Chem 11
FINAL EXAM REVIEW
Name:____KEY_________
Block:_________________
Part I: Safety
1. A __FIRE BLANKET_____ is used to spread over and put out a small fire on the workbench.
All reactions involving hazardous or irritating volatile chemicals should be carried out in a
__FUMEHOOD__. Never add water to concentrated _ACID_. Never return unused chemicals to their
original container, this could cause _CONTAMINATION or REACTION__. Long hair should be
_TIED UP_ during experiments. Broken glass and spilled chemicals must be _CLEANED UP /
REPORTED__. Always handle hot test tubes with _TESTTUBE CLAMPS __. Acid / Alkali burns are
more serious than acid / alkali burns because _YOU DON’T FEEL THE BURNING RIGHT AWAY _.
Part II: Significant Figures
1. How many sig figs?
a) 1 476 765
__7 ______________
e) 3 000 000
__1 ______________
b) 0.004556
__4 ______________
f) 1090
__3 ______________
c) 146008
__6 ______________
g) 3.0045
__5 ______________
d) 0.010101
__5 ______________
h) 5.0005
__5 ______________
2. Calculate the following, rounding off to the appropriate number of sig figs:
= __3.32 x 105 __
f) 108 x 10-3
b) 11 470 x 64.07
= __7.349 x 105 _
g) (3 x 104)(2 x 10-6) = __6 x 10-2 ____
c) 14.7 x 164.3
= __2.42 x 103 __
d) 447 954 – 69.01
= __447 885 ___
e) 6 478.1 – 24
= __6454 ______
a) 6764
x 49.1
h)
= __105 _______
5.2  10 3
1.3  10 4
= __4.0 x 10-3 __
3. Write the following in 3 sig figs:
a) 1.072
__1.07 _______
d) 7.500
__7.50 _______
b) 721 746
__7.22 x 105 __
e) 0.6306
__6.31 x 10-1 __
c) 76 549
__7.65 x 104 __
f) 0.004559 __4.56 x 10-3 __
Part III: Chemical Formulae
1. Give the name or formula of the following:
a) magnesium hydroxide ___Mg(OH)2 ___
g) KCl___potassium chloride __________
b) iron II bromide___FeBr2 ____________
h) SnF4___tin(IV) fluoride ____________
c) H2SO4__sulphuric acid _____________
i) LiNO2__lithium nitrite _____________
d) HBrO____hydrogen hypobromide ___
j) PCl3___phosphorous trichloride _____
e) copper I perchlorate__CuClO4 _______
k) lithium acetate__LiCH3COO ________
f) sulphur trioxide___SO3 _____________
l) sodium phosphide___Na3O __________
2. How many atoms in each of the following formulae?
a) BaSO4
__1-Ba, 1-S, 4-O ___
c) H3PO4
__3-H, 1-P, 4-O ____
b) CuSO4·5H2O
1-Cu, 1-S, 9-O, 10-H
d) Fe2(SO4)3
__2-Fe, 3-S, 12-O ___
3. Classify the following as a chemical or physical change:
a) melting butter
__P ______________
d) dissolving sugar __P ______________
b) baking muffins
__C ______________
e) silver tarnishing __C ______________
c) electrolysis
__C ______________
f) distillation
__P ______________
4. Classify the following as a solution, suspension, or pure substance (element or compound):
a) sugar and water
__SOLUTION _____
d) gold
_P.S. (ELEMENT) _
b) flour and water
__SUSPENSION ___
e) copper II sulphate P.S. (COMPOUND)
c) glass
__SOLUTION _____
f) oil and water
__SUSPENSION ___
Part IV: The Mole
1. State Avogadro’s Hypothesis: _EQUAL VOLUMES OF GASES (AT THE SAME TEMP. AND
PRESSURE) CONTAIN EQUAL NUMBERS OF PARTICLES. ____________________________
2. Calculate the molar mass of the following:
a) HNO3
_63.0 g/mol _
b) Pb(NO3)2_331.2 g/mol
c) LiCl
_42.5 g/mol _
e) MgCO3 _84.3 g/mol __
d) C6H22O11_270.0 g/mol
f) Ag2SO4 _311.9 g/mol _
3. How many atoms of oxygen are contained in 22.0 g of CO2 (g)?
1 mol CO 2 6.02  10 23 molec. CO 2
2 atoms O
22.0 g CO 2 


