CHAPTER 1 & 2
Chemistry
Matter & Change
CHEMISTRY
STUDY OF COMPOSITION AND BEHAVIOR OF MATTER
“What stuff is made of and how it acts”
Organic Chemistry:
Study of carbon compounds
Inorganic Chemistry: Study of non carbon compounds
Analytical Chemistry: Study of composition of substances
Physical Chemistry:
Study of behavior of substances
Biochemistry:
Study of the chemistry of living things
How Chemistry is Used

Pure Chemistry:
Knowledge for knowledge’s sake. Research to
learn how something works. May lead to and
application.
Ex: Research for synthetic rubber 1940’s
o Applied Chemistry
Research directed to a specific goal or
application.
Ex: Silly Putty 1950’s
Scientific Method

Systematic problem solving approach
 Observations
Noticing a problem (car won’t start)
• Hypothesis (battery dead)
Possible explanation
• Experiment
Procedure used to test the hypothesis (jump start?)
Manipulated Variable – Independent Variable
Variable you change during an experiment.
Responding Variable- Dependent Variable
Variable you observe during the experiment
Scientific Method Continued
THEORY:
Tested model that explains WHY an
experiment gives certain results.
Ex: Atomic Theory
LAW:
Model of atom has changed
over time.
Statement that summarizes the results of many
observations and experiments. Can be proven
and usually is an equation.
Ex: Law of Gravity (objects fall at a rate of 9.8
meters per second)
PROPERTIES OF MATTER
MATTER: Anything that has mass and takes up space
MASS: Amount of substance and object contains
WEIGHT:
Earth’s attraction for an object
GRAVITY
VOLUME: Amount of space an object takes up
PHYSICAL PROPERTY
•QUALITY OF A SUBSTANCE that can be analyzed
without changing the composition of the substance,
Ex: color, odor, density, MP, BP, conductivity
CHEMICAL PROPERTY
• ability of a substance to undergo a chemical reaction
and form new substances
Ex: sodium explodes in water,
iron nail rusts, wood burns
Changes in Matter
Change in a substance that does
Physical Change: not change composition. Same
substance in the beginning and end.
Ex: cutting, grinding, tearing, painting, phase change
Chemical Change
Change in the composition of a substance.
Different substance in the end.
Ex: burning, rusting, chemical reactions
Demo: SUGAR + WATER
REACTANTS
C12H22O11
+
YIELD
H2O
PRODUCTS
 C12H22O11 + H2O
STARTING AND ENDING MATERIALS ARE THE SAME:
PHYSICAL CHANGE
DEMO: SUGAR + SULFURIC ACID
REACTANTS
YIELD
PRODUCTS
C12H22O11 + H2SO4  12 C + SO3 +12 H2O
STARTING AND ENDING MATERIALS ARE DIFFERENT:
CHEMICAL CHANGE
INDICATORS OF A CHEMICAL CHANGE
COLOR CHANGE
ODOR CHANGE
ENERGY CHANGE
FORMATION OF A GAS
FORMATION OF A
PRECIPITATE- (solid
formed from 2 aqueous
solutions)
NOT EASILY REVERSED
What’s happening during a
chemical reaction?
Only the OUTER SHELL ELECTRONS called
(Valence Electrons) of atoms are involved.
atoms Combine, break away or rearrange
Law of Conservation of Mass
Matter is not created or destroyed.
Mass reactants = Mass of products
Energy Changes
Both physical and chemical changes involve energy changes
Types of energy include heat, light, bond energy
ENDOTHERMIC Needs or requires energy (heat), takes
heat in, surroundings feel cooler
Energy is a (REACTANT)
EXOTHERMIC
Gives off or releases energy (heat),
gives off heat, feels warmer.
Energy is a (PRODUCT)
Law of Conservation of Energy
Energy is not created or destroyed.
Energy of reactants = Energy of products
States of Matter
Density
Movement
shape
volume
D = mass/volume
solid
Packed very
close together,
incompressible
Packed close
liquid together,
incompressible
Very far apart
gas (99%empty
space),
compressible
Vibrate
in place
Slide past
each other
Rapid,
random
straight line
definite
indefinite
indefinite
definite
definite
indefinite
Phase Changes
HEAT IN (ENDOTHERMIC)
MELTING
BOILING
SOLID ========== LIQUID =========== GAS
HEAT OUT (EXOTHERMIC)
FREEZING
H2O: ICE
CONDENSATION
WATER
* WATER VAPOR
*The term VAPOR is used when a substance that is normally
a liquid or solid at room temperature is in a gaseous state.
Types of Matter
Substance
(homogeneous)
Mixture
Definite composition
(_________________________)
Variable
composition
(______________________)
Separated physically
(______________________)
Element
Compound
Homogeneous
Heterogeneous
Separated chemically
(_______________________)
One kind of atom
Element _____________________
Found
on periodic table, H, He
______________________________
solution; one phase
Homogeneous (______________________)
Same
throughout; koolaid, jello
_____________________________
Chemical blend
Compound ____________________
Not the same
Heterogeneous _________________
of 2 or more elements
______________________________
throughout;
different phases
_____________________________
H O, NaCl, BaSO
2
4
(_____________________________)
Chunky soup, salad, soil
_____________________________
Comparison of Compound VS Mixture
Compound
Mixture
1. Chemically combined
Physically combined
2. Can only be separated by
chemical means.
Can be separated
physically.
3. Components are present in a Components may be
definite proportion by weight present in any proportion
4. Compound has different
properties than its individual
components.
Components in mixture
keep their original
properties.
Chemical Symbols
- Every element has a symbol - Symbol consists of
1 or 2 letters, first is capitalized
-Some named for Greek and Latin names
- Ex: Sodium (Natrium) – Na; Iron (Ferrous) Fe
-Chemical Formulas
Combination of elements to represent
compounds.
Ex: C12H22O11 sugar; H2O water
Reaction symbols

solid (s)

* liquid
(l)
* The following are the only
liquids used during a
Water, Bromine & Mercury
chemical reaction
Everything else in a liquid state is an


gas (g)

gas as a product
precipitate ( ) or (ppt.)

aqueous (aq)
Aqueous Solution
( )
Solid product formed from
2 aqueous solutions
Dissolved in water.