Chemistry 1010 Review Tutorial Questions
December 2013
1) Naming Elements and Compounds
Formula/Symbol
Al2O3
Ca3N2
HClO4
Mg2+
NaF
(NH4)2SO4
CuClO4
K2CrO4
HlO3(aq)
Ag2O
HBrO(aq)
Li2S
Cl2O7
HF(aq)
CrSO4
Na2CO3 .10H2O
K2SO3
Cr(OH)3
Co2S3
Co(HCO3)2
Fe2(CO3)3
Fe2O3
Cu2SO4
OF2
Cu(NO3)2
MgS
MgCl2
Name
Name
Cobalt (II) phosphate octahydrate
Nitrous Acid
Diboron Tetrachloride
Barium Chloride Hexahydrate
Phosphours Tribromide
Copper (II) Sulfate Pentahydrate
Disulfur Dichloride
Aluminum Hydroxide
Calcium Phosphate
Magnesium Nitride
Copper (II) Phosphate
Sodium Carbonate Decahydrate
Silver Nitrate
Percloric Acid
Phosphoric Acid
Ammonium Nitrate
Sodium Chromate
Calcium Nitrate
Sodium Carbonate Monohydrate
Dinitrogen Pentaoxide
Magnesium Phosphate
Sodium Sulfite
Carbon Tetrabromide
Magnesium Perchlorate
Hexahydrate
Ammonium Iodide
Lithium Chloride Monohydrate
Lithium Sulfite
Formula/Symbol
2) Balancing Chemical Equations
__N2O5 + __H2O → __HNO3
__MnO2 + __HCl → __MnCl2 + __Cl2 + __H2O
__Na2S2O3 + __I2 → __NaI + __Na2S4O6
__Al4C3 + __H2O → __Al(OH)3 + __CH4
__Ca3(PO4)2 + __C → __Ca3P2 + __CO
3) Predict whether the following compounds are soluble in water
a)
b)
c)
d)
e)
f)
PbSO4
KNO3
Ca(CH3COO)2
Hg2Cl2
SrCO3
LiCl
4) Write molecular, complete and net ionic equations for the following reactions. Also, classify
each reaction as precipitation, redox , acid/base, gas evolution or no reaction:
a) When Ca metal and hydrochloric acid are mixed
b) A solution of aqueous Barium Hydroxide is mixed with Nitric Acid
c) Aqueous Sodium Carbonate reacts with Hydrochloric Acid
d) Aqueous Barium Chloride reacts with Sodium Sulfate
e) Solid zinc reacts with Hydrochloric acid
f) Aqueous Silver Nitrate reacts with aqueous Magnesium Chloride
g) Aqueous solutions of Lead (II) nitrate and Sodium Chloride
h) Solutions of Sodium Phosphate and Iron (II) Chloride
i) Ca(s) + AgNO3 ->
j) HNO3(aq) + Ba(OH)2 (aq) ->
k) Pb(NO3)2 (aq) + NaI (aq) ->
Write molecular, complete and net ionic equations for the following reactions.
a) Aqueous Cobalt (II) Chloride reacts with aqueous Silver Nitrate
b)
c)
d)
e)
f)
g)
h)
i)
j)
k)
l)
m)
n)
o)
p)
q)
Nitric Acid reacts with aqueous Calcium Hydroxide
Aluminum Metal reacts with aqueous Coper (II) Chloride
Solutions of Copper (II) Chloride reacts with Silver Nitrate
Zinc solid reacts with Copper (II) Sulfate
Ammonia solution reacts with Hydrochloric Acid
The reaction between Sodium metal and Water
The combustion of Methane (CH4) gas in Oxygen
Neutralization reaction between Sulfuric Acid and aqueous Potassium Hydroxide
Chromium (III) Chloride solution reacts with Sodium Sulfide to give a black ppt.
Silver Nitrate solution reacts with Sodium Chloride to give a white ppt.
Ammonium Phosphate solution reacts with Nickel (II) Chloride
Aqueous Barium Hydroxide reacts with Nitric Acid
Aqueous Chromium (III) Sulfate reacts with aqueous Ammonium Carbonate
Aqueous Phosphoric Acid reacts with aqueous Calcium Hydroxide
Solutions of Copper (II) Sulfate reacts with Strontium Nitrate (Sr(NO3)2)
A strip of Zinc is added to a solution of Lead (II) Nitrate
5) Assign oxidation numbers to each of the atoms indicated
a)
b)
c)
d)
e)
f)
g)
Nb in Nb2O5
P in HPO42–
Ga in Ga(H2PO4)3
N in N2H5+
Cl in Cl2(g)
Fe3+
C in CH2Cl2
6) Determine whether each of the following is a redox reaction by assigning oxidation numbers.
If it is, identify the oxidizing and reducing agents:
a) CuCl2(aq) + Al(s) → AlCl3(aq) + Cu(s)
b) KSO4(aq) + Ba(NO3)2(aq) → BaSO4(s) + KNO3(aq)
c) Na(s) + Au(NO3)3(aq) → NaNO3(aq) + Au(s)
7) Balance the following Redox Reactions under acidic and basic conditions.
a) C4H4O6- (aq) + ClO3- (aq)  CO3- (aq) + Cl- (aq)
b) H2O2 (aq) + Cl2O7 (aq)  ClO2- (aq) + O2 (g)
c) Tl2O3 (aq) + NH2OH  TlOH (s) + N2 (g)
d) Mn(OH)2 (s) + MnO4- (aq)  MnO2 (s)
e) S4O6 2- (aq) + Al (s)  H2S (aq) + Al3+ (aq)