Worksheets - Answers
Grade 11 University Level
Unit 1
Nomenclature
Worksheet 1 – Nomenclature 1
Worksheet 2 – Nomenclature 2
Worksheet 3 – Nomenclature 3
Worksheet 4 – Nomenclature 4
Worksheet 5 –Nomenclature 5
Read Pgs 52 – 65 Q# Pg 66 2 – 6
Types of Reactions
No Worksheet – Chemical Equations
Read Pgs 72 – 78 Q# Pg 79 1 – 6
Worksheet 6 – Balancing Chemical Equations
Worksheet 7 – Types of Reactions
Read Pgs 79 – 86, Q# Pg 86 1 – 5
Worksheet 8 – Types of Reactions
Read Pgs 87 – 102 Q# Pg 103 3 – 5
Worksheet 9 – Net Ionic Equations
Atomic Structure
Worksheet 10 – Aufbau Diagrams
Read Pgs 4 – 14, Pg 14, Q# 1 – 6
Worksheet 11 – Blank Periodic Table
Worksheet 12 – Energy Level Diagrams
Worksheet 13 – Electron Configurations
Worksheet 14 – Orbital and Energy Level
Diagrams
Worksheet 15 – Quantum Numbers
Worksheet 16 – Atomic Structure Review
Unit 2
Periodicity
Worksheet 17 – Periodic Trends
Read Pgs 15 – 25 Pg 26 Q# 1 - 7
Worksheet 18 – Alkali Metals and Halogens
Pg 30 Q# 1 – 15, 17
Bonding
No Worksheet – Ionic Compounds
Read Pgs 34 – 40, Pg 41 Q# 1,2,4,5
No Worksheet – Covalent Compounds
Read Pgs 41 – 51, Pg 51 Q# 1 – 6
No Worksheet – Ionic/Covalent Structural Formula
Worksheet 19 – Polarity
Read Pgs 48 – 50, Pgs 51 Q# 7
No Worksheet – Unit 2 Review
Pgs 70 – 71 Q# 1 – 18,
Worksheet 1 – Nomenclature 1
1. Write the formulas for each of the following compounds:
a) calcium fluoride
CaF2
b) sodium sulfide
Na2S
c) aluminum nitride
AlN
d) aluminum chloride
AlCl3
e) potassium oxide
K2O
f) calcium chloride
CaCl2
g) copper (II) sulfide
CuS
h) lead (II) bromide
PbBr2
i) silver iodide
AgI
j) barium nitride
Ba3N2
k) iron (II) fluoride
FeF2
l) manganese (IV) oxide
MnO2
m) mercury (II) sulfide
HgS
n) ferric oxide
Fe2O3
o) cuprous nitride
Cu3N
p) antimony (V) iodide
SbI5
q) cesium carbide
Cs4C
r) strontium phosphide
Sr3P2
2. Write the names for the following compounds:
a) lime, CaO(s)
calcium oxide
b) road salt, CaCl2(s)
calcium chloride
c) magnesia, MgO(s)
magnesium oxide
d) bauxite, Al2O3(s)
aluminum oxide
e) zinc ore, ZnS(s)
zinc sulfide
f) cassiterite, SnO2(s)
tin (IV) oxide
3. Write the IUPAC and Classical names for the following compounds if needed:
a) Na2O(s)
sodium oxide
b) SnCl4(s)
tin (IV) chloride
c) ZnI2(s)
zinc iodide
d) SrCl2(s)
strontium chloride
e) AlBr3(s)
aluminum bromide
f) PbCl4(s)
lead (IV) chloride
stannic chloride
plumbic chloride
4. Write the chemical formulas and names for the compounds formed by the pairs of
elements below:
a) strontium and oxygen
SrO
strontium oxide
b) sodium and sulfur
Na2S
sodium sulfide
c) barium and fluorine
BaF2
barium flrouide
d) silver and iodine
AgI
silver iodide
e) calcium and bromine
CaBr2
calcium bromide
f) lithium and chlorine
LiCl
lithium chloride
Worksheet 2 – Nomenclature 2
1. For each of the following compounds use stock and classical naming systems when
needed:
a) NaNO3(s)
sodium nitrate
-found in tobacco
b) NaNO2(s)
sodium nitire
-a meat preservative
c) Cu(NO3)2(s)
copper (II) nitrate
cupric nitrate
-blue solution in water
d) CuNO3(s)
copper (I) nitrate
cuprous nitrate
-green solution in water
e) Al2(SO3)3(s)
aluminum sulfite
-a food additive in pickles
f) Ca(OH)2(s)
calcium hydroxide
-firming agent in fruit products
g) PbCO3(s)
lead (II) carbonate
plumbous carbonate
-cerussite, a mineral
h) Sn3(PO4)2(s)
tin (II) phosphate
stannous phosphate
-use to fix paints to silk
i) Fe2(SO4)3(s)
iron (III) sulfate
ferric sulfate
-a mineral found on Mars
2. Write the chemical formula for each of the following compounds:
a) calcium carbonate
CaCO3
-active ingredient in antacids
b) sodium bicarbonate
NaHCO3
-a foaming agent added to foods
c) sodium hypochlorite
NaClO
-a component of bleach
d) calcium sulfate
CaSO4
-plaster of Paris
e) ammonium nitrate
NH4NO3
-used in fertilizer
f) ammonium phosphate
(NH4)PO4
-a leavening agent added to foods
g) copper (II) sulfate
CuSO4
-used as a fungicide
h) sodium hydroxide
NaOH
-a strong base used as a washing agent
i) potassium permanganate
KMnO4
-a traditional antiseptic
3. Use IUPAC and Archaic systems (if necessary) to name each of the following
compounds:
a) LiClO3(s)
lithium chlorate
b) BaSO4(s) )
barium sulfate
c) Hg2CO3(s)
mercury (II) carbonate
d) Mg(NO3)2(s)
magnesium nitrate
e) Fe(BrO3)3(s)
iron (III) bromate
f) Na3PO4(s)
sodium phosphate
g) NH4IO3(s)
ammonium iodate
h) AuC2H3O2(s)
gold (I) acetate
i) Zn3(PO4)2(s)
zinc phosphate
j) Sb(ClO3)5(s)