 6.02 1023 atoms O
44.0 g CO 2
1 mol CO 2
1 molec. CO 2
4. How many molecules of carbon dioxide are there in 22.0 g of the gas?
1 mol CO 2 6.02  10 23 molec. CO 2
22.0 g CO 2 

 3.01 1023 molec.CO2
44.0 g CO 2
1 mol CO 2
5. How many moles is 19.2 g of NaCl?
1 mol NaCl
19.2 g NaCl 
 0.328 mol NaCl
58.5 g NaCl
6. What is the mass of 3.2 moles of HgNO3?
262.6 g HgNO 3
3.2 mol HgNO 3 
 8.4  102 g HgNO 3
1 mol HgNO 3
7. What is the mass of 4.5 L of CO2 (g) at STP?
1 mol CO 2 44.0 g CO 2
4.5 L CO 2 

 8.8 g CO2
22.4 L CO 2 1 mol CO 2
8. How many molecules are there in 4.5 L CO2 (g)?
1 mol CO 2 6.02  10 23 molec. CO 2
4.5 L CO 2 

 1.2  1023 molec.CO2
22.4 L CO 2
1 mol CO 2
9. A compound is composed of 19.01 g of carbon, 18.48 g of nitrogen, 25.34 g of oxygen and 1.58 g of
hydrogen. Find the empirical formula of this compound.
1 mol C
1 mol O
19.01 g C 
 1.58 mol C 25.34 g O 
 1.58 mol O
12.0 g C
16.0 g O
1 mol N
1 mol H
18.48 g N 
 1.32 mol N 1.58 g H 
 1.58 mol H C1.2N1O1.2H1.2  C6N5O6H6
14.0 g N
1.0 g H
10. A 7.30 g sample of a hydrocarbon is burned to give 23.8 g of CO2 and 7.30 g of H2O. What is the
empirical formula of the compound?
1 mol CO 2
1 mol C
CH + O2  CO2 + H2O 23.8 g CO 2 

