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2 DIVERSITY OF MATTER
Eclipse (Pink Floyd ndashThe Dark side of the Moon)
All that you touchAll that you seeAll that you tasteAll you feelAll that you loveAll that you hateAll you distrustAll you saveAll that you giveAll that you dealAll that you buybeg borrow or steal
All you createAll you destroyAll that you doAll that you sayAll that you eateveryone you meetAll that you slighteveryone you fightAll that is nowAll that is goneAll thats to comeAnd everything under the sun is in tune ()But the sun is eclipsed by the moon
And is made of MATTER
hellipMatter is anything that occupies space
hellipMatter is anything that occupies space
States of Matter
The Four States of Matter
SolidLiquidGasPlasma
4
States of Matter
The Four States of Matter
We assume the KINETIC THEORY OF MATTER that all matter is made of tiny particles always in motion
Basis of Classification of the Four TypesBased upon particle arrangementBased upon energy of particlesBased upon distance between particles
5
States of Matter
Solids Particles of solids are tightly packed vibrating
about a fixed position Solids have a definite shape and a definite
volume Solids have an infinite number of free surfaces
6
States of MatterMicroscopic Explanation for Properties of
Solids
Solids have a definite shape and a definite volumebecause the particles are locked into place
Solids are not easily compressible because there is little free space between particles
Solids do not flow easily because the particles cannot moveslide past one another
7
States of Matter Liquids
Particles of liquids are tightly packed but are far enough apart to slide over one another
Liquids have an indefinite shape and a definite volume
Liquids have one free surface
8
States of MatterMicroscopic Explanation for Properties of
Liquids
Liquids have an indefinite shape because the particles can slide past one another
Liquids are not easily compressible and have a definite volume because there is little free space between particles
Liquids flow easily because the particles can moveslide past one another
9
States of Matter Gases
Particles of gases are very far apart and move freely Gases have an indefinite shape and an indefinite
volume Gases have no free surfaces
10
Microscopic Explanation for Properties of Gases
Gases have an indefinite shape and an indefinite volume because the particles can move past one another
Gases are easily compressible because there is a great deal of free space between particles
Gases flow very easily because the particles randomly move past one another
11
States of Matter
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Eclipse (Pink Floyd ndashThe Dark side of the Moon)
All that you touchAll that you seeAll that you tasteAll you feelAll that you loveAll that you hateAll you distrustAll you saveAll that you giveAll that you dealAll that you buybeg borrow or steal
All you createAll you destroyAll that you doAll that you sayAll that you eateveryone you meetAll that you slighteveryone you fightAll that is nowAll that is goneAll thats to comeAnd everything under the sun is in tune ()But the sun is eclipsed by the moon
And is made of MATTER
hellipMatter is anything that occupies space
hellipMatter is anything that occupies space
States of Matter
The Four States of Matter
SolidLiquidGasPlasma
4
States of Matter
The Four States of Matter
We assume the KINETIC THEORY OF MATTER that all matter is made of tiny particles always in motion
Basis of Classification of the Four TypesBased upon particle arrangementBased upon energy of particlesBased upon distance between particles
5
States of Matter
Solids Particles of solids are tightly packed vibrating
about a fixed position Solids have a definite shape and a definite
volume Solids have an infinite number of free surfaces
6
States of MatterMicroscopic Explanation for Properties of
Solids
Solids have a definite shape and a definite volumebecause the particles are locked into place
Solids are not easily compressible because there is little free space between particles
Solids do not flow easily because the particles cannot moveslide past one another
7
States of Matter Liquids
Particles of liquids are tightly packed but are far enough apart to slide over one another
Liquids have an indefinite shape and a definite volume
Liquids have one free surface
8
States of MatterMicroscopic Explanation for Properties of
Liquids
Liquids have an indefinite shape because the particles can slide past one another
Liquids are not easily compressible and have a definite volume because there is little free space between particles
Liquids flow easily because the particles can moveslide past one another
9
States of Matter Gases
Particles of gases are very far apart and move freely Gases have an indefinite shape and an indefinite
volume Gases have no free surfaces
10
Microscopic Explanation for Properties of Gases
Gases have an indefinite shape and an indefinite volume because the particles can move past one another
Gases are easily compressible because there is a great deal of free space between particles
Gases flow very easily because the particles randomly move past one another
11
States of Matter
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
hellipMatter is anything that occupies space
hellipMatter is anything that occupies space
