Changes in Matter - Read p. 17 and complete the table below.
Physical change
Description:
Chemical Change
Description:
Change that forms a NEW
substance that is made from
the original substance (same
elements).
Alters the appearance of a
material but NO NEW
substance is made!!
Stampedes 
Stampedes
Stampedes  made + steps
**two new words from original word**
**same word, just different style/font**
Examples:
Examples:
 Change states of matter
 Break something apart
 Mix something(s) together
 Rust on a car/bike
 Wood/anything burning
 Baking a cake
 Digestion/photosynthesis!
Evidence for Chemical Reactions - Read p. 18-19 and complete the table below.
Description
Color Change
Precipitation
Gas production
Changes in
temperature or
energy
Changes in
properties
Examples
End products are a different
color than original material.
-
Leaves in the fall
Fruit turning brown
Copper penny turning green
Solid that forms when two
liquids react.
-
Soap scum
Bubbles can be seen (oxygen,
carbon dioxide, hydrogen)
-
Baking soda and vinegar
Alka-seltzer and water
Increase/decrease in
temperature; observation of
heat, light, sound
-
Burning natural gas
Glow stick
Cold/hot packs
Change in texture, appearance,
etc.
-
Baking bread
Frying an egg
Observing Chemical Change – Review and Reinforce
Part A: Classify the following changes as either physical or chemical changes. Explain each answer.
1. A piece of paper is cut into many pieces. PHYSICAL – still paper, just in smaller pieces.
2. A piece of paper is set on fire. CHEMICAL – color change, energy release.
3. A sidewalk is warmed by the heat of the sun. PHYSICAL – still sidewalk, just warmer!
4. Salt crystals appear when a glass of saltwater is left on a windowsill for several days. PHYSICAL – water
evaporates (state change) leaving salt behind.
5. A can of soda tastes flat after being left open for several hours. PHYSICAL – all the dissolved CO2
escapes liquid.
6. A piece of ice melts into a puddle of water. PHYSICAL – state change (solid to liquid).
7. A copper bracelet turns green. CHEMICAL – color change with new material produced.
8. A piece of banana turns brown after being cut. CHEMICAL – color change on outside of fruit.
9. A plant uses sunlight to produce stored energy. CHEMICAL – new material made (sugar is stored
energy).
Part B: Complete the following table. Describe changes in properties that you might notice during each process and
state whether the changes are chemical or physical.
Changes in Matter
Event
Baking a cake
Burning a log
Freezing water
Observable Changes
Type of Change
10. “liquid” sticky mixture changes into spongy,
fluffy cake.
11. chemical
12. solid wood (light in color) change to ash (dark
to white in color); energy (heat/light) released.
13. chemical
14. liquid water solidifies into ice (phase change).
15. physical
Chemical Interactions
Part A:
Valence electrons and Electron dot diagrams - Use the examples in Figure 6 on p. 57 to draw
electron dot diagrams for the following elements.
Element
Symbol
# valence
electrons
E-dot
diagram
Element
Chlorine
Cl
7
Cl
Phosphorus
P
5
Oxygen
O
6
Argon
Ar
8
Sodium
Na
1
Aluminum
Al
3
Barium
Ba
2
Silicon
Si
4
Part B:
Symbol # valence
electrons
E-dot
diagram
How many of each element is needed?? – Use the examples above to help you determine how many
of each element would be needed to make ‘happy’ atoms! Remember, elements in the same group
(column) have the same number of valence electrons (i.e. their E-dot diagrams would look the same!!)
Elements
Number of each
Formula (p.25)
Sodium + Chlorine
1
1
NaCl
Barium + Oxygen
1
1
BaO
Aluminum + Fluorine
1
3
AlF3
Magnesium +Phosphorus
3
2
Mg3P2
Potassium + Sulfur
2
1
K2S
Aluminum + Oxygen
2
3
Al2O3
Lithium+ Bromine
1
1
LiBr
Hydrogen + Oxygen
2
1
H2O
Beryllium + Iodine
1
2
BeI2
Aluminum + Nitrogen
1
1
AlN
Structure of a Chemical Equation
Reactants
Reactants
(p. 26)
Products
Products
Conservation of Mass and Balanced Chemical Equations (p. 26-28)
Part A:
Writing Chemical Formulas - Use your knowledge from the previous section to write the chemical
formula for each element combination.
F
H
N
S
Br
O
HF
H3N
H2S
HBr
H2O
Na
NaF
Na3N
Na2S
NaBr
Na2O
Mg
MgF2
Mg3N2
MgS
MgBr2
MgO
Ca
CaF2
Ca3N2
CaS
CaBr2
CaO
Al
AlF3
AlN
Al2S3
AlBr3
Al2O3
Part B:
Balancing Chemical Equations – Use some of the examples from above to write and balance
chemical equations. **Did not complete in class**
Reactant
+
Reactant
Yields
H
+
O