antimony (V) chlorate
antimonic chlorate
k) MnSO4(s)
manganese (II) sulfate
manganous sulfate
l) KBrO(s)
potassium hypobromite
m) AlPO5(s)
aluminum perphosphate
mercurous carbonate
ferric bromate
aurous acetate
4. Write the chemical formulas for each of the following molecules:
a) nitrogen
N2
b) carbon dioxide
CO2
c) carbon monoxide
CO
d) nitrogen dioxide
NO2
e) nitrogen monoxide
NO
f) dinitrogen monoxide
N2O
g) dinitrogen tetroxide
N2O4
h) sulfur dioxide
SO2
i) diiodine pentoxide
I2O5
j) silicon tetrafluoride
SiF4
k) boron trifluoride
BF3
l) phosphorus triiodide
PI3
m) diphosphorus pentoxide
P2O5
n) hexanitrogen heptachloride
N6Cl7
5. Rename each of the following compounds using the Stock system and give the chemical
formula for each compound:
a) ferrous sulfide
FeS
iron (II) sulfide
b) plumbic bromide
PbBr4
lead (IV) bromide
c) stannous chloride
SnCl2
tin (I) chloride
d) cuprous hypophosphite Cu3PO2
copper (I) hypophosphite
e) stannic chlorite
Sn(ClO2)4
tin (IV) chlorite
f) ferrous bromate
Fe(BrO3)2
iron (II) bromate
g) ferric chlorite
Fe(ClO2)3
iron (III) chlorite
h) plumbic sulfate
Pb(SO4)2
lead (IV) sulfate
i) titaniumic arsenite
Ti3(AsO3)
titanium (IV) arsenite
j) arsenous nitrite
As(NO2)3
arsenic (III) nitrite
k) cobaltic acetate
Co(C2H3O2)3 cobalt (III) acetate
6. Name the following compounds:
a) SF6(g)
sulfur hexafluoride
b) N2O3(g)
dinitrogen trioxide
c) NO2(g)
nitrogen dioxide
d) PCl3(l)
phosphorus trichloride
e) PCl5(s)
phosphorus pentachloride
f) S5P4(s)
pentasulfur tetraphosphide
g) Se2F(s)
diselenium monoflrouide
h) N2I7(s)
dinitrogen heptaiodide
Worksheet 3 – Nomenclature 3
1. Name the following hydrated compounds:
a) CuSO4•5H2O
copper (II) sulfate pentahydrate
b) Na2SO4•10H2O
sodium sulfate decahydrate
c) MgSO4•7H2O
magnesium sulfate heptahydrate
d) LiNO3•3H2O
lithium nitrate trihydrate
e) CaSO3•8H2O
calcium sulfite octahydrate
2. Write the chemical formulas for the following hydrates:
a) iron(III) oxide trihydrate
Fe2O3•3H2O
-rust
b) aluminum chloride hexahydrate
AlCl3•6H2O
-component of antiperspirant
c) sodium thiosulfate pentahydrate
NaS2O3•5H2O
-photographic “hypo”
d) cadmium (II) nitrate tetrahydrate
Cd(NO3)2•4H2O
-photographic emulsion
e) lithium chloride tetrahydrate
LiCl•4H2O
-in fireworks
f) calcium chloride dihydrate
CaCl2•2H2O
-deicer
3. Write the names of the following bases:
a) KOH(aq)
potassium hydroxide
b) Ca(OH)2(aq)
calcium hydroxide
4. Write the formulas of the following bases:
a) aqueous magnesium hydroxide
Mg(OH)2(aq)
b) aqueous sodium hydroxide
NaOH(aq)
c) aqueous aluminum hydroxide
Al(OH)2(aq)
5. Write the chemical formulas for the following compounds:
a) aqueous hydrogen chloride
HCl(aq)
b) hydrochloric acid
HCl(aq)
c) aqueous hydrogen sulfate
H2SO4(aq)
d) sulfuric acid
H2SO4(aq)
e) aqueous hydrogen acetate
CH3COOH(aq)
f) acetic acid
CH3COOH(aq)
g) aqueous hydrogen nitrite
HNO3(aq)
h) nitric acid
HNO3(aq)
i) hydrobromic acid
HBr(aq)
j) hyposulfurous acid
H2SO2(aq)
k) hydroiodic acid
HI(aq)
l) aqueous hydrogen perchlorate
HClO4(aq)
6. Name each of the following compounds using both the “classical” and the “IUPAC”
nomenclature systems:
a) H2SO3(aq)
aqueous hydrogen sulfite
sulfurous acid
b) H3PO4(aq)
aqueous hydrogen phosphate
phosphoric acid
c) HCN(aq)
aqueous hydrogen cyanide
hydrocyanic acid
d) H2CO3(aq)
aqueous hydrogen carbonate
carbonic acid
e) H2S(aq)
aqueous hydrogen sulfide
hydrosulfuric acid
f) HCl(aq)
aqueous hydrogen chloride
hydrochloric acid
g) H2SO4(aq)
aqueous hydrogen sulfate
sulfuric acid
h) H3PO3(aq)
aqueous hydrogen phosphite
phosphorous acid
Worksheet 4 – Nomenclature 4
1. Write the chemical names for each of the following compounds.
- be sure to include both Stock and Classical Names for any compounds
with polyvalent ions.
- also if it is a binary or ternary acid be sure to include both IUPAC and
classical system names.
a) MgCl2(aq)
magnesium chloride
b) FeO(s)
iron (II) oxide
c) Cs2S2O3
cesium thiosulfate
d) Cu3(AsO4)2
copper (II) arsenate
cupric arsenate
e) Cu3AsO4
copper (I) arsenate
cuprous arsenate
f) SrCl2•3H2O
strontium chloride trihydrate
g) HI(g)
hydrogen iodide
h) HI(aq)
aqueous hydrogen iodide
i) O8Cl4
octaoxygen tetrachloride
j) H3PO4(aq)
aqueous hydrogen phosphate
k) CaHPO4(aq)
calcium hydrogen phosphate
l) P3F9
triphosphorus nonafluoride
m) BeS
beryllium sulfide
n) AuI3
gold (III) iodide
o) KMnO4(s)
potassium permanganate
p) (NH4)OH(aq)
ammonium hydroxide