 0.541mol C
44.0 g CO 2 1 mol CO 2
1 mol H 2 O
2 mol H
7.30 g H 2 O 

 0.811mol H C0.541H0.811  C2H3
18.0 g H 2 O 1 mol H 2 O
11. Find the percent composition of a compound which is 10.12 g of aluminum and 17.93 g of sulphur.
10.12 g Al  28.05 g  100%  36.1% Al 17.93 g S  28.05 g  100%  63.9 % S
12. A compound is composed of 7.20 g of carbon, 1.20 g of hydrogen and 9.60 g of oxygen. The molar mass
of the compound is 180 g. Find the empirical formula and the molecular formula of this compound.
1 mol C
1 mol O
1 mol H
 0.600 mol C 9.60 g O 
 0.600 mol O 1.20 g H 
 1.20 mol H
12.0 g C
16.0 g O
1.0 g H
30.0 g CH 2 O
C0.6H1.2O0.6  CH2O (empirical) 180 g/mol  n 
n = 6  C6H12O6 (molecular)
1 mol CH 2 O
Part V: Chemical Reactions
7.20 g C 
1. Balance the following equations:
Classification:
a) _2_ K + _2_ H2O  _2_ KOH + ___ H2
__single replacement ________
b) _4_ FeS2 + _11 O2  _2_ Fe2O3 + _8_ SO2
__combustion ______________
c) ___ Br2 + _2_ KI  _2_ KBr + ___ I2
__single replacement ________
d) _2_ C15H30 + _45 O2  _30 CO2 + _30 H2O
__combustions _____________
e) _2_ AgNO3 + ___ CuCl2  _2_ AgCl + ___ Cu(NO3)2
__double replacement _______
f) ___ CaC2 + _2_ O2  ___ Ca + _2_ CO2
single replacement / combustion
g) _2_ HgO  _2_ Hg + ___ O2
__decomposition ____________
2. Classify each equation in question #1 as synthesis, decomposition, combustion, single replacement,
double replacement, or neutralization (water forming).
3. Complete the equation and balance it afterwards.
a) _2_ C6H6 + _15 O2  6 H2O + 12 CO2
b) ___ Pb + ___ KNO3  No Reaction
c) ___ ZnSO4 + ___ SrCl2  SrSO4 + ZnCl2
4. Give an example of a reaction that is exothermic and one that is endothermic. On which side of the
equation must the energy term be in each case? examples vary…
A + B  C + ENERGY (exothermic)
A + ENERGY  B + C (endothermic)
5. Write the following equations in chemical notation and balance if needed (include subscripts):
a) solid calcium carbonate when heated decomposes into solid calcium oxide and carbon dioxide gas.
CaCO3 (s)  CaO (s) + CO2 (g)
b) aqueous lead II nitrate combines with aqueous potassium chromate to form solid lead II chromate and
aqueous potassium nitrate.
Pb(NO3)2 (aq) + K2CrO4 (aq)  PbCrO4 (s) + 2 KNO3 (aq)
c) hydrogen gas and nitrogen gas combine to form ammonia gas.
3 H2 (g) + N2 (g)  2 NH3 (g)
Part VI: Stoichiometry
1. 5 g of silver reacts with nitric acid to form nitrogen monoxide, silver nitrate and water.
a) Write the balanced equation.
3 Ag + 4 HNO3  NO + 3 AgNO3 + 2 H2O
b) Calculate the # of moles of silver nitrate produced.
1 mol Ag 3 mol AgNO 3
5 g Ag 

 0.05 mol AgNO3
107.9 g Ag
3 mol Ag
c) Calculate the # of grams of nitric acid required in the reaction.
1 mol Ag 4 mol HNO 3 63.0 g HNO 3
5 g Ag 


 4 g HNO3
107.9 g Ag
3 mol Ag
1 mol HNO 3
2. When 5.45 g of KClO3 decomposes, potassium chloride and oxygen gas are produced.
a) Write the balanced equation.
2 KClO3  2 KCl + 3 O2
b) How many moles of potassium chloride are produced?
1 mol KClO 3
2 mol KCl
5.45 g KClO 3 

 0.0445mol KCl
122.5 g KClO 3 2 mol KClO 3
c) How many grams of oxygen are produced?
1 mol KClO 3
3 mol O 2
32.0 g O 2
5.45 g KClO 3 


 2.14 g O 2
122.5 g KClO 3 2 mol KClO 3 1 mol O 2
3. When solid calcium oxide decomposes, it produces solid calcium and oxygen gas.
a) Write the balanced equation.
2 CaO  2 Ca + O2
b) How many moles of calcium are produced from 31 g of calcium oxide?
1 mol CaO 2 mol CaO
31 g CaO 

 0.55 mol Ca
56.1 g CaO 2 mol Ca
c) How many grams of calcium oxide will produce 21.5 g of oxygen?
1 mol O 2 2 mol CaO 56.1 g CaO
21.5 g O 2 


 75.3 g CaO
32.0 g O 2 1 mol O 2
1 mol CaO
4. If 3.78 g of fluorine are reacted with 10.5 g of hydrogen to produce hydrogen fluoride, which reactant is
in excess and which reactant is the limiting reagent? Determine the mass of the excess and the mass of
the product formed.
F2 + H2  2 HF
1 mol H 2
1 mol F2
 5.21mol H2 Excess
3.78 g F2 
 0.0995mol F2 Limiting 10.5 g H 2 
2.016 g H 2
38.0 g F2
2.016 g H 2
(5.21 mol H 2 - 0.0995 mol H 2 used) 
 10.3 g H 2 Excess
1 mol H 2
2 mol HF 20.0 g HF
0.0995 mol F2 

