Darien High School
Chemistry 400 Honors – Mr. Heberton
Unit 2 - Part 2
Chemical Reactions
and Balancing
2H2O(l)  H2(g) + O2(g)
SERIES (s) + 2Al(NO3)3(aq)
2Al(s) + 3Pb(NO3)2(aq) ACTIVITY
 3Pb
C6H12O6(s) + 6O2(g)  6CO2(g) + 6H2O(g)
Metals
Li
Rb
K
Ba
Sr
Ca
Na
Mg
Al
Mn
Zn
Cr
Fe
Cd
Co
Ni
Sn
Pb
H2
Sb
Bi
Cu
Hg
Ag
Pt
Au
Nonmetals

React with cold H2O and acids, replacing
hydrogen.

React with oxygen, forming oxides.

React with steam (but not cold H2O ) and
acids, replacing hydrogen.

React with oxygen forming oxides.



Do not react with H2O.
React with acids, replacing hydrogen.
React with oxygen forming oxides.

React with oxygen, forming oxides.

Fairly unreactive, forming oxides only
indirectly.
F2
Cl2
Br2
I2
M
o
r
e
A
c
t
i
v
e
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Chemical Reactions Vocabulary
Part I
Chemical reaction-
Reactants-
Products-
Word Equations-
Chemical Equations-
Coefficient-
Aqueous Solution
Part II
Synthesis Reaction-
Decomposition Reaction-
Combustion Reaction-
Single Replacement Reaction-
Double Replacement Reaction-
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1. Balance the following equations. Make sure that you use the lowest possible whole
number coefficients.
Example
a. _3__C + _4__H2 → __1_C3H8 (but no need to write “1” as a coefficient)
b. 2H2O + O2 → 2H2O2
c. S8 + 12O2 → 8SO3
d. N2 + 3H2 → 2NH3
e. 4P + 5O2 → 2P2O5
f. 2CaO + MnI4 → MnO2 + 2CaI2
g. 2Ag2O → 4Ag + O2
h. CH4 + 2O2 → CO2 + 2H2O
i. 2C6H6 + 15O2 → 6H2O + 12CO2
j. 4NaI + Pb(SO4)2 → PbI4 + 2Na2SO4
k. 2HNO3 + Mg(OH)2 → 2H2O + Mg(NO3)2
l. Fe2O3 + 3H2O → 2Fe(OH)3
m. C2H2 + 2H2 → C2H6
n. CF4 + 2Br2 → CBr4 + 2F2
o. 2NaBr + Ca(OH)2 → CaBr2 + 2NaOH
p. 2NH3 + H2SO4 → (NH4)2SO4
q. 4NH3 + 5O2 → 4NO + 6H2O
r. Li3N + 3NH4NO3 → 3LiNO3 + (NH4)3N
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Balance the following equations. Make sure that you use the lowest possible whole number
coefficients. ALSO note the type of reaction to the right of the equation.
Example:
a. 2KClO3 → 2KCl + 3O2
Decomposition
b. 2H2 + O2 → 2H2O
Synthesis
c. 2NaCl + F2 → 2NaF + Cl2
Single Replacement
d. 2AlBr3 + 3K2SO4 → 6KBr + Al2(SO4)3
Double Replacement
e. C3H8 + 5O2 → 3CO2 + 4H2O
Combustion
f. 2NaBr + CaF2 → 2NaF + CaBr2
Double Replacement
g. 4C5H9O + 27O2 → 20CO2 + 18H2O
Combustion
h. 2C8H18 + 25O2 → 16CO2 + 18H2O
Combustion
i. FeCl3 + 3NaOH → Fe(OH)3 + 3NaCl
Double Replacement
j. 2Na + 2H2O → 2NaOH + H2
Single Replacement
k. H3PO4 + 3NaBr → 3HBr + Na3PO4
Double Replacement
l. 2K + MgBr2 → 2KBr + Mg
Single Replacement
m. 2Fe(OH)3 → Fe2O3 + 3H2O
Decomposition
n. 2HCl + CaCO3 → CaCl2 + H2O + CO2
Double Replacement/Synthesis
o. HNO3 + NaHCO3 → NaNO3 + H2O + CO2
Double Replacement/Synthesis
p. 2VF5 + 10HI → V2I10 + 10HF
Double Replacement
q. H2SO4 + 2NaNO2 → 2HNO2 + Na2SO4
Double Replacement
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Directions: 1. Write the skeletal formula equation showing all appropriate symbols (aq, s, l, g)
2. Name the type of reaction
3. Balance the equation
Aluminum reacts in the air to form aluminum oxide.
4Al(s) + 3O2 (g)  2Al2O3 (s)
Synthesis