q) HCl(aq)
aqueous hydrogen chloride
hydrochloric acid
r) HBrO2(aq)
aqueous hydrogen bromite
bromous acid
s) HCN(aq)
aqueous hydrogen cyanide
hydrocyanic acid
t) HBrO2(g)
hydrogen bromite
ferrous oxide
hydroiodic acid
phosphoric acid
auric iodide
u) LiH2PO4(aq)
lithium dihydrogen phosphate
v) Al(H2PO2)3(aq)
aluminum dihydrogen phosphate
w) AlCl3•8H2O
aluminum chloride octahydrate
x) S3Cl5
trisulfur pentachloride
y) Ti3N4
titanium (IV) nitride
z) Sr(ClO)2(s)
strontium hypochlorite
aa) HNO(aq)
aqueous hydrogen hyponitrite
bb) FrIO2
francium iodite
cc) (NH4)3AsO3
ammonium arsenite
dd) HgMnO4
mercury (I) permanganate
ee) HBr(g)
hydrogen bromide
ff) H2SO4(aq)
aqueous hydrogen sulfate
gg) N2O2
dinitrogen dioxide
hh) XeF6
xenon hexaflouride
ii) H2SO3(aq)
aqueous hydrogen sulfite
sulfurous acid
jj) HBr(aq)
aqueous hydrogen bromide
hydrobromic acid
kk) BeHSO3(aq)
beryllium hydrogen sulfite
ll) RbClO4
rubidium perchlorate
mm) H2CO3(aq)
aqueous hydrogen carbonate
carbonic acid
nn) H2CO4(aq)
aqueous hydrogen percarbonate
percarbonic acid
oo) H2Se(aq)
aqueous hydrogen selenide
hydroselenic acid
pp) BaSO2•10H2O
barium hydrosulfite decahydrate
qq) Pb(HCO)4
lead (II) hypocarbonite
plumbous hypocarbonite
rr) Fe2(HCO4)3
iron (III) percarbonate
ferric percarbonate
ss) H2O
dihydrogen monoxide
water
titaniumic nitride
hyponitrous acid
mercurous permanganate
sulfuric acid
Worksheet 5 –Nomenclature 5
1. Write the chemical formulas of the following compounds:
a) radium oxide
RaO
b) hexanitrogen difluoride
N6F2
c) tin (IV) permanganate
Sn(MnO4)4
d) cupric carbonite
CuCO2
e) aqueous hydrogen iodide
HI(aq)
f) magnesium dihydrogen phosphate
Mg(H2PO4)2
g) cuprous nitrite dehydrate
CuNO2∙10H2O
h) hypobromous acid
HBrO(aq)
i) aqueous hydrogen hypobromite
HBrO(aq)
j) hydrogen bromide
HBr(g)
k) aqueous hydrogen bromide
HBr(aq)
l) hydrobromic acid
HBr(aq)
m) ammonium phosphate
(NH4)3PO4
n) titaniumic chloride
TiCl4
o) oxygen dichloride
OCl2
p) aluminum nitride
AlN
q) potassium dichromate
K2Cr2O7
r) phosphoric acid
H3PO4(aq)
s) phosphorous acid
H3PO3(aq)
t) hydrogen cyanide
HCN
u) lithium iodite
LiIO2
v) ammonium thiosulfate
(NH4)2S2O3
w) antimonic persulfate
Sb2(SO5)5
x) aqueous hydrogen sulfate
H2SO4(aq)
y) sulfuric acid
H2SO4(aq)
z) aluminum hydrogen hypocarbonite
Al(HCO)3
aa) octasulfur decachloride
S8Cl10
bb) pernitric acid
HNO4(aq)
cc) aqueous hydrogen pernitrate
HNO4(aq)
dd) cuprous chloride hexahydrate
CuCl∙6H2O
ee) nickelic phosphide
NiP
ff) lithium iodate
LiIO3
gg) diphosphorus tetraiodide
P2I4
hh) potassium thiosulfate
K2S2O3
ii) calcium hydrogen phosphate
CaHPO4
jj) aqueous magnesium hydroxide
Mg(OH)2(aq)
kk) hydrochloric acid
HCl(aq)
ll) acetic acid
CH3COOH(aq)
mm) cobalt (III) dichromate
Co2(Cr2O7)3
nn) mercury (I) carbide
Hg4C
oo) titaniumous hydrogen sulfide
Ti(HS)3
pp) cesium cyanate
CsOCN
qq) nonanitrogen trifluoride
N9F3
rr) nickel (III) oxide
Ni2O3
ss) hypophosphorous acid
H3PO2(aq)
tt) perphosphoric acid
H3PO5(aq)
uu) aqueous hydrogen perphosphate
H3PO5(aq)
vv) persulfuric acid
H2SO5(aq)
Worksheet 6 - Balancing Chemical Equations
1. Write balanced equations for the following reactions:
a) The reaction of ammonia with iodine forms aqueous nitrogen triiodide and
hydrogen gas.
___________________________________________________________________
b) When heated mercury (II) oxide decomposes into mercury and oxygen gas.
___________________________________________________________________
c) The reaction of iron (III) oxide with carbon produces carbon monoxide and iron.
___________________________________________________________________
d) The combustion of ammonia produces nitrogen monoxide and water
___________________________________________________________________
e) Magnesium reacts with sulfuric acid, forming magnesium sulfate and releasing hydrogen
gas.
___________________________________________________________________
f) Ethane, CH3CH3, burns in oxygen gas to form carbon dioxide and water.
___________________________________________________________________
g) Potassium chlorate, a good oxidizing agent, will readily produce potassium chloride and
oxygen gas.
___________________________________________________________________
h) Sulfuric acid is produced by reacting sulfur dioxide with oxygen gas, and water.
___________________________________________________________________
2. Balance the following equations
a)
Li2O(s)
+
H2O(l)