Al
+
S

Na
+
Br

Mg
+
F

Ca
+
S

Na
+
O

H
+
Br

Na
+
N

Al
+
F

Product (formula)
Identifying Balanced and Unbalanced Equations
Part A:
Identify which equations below are balanced (B) and which are unbalanced (U) by writing the
corresponding letter on the line.
Part B:
If the equation is UNBALANCED, then use the space provided to balance the equation.
_________1.
Pb(NO3)2 +
2KI

PbI2
_________2.
2H2
+
O2

2H2O
Balanced 3.
CuSO4
+
Zn

ZnSO4
_________4.
ZnS
+
2O2

ZnSO4
Balanced 5.
2NaOH
+
CO2

Na2CO3
Balanced 6.
H2
+
Cl2

2HCl
_________7.
2Mg
+
O2

2MgO
_________8.
2Na
+
3H2O

Balanced 9.
NaOH
+
HCl
_________10.
N2
+
_________11.
2Al
_________12.
_________13.
+
2KNO3
+
Cu
+
H2 O
2H2
+
2NaOH

NaCl
+
H2 O
3H2

2NH3
+
3H2SO4

Al2(SO4)3 +
3H2
As2O5
+
3H2O

2H3AsO4
2C
+
O2

2CO
Classifying Chemical Reactions
Type of
Reaction
Synthesis
(p. 29-31)
Description
General example
Specific
example(s)
When two or more substances
combine to make a more
complex substance.
A + B  AB
2Na + Cl2  2NaCl
CaO + H2O  Ca(OH)2
ONE PRODUCT!!
Decomposition
Breakdown of compounds into
simpler products.
AB  A + B
2H2O2  2H2O + O2
2NaN3  2Na + 3N2
ONE REACTANT!!
When one element replaces
another in a compound.
Replacement
(single)
2 REACTANTS
2 PRODUCTS
Replacement
(double)
2 REACTANTS
2 PRODUCTS
**Always have one single/lone
element on reactant/product
side**
When two elements in
different compounds change
place.
Fe + CuSO4  Cu +
FeSO4
A + BX  B + AX
2Na + 2H2O  2NaOH +
H2
AB + XY  XB + AY
HCl + NaOH  NaCl +
H2O
MgCl2 + K2S  MgS +
2KCl
**Always have compounds on
reactant/product sides**
Balancing Synthesis Reactions – balance the following examples of synthesis reactions.
1.
P4
+
5O2

P4O10
2.
2H2
+
O2

2H2O
3.
NaOH
+
CO2

Na2CO3
4.
2CO
+
O2

2CO2
5.
K2S
+
2O2

K2SO4
6.
2Li
+
Cl2

2LiCl
+
H2 O
Balancing Decomposition Reactions – balance the following examples of
decomposition reactions.
1.
2HClO

O2
+
2HCl
2.
CaC2O4

Ca
+
2CO2
3.
PtCl4

Pt
+
2Cl2
4.
2H2O2

2H2O
+
O2
5.
2BaO2

2BaO
+
O2
6.
2KClO3

2KCl
+
3O2
Identifying and Balancing Replacement Reactions
Part A:
Identify the following equations as either single replacement (SR) or double replacement (DR).
Part B:
Balance each of the equations of replacement reactions below. *Balanced
SINGLE
1.*
SnCl2
+
Fe

