Practice Worksheet - Chemistry

Chemistry 1010 Review Tutorial Questions December 2013
1) Naming Elements and Compounds
Formula/Symbol Name Name Formula/Symbol
Al 2 O 3
Ca 3 N 2
HClO 4
Mg 2+
NaF
(NH 4 ) 2 SO 4
CuClO 4
K 2 CrO 4
HlO 3 (aq)
Ag 2 O
HBrO(aq)
Li 2 S
Cl 2 O 7
HF(aq)
CrSO 4
Na 2 CO . 3 10H 2 O
K 2 SO 3
Cr(OH) 3
Co 2 S 3
Co(HCO 3 ) 2
Fe 2 (CO 3 ) 3
Fe 2 O 3
Cu 2 SO 4
OF 2
Cu(NO 3 ) 2
MgS
MgCl 2
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

2) Balancing Chemical Equations
__N 2 O 5 + __H 2 O → __HNO 3
__MnO 2 + __HCl → __MnCl 2 + __Cl 2 + __H 2 O
__Na 2 S 2 O 3 + __I 2 → __NaI + __Na 2 S 4 O 6
__Al 4 C 3 + __H 2 O → __Al(OH) 3 + __CH 4
__Ca 3 (PO 4 ) 2 + __C → __Ca 3 P 2 + __CO
3) Predict whether the following compounds are soluble in water
a) PbSO 4
b) KNO 3
c) Ca(CH 3 COO) 2
d) Hg 2 Cl 2
e) SrCO 3
f) 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) + AgNO 3 ->
j) HNO 3 (aq) + Ba(OH) 2 (aq) ->
k) Pb(NO 3 ) 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

) Nitric Acid reacts with aqueous Calcium Hydroxide
c) Aluminum Metal reacts with aqueous Coper (II) Chloride
d) Solutions of Copper (II) Chloride reacts with Silver Nitrate
e) Zinc solid reacts with Copper (II) Sulfate
f) Ammonia solution reacts with Hydrochloric Acid
g) The reaction between Sodium metal and Water
h) The combustion of Methane (CH4) gas in Oxygen
i) Neutralization reaction between Sulfuric Acid and aqueous Potassium Hydroxide
j) Chromium (III) Chloride solution reacts with Sodium Sulfide to give a black ppt.
k) Silver Nitrate solution reacts with Sodium Chloride to give a white ppt.
l) Ammonium Phosphate solution reacts with Nickel (II) Chloride
m) Aqueous Barium Hydroxide reacts with Nitric Acid
n) Aqueous Chromium (III) Sulfate reacts with aqueous Ammonium Carbonate
o) Aqueous Phosphoric Acid reacts with aqueous Calcium Hydroxide
p) Solutions of Copper (II) Sulfate reacts with Strontium Nitrate (Sr(NO3)2)
q) A strip of Zinc is added to a solution of Lead (II) Nitrate
5) Assign oxidation numbers to each of the atoms indicated
a) Nb in Nb 2 O 5
b) P in HPO 4
2–
c) Ga in Ga(H 2 PO 4 ) 3
d) N in N 2 H 5
+
e) Cl in Cl 2(g)
f) Fe 3+
g) C in CH 2 Cl 2
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) CuCl 2(aq) + Al (s) → AlCl 3(aq) + Cu (s)
b) KSO 4(aq) + Ba(NO 3 ) 2(aq) → BaSO 4(s) + KNO 3(aq)
c) Na (s) + Au(NO 3 ) 3(aq) → NaNO 3(aq) + Au (s)

7) Balance the following Redox Reactions under acidic and basic conditions.
a) C 4 H 4 O - 6 (aq) + ClO - 3 (aq) CO - 3 (aq) + Cl - (aq)
-
b) H 2 O 2 (aq) + Cl 2 O 7 (aq) ClO 2 (aq) + O 2 (g)
c) Tl 2 O 3 (aq) + NH 2 OH TlOH (s) + N 2 (g)
d) Mn(OH) 2 (s) + MnO - 4 (aq) MnO 2 (s)
2-
e) S 4 O 6 (aq) + Al (s) H 2 S (aq) + Al 3+ (aq)