LiOH(aq)
b)
Na(s)
+
Cl2(g)

NaCl(s)
c)
Al2O3(s)
+
H2(g)

Al(s) + H2O(l)
d)
Fe(s)
+
O2(g)

Fe2O3(s)
e)
Al(s)
+
HCl(aq)

f)
Al(s)
+
O2(g)

g)
KMnO4(s) +
HCl(aq)

Cl2(g) +

MgCl2(aq)
+
NH4NO3(aq)
i)
Pb(C2H5)(l)
+
O2(g)

j)
Ca(s)
H2O(l)

+
H2(g)
Al2O3(s)
MnCl2(aq) +
h)
+
AlCl3(aq)
KCl(aq) +
Mg(NO3)2(aq) +
PbO(s) +
H2(g)
H2O(l)
NH4Cl(aq)
CO2(g) +
+
H2O(l)
Ca(OH)2(aq)
Worksheet 7 – Types of Reactions
For the following reactions identify:
a) the type of reaction
b) predict the products (be sure to include states of matter)
c) balance the equation
Write “no reaction” if nothing happens.
Type of Reaction
1. CaSO4(s) 
CaO(s) + SO3(g)
decomposition
2. Cl2(aq) + NaI(aq) 
I2(aq) + NaCl(aq)
single-displacement
3. Zn(s) + CuCl2(aq) 
Cu(s) + ZnCl2(aq)
single-displacement
4. KOH(aq) + MgCl2(aq) 
KCl(aq) + Mg(OH)2(s)
double-displacement
5. Li2O(s) + CO2(g) 
Li2CO3(s)
synthesis
6. Al(s) + H2O(l) 
Al(OH)3(s) + H2(g)
single-displacement
7. Mg(s) + Zn(NO3)2(aq) 
Mg(NO3)2(aq) + Zn(s)
single-displacement
8. Sn(s) + HCl(aq) 
SnCl2(aq) + H2(g)
single-displacement
9. Hg2(NO3)2(aq) + NaCl(aq) 
NaNO3(aq) + HgCl(s)
double-displacement
10. Na2CO3(aq) + H3PO4(aq) 
Na3PO4(aq) + H2O(l) + CO2(g) double/decomposition
11. Zn(s) + O2(g) 
ZnO(s)
synthesis
12. Br2(aq) + MgI2(aq) 
MgBr2(aq) + I2(aq)
single-displacement
13. S(s) + O2(g) 
SO2(g)
synthesis
14. CaO(s) + H2O(l) 
Ca(OH)2(aq)
synthesis
15. Cu(s) + Hg(NO3)2(aq) 
No Reaction
16. KOH(aq) + HClO(aq) 
KClO(aq) + H2O(l)
double-displacement
17. Ni(s) + CuSO4(aq) 
NiSO4(aq) + Cu(s)
single-displacement
18. H2(g) + Cl2(g) 
HCl(g)
synthesis
19. NH4NO3(aq) + KOH(aq) 
KNO3(aq) + H2O(l) + NH3(g)
double/decomposition
20. NaOH(aq) + H2SO4(aq) 
Na2SO4(aq) + H2O(l)
double displacement
21. F2(aq) + AlCl3(aq) 
AlF3(aq) + Cl2(aq)
single-displacement
22. Al(NO2)3(s) 
Al2O3(s) + NO(g)
decomposition
23. CsNO3(aq) + Na2S(aq) 
No Reaction
24. BaO(s) + ClO2(g) 
BaClO3(s)
synthesis
25. Ca(s) + HIO3(aq) 
CaIO3(aq) + H2(g)
single-displacement
26. NH4Cl(aq) + Al(OH)3(aq) 
AlCl3(aq) + H2O(l) + NH3(g)
double/decomposition
27. Na(s) + CuCl(aq) 
NaCl(aq) + Cu(s)
single-displacement
Worksheet 8 – Types of Reactions
In each of the following identify the type of reaction and then state the products.
1. Na3PO4(aq) + CaBr2(aq)

NaBr(aq) + Ca3(PO4)2(s)
2. Pb(NO3)2(aq) + HCl(aq)

PbCl2(s) + HNO3(aq)
3. Na2CO3(aq) + KF(aq)

No Reaction
4. AgNO3(aq)

Cu(NO3)2(aq) + Ag2SO4(s)

NiF(aq) + AgCl(s)

No Reaction

CaO(s) + CO2(g)
+ O2(g)

P2O3(g)
9. RbNO3(aq) + BeF2(aq)

No Reaction
10. AgNO3(aq)
Cu(s)

Cu(NO3)2(aq) + 2 Ag(s)
11. Li2SO3(aq) + HNO3(aq)

LiNO3(aq) + H2O(l) +SO2(g)
12. Na2O(s)
+ H2O(l)

NaOH(aq)
13. HNO3(aq)
+ Ca(OH)2(aq)

Ca(NO3)2(aq) + H2O(l)

Na3PO4(aq) + H2O(l) +NH3(g)

Al(NO3)3(aq) + Sn(s)
O2(g)

CO2(g) + H2O(l)
+ CaSO4(aq)

No Reaction
+ SO2(g)

BeSO3(s)
+ Br2(l)

PbBr2(s) or
Ti3(PO3)4(s)