States of Matter
The Four States of Matter
SolidLiquidGasPlasma
4
States of Matter
The Four States of Matter
We assume the KINETIC THEORY OF MATTER that all matter is made of tiny particles always in motion
Basis of Classification of the Four TypesBased upon particle arrangementBased upon energy of particlesBased upon distance between particles
5
States of Matter
Solids Particles of solids are tightly packed vibrating
about a fixed position Solids have a definite shape and a definite
volume Solids have an infinite number of free surfaces
6
States of MatterMicroscopic Explanation for Properties of
Solids
Solids have a definite shape and a definite volumebecause the particles are locked into place
Solids are not easily compressible because there is little free space between particles
Solids do not flow easily because the particles cannot moveslide past one another
7
States of Matter Liquids
Particles of liquids are tightly packed but are far enough apart to slide over one another
Liquids have an indefinite shape and a definite volume
Liquids have one free surface
8
States of MatterMicroscopic Explanation for Properties of
Liquids
Liquids have an indefinite shape because the particles can slide past one another
Liquids are not easily compressible and have a definite volume because there is little free space between particles
Liquids flow easily because the particles can moveslide past one another
9
States of Matter Gases
Particles of gases are very far apart and move freely Gases have an indefinite shape and an indefinite
volume Gases have no free surfaces
10
Microscopic Explanation for Properties of Gases
Gases have an indefinite shape and an indefinite volume because the particles can move past one another
Gases are easily compressible because there is a great deal of free space between particles
Gases flow very easily because the particles randomly move past one another
11
States of Matter
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
States of Matter
The Four States of Matter
SolidLiquidGasPlasma
4
States of Matter
The Four States of Matter
We assume the KINETIC THEORY OF MATTER that all matter is made of tiny particles always in motion
Basis of Classification of the Four TypesBased upon particle arrangementBased upon energy of particlesBased upon distance between particles
5
States of Matter
Solids Particles of solids are tightly packed vibrating
about a fixed position Solids have a definite shape and a definite
volume Solids have an infinite number of free surfaces
6
States of MatterMicroscopic Explanation for Properties of
Solids
Solids have a definite shape and a definite volumebecause the particles are locked into place
Solids are not easily compressible because there is little free space between particles
Solids do not flow easily because the particles cannot moveslide past one another
7
States of Matter Liquids
Particles of liquids are tightly packed but are far enough apart to slide over one another
Liquids have an indefinite shape and a definite volume
Liquids have one free surface
8
States of MatterMicroscopic Explanation for Properties of
Liquids
Liquids have an indefinite shape because the particles can slide past one another
Liquids are not easily compressible and have a definite volume because there is little free space between particles
Liquids flow easily because the particles can moveslide past one another
9
States of Matter Gases
Particles of gases are very far apart and move freely Gases have an indefinite shape and an indefinite
volume Gases have no free surfaces
10
Microscopic Explanation for Properties of Gases
Gases have an indefinite shape and an indefinite volume because the particles can move past one another
Gases are easily compressible because there is a great deal of free space between particles
Gases flow very easily because the particles randomly move past one another
11
States of Matter
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
States of Matter
The Four States of Matter
We assume the KINETIC THEORY OF MATTER that all matter is made of tiny particles always in motion
Basis of Classification of the Four TypesBased upon particle arrangementBased upon energy of particlesBased upon distance between particles
5
States of Matter
Solids Particles of solids are tightly packed vibrating
about a fixed position Solids have a definite shape and a definite
volume Solids have an infinite number of free surfaces
6
States of MatterMicroscopic Explanation for Properties of
Solids
Solids have a definite shape and a definite volumebecause the particles are locked into place
Solids are not easily compressible because there is little free space between particles
Solids do not flow easily because the particles cannot moveslide past one another
7
States of Matter Liquids
Particles of liquids are tightly packed but are far enough apart to slide over one another
Liquids have an indefinite shape and a definite volume
Liquids have one free surface
8
States of MatterMicroscopic Explanation for Properties of
Liquids
Liquids have an indefinite shape because the particles can slide past one another
Liquids are not easily compressible and have a definite volume because there is little free space between particles
Liquids flow easily because the particles can moveslide past one another
9
States of Matter Gases