Sodium oxide reacts at room temperature with water to form sodium hydroxide.
Na2O (s) + H2O (l)  2NaOH (aq)
Synthesis
Aqueous solutions of sulfuric acid and sodium hydroxide react to form aqueous sodium sulfate and
water.
H2SO4 (aq) + 2NaOH (aq)  Na2SO4 (aq) + 2H2O (l)
Double Replacement or Neutralization
Solid aluminum reacts with aqueous zinc chloride to produce solid zinc metal and aqueous aluminum
chloride.
2Al (s) + 3ZnCl2 (aq)  3Zn (s) + 2AlCl3 (aq)
Single Replacement
Nitrogen gas reacts with oxygen gas to form dinitrogen monoxide gas.
2N2 (g) + O2 (g)  2N2O (g) Synthesis
Potassium bromide decomposes to form potassium metal and bromine liquid.
2KBr (s)  2K(s) + Br2 (l) Decomposition
Mercury (II) oxide when heated forms mercury and oxygen gas.
Heat
2HgO (s)  2 Hg + O2 (g) Decomposition
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Zinc reacts with aqueous sulfuric acid to form zinc sulfate and liberates hydrogen gas.
Zn (s) + H2SO4 (aq)  ZnSO4 (aq) + H2 (g)
Single Replacement
Magnesium nitride and water combine to form magnesium hydroxide and aqueous ammonia.
Mg3N2 (s) + 6H2O (l)  3Mg(OH)2 (s) + 2NH3 (aq)
Double Replacement
Propane gas (C3H8) burns in air to produce carbon dioxide gas and water vapor.
C3H8 (g) + 5O2 (g)  3CO2 (g) + 4H2O (g) Combustion
Nitrogen gas reacts with hydrogen gas to form gaseous ammonia.
N2 (g) + 3H2 (g)  2NH3 (g)
Synthesis
Calcium reacts with aqueous aluminum chloride to form aqueous calcium chloride and aluminum
metal.
3Ca (s) + 2AlCl3 (aq)  3CaCl2 (aq) + 2Al (s)
Single Replacement
At high temperatures, aluminum oxide decomposes.
Heat
2Al2O3 (s)  4Al (s) + 3O2 (g)
Decomposition
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Directions:
For each problem, complete the following:
1. Use the Activity Series to determine if the reaction will occur
2. Write the formula equation showing all reactants and predicted products.
3. Balance the equation
Solid nickel (II) reacts with aqueous copper (II) chloride.
Ni (s) + CuCl2 (aq)  NiCl2 (aq) + Cu (s)
Aqueous iron (II) sulfate reacts with solid copper (II).
FeSO4 (aq) + Cu (s)  NR (No Reaction)
Calcium reacts with water at 50°C.
Ca (s) + 2H2O (l)  Ca(OH)2 (aq) + H2 (g)
Zinc dust reacts with aqueous lead (II) nitrate.
Zn (s) + Pb(NO3)2 (aq)  Zn(NO3)2 (aq) + Pb (s)
Tin (II) reacts with aqueous sulfuric acid.
Sn (s) + H2SO4 (aq)  SnSO4 (aq) + H2 (g)
Solid manganese (II) reacts with water at 50°C.
Mn (s) + H2O (l)  NR (water needs to be in steam form, i.e. at 100oC)
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Magnesium bromide + chlorine
MgBr2 (s) + Cl2 (g)  MgCl2 (s) + Br2 (g)
Aqueous Silver nitrate + zinc chloride
2AgNO3 (aq) + ZnCl2 (aq)  2AgCl (s) + Zn(NO3)2 (aq)
Sulfuric acid solution + sodium hydroxide
H2SO4 (aq) + 2NaOH (s)  Na2SO4 (aq) + 2H2O (l)
Acetic acid + copper
CH3COOH (aq) + Cu (s)  NR
Silver + copper(II) sulfate
Ag (s) + CuSO4 (aq)  NR
Nitric acid + iron(III) hydroxide
6HNO3 (aq) + 2Fe(OH)3 (s)  2Fe(NO3 )3 (aq) + 6H2O (l)
Magnesium chloride + silver nitrate
MgCl2 (aq) + 2AgNO3 (aq)  Mg(NO3)2 (aq) + 2AgCl (s)
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