TiO2(s) + PO2(g)

HBrO3(aq)

HIO4(aq)

H2O(l) + PO4(g)
5. AgF(aq)
+ NiCl2(aq)
6. Pb(s)
+ FeSO4(aq)
7.
CaCO3(s)
8. P4(s)
14. NaOH
15. Al(s)
16. C3H6(g)
17. Na(s)
18. BeO(s)
19. Pb(s)
20.
21. H2O(l)
22. IO3(g)
23.
+ CuSO4(aq)
+
+ (NH4)3PO4
+ Sn(NO3)2(aq)
+
+ BrO2(g)
+ H2O(l)
H3PO5(aq)
PbBr4(s)

Rb2O(s) + H2O(l)
25. CoBr3(aq) + I2(s)

No Reaction
26. CoBr3(aq)
+ Cl2(g)

CoCl3(aq) + Br2(l)
+ HNO3(aq)

KNO3(aq) + H2S(g)

Ni(OH)2(aq) + H2(g)

Mg(s) + Cl2(g)

NaCl(aq) + H2O(l)
24.
27. K2S(aq)
28. H2O(l)
29.
30. HCl(aq)
RbOH(aq)
+
Ni(s)
MgCl2(s)
+ NaOH(aq)
Worksheet 9 – Net Ionic Equations
1. Write the balanced chemical equation, total ionic equation, and net ionic equation for the
reaction of sodium iodide solution and aqueous bromine.
Balanced Equation: 2NaI(aq) + Br2(aq)  2NaBr(aq)
Total Ionic Equation: 2Na+(aq) + 2I-(aq) + Br2(aq) 
2Na+(aq) + 2I-(aq) + Br2(aq) 
Net Ionic Equation: 2I-(aq) + Br2(aq)  2Br-(aq) +
+ I2(aq)
2Na+(aq) + 2Br-(aq) + I2(aq)
2Na+(aq) + 2Br-(aq) + I2(aq)
I2(aq)
2. Write the balanced chemical equation, total ionic equation, and net ionic equation for the
reaction of lead (II) nitrate solution and potassium chloride solution.
Balanced Equation: Pb(NO3)2(aq) + 2KCl(aq)  2KNO3(aq) + PbCl2(s)
Total Ionic Equation: Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + 2Cl-(aq)  2K+(aq) + 2 NO3-(aq) + PbCl2(s)
Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + 2Cl-(aq)  2K+(aq) + 2 NO3-(aq) + PbCl2(s)
Net Ionic Equation: Pb2+(aq) + 2Cl-(aq)  PbCl2(s)
3. Write the balanced chemical equation, total ionic equation, and net ionic equation for the
reaction of sodium carbonate solution and hydrochloric acid.
Balanced Equation: Na2CO3(aq) + 2HCl(aq)  2NaCl(aq) + H2O(aq) + CO2(aq)
Total Ionic Equation: 2Na(aq)+ CO32-(aq)+2H+(aq)+2Cl-(aq)  2Na+(aq) + 2Cl-(aq) + H2O(aq) + CO2(aq)
2Na(aq)+ CO32-(aq)+2H+(aq)+2Cl-(aq)  2Na+(aq) + 2Cl-(aq) + H2O(aq) + CO2(aq)
Net Ionic Equation: CO32-(aq) + 2H+(aq)  H2O(aq) + CO2(aq)
4. Write the net ionic equation for each of the following reactions:
a) When aqueous sodium carbonate solution is added to a solution of calcium
chloride, solid calcium carbonate is formed and sodium chloride remains in
solution.
Balanced Equation: Na2CO3(aq) + CaCl2(aq)  2NaCl(aq) + CaCO3(s)
Total Ionic Equation: 2Na+(aq)+ CO32-(aq) + Ca2+(aq) +2Cl-(aq) 2Na+(aq)+2Cl-(aq)+ CaCO3(s)
2Na+(aq)+ CO32-(aq) + Ca2+(aq) +2Cl-(aq) 2Na+(aq)+2Cl-(aq)+ CaCO3(s)
Net Ionic Equation: CO32-(aq) + Ca2+(aq) CaCO3(s)
b) When solid magnesium metal is added to a solution of zinc chloride, solid zinc
metal is formed, leaving a solution of magnesium chloride
Balanced Equation: ZnCl2(aq) + Mg(s)  MgCl2(aq) + Zn(s)
Total Ionic Equation: Zn2+(aq) + 2Cl-(aq) + Mg(s)  Mg2+(aq) + 2Cl-(aq) + Zn(s)
Zn2+(aq) + 2Cl-(aq) + Mg(s)  Mg2+(aq) + 2Cl-(aq) + Zn(s)
Net Ionic Equation: Zn2+(aq) + Mg(s)  Mg2+(aq) + Zn(s)
c) When sodium iodide solution is mixed with aqueous lead (II) nitrate, a yellow
lead (II) iodide precipitate is formed, leaving a solution of sodium nitrate.
Balanced Equation: 2NaI(aq) + Pb(NO3)2(aq)  2NaNO3(aq) + PbI2(s)
Total Ionic Equation: 2Na+(aq) +2I-(aq)+ Pb2+(aq)+ 2NO3-(aq)2Na+(aq) + 2NO3-(aq) + PbI2(s)