Particles of gases are very far apart and move freely Gases have an indefinite shape and an indefinite
volume Gases have no free surfaces
10
Microscopic Explanation for Properties of Gases
Gases have an indefinite shape and an indefinite volume because the particles can move past one another
Gases are easily compressible because there is a great deal of free space between particles
Gases flow very easily because the particles randomly move past one another
11
States of Matter
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
States of Matter
Solids Particles of solids are tightly packed vibrating
about a fixed position Solids have a definite shape and a definite
volume Solids have an infinite number of free surfaces
6
States of MatterMicroscopic Explanation for Properties of
Solids
Solids have a definite shape and a definite volumebecause the particles are locked into place
Solids are not easily compressible because there is little free space between particles
Solids do not flow easily because the particles cannot moveslide past one another
7
States of Matter Liquids
Particles of liquids are tightly packed but are far enough apart to slide over one another
Liquids have an indefinite shape and a definite volume
Liquids have one free surface
8
States of MatterMicroscopic Explanation for Properties of
Liquids
Liquids have an indefinite shape because the particles can slide past one another
Liquids are not easily compressible and have a definite volume because there is little free space between particles
Liquids flow easily because the particles can moveslide past one another
9
States of Matter Gases
Particles of gases are very far apart and move freely Gases have an indefinite shape and an indefinite
volume Gases have no free surfaces
10
Microscopic Explanation for Properties of Gases
Gases have an indefinite shape and an indefinite volume because the particles can move past one another
Gases are easily compressible because there is a great deal of free space between particles
Gases flow very easily because the particles randomly move past one another
11
States of Matter
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
States of MatterMicroscopic Explanation for Properties of
Solids
Solids have a definite shape and a definite volumebecause the particles are locked into place
Solids are not easily compressible because there is little free space between particles
Solids do not flow easily because the particles cannot moveslide past one another
7
States of Matter Liquids
Particles of liquids are tightly packed but are far enough apart to slide over one another
Liquids have an indefinite shape and a definite volume
Liquids have one free surface
8
States of MatterMicroscopic Explanation for Properties of
Liquids
Liquids have an indefinite shape because the particles can slide past one another
Liquids are not easily compressible and have a definite volume because there is little free space between particles
Liquids flow easily because the particles can moveslide past one another
9
States of Matter Gases
Particles of gases are very far apart and move freely Gases have an indefinite shape and an indefinite
volume Gases have no free surfaces
10
Microscopic Explanation for Properties of Gases
Gases have an indefinite shape and an indefinite volume because the particles can move past one another
Gases are easily compressible because there is a great deal of free space between particles
Gases flow very easily because the particles randomly move past one another
11
States of Matter
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
States of Matter Liquids
Particles of liquids are tightly packed but are far enough apart to slide over one another
Liquids have an indefinite shape and a definite volume
Liquids have one free surface
8
States of MatterMicroscopic Explanation for Properties of
Liquids
Liquids have an indefinite shape because the particles can slide past one another
Liquids are not easily compressible and have a definite volume because there is little free space between particles
Liquids flow easily because the particles can moveslide past one another
9
States of Matter Gases
Particles of gases are very far apart and move freely Gases have an indefinite shape and an indefinite
volume Gases have no free surfaces
10
Microscopic Explanation for Properties of Gases
Gases have an indefinite shape and an indefinite volume because the particles can move past one another
Gases are easily compressible because there is a great deal of free space between particles
Gases flow very easily because the particles randomly move past one another
11
States of Matter
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
States of MatterMicroscopic Explanation for Properties of
Liquids
Liquids have an indefinite shape because the particles can slide past one another
Liquids are not easily compressible and have a definite volume because there is little free space between particles
Liquids flow easily because the particles can moveslide past one another
9
States of Matter Gases
Particles of gases are very far apart and move freely Gases have an indefinite shape and an indefinite
volume Gases have no free surfaces
10
Microscopic Explanation for Properties of Gases
Gases have an indefinite shape and an indefinite volume because the particles can move past one another
