CHEMISTRY
Reactions Unit
Day 1:
Objectives 8.1.1, 8.1.2
Before class:
Read section pages 241 – 247
Answer the following. Complete sentences are not needed.
1. Define: a. chemical reaction, b. chemical equation, c. precipitate,
d. catalyst, e. reversible reaction
2. In a chemical equation, a coefficient indicates
a. the exact amount of substance used as products in a
chemical equation
b. the relative number of moles of substance in a reaction
c. the correct formulas of the reactants and products
d. that a precipitate has formed
3. Chemical equations must be balanced in order to satisfy
a. the law of inverse proportions
b. the Pauli exclusion principle
c. the law of conservation of energy
d. the law of conservation of mass
After class:
Write the letter of the best answer.
1. Which coefficients would you add to balance the chemical equation
Fe + O2  Fe2O3?
a. 2, 3, 1
b. 3, 2, 1
c. 4, 3, 2
d. The equation is already balanced
2. Which sentence is a correct translation for the equation
4Fe(s) + 3O2(g)  2Fe2O3(s)
a. Iron and dioxygen react to form bi-iron trioxide
b. Solid iron and gaseous oxygen react to form solid iron (III) oxide
c. Solid iron and solid oxygen react to form iron trioxide
d. Iron and oxygen react to form gaseous iron(III) oxide
3. Copy the table and write the symbol that corresponds to each
explanation
Explanation
Symbol
A reaction is carried out at 20°C
A reactant or product in the solid state
Indicator of a gaseous reactant
Indicator of a solid precipitate
Indicates a reversible reaction
Indicates that reactants are heated
CHEMISTRY
Reactions Unit
4. Create a chart or checklist to help you remember the characteristics of
a chemical equation. Use a form that makes sense to you and include
examples.
Day 2:
Objectives 8.1.3, 8.1.4
Before class:
Read section pages 247 – 254
Answer the following. Complete sentences are not needed.
1. What three pieces of information are revealed by a chemical
equation?
2. What are the four steps to balancing a chemical equation?
During class:
1. Example: 2H2O  2H2 + O2
2. Example: Solid calcium metal reacts with water to form aqueous calcium
hydroxide and hydrogen gas.
3. Example: Nitrogen dioxide gas reacts with water to form aqueous nitric acid and
nitrogen monoxide gas.
4. You try: Solid potassium chlorate decomposes to form solid potassium chloride
and oxygen gas.
5. You try:
H2SO4(aq) +
BaCl2(aq) 
HCl(aq) +
BaSO4(s)
Al2O3(s) +
H2SO4(aq) 
Al2(SO4)3(aq) +
H2O(l)
After class:
Write the letter of the best answer.
2. For a chemical equation to be balanced
a. only the number of atoms must be the same in the reactants and
the products
b. the coefficients of the products must be greater than the
coefficients of the reactants
c. the coefficients of the reactants must be greater than the
coefficients of the products
d. the number and types of atoms must be the same in the
products and reactants
3. According to the reaction 2Fe2O3 + 3C  4Fe + 3CO2, how many
relative grams of carbon dioxide are produced?
a. 36.03 g
b. 44.01 g
c. 84.03 g
d. 132.03 g
CHEMISTRY
Reactions Unit
4. Which shows a correctly balanced chemical equation?
a. Ca + O  2CaO
b. MgO + HCl  MgCl + OH–
c. H2SO4 + NaOH  Na2SO4 + H2O
d. NH4NO2  N2H3 + H2O
5. Which shows a correctly balanced chemical equation?
a. 2Mg + O2  2MgO
b. C3H8 + O2  CO2 + H2O
c. Ca3PO4 + H2SO4  CaSO4 + H3PO4
d. 2K + H2 + OH–  2KOH + H2
6. Write balanced chemical equations for each of these chemical reactions
a. Methane and oxygen react to form hydrogen and carbon dioxide
b. Methane and chlorine react to form carbon tetrachloride and
hydrochloric acid
c. Hydrochloric acid and barium hydroxide react to form barium
chloride and water
d. Silicon dioxide and hydrofluoric acid react to form silicon
tetrafluoride and water.
e. Potassium chloride and lead (II) nitrate react to form potassium
nitrate and lead (II) chloride
Day 3:
Objectives 8.1.1, 8.1.2, 8.1.3, 8.1.4
During class:
Copy and balance the following equations. If it is already balanced, write
“balanced”.
1. NaNO3 + PbO  Pb(NO3)2 + Na2O
2. AgI + Fe2(CO3)3  FeI3 + Ag2CO3
3. C2H4O2 + O2  CO2 + H2O
4. ZnSO4 + Li2CO3  ZnCO3 + Li2SO4
5. V2O5 + CaS  CaO + V2S5
6. Mn(NO2)2 + BeCl2  Be(NO2)2 + MnCl2
7. AgBr + GaPO4  Ag3PO4 + GaBr3
8. H2SO4 + B(OH)3  B2(SO4)3 + H2O
9. S8 + O2  SO2
10. Fe + AgNO3  Fe(NO3)2 + Ag
11. HCl(aq) + Fe2O3(s)  FeCl3(aq) + H2O(l)
12. Li(s) + O2(g)  Li2O(s)
13. MgCO3(s)  MgO(s) + CO2(g)
14. Fe3O4(s) + H2(g)  Fe(s) + H2O(l)
15. C6H5OH(aq) + O2(g)  CO2(g) + H2O(l)
CHEMISTRY
Reactions Unit
16. KClO4(aq)  KCl(aq) + O2(g)
17. AgNO3(aq) + H2S(g)  Ag2S(s) + HNO3(aq)
18. Cl2(g) + KI(aq)  KCl(aq) + I2(l)
19. FeCl3(aq) + NaOH(aq)  Fe(OH)3(s) + NaCl(aq)
Write and balance a formula equation for each reaction.