2Na+(aq) +2I-(aq)+ Pb2+(aq)+ 2NO3-(aq)2Na+(aq) + 2NO3-(aq) + PbI2(s)
Net Ionic Equation: 2I-(aq) + Pb2+(aq)  PbI2(s)
5. Write the net ionic equation for each of the following reactions.
a) An aqueous solution of sodium sulphide reacts with hydrochloric acid to produce
hydrogen sulphide gas and a solution of sodium chloride.
Balanced Equation: Na2S(aq) + 2HCl(aq)  2NaCl(aq) + H2S (g)
Total Ionic Equation: 2Na+(aq) + S2-(aq)+ 2H+(aq) + 2Cl-(aq)2Na+(aq) +2Cl-(aq) +H2S(g)
2Na+(aq) + S2-(aq)+ 2H+(aq) + 2Cl-(aq)2Na+(aq) +2Cl-(aq) +H2S(g)
Net Ionic Equation: S2-(aq)+ 2H+(aq) H2S(g)
b) An aqueous solution of potassium hydroxide reacts with nitric acid to give a
solution of potassium nitrate and water.
Balanced Equation: KOH(aq) + HNO3(aq)  KNO3(aq) + H2O(l)
Total Ionic Equation: K+(aq) + OH-(aq) + H+(aq) + NO3- (aq)  K+(aq) + NO3- (aq) + H2O(l)
K+(aq) + OH-(aq) + H+(aq) + NO3- (aq)  K+(aq) + NO3- (aq) + H2O(l)
Net Ionic Equation: OH-(aq) + H+(aq)  H2O(l)
Worksheet 13 – Electron Configurations of Atoms
1) Write the full and shorthand (condensed) electron configurations for each of the
following atoms.
a)
b)
c)
d)
e)
f)
g)
h)
i)
j)
k)
l)
phosphorus
1s22s22p63s23p3
beryllium
1s22s2
fluorine
1s22s22p5
calcium
1s22s22p63s23p64s2
zinc
1s22s22p63s23p64s23d10
2
2
6
2
tellurium, 1s 2s 2p 3s 3p64s23d104p65s24d105p4
sodium
1s22s22p63s1
nickel
1s22s22p63s23p64s23d8
oxygen
1s22s22p4
iron
1s22s22p63s23p64s23d6
magnesium
1s22s22p63s2
aluminum
1s22s22p63s23p1
[Ne]3s23p3
[He]2s2
[He]2s22p5
[Ar]4s2
[Ar]4s23d10
[Kr] 5s24d105p4
[Ne]3s1
[Ar]4s23d8
[He]2s22p4
[Ar]4s23d6
[Ne]3s2
[Ne]3s23p1
2) Write shorthand (condensed) electron configuration for each of the following atoms.
a)
b)
c)
d)
e)
[Xe]6s24f11
[Xe]6s24f145d6
[Xe]6s24f145d106p2
[Rn]7s2
[Rn]7s25f146d5
holmium
osmium
lead
radium
bohrium
3) Determine which elements have the following electron configurations:
a) 1s22s22p63s23p4 S
b) 1s22s22p63s23p64s23d104p65s1
c) [Kr] 5s24d105p3 Sb
d) [Xe] 6s24f145d6
e) [Rn] 7s25f11
Os
Es
4) Determine which electron configurations are not valid.
a) 1s22s22p63s23p64s24d104p5 no
b) 1s22s22p63s33d5 no
c) [Ra] 7s25f8 no
d) [Kr] 5s24d105p5 yes
e) [Xe] no – better to put [Kr]5s24d105p6
Rb
5) Which block of the periodic table are each of the following elements located in?
a) einsteinium
f
b) polonium
p
c) rutherfordium
d
d) francium
s
6) Without looking at the periodic table, identify the group number, period number, and
block of an atom that has each of the following electron configurations.
a) [Ne]3s1
group 1, period 3, s block
b) [He]2s2
group 2, period 2, s block
c) [Kr]5s24d105p5
group 17, period 5, p block
7) What is the number of orbitals in each of the following subshells?
a) 2s
1
b) 4p 3
c) 3d 5
d) 1p 0
e) 4f
7
f) 2p
g) 2d 5
h) 6g 9
3
8) What is the maximum number of electrons in each of the following subshells?
a) 2s
2
b) 4p 6
c) 3d 10
d) 1p 0
e) 4f
14
f) 2p
g) 2d 10
h) 6g 18
6
Worksheet 14 – Orbital and Energy Level Diagrams
1) Identify and correct the errors in each of the following valence shell orbital diagrams:
Element
s orbital
p orbitals
a) carbon