Gases are easily compressible because there is a great deal of free space between particles
Gases flow very easily because the particles randomly move past one another
11
States of Matter
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
States of Matter Gases
Particles of gases are very far apart and move freely Gases have an indefinite shape and an indefinite
volume Gases have no free surfaces
10
Microscopic Explanation for Properties of Gases
Gases have an indefinite shape and an indefinite volume because the particles can move past one another
Gases are easily compressible because there is a great deal of free space between particles
Gases flow very easily because the particles randomly move past one another
11
States of Matter
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Microscopic Explanation for Properties of Gases
Gases have an indefinite shape and an indefinite volume because the particles can move past one another
Gases are easily compressible because there is a great deal of free space between particles
Gases flow very easily because the particles randomly move past one another
11
States of Matter
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
States of MatterPlasma
A plasma is an ionized gas at very high temperature
A plasma is a very good conductor of electricity and is affected by magnetic fields
It is by far the most common form of matter Plasma in the stars and in the tenuous space between them makes up over 99 of the visible universe and perhaps most of that which is not visible
12
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
States of Matter
13
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
States of MatterMicroscopic Explanation for Properties of
Plasmas
Plasmas have an indefinite shape and an indefinite volume because the particles can move past one another
Plasmas are easily compressible because there is a great deal of free space between particles
Plasmas are good conductors of electricity and are affected by magnetic fields because they are composed of ions (negatively charged electrons and positively charged nuclei)
14
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
States of Matter The Four States of
MatterThe Classification and Properties of
Matter Depend Upon Microscopic Structure
Particle arrangement Particle energy Particle to particle distance 15
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Gases Solids and Liquids
Phase
Particle Properties
Spacing Energy Motion Volume Shape
Solid
Liquid
Gas
close low vibrational definite definite
close moderate rotational definite indefinite
far apart high translational indefinite indefinite
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Physical properties are those that we can measure without changing the identity of the substance we are studying
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
The physical properties can be observed or measured
Hardness color melting point and density are all physical properties
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Intensive properties do not depend on the size of the sample of matter and can be used to identify substances
density color melting and boiling point hellip
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Extensive properties depend on the quantity of the sample
mass area volume hellip
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
All matter regardless of state undergoes physical and chemical changes
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
A physical change occurs when the substance changes state but does not change its chemical composition
For example
bullwater freezing into icebullcutting a piece of wood into smaller piecesbullbreaking a paper
The form or appearance has changed but the physical properties of that substance are the same
Melting point Density Boiling point Color Vapor pressure Electrical conductivity Solubility Hardnesshelliphellip
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Chemical properties describe the way a substance can change or react to form other substances These properties then must be determined using a process that changes the identity of the substance of interest
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
A chemical change occurs when a substance changes into something new
This occurs due to heating chemical reaction etc You can tell a chemical change has occurred if the density melting point or freezing point of the original substance changes Many common signs of a chemical change can be seen (bubbles forming mass or colour changed etc)
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Mixtures are two or more substances that are NOT chemically combined
Mixtures do not
middot Have constant boiling points
middot Have constant melting points
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Variable compositionComponents retain their
characteristic propertiesMay be separated into pure
substances by physical methodsMixtures of different
compositions may have widely different properties
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Heterogeneous mixtures are composed of large pieces that are easily separated by physical means (ie density polarity metallic properties)
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Do not have same composition throughout
