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Properties and States of Matter
Objectives
• Describe the two properties of all matter.
• Describe the difference between a pure substance and a mixture.
• Define physical properties.
• Define chemical properties.
• Explain how matter is organized.
Chapter 3 Section 1 Properties of Matter
What is Matter?
• Matter has mass and takes up space.–Everything you can see in the universe is matter.
• Atoms are the Building Blocks of Matter •All matter is made from particles called atoms. •Atom is the smallest unit of matter that has unique properties.
Chapter 3 Section 1 Properties of Matter
Flow Chart Of MatterMATTER
PURE SUBSTANCEMIXTURE
ELEMENT
HOMOGENEOUSHETEROGENEOUS
COMPOUND
physical change
chemical change
solutions
Pure Substances
• A pure substance consists of one type of atom or one type of molecule.
•A pure substance may be an element or a compound.•A molecule is not necessarily a compound.
Chapter 3 Section 1 Properties of Matter
Pure Substances, continued
• Elements: A Single Type of Atom •Elements cannot be broken down chemically or physically. •An element is a single kind of atom.
• There are more than 100 different elements.
• Three Major Categories of Elements•Metals•Metalloids•Non-metals
Chapter 3 Section 1 Properties of Matter
Chapter 3 Section 1 Properties of Matter
Pure Substances, continued
• Molecules & Compounds• A Molecule is two or more atoms joined by
chemical bonds•A molecule has a fixed composition•all of its molecules have the same atoms in the same proportion.
• A compound is a molecule of two or more different atoms joined by chemical bonds.
Chapter 3 Section 1 Properties of Matter
Chapter 3 Section 1 Properties of Matter
Mixtures
• A mixture contains two or more pure substances.•A homogeneous mixture is uniform throughout, such as apple juice. •A heterogeneous mixture is not uniformly mixed, such as salad dressing.
• A mixture can be separated with physical methods
Chapter 3 Section 1 Properties of Matter
Mixtures, continued
• A Solution is a mixture that appears to be a single substance.
•The particles are too small to be affected by gravity and do not separate.
•Salt water•Many solutions are liquids, but may also be a gas or solid.
•air
Chapter 3 Section 1 Properties of Matter
Mixtures, continued
• Suspensions •A mixture where the particles eventually settle out. •May be gas or liquid.
• Colloids •A mixture that has particles larger than a solution•Particles do not settle out. •May be solid, liquid, or gas.
Chapter 3 Section 1 Properties of Matter
Identifying Matter with Physical Properties
• A physical property is a characteristic of a substance that can be observed or measured.
• Examples are mass, density, color, hardness, melting point, boiling point.
Chapter 3 Section 1 Properties of Matter
Identifying Matter with Physical Properties, continued
• Mass and Weight •The amount of matter in an object is called mass. •Mass is constant at any place in the universe, because the amount of matter does not change.
Chapter 3 Section 1 Properties of Matter
Physical States of Matter
Solid LiquidGas
Plasma
Solid
Particles are tightly compactParticles vibrate without the ability to move freelyDefinite shape and volumeSolid Animation
Liquid
Particles are tightly compact, but able to move around close to each otherNo definite shape, but definite volumeLiquid Animation
Gas
Particles can easily spread out or move close togetherParticle move freely and with a lot of energyNo definite shape or volumeGas Simulation
PlasmaExist at extremely high temperatures (several million degrees Celsius)Particles are broken apartParticles move freely and with extremely high energyThis form is not too common on earth, however it is the most common form of matter in the universeNo definite shape or volume?Examples: Florescent and neon lights, lightning, aurora borealis
Why do you think this is the most common
form/state of matter in the universe?
Energy and the States of Matter
The physical states of matter result from the amount of energy the particles composing the matter have. Basically, more energy means more movement for the particles and less energy means less movement. Energy/Temperature and Matter
If you were to compare an ice cube and the steam created from boiling water, which would you think has more energy?
Properties of MatterChemical Property
Any property of matter that describes a substance based on its ability to change into a new substanceExamples
flammabilityreactivity with vinegarreactivity with oxygen
Iron + Oxygen Iron oxide (rust)2Fe + 3O2 Fe2O3
Chemical or Physical Property?