Correct:



b) sulfur




Correct:




c) aluminum


Correct:


2) Consider the valence level electron configurations of the following five elements:
Element
s orbital p orbitals
1



2

3

4



5





a) Which of the above elements are metals? 2, 3, 4 could be metals
b) Which of the above elements would form an ion with a +2 charge? 3, possibly 4
c) Which of the above elements is a noble gas? 1, possibly 3 a halogen? 5
d) Which of the above elements has the same configuration as S2- ? 1
3) Write the orbital occupied by the last electron of each of the following elements:
As
W
Li
U
O
Rn
V
4p
5d
2s
5f
2p
6p
3d
4) Draw an orbital diagram for each of the following.
a) a cobalt atom (Co)


1s
2s




2p

3s


3p



4s





3d
b) a sulfide ion S2–


1s
2s




2p

3s


3p
4s
c) a cadmium ion (Cd2+)


1s
2s


4p





2p

5s

3s




3p




4s

4d
5) Draw a complete energy level diagram (vertical) for an atom of iron, Fe.


3d
Worksheet 15 – Quantum Numbers
1. State the four quantum numbers and the possible values they may have.
n = 1,2,3,4,5,6,7,8 , l = 0,1,2,3 , ml = -l...+l , ms = +½ , -½
2. Name the orbitals described by the following quantum numbers
a. n = 3, L = 0
b. n = 3, L = 1
c. n = 3, L = 2
d. n = 5, L = 0
,
,
,
,
3s
3p
3d
5s
3. Give the n and L values for the following orbitals
a. 1s
b. 3s
c. 2p
d. 4d
e. 5f
,n=1l=0
,n=3l=0
,n=2l=1
,n=4l=2
,n=5l=3
4. Place the following orbitals in order of increasing energy:
1s, 3s, 4s, 6s, 3d, 4f, 3p, 7s, 5d, 5p
, 1s, 3s, 3p, 4s, 3d, 5p, 6s, 5d, 7s
5. What are the possible mL values for the following types of orbitals?
a. s
b. p
c. d
d. f
,0
, -1, 0, +1
, -2, -1, 0, +1, +2
, -3, -2, -1, 0, +1, +2, +3
6. How many possible orbitals are there for n =
a. 4
b. 10
, 16
, 100
7. How many electrons can inhabit all of the n=4 orbitals?
32
8. Tabulate all of the possible orbitals (by name, i.e. 4s) for n=4 and give the three quantum
numbers which define each orbital.
4s n = 4, l = 0, ml = 0
4p n = 4, l = 1, ml = -1, 0, +1
4d n = 4, l = 2, ml = -2, -1, 0, +1, +2
4f n = 4, l = 3, ml = -3, -2, -1, 0, +1, +2, +3
9. Write electron configurations for the following atoms:
a. H 1s1
d. F 1s22s22p5
b. Li 1s22s1
e. Br 1s22s22p63s23p64s23d104p5
2 2 3
c. N 1s 2s 2p
Worksheet 16 - Atomic Structure Test Review
1) Which one of the following statements regarding Rutherford’s gold foil experiment is TRUE?
a) Rutherford predicted that most of the alpha particles would pass straight through the
foil because atoms are mainly empty space.
b) Rutherford predicted that the alpha particles that hit negative particles would bounce
back towards the radioactive source.
c) The actual experimental results led Rutherford to conclude that atoms have a central
positive core because most of the alpha particles were deflected at large angles.
d) Since most of the alpha particles passed straight through the foil without deflection,
Rutherford concluded that atoms are mainly empty space.
e) The most surprising thing about the experimental results was that only some of the
alpha particles were deflected at large angles.
2) In Thomson’s model of the atom:
a) negative particles are embedded within a sphere of positive charge
b) atoms are tiny, indivisible spheres
c) positive particles are embedded within a sphere of negative charge
d) there is a positive nucleus surrounded by empty space
3) Which one of the following could be the electron configuration for an element with the
following Lewis diagram?
a) 1s22s1
b) 1s22s22p3
c) 1s22s22p1
d) [Ar]4s23d3
X
e) more than one are correct
4) The species with the following energy level diagram is:
a) Ne
b) Na
c) Na+
d) K
e) Cl–
5) In the emission spectrum of hydrogen, which electronic transition would produce a line in the
visible region of the electromagnetic spectrum?
a) n = 2  n = 1
b) n = 3  n = 2
c) n = 2  n = 3
d) n =   n = 1
6) How many unpaired electrons are in the ground state energy level diagram for an atom of
sulfur?
a) 1
b) 2
c) 3
d) 4
e) 5
7) Which of the following particles has the same electron configuration as krypton?
a) Ga3+
b) Ga3–
c) Sn4+
d) Sn2+
e) As3–
8) Complete the following table:
Symbol
Name of
of
Atomic
Element
Atom Number
or Ion
Mass
Number
Number
of
Protons
Number
of
Neutrons
Number
of
Electrons
Overall
Charge
a
beryllium
Br
4
9
4
5
4
0
b
fluorine
F-
9
19
9
10
10
1-
c
iron
Fe3+
26
56
26
30
23
3+
d
selenium
Se2-
34
79
34
45
36
2-
9) Write the full electron configuration for each of the following atoms:
a) strontium
1s22s22p63s23p64s23d104p65s2
1s22s22p63s23p64s23d104p2
b) germanium
10) Write the shorthand electron configuration for each of the following atoms:
a) silicon
[Ne]3s23p2
b) molybdenum
[Kr]5s24d4
c) terbium
[Xe]6s24f9
d) gold
[Xe]6s24f145d9
e) seaborgium
[Rn]7s25f146d4
11) Draw orbital diagrams for each of the following ions (shorthand), indicate which electrons
have been gained/lost:
a) Cu+
4s
↑
3d
↑↓ ↑↓ ↑↓ ↑↓ ↑↓
b) Pb2+
6s
↑↓
5d
↑↓ ↑↓ ↑↓ ↑↓ ↑↓
6p
↑
↑
4s
↑↓
3d
↑↓ ↑↓ ↑↓ ↑↓ ↑↓
4p
↑↓ ↑↓ ↑↓
5s
↑↓
4d
↑↓ ↑↓ ↑↓ ↑↓ ↑↓
5p
↑↓ ↑↓ ↑↓
6s
↑↓
5s
↑↓
4d
↑↓ ↑↓ ↑↓ ↑↓ ↑↓
5p
↑
c) Br–
d) Sb3–
e) Ba2+
f) Sn4+
12) What is the maximum number of electrons in:
a) n = 3 , 18
b) 3d , 10
d) 4f
, 14
e) 2s , 2
↑
c) 6p , 6
f) n = 5 , 50
g) all d orbitals of curium, Cm , 30
13) State the four quantum numbers for each of the following:
a) the 31st electron of Ga
, 4, 1, -1, +½
b) the 12th electron of magnesium
, 3, 0, 0, -½
c) the 80th electron of mercury
, 4, 2, +2, -½
d) the 54th electron of xenon
, 5, 1, +1, -½
e) the 68th electron of holmium
, 4, 3, 0, +½
Worksheet 17 - Periodic Trends
1) Which of the following elements has the largest atomic radius?
a) beryllium
b) carbon
c) nitrogen
d) oxygen
2) Which of the following elements has the smallest atomic radius?
a) sulfur
b) selenium
c) oxygen
d) tellurium
3) Which of the following elements has the smallest first ionization energy?
a) strontium
b) calcium
c) barium
d) magnesium
4) Which of the following elements has the largest first ionization energy?