 3.98 g HF
1 mol F2
1 mol HF
5. If 25.26 g of copper react with an excess of chlorine, 50.52 g of copper II chloride are produced.
Calculate the theoretical and the percent yield.
Cu + Cl2  CuCl2
1 mol Cu 1 mol CuCl 2 134.5 g CuCl 2
25.26 g Cu 


 53.5 g CuCl2
63.5 g Cu
1 mol Cu
1 mol CuCl 2
50.52 g CuCl 2
actual yield
% yield 
 100% 
 100%  94.4%
theoretica l yield
53.5 g CuCl 2
6. How many moles are there in 10.6 L of SO2 (g) at STP?
1 mol
10.6 L SO 2 
 0.473 mol SO2
22.4 L
7. What is the mass in grams of 3.45 mL of O2 (g) at STP?
1 mol 32.0 g O 2
0.00345 L O 2 

 0.00493g O 2
22.4 L 1 mol O 2
8. How many atoms are there in 15.0 L of Ar (g) at STP?
1 mol 6.02  10 23 atoms Ar
15.5 L Ar 

 4.03 1023 atoms Ar
22.4 L
1 mol Ar
Part VII: Gases
1. If 2.00 mole of O2 (g) occupy 200 L at 0 C, what is the pressure of the O2?
kPaL
(2.00 mol)(8.31
)(273 K)
nRT
molK

 22.7 kPa
PV=nRT P 
V
200 L
2. How many moles of N2 (g) can be contained in a 3.50 L cylinder at 45 C and 202.6 kPa?
PV (202.6 kPa)(3.50 L)
n

 0.268 mol N 2
kPaL
RT
(8.31
)(318 K)
molK
3. A gas sample at 7 C and 304 kPa pressure contains 1.30 x 1022 molecules. What is the volume of the
gas?
kPaL
(0.0216 mol)(8.31
)(280 K)
nRT
molK
V

 0.165 L
P
304 kPa
4. The reaction of 2 K (s) + 2 H2O (l)  2 KOH (aq) + H2 (g) produced 45.3 mL of H2 (g) at a
temperature of 22 C and 97.8 kPa pressure. What mass of K (s) was used in the reaction?
2 mol K 39.1 g K
PV (97.8 kPa)(0.0453 L)