FeCl2
+
Sn
DOUBLE
2.*
CoCl2
+
Ca(OH)2

CaCl2
+
Co(OH)2
SINGLE
3.
2HCl
+
Cu

CuCl2
+
H2
DOUBLE
4.
CdCl2
+
H2 S

CdS
+
2HCl
DOUBLE
5.
BaCl2
+
K2CrO4

BaCrO4
+
2KCl
DOUBLE
6.
PCl3
+
3AgF

PF3
+
3AgCl
SINGLE
7.*
CuSO4
+
Zn

ZnSO4
+
Cu
SINGLE
8.
2HNO3
+
Ba

Ba(NO3)2 +
H2
SINGLE
9.
3MnO2
+
4Al

2Al2O3
3Mn
+
Identifying and Balancing Chemical Reactions
Part A:
Identify each of the following reactions as Synthesis (S), Decomposition (D), Single
Replacement (SR), or Double Replacement (DR).
Part B:
Balance each of the equations below if needed. (*6 are balanced!!)
Double R 1.
CoCl2
+
H2 O

CoO
+
2HCl
Single R
NiO2
+
C

CO2
+
Ni
2.*
Double R 3.
Pb(NO3)2 +
2NaCl

PbCl2
+
2NaNO3
Double R 4.*
HCl
+
NaOH

NaCl
+
H2 O
Decomp
5.*
CaCO3

CaO
+
CO2
Single R
6.
CoF3
+
3S

3SF
+
Co
Synthesis 7.*
Mg
+
Br2

MgBr2
Double R 8.
NiSO4
+
2NaOH

Ni(OH)2
+
Na2SO4
Synthesis 9.*
MoO3
+
MnO

MnMoO4
Single R
10.
C2H2O4
+
2Na

Na2C2O4
+
H2
Decomp
11.*
Cu(OH)2

CuO
+
H2 O
Double R 12.
2HF
+
Li2CO3

2LiF
+
H2CO3
Double R 13.
CaCl2
+
2AgNO3

Ca(NO3)2 +
2AgCl
Controlling Chemical Reactions - Read p.32-34 and complete the table.
Exothermic Reaction
Endothermic Reaction
Description:
A reaction that releases energy in the form
of heat.
Description:
A reaction which absorbs energy (absorbs
heat…feels cold!)
EXO  OUT!! (to release)
ENDO  IN!! (take in)
Examples:
Examples:
Gasoline + oxygen
Baking soda + vinegar
Activation energy – the minimum about of energy needed to start a chemical
reaction.
Rates of Chemical Reactions – Read p. 34-37 and complete the table below.
The rate (how fast or slow) of a chemical reaction is affected by such factors as concentration, surface area, and
temperature, and by using substances called catalysts and inhibitors.
Factor
Description
Concentration The amount of one material in a given
Effect on reaction
Surface area
The amount of exposed surface of a
material.
Increase concentration,
increase particles available to
react.
Increase surface area,
increases rate of reaction.
Temperature
Change temperature changes how fast
particles move (increase contact and
increase energy)
Increase temp, increase
reaction rate; decrease temp.,
decrease reaction rate.
volume of another material.
Catalysts
Material that increases the rate of
reaction by decreasing the activation
energy (NOT permanently changed…not a
reactant!)
Add catalyst, increase
reaction rate.
Inhibitors
Material used to decrease the rate
of a reaction.
Add inhibitor, decrease
reaction rate.
Packet p. 21 – Answer Key
1. batter rises (gas produced) and
sticky batter turns fluffy.
2. chemical
3. wood turns to ash (black/white
in color); heat/light energy
produced.
6. physical
7. physical change
8. matter
9. exothermic
10. endothermic
4. chemical
11. chemical reaction
5. state change from liquid to
solid
12. precipitate
13. chemistry
Packet p. 22 – Answer Key
1. FeS + HCl  FeCl2 + H2S
6. c
2. Na + F2  NaF
7. g
3. HgO  Hg + O2
8. f
4. 2 molecules of Hydrogen (H2)
and 1 molecule of Oxygen (O2)
produces 2 molecules of water
(H2O)
9. a
5. the reactants include 4 atoms
of Hydrogen (2H2) and 2 atoms of
Oxygen (O2) and the products are
the same – 4 atoms of Hydrogen
with 2 atoms of Oxygen (2H2O).
12. b
10. e
11. h
13. d