1. Paper is white
2. Boiling point of H2O is 100oC
3. Zinc reacts with hydrochloric acid and creates hydrogen gas
4. Nitrogen does not burn
5. Sulfur smells like rotten eggs
Chemical Property
Chemical Property
Physical Property
Physical Property
Physical Property
Comparing Physical and Chemical Properties
Substance/Matter Physical Property Chemical Property
Helium Less dense than air Nonflammable
Wood Grainy texture Flammable
Baking soda White powder Reacts with vinegar to produce bubbles
Powdered sugar White powder Does not react with vinegar
Rubbing alcohol Clear liquid Flammable
Red food coloring Red color Reacts with bleach and loses color
Iron Malleable Reacts with oxygen
Changes in MatterPhysical Change
a change in shape, size, color, or statea change without a change in chemical compositiona change that is reversibleThe Mixtures LabExamples
tearing paper cutting your hair change in state
Changes in States(Physical Changes)
Melting
Vaporization
(Evaporation/Boiling)
Freezing
Condensation
All changes in state require a change in energy
Sublimation
Solid
Liquid
Gas
PlasmaDisposition
Liquid
Gas
Plasma
Liquid
Gas
All changes in state require a change in energy
Plasma
Liquid
Gas
States of Matter Simulation
Simulation 1
Simulation 2
This is what happens when energy is added and taken away
Changes in MatterChemical Change
a change in which a substance becomes another substance having different propertiesa change that is not reversible using ordinary physical means Changes that usually cause heat, sound, light, odor, fizzing/foaming, color changes
You usually need more than one of the above characteristics to be considered a chemical
change!
Examplescombining sulfuric acid and sugar
burning a piece of woodsoured milk
Chemical or Physical Change?
1. Bending a Paper Clip
2. Baking a cake
3. The sublimation of carbon dioxide
4. Crushing an aluminum can
5. Vinegar and baking soda combining to create salt and water
Chemical Change
Chemical Change
Physical Change
Physical Change
Physical Change
Section 1 Properties of MatterChapter 3
Section 2 Objectives
• Define the law of conservation of mass.
• Describe the difference between physical and chemical changes.
• Explain why some changes are reversible and some are not.
Chapter 3Section 2 Physical and Chemical Changes
Conservation of Mass
• Mass is not created or destroyed in ordinary chemical or physical changes.
• In ordinary physical or chemical changes, the amount of matter, which is called mass, does not change.
Chapter 3Section 2 Physical and Chemical Changes
Conservation of Mass Lab
1. Weigh a clean, dry cup: _________2. Add a small amount of vinegar and re-weigh: ____3. Amount of Vinegar = (#2 - #1) = ______________4. Weigh a 2nd clean, dry cup:_________5. Add a small amount of baking soda and re-
weigh:_______6. Amount of Baking soda = (#5 - #4) = __________7. Total Mass of reactants: (#6 + #3) = __________8. SLOWLY add the baking soda to the vinegar. If it
overflows, you have to start over.9. Weigh the resulting mixture and cup: _______10.Total Mass of Products (#9 - #1)= ___________11.Was Conservation of Mass upheld? Does #10 =
#7? Explain why or why not.
Physical Changes in Our World
• A physical change is any change in which the properties of a substance, but not the identity of the substance, change.
• The next slide shows the physical changes that occur when sulfur and salt are separated.
Chapter 3Section 2 Physical and Chemical Changes
Chapter 3Section 2 Physical and Chemical Changes
Physical Changes in Our World, continued
• Physical Changes in Nature •Movement of soil and rock •Ponds freezing•Water freezing or melting
• Physical Changes in Industry •Making sugar •Building furniture
Chapter 3Section 2 Physical and Chemical Changes
Chemical Change in Our World
• A chemical change occurs when new substances are formed
•Different identity •Different physical properties.
• A Chemical Change producing new substances are also called chemical reactions.