 0.141g K
n

 0.00181 mol H 2 0.00181 mol H 2 
kPaL
1 mol H 2 1 mol K
RT
(8.31
)(295 K)
molK
Part VIII: Composition of the Atom
1. Fill in the table:
symbol
At. #
At. Mass
#p
#n
#e
C
6
12
6
6
6
Au
79
197
79
118
79
Zn
30
65
30
35
30
He
2
4
2
2
2
Cs
55
133
55
78
55
Br-
35
80
35
45
36
Eu
63
152
63
89
63
Sc3+
21
45
21
24
18
2. Define “isotope” and give 3 examples.
Atoms of the same element with different mass numbers (different #s of neutrons)
Examples will vary
Part IX: The Periodic Table
1. State how each of the following varies as you go across a row or down a column of the periodic table:
a) electronegativity:
b) atomic radius:
See textbook / notes
c) ionization energy:
d) metallic properties:
2. How many electrons must each halogen atom gain to be isoelectronic (same number of electrons) with
the adjacent noble gas? What charge does each halogen atom have when it is isoelectronic with the
adjacent noble gas?
gain 1 electron  becomes -1 charge
3. Give the electron configuration of the following:
a) Li__1s22s1 ___________________________
e) Ba__[Xe] 6s2_________________________
b) C__1s22s22p2 ________________________
f) Br__[Ar] 4s23d104p5___________________
c) Ca__1s22s22p63s23p64s2 ________________
g) Br1-__[Ar] 4s23d104p6 _________________
d) Ca2+__1s22s22p63s23p6 _________________
h) P3-__[Ne] 3s23p6 ______________________
Part X: Chemical Bonding
1. Identify the bond type of the following (hint: use your table of electronegativities):
a) HBr
__Ionic _________
d) I2
__Covalent _____
g) LiCl
b) HCl
__Ionic _________
e) PCl3
__Covalent _____
h) MgO __Ionic__________
c) H2
__Covalent ______
f) CCl4 __Covalent _____
i) AsF3 __Covalent ______
2. Draw electron-dot structures (Lewis structures) for the following:
a)
b)
c)
·
········
··
Na
d)
Ne
e)
Mg
f)
··
········
····
H-
g)
O2-
h)
Si
i)
__Ionic__________
········
···
Sr2+
Al
········
N3-
3. What must be the charge on the following atoms in order for them to be stable? Why must this be so?
a) Ca2+
b) P3-
c) Cl-
d) B3+
4. Draw electron-dot structures for the following compounds:
a) NH3
c) CO2
e) C2H4
b) H2O
d) SO32-
f) MgCl2
5. How does the bond distance vary between a single, double, and triple bond? Which one requires more
energy to break?
C---------C C===C C≡C
triple bonds require more energy to break
Part XI: Solutions
1. Draw a table which classifies matter based on its composition (i.e. classify mixtures and pure substances
into mechanical mixtures, suspensions, solutions, elements and compounds). Then classify this table
based on its differences in properties (i.e. using homogeneous and heterogeneous classifications).
See Textbook / Notes
2. Differentiate between the following terms:
a) saturated / unsaturated:
b) miscible / immiscible:
c) soluble / insoluble:
See textbook / notes
3. Write dissociation equations for the following (make sure that they are balanced!):
a) NaCl (s)  Na+(aq) + Cl-(aq)
b) KNO3 (s)  K+(aq) + NO3-(aq)
c) NH4Cl (s)  NH4+(aq) + Cl-(aq)
d) Fe2(SO4)3 (s)  2 Fe3+(aq) + 3 SO42-(aq)
4. How many grams of NaCl are there in 250 mL of a 2.50 M solution?
2.50 mol 58.5 g
0.250 L 

 37 g NaCl
1L
1 mol
5. What volume of 0.750 M solution could be prepared from 500 g of Na2SO4?
1 mol
1L
500 g Na 2SO 4 

5L
142 g 0.750 mol
6. What is the molarity of a solution containing 250 g of CaCl2 in 1500 mL of solution?
250 g 1 mol

 1.5 M
1.500 L 111 g
7. One litre of 12.0 M HCl is diluted to 20.0 litres. What is the molarity of the diluted solution?
1L
12.0 M 
 0.600 M
20.0 L
8. To what volume must 100 mL of 6.00 M HCl be diluted in order that the resulting solution be 1.00 M?
0.1 L
6.00 M 
 1.00 M x = 0.6 L (600 mL)
x
9. If 90 mL of 0.35 M HNO3 is added to 50 mL of 0.40 M NaNO3, what is the concentration of all of the
ions in the final solution?
0.090 L
0.050 L
[HNO 3 ]  [H  ]  0.35 M 
 0.2 M [NaNO3 ]  [Na  ]  0.40 M 
 0.1M
0.140 L
0.140 L
[NO 3- ]  [HNO 3 ]  [NaNO3 ]  0.2 M  0.1M  0.3 M
10. Write the net ionic equations and state which ions are the spectator ions for each of the reactions that
occur when we mix the following:
a) AgNO3 / K2CO3
2 Ag+(aq) + CO32-(aq)  Ag2CO3 (s)
K+, NO3-
b) FeBr3 / KOH
Fe3+(aq) + 3 OH-(aq)  Fe(OH)3 (s)
K+, Br-
c) Na3PO4 / MgSO4
3 Mg2+(aq) + 2 PO43-(aq)  Mg3(PO4)2 (s)
Na+, SO42-
d) Cr2(SO4)3 / (NH4)2SO3
2 Cr3+(aq) + 3 SO32-(aq)  Cr2(SO3)3 (s)
NH4+, SO42-
Part XII: Acids & Bases
1. Give 5 characteristics of acids and 5 characteristics of bases.
See Textbook / Notes
2. 28.7 mL of 0.452 M KOH are required to neutralize 35.0 mL of HBr solution. What is the concentration
of the HBr?
0.0130 mol
mol OH -  mol H   0.0287 L  0.452 M  0.0130mol [H  ]  [HBr] 
 0.371M
0.0350 L
3. What volume of 0.230 M Ca(OH)2 is required to neutralize 50.0 mL of 0.560 M HCl? Write out your
balanced equation first.
Ca(OH)2 (aq) + 2 HCl (aq)  CaCl2 (aq) + 2 H2O (l)
mol HCl  0.0500 L  0.560 M  0.0280mol
1 mol Ca(OH) 2
1L
0.0280 mol HCl 