Components are distinguishableExamples fruit salad vegetable soup wood granite etc
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Solutions are homogenous Therefore they are easily separated by physical methods like distillation or evaporation
Examples
bull Sugar water
bull Stainless steel
bull Salt water
bull Wine
bull Brass
bull Air
bull Cola drink
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Separating Mixtures
Dirty water
Oil and Water
Saltwater
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
SettlingDensity causes
parts of the mixture to settle to the bottom
This process is used during water filtration Contaminants sink and clearer water is skimmed off
31
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Filtration
A mixture is passed through material with many holes Anything larger than the hole is trapped while the rest of the mixture passes through
Examples Dirty water lab Precipitation lab
32
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
CrystallizationThe separation
process in which the solvent is evaporated leaving crystals of solute behind Examples
Rock candy Saltwater lab
33
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
DistillationThe separation process in which the desired
component is evaporated from the solution and collected
Water is boiled and the steam is collected As the steam cools it condenses to form pure water and anything that was dissolved in the water is left behind
34
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
ChromatographyThis process is mostly
used to identify substances
As the substance is drawn up the material (eg filter paper) it carries the solutes with it
The least dense are drawn farthest up the filter paper
Example Chromatography lab- green
plant pigment
35
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
A substance is matter of a particular kind
A substance cannot be further broken down or purified by physical means
Each substance has its own characteristic properties that are different from the set of properties of any other substance
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Fixed composition
Properties do not vary
Cannot be separated into simpler substances by physical methods (physical changes)
Can only be changed in identity and properties by chemical methods
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Compounds
Can be decomposed into simpler substances by chemical changes always in a definite ratio
Water Sugar Salt Ammonia Propane
Elements
Cannot be decomposed into simpler substances by chemical changes
Gold Iron Sulfur Oxygen Chlorine
Water always contains 889 oxygen and 111 hydrogen
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
HOMOGENEOUS HETEROGENEOUS
SOLUTION
COMPOUND ELEMENT
HAS IT UNIFORM PROPERTIES
YES NO MIXTURE
Has it always the same composition and properties
YES PURE SUBSTANCENO MIXTURE
Can it be broken down into a simpler substance by a chemical reaction
YES NOSpring waterBronzeAirBleachCoca-Cola
Water SugarSulfuric acidSalt
GoldOxygeneCopper
MATERIAL SYSTEM
Wood GraniteHamburgerPencil
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Solutions
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
DefinitionsA solution is a homogeneous mixture
A solute is dissolved in a solvent Solute is present in the smaller amount
The solvent is present in the larger amount
an aqueous solution has water as solvent
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Solutions
Solute
Solvent
When the solvent is water the solution is said to be aqueous
a homogenous mixture of 2 or more substances
the substance present in the larger amount
is(are) the substance(s) present in the smaller amount(s)
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Types of solutions
1048708 Gases Gases dissolved in gases (air) Liquids dissolved in gases (humid air) Solids dissolved in gases (moth balls )
1048708 Liquids Gases in liquids (air dissolved in water) Liquids in liquids (ethanol in water) Solids in Liquids (salt in water)
1048708 Solids Gases in solids (H2 in Pt) Liquids in solids (HgAg amalgam) Solids in solids (Cr in Fe alloy)
() bolas antipolilla
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Terminology
Solubility The maximum amount of solute that will dissolve in a solvent
Dilute A solution that contains relatively little solute
Concentrated A solution that contains a relatively large amount of solute
Saturated is one where the concentration is at a maximum - no more solute is able to dissolve
Supersaturated A solution that contains more than the solubility limit
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
ConcentrationConcentration is the amount of solute in a given amount of either solution or solvent
100)( xsolutionmasssolutemass
ww
100)( xsolutionvolumesolutevolume
vv
solutionofliterssoluteofgrams
Lg
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Factors Affecting Solubility
1 Nature of Solute Solvent
- Like dissolves like
2 Temperature -SolidsLiquids- Solubility increases with TemperatureGases - Solubility decreases with Temperature
3 Pressure Factor -SolidsLiquids - Very little effectGas - Solubility increases with Pressure
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Solubilities of Solids vs Temperature
Solubilities of Gases vs Temperature
Solubilities of Gases vs Temperature
