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Chapter 2 Note-Packet
Introduction to Matter
Section 1
Chapter 2 Chapter 2 NotesNotes
Anything that has mass and takes
up space
Matter
The study of properties of
matter and how matter changes
Chemistry
A single kind of matter that is pure
Substance
The same composition and
properties
Always has
Physical properties
Chemical properties
Matter has two kinds of properties
Chapter 2 Chapter 2 NotesNotes
Characteristic of a pure substance that can be seen without
changing it into another substance
Physical property
Liquid water freezing into ice
Example
Characteristic of a pure substance that
describes its ability to change into different
substances
Chemical property
Iron combines with oxygen to
form rust
Example
Properties of Matter
Can be used to classify matter
Chapter 2 Chapter 2 NotesNotes
Pure substance that cannot be broken
down into any other substance by
chemical or physical means
Element Elements are the simplest substance!
The basic particle from which all elements are
madeAtoms
A chemical bond forms- a force of
attraction between the two atoms
When atoms combine
Group of 2 or more atoms held
together by a chemical bond
Molecules
Two Hydrogen atoms and one Oxygen atom forms water
Example
Chapter 2 Chapter 2 NotesNotes
Pure substance made of two or more different elements
chemically combined in a set ratio
Compounds
Shows the elements in a
compound and the ratio of atoms
Chemical Formula
CO2The ratio of
Carbon to Oxygen is 1:2
Chemical Formula
COA different ratio
equals a different compound
Elements that are chemically combined
have different properties from the uncombined
elements
Chapter 2 Chapter 2 NotesNotes
A mix of two or more substances that retain their own properties
MixtureContrast
Compounds- The combined elements change their properties.
Mixtures- The combined elements keep their properties.
Mixture where you cannot see the different parts
Mixture where you can see the
different parts
Heterogeneous Homogeneous
Dissolved sugar in water
Salad in a bowl
A homogeneous mixture is called a
solution
Examples
Section 2
The measure of the force of
gravity on you
WeightThe measure of the amount of matter in an
object
Mass
Does not change with location
The amount of space that matter
occupies
Volume The mass of a material in a given
volume
Density
Volume = Length x Width x Height
Liter (L), milliliter (mL) and cubic
centimeter (cm3)
Density = Mass
Volume
Relates to
Units
Formula
Formula
g / cm3
Units
Grams (g)
Units
Section 3
When a substance changes, but is still the same substance
after the change
Physical Change
When a substance changes into a new
substance with properties different from
the original
Chemical Change
Changes of state
Changes of shape or form
Combination of fuel with oxygen
Using electricity to break down compounds
Combination of substance with
oxygen
Combining metals with substances,
producing dark coat on metal
Combustion
Electrolysis
Oxidation Tarnishing
A change in matter that produces one
or more new substances
Chemical Reactions
Chemical changes occur when bonds
break and new bonds form
Evidence for chemical
Reactions, or changes
A color change may signal that a chemical change
has occurred
Changes in Color
A solid that forms from solution during a chemical reaction
is a precipitate
Precipitate may form
If a chemical change occurs from liquids or solids, a
gas may form
A gas may form
The next video shows a color change, and a
precipitate!
The ability to do work or cause
change
Energy
Chemical or physical changes in matter includes a change in energy
The average energy from the
random motion of matter particles
The total energy of all the particles
in an object
Temperature Thermal Energy Always flows from hot to cold
Change in which energy is taken in
Change in which energy is released
Endothermic Change Exothermic Change
Law of Conservation of
Mass
Matter cannot be created or destroyed
Matter can only be changed!
All the atoms present at the start
of a reaction are present at the end
In a chemical reaction, the total mass of the
reactants must equal the total mass of the
products
+
Iron (6 atoms) Sulfur (6 atoms) Iron Sulfide (12 atoms)
Section 4
The energy of matter in motion
Kinetic Energy
The energy an object has because
of its position
Potential Energy
Energy stored in chemical bonds
Chemical Energy
Energy form that travels through space as waves
Electromagnetic Energy Energy of electrically charged
particles moving from one place to
another
Electric Energy
Forms of Energy
Chemical energy may be changed to other forms of energy. Other forms of energy may also be changed to chemical energy!
Chapter 2 Chapter 2 NotesNotes
Matter
Chemistry
Substance
Always has
Matter has two kinds of properties
Chapter 2 Chapter 2 NotesNotes
Physical property
Example
Chemical property
Example
Properties of Matter
Chapter 2 Chapter 2 NotesNotesElement Elements are the
simplest substance!
Atoms
When atoms combine
Molecules
Example
Chapter 2 Chapter 2 NotesNotesCompounds Chemical Formula
CO2
Chemical Formula
CO
Chapter 2 Chapter 2 NotesNotesMixture
Contrast
Compounds- _________________________________________________________________________________________________________________
Mixtures- ______________________________________________________
Heterogeneous
Homogeneous
Examples
Weight Mass
Volume
Density
Relates to
Units
Formula
Formula
Units
Units
Physical Change Chemical Change
Combustion
Electrolysis
Oxidation Tarnishing
Chemical Reactions
Evidence for chemical
Reactions, or changes
Changes in Color
Precipitate may form
A gas may form
Energy
Temperature Thermal Energy
Endothermic Change Exothermic Change
+
__________________ __________________ __________________________
Kinetic Energy Potential Energy
Chemical Energy Electromagnetic Energy
Electric Energy
Forms of Energy
________________________________________________________________________________________________________________________________________________________________________________________________________________________________________