 0.0609L
2 mol HCl
0.230 mol Ca(OH) 2
Part XIII: Organic Chemistry
1. Explain what is wrong with each of the following. If a given name is incorrect, provide the correct name.
a)
H3C
c)
CH3
CH
CH
HC
H3C
CH
CH3
OH
propanol
2-propanol
C
CH3
1,2,3-trimethyl-1-cyclobutene
2,3,4-trimethyl-1-cyclobutene
d) H3C
CH3 CH CH3
CH3
b) 2-bromo-4-hexyne
5-bromo-2-hexyne
too many bonds on circled carbon
2. Draw the following compounds. Include all hydrogens.
a) 2,3-dimethylheptane
e) 1,4-dimethyl-3-propylbenzene
CH3 CH3
H3C
CH3
CH CH CH2 CH2 CH2 CH3
H
H
b) 1-hexanol
H
O
H
H
H
H
H
H
C
C
C
C
C
C
H
H
H
H
H
H
H
CH2 CH2 CH3
H
CH3
f) methylcyclohexane
HC
c) 1,2-difluorocyclopropane
F
F
C
H
H2C
C
g) trans-2-pentene
H
H
CH2
CH2
H3C
CH2 CH
C
CH3
CH2
H2C
CH2
CH2
C
H3C
H2C
H2C
CH2 CH3
C
d) 4-ethyl-3-octene
CH3
H
h) cis-3-hexene
H3C
CH2
C
CH2 CH3
C
H
CH2 CH2 CH2 CH2 CH3
H
3. Name the following molecules.
CH3
CH2 CH2 CH3
a) H3C CH CH2 CH3 methylbutane
f)
CH3
H3C CH2 CH CH CH2 CH2 CH3
H3C
CH2
C
C
Br
Cl
C
C
Cl
Cl
h)
c)
trichloromethane
H
cis-4-methyl-2-pentene
Br
C
I
i) Br
Br 1-bromo-2-iodocyclobutane
d)
C
CH3 trans-1,2-dibromopropene
H3C CH2 CH2
C
C
C
OH
C
e)
1-butanol
C
CH2 CH2 CH CH3
H
C
C
C
6-bromo-2-heptyne
4-ethyl-3-methylheptane
C
C
g)
CH3
b)
propylbenzene
j)
H
cis-4-octene
CH2 CH2 CH3
C
H
4. Match the following descriptions to the appropriate compounds:
a) propyne
__6 _______________
f) an amide
b) an aldehyde
__10 ______________
g) an unsaturated fatty acid__4 __________
c) ethene
__1 _______________
h) an ether
d) a ketone
__7 _______________
i) metadibromobenzene__3 ____________
e) glycerol
__8 _______________
j) an ester
(1) C2H4
__11 ____________
__9 _____________
__2 _____________
Br
O
C
(2) H3C
O
CH3
(3)
Br
O
C
(4) HO
Br
O
O
C
(7) H3C
(5)
Br
HO
CH2
HO
CH
(8) HO
C
C
C
CH3
CH2
C
(9) H3C CH2 O CH2 CH3
(6)
(10) H3C
H
O
C
(11) H3C
NH2
(12) C2H2
(13) H3C OH
O
C
(14) HO