a) bromine
b) potassium
c) arsenic
d) calcium
5) Which of the following elements has the highest electron affinity?
a) chlorine
b) silicon
c) sodium
d) phosphorus
6) Which element in the following sets should have the largest atomic radius, and why?
a) boron, lithium, or fluorine
b) potassium, lithium, or sodium
7) Which element in the following pairs has the higher first ionization energy?
a) cesium or gold
b) sulfur or phosphorus
c) magnesium or aluminum
d) neon or krypton
e) oxygen or selenium
f) barium or calcium
8) Which element in the following sets loses an electron most readily, and why?
a) boron, lithium, or fluorine
b) potassium, lithium, or sodium
- lowest ionization energy/largest size - lowest ionization energy/largest size
- electron farther from attractive positive force of nuceleus
9) List each of the following sets in order of increasing radius:
a) Ne, Na+, O2–
Na+, Ne, O2–
b) Mg2+, Na+, Al3+
Al3+, Mg2+, Na+
3–
2–
1–
c) N , O , F
N3–, O2–, F1–
10) The ion Na+ and the atom Ne have the same electron configuration. To remove an electron
from gaseous neon atoms requires 2081 kJ/mol. To remove an electron from a gaseous Na+ ion
requires 4562 kJ/mol. Why are these values not the same?
Both have 10 electrons (2 electrons in first shell, 8 in second), but Ne has 10 protons
in nucleus and Na+ has 11 protons in nucleus. (ENC of Ne is 0, ENC of Na+ is +1)
The 11 protons are holding on to the electrons more strongly than neon’s 10
protons, therefore it would take more energy to remove an electron from Na+.
(Note: You should draw/write configurations, orbital diagram or Bohr-Rutherford
diagrams in your answer.)
11) The second ionization energy of magnesium is only about twice as great as the first
ionization energy. However, the third ionization energy is about ten times as great as the first.
Why does it take so much more energy to remove the third electron from magnesium?
A magnesium atom has 2 electrons in the valence shell. Once the first two electrons
are removed, the third electron is a whole shell closer to the nucleus, therefore it
would require significantly more energy to remove this electron. (You should
draw/write configurations, orbital diagrams, or a Bohr-Rutherford diagram in your
answer.)
12) The following graph shows the melting points (and boiling points) of the period 3 elements.
a) Why is there a general increase in melting point for Na, Mg, and Al?
Smaller radius and increased nuclear charge cause increased strength of metallic bonding.
b) Why does Si have the highest melting point?
Si is the only element in the period that exists as a network covalent structure.
c) Why is there a general decrease in melting point for P4, S8, and Cl2?
Molecules with larger mass/size experience stronger intermolecular forces (van der Waals’
forces), thus S8 has slightly higher m.p. than P4, and Cl2 is lower than both of the others.
d) Why do the noble gases have the lowest melting point?
Noble gases exist as single, diatomic elements, therefore very low van der Waals forces.
13) Although the first ionization energy of K is smaller than that of Ca, the second ionization
energy of K is much higher than that of Ca. Why is this so?
Potassium has one valence electron, while calcium has two valence electrons. Once
the first electrons have been removed, the second electron of potassium is in the
third shell, while the second electron of calcium is still in the fourth shell. It would
require much more energy to remove the second electron from potassium because it
is much closer to the nucleus. (You should draw/write configurations, orbital
diagrams, or Bohr-Rutherford diagrams in your answer.)
14) Element
AA
BB
CC
I1
531
2090
523
I2
1087
3135
8360
I3
6270
4180
11704
I 1 = 1st ionization energy (kJ/mol)
I 2 = 2nd ionization energy (kJ/mol)
I 3 = 3rd ionization energy (kJ/mol)
a) Which of the above elements would most likely be an alkali metal?
CC would most likely be the alkali metal (group 1) because there is a big jump in
ionization energy from I1 to I2 indicating that the second electron is a shell closer to
the nucleus than the first.
b) Which of the above elements would most likely be a noble gas?
BB would most likely, of the three elements above, to be a noble gas because there is
no big jump in ionization energy. AA is a Group 2 element.
Worksheet 18 - Alkali Metals and Halogens
1) State whether each of the following properties increase or decrease going down the alkali
metal group.
a) atomic radius
increases
b) ionic radius
increases
c) ionization energy decreases
d) electronegativity
decreases
e) reactivity
decreases
2) State whether each of the following properties increase or decrease going down the
halogen group.
a) atomic radius
increases
b) ionic radius
increases
c) ionization energy decreases
d) electronegativity
decreases
e) reactivity
decreases
3) What is the state of matter at room temperature for each of the following?
a) F2
gas
b) Cl2
gas
c) Br2
liquid
d) I2
solid
4) For each of the following, circle the correct element.
Li
Si
S
metal
N
P
As
smallest ionization energy
K
Ca
Sc
largest atomic mass
S
Cl
Ar
member of the halogen family
Al
Si
P
greatest electron affinity
Ga
Al
Si
largest atomic radius
V
Nb
Ta
largest atomic number
Te
I
Xe
member of noble gases
Si
Ge
Sn
4 energy levels
Li
Be
B
member of alkali metals
As
Se
Br
6 valence electrons
H
Li
Na
nonmetal
Hg
Tl
Pb
member of transition metals
Na
Mg
Al
electron distribution ending in s2 p1
Pb
Bi
Po
metalloid
B
C
N
gas at room temperature
Ca
Sc
Ti
electron distribution ending in s2 d2
Worksheet 19 – Polarity
In each of the following problems, rank the molecules from lowest to highest polarity:
1)
PF3, LiOH, SF2, NF3
NF3 < SF2 < PF3 < LiOH
2)
Ni(OH)3, N2H2, CH3OH, C2H5OH
N2H2 < C2H5OH < CH3OH < Ni(OH)3
3)
B2F4, H2C2O4, CuCl2, CF2O
NO2 < SO < SeCl2 < PbCl2
4)
PH3, PF3, NH3, NF3
PH3 < NH3 < NF3 < PH3
5)
H2O, H2S, HF, H2
H2 < H2S < H2O < HF