Chapter 3Section 2 Physical and Chemical Changes
Chemical Change in Our World, continued
• Chemical Changes in Nature •Photosynthesis •Digestion.
• Physical Changes in Industry •Making metal •Refining oil for gasoline.
Chapter 3Section 2 Physical and Chemical Changes
Are Physical and Chemical Changes Reversible?
• Most physical changes are reversible •Physical changes only affect the matter’s form.
• Most chemical changes are not reversible.
Chapter 3Section 2 Physical and Chemical Changes
Section 3 Objectives
• Explain why particles in matter are always in motion.
• Compare the properties of solids, liquids, and gases.
• Explain the behavior of gases.
• Describe plasma.
Chapter 3 Section 3 States of Matter
Particles of Matter in Motion
• There are movements in matter that are too small to see or feel.
• Particles in matter are always in motion because particles have energy.
Chapter 3 Section 3 States of Matter
Particles of Matter in Motion, continued
• States of Matter Determined by Particle Energy The more energy a particle has, the faster it moves.
• Particle energy and movement determines the physical forms of matter, or the states of matter.
• Four states of matter are solid, liquid, gas, and plasma.
•They are physically different because their particles have different amounts of energy.
Chapter 3 Section 3 States of Matter
Chapter 3 Section 3 States of Matter
Physical Differences Between States of Matter
• Solids Have Rigid Structure •Particles are fixed into place
• water molecules in ice. •Does not change shape or size.
• Temperature measures the energy of the particles. •The temperature at which a solid change to liquid is called its melting point.
Chapter 3 Section 3 States of Matter
Physical Differences Between States of Matter, continued
• Liquids •A liquid assumes the shape of its container. •Molecules are in contact with each other, but are not held rigidly in place.
• A liquid has a definite volume but no definite shape.
Chapter 3 Section 3 States of Matter
Physical Differences Between States of Matter, continued
• Gas •The particles of matter have enough energy to escape their attraction to each other. •Due to their high energy and rapid motion, particles of a gas fill whatever volume is available.
• A gas has no definite shape and no definite volume.
Chapter 3 Section 3 States of Matter
Physical Differences Between States of Matter, continued
• Changing from One State to Another •Changes occur when energy is added to or removed from a substance.
• The change from a liquid to a gas is called evaporation or boiling.
•Energy is added to the liquid to cause its molecules to escape the attraction to one another.
Chapter 3 Section 3 States of Matter
Physical Differences Between States of Matter, continued
• When a gas is cooled, attractions between the particles becomes stronger and the gas condenses into a liquid.
• When a liquid changes to a solid, it freezes. The liquid cools enough for attractions between the particles to lock the particles into fixed positions.
Chapter 3 Section 3 States of Matter
Section 3 States of MatterChapter 3
Solid, Liquid and Gas
Behavior of Gases
• The volume of a gas is the amount of space taken up by the gas particles in a container.
• Temperature Heat causes a gas to expand because the molecules have more energy. Cold causes the gas to contract because the molecules move slower.
Chapter 3 Section 3 States of Matter
Behavior of Gases, continued
• Volume The volume of a gas depends on the container that holds the gas.
• Pressure measures the amount of force exerted per unit area of a surface. When air particles collide within a container, they exert more pressure.
• In the next slide, the beach ball has less pressure because it has fewer gas particles.
Chapter 3 Section 3 States of Matter
Chapter 3 Section 3 States of Matter
Plasma: A Fourth State of Matter
• Plasma is a state of matter that starts as a gas and then becomes ionized. Its properties differ from those of a solid, liquid, or gas.
• Plasma is created when energy is added to a gas. Plasma is similar to a gas in that it has no fixed shape, but it is different in that it conducts electric current and is attracted to magnetic fields.
Chapter 3 Section 3 States of Matter
Concept Mapping
Chapter 3 Properties and States of Matter
Use the terms below to complete the concept map on the next slide.
changes of state
melting
evaporating
solid
liquid
condensing
chemical formulas
Chapter 3 Properties and States of Matter
Chapter 3 Properties and States of Matter
End of Chapter 3 Show
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