20. Aluminum + Chlorine  Aluminum Chloride
21. Lead + Copper (I) Nitrate  Copper + Lead (II) Nitrate
22. Barium Chloride + Potassium Carbonate  Barium Carbonate +
Potassium Chloride
23. Glucose (C6H12O6) + Oxygen  Carbon Dioxide + Water
24. Aluminum Sulfate + Calcium Hydroxide  Aluminum Hydroxide +
Calcium Sulfate
25. Sodium + Chlorine  Sodium Chloride
26. Copper + Silver Nitrate  Copper(II) Nitrate + Silver
Day 4:
Objectives 8.2.1, 8.2.2, 8.2.3, 8.2.4
Before class:
Read pages 256 – 262
Answer the following. Complete sentences are not needed.
1. Which type of reaction occurs when an acid disintegrates to
become a nonmetal oxide and water?
a. synthesis
b. double replacement
c. single replacement
d. decomposition
2. Which type of reaction occurs when bromine and lithium iodide
react to form lithium bromide and iodine?
a. decomposition
b. single replacement
c. synthesis
d. double replacement
3. Which is an example of a synthesis reaction?
a. Water becomes ice when it is subjected to temperatures
below
0 °C.
b. A flame ignites when a stove’s burner is turned on.
c. Liquid coffee is produced when water drips through ground
coffee at high temperature.
d. Iron turns to rust when it is exposed to oxygen.
CHEMISTRY
Reactions Unit
After class:
Write the letter of the best answer.
1. In the equation 2Mg(s) + O2(g)  2MgO(s),
MgO is
a. an oxide
b. a reactant
c. a precipitate
d. an oxyacid
2. Which is a correctly balanced equation that represents a decomposition
reaction?
a. H2CO3  H2O + CO2
b. C4H10O  CO2 + H2O
c. NH4NO2  NH3 + H2O
d. both a and c
3. Which equations show synthesis reactions?
a. 2Na + Cl2  2NaCl
b. Zn + 2HCl  ZnCl2 + H2
c. 2Br + 2LiI  2LiBr + I2
d. 4Fe + 3O2  2Fe2O3
e. 2H2O  2H2 + O2
f. 2Ca + O2  2CaO
g. 2Mg + O2  2MgO
h. H2CO3  CO2 + H2O
Day 5:
Objectives 8.2.4. 8.2.5
Before class:
Read pages 262 – 264
Answer the following. Complete sentences are not needed.
1. Define and show an example of: a. double-replacement reaction,
b. combustion reaction
After class:
1. Perform the QuickLAB on page 264.
2. Copy and complete the chart below. Use the following reactions below
as your examples
Zn + 2HCl  ZnCl2 + H2
CH4 + 2O2  CO2 + 2 H2O
2Mg + O2  2MgO
MgCO3 + 2HCl  MgCl2 + H2CO3
2KCl + Pb(NO3)2  2KNO3 + PbCl2
C7H16 + 11O2  7CO2 + 8H2O
2Al2O3  4Al + 3O2
2Na + 2H2O  2NaOH + H2
CHEMISTRY
Reactions Unit
Reaction Type
synthesis
decomposition
single-replacement
double-replacement
combustion
Description
General equation
Example(s)
Day 6:
Objectives 8.3.1. 8.3.2
Before class:
Read section 8 – 3
Answer the following. Complete sentences are not needed.
1. Define: activity series
During class:
1. Example: Using table 8-3, predict whether the following reactions will occur. If
they will, write the products and balance the equation.
MgCl2(aq) + Zn(s) 
Al(s) + H2O(g) 
2. You try: Using table 8-3, predict whether the following reactions will occur. If
they will, write the products and balance the equation.
Cd(s) + O2(g) 
I2(s) + KF(g) 
After class:
Write the letter of the best answer.
1. Which reaction would not be predicted to occur by the activity series?
a. Ni + O2
b. Au + H2
c. Sr + H2O
d. Pb + HCl
2. Use the activity series to predict whether each of the possible reactions
listed below will occur. For the reactions that will occur, write a
balanced equation showing the reactants and products.
a. Rb(s) + H2O(g) 
b. Zn(s) + H2O(l) 
c. Mg(s) + HCl(aq) 
d. Fe(s) + H2O(g) 
e. Pt(s) + H2O(l) 
f. Al(s) + O2(g) 
CHEMISTRY
Reactions Unit
Complete each sentence below.
3. When Mg, Al, Mn, or Zn reacts with oxygen, the result
is__________________
4. When Ni reacts with acid, it ______________________________________
5. The metals Ag and Pt are __________________ reactive than Co and Rb.
6. Activity series are used to predict_________________________________.
Day 7:
All Objectives
Before class:
Organize your handouts from each day. Miss Becker will be checking
that you have them all during class.
You should have days 1 – 6.
During class:
The following questions are suggested for study. They are not graded. They are not
required. I recommend reading through them, and working through the ones that don’t
seem obvious to you.
Chapter 8 review 1, 8, 11, 15, 16, 18, 20, 21, 24, 27 – 29, 35