CHEMISTRY 11
REVIEW SHEET
Final Exam Review
Introduction to Chemistry
1.
An old barometer hanging on the wall of a mountain hut has a reading of 25.5 inches of
mercury. If 1 inch of mercury equals 0.0334 atm (atmoshperes) and 1 atm = 101.3 kPa
and 1 kPa = 7.50 torr. What is the pressure reading of the barometer in torr?
2.
If sugar is $9.80 for 10 kg, what is the cost of: (a) 90.0 kg of sugar?
(b) 6.00 tonnes of
sugar (recall 1 tonne = 1000 kg)?
QUANTITY
WRITTEN UNIT
UNIT SYMBOL
PREFIX AND UNIT SYMBOLS
EXPONENTIAL EQUIVALENTS
length
mass
time
amount of substance
volume
WRITTEN PREFIX AND UNIT
1.3 kilograms
1.25 µmol
7.25 x 106 t
37.5 mmol
38.3 dekametres
93.5 cL
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CHEMISTRY 11
3.
Convert the following:
(a)
4.
REVIEW SHEET
2.25 mL into L
(c)
3125 ML into kL
(e)
25 cm/µs into km/s
If 1 L of granite has a mass of 5.50 kg,
(a)
what is the mass of 7.00 L of granite?
(b)
what is the volume occupied by 22 kg of granite?
5.
A student measured the volume of an iron nail to be 0.880 mL and found that the mass
was 6.92 g. What is the density of the iron?
6.
A sample of vegetable oil had a density of 0.916 g/mL. Calculate the mass of 0.250 L of
the oil.
7.
What volume would 2.86 g of silver occupy? The density of silver is 10.5 g/mL.
8.
Write the following numbers in scientific notation:
(a)
9.
(c)
21 700 000
(e)
95 007 000
(e)
2.57 x 106
Write the following numbers in decimal notation:
(a)
10.
23 000
2.25 x 103
(c)
3.125 x 10-4
How many significant figures does each of the following measurements have?
(a)
3218.04 cm
(c)
6.84 x 10-4 mmol
(e)
2500 s
(b)
250.000 mL
(d)
9 000 000 µs
(f)
5.2500 x 10-6 cg
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CHEMISTRY 11
11.
Determine the volumes of the following graduated cylinders:
12.
Determine the reading on the following scales:
REVIEW SHEET
13 State the rule for rounding to the correct number of significant figures after multiplying
or dividing numbers.
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CHEMISTRY 11
14.
REVIEW SHEET
Perform the indicated operations and the give the answer to the correct number of
significant figures.
15.
(a)
35.8 x 0.12
(d)
1750 x (6.7254 x 102)
(b)
128.62 ÷ 9.25
(e)
(6.1428 x 103) ÷ 0.004810
In the following mixed calculations perform multiplications and divisions before doing
the additions and subtractions. Keep track of the number of significant figures at each
stage of a calculation.
(a)
65.00 x 0.24000 – 15.78 x 0.148
(d)
16. Which of the following statements describe physical properties and which describe chemical
properties?
(a)
glass is transparent
(d)
copper conducts electricity
(b)
salt melts at 801°C
(e)
fumes from ammonia and
(c)
Adding lye to fat makes soap
hydrochloric acid mix to
produce a white smoke
17.
Which of the following are intensive properties and which are extensive?
(a)
shape
(c)
length
(e)
time to dissolve
(b)
smell
(d)
colour
(f)
density
18.
Briefly describe the characteristics of solids, liquids, and gases.
19.
Classify each of the following as one of element, compound, solution, or mechanical
mixture.
(a)
gravel
(d)
iron
(g)
orange juice
(b)
coffee
(e)
water
(h)
ammonia
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CHEMISTRY 11
20.
21.
REVIEW SHEET
Classify each of the following as one of an atom, molecule, or ion.
(a)
NH3
(c)
Pb
(e)
SO42-
(b)
Cr2O72-
(d)
PCl5
(f)
Co
How can you separate all the components in a mixture containing sand, iron filings,
water, gasoline, red water-soluble dye, and blue water-soluble dye? In pure form the
dyes are powders.
22.
Which of the following represents the cooling curve for a pure substance. Explain how
you know.
23.
Classify each of the following as either a chemical (primarily) or physical change.
(a)
formation of fog
(d)
rusting nail
(b)
burning paper
(e)
dissolving salt into water
(c)
plant growing
(f)
filtering sand and water
24.
List 4 characteristics of metals.
25.
List 4 characteristics of nonmetals.
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CHEMISTRY 11
26.
27.
Indicate which terms apply to each species. There is more than one term which applies to
each species.
N (neutral)
C (cation)
A (anion)
M (monatomic)
D (diatomic)
P (polyatomic)
(a)
SO42-
(c)
Ba2+
(e)
N2H5+
(b)
NH3
(d)
ClO-
(f)
Fe
Write the formulae for the following ionic compounds.
(a)
28.
(b)
Na2HPO4
diphosphorus trichloride
(b)
oxygen diiodide
S4N2
(b)
ClF3
zinc perchlorate hexahydrate
(b)
iron (III) sulphate nonhydrate
(c)
Co3(PO4)2•8H2O
Name the following hydrated compounds.
(a)
33.
Ag3PO4
Write the formulae for the following hydrated compounds.
(a)
32.
uranium (IV) sulphate
Name the following covalent compounds.
(a)
31.
(b)
Write the formulae for the following covalent compounds.
(a)
30.
calcium dihydrogen phosphate
Name the following ionic compounds.
(a)
29.
REVIEW SHEET
FeSO4•5H2O
Write the formulae for the following acids.
(a)
sulphuric acid
(c)
acetic acid
(b)
nitric acid
(d)
hydrochloric acid
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CHEMISTRY 11
34.
REVIEW SHEET
Name the following acids.
(a)
HF
(c)
H3PO4
(b)
H2SO3
(d)
HNO2
The Mole Concept
35.
Review the following terms: arbitrary mass, Avogadro’s hypothesis, mole, atomic
mass, molar mass, molar volume, STP, density, empirical formula, molecular formula,
empirical mass, concentration, dilution, molarity.
36.
Calculate the molar mass of each of the following.
NCl3
(a)
37.
NiSO4•7H2O
(b)
Cr(NO3)3•9H2O
(b)
5.64 x 10-5 mol of AuCl3
(b)
6.48 kg of KMnO4
Calculate the mass of the following.
(a)
39.
Al2(SO4)3
Calculate the molar mass of each of the following.
(a)
38.
(b)
4.50 mol of PCl3
Calculate the number of moles in the following.
(a)
85.6 g of CaO
40.
Calculate the molar mass of 0.00496 mol sample of cholesterol has a mass of 1.894 g
41.
What is STP and what are the experimental conditions of STP?
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CHEMISTRY 11
42.
Calculate the volume at STP occupied by the following.
(a)
43.
645 mL of SO2(g)
1 molecule of CH3CO2H
(b)
2.56 mol of (NH4)3PO4
1 Pb atom
(b)
5.62 x 1018 Fe(OH)3 molecules
60.5 g of AlCl3
(b)
84.6 mL of HCl(g) at STP
8.27 x 1020 molecules of O2(g)
(b)
125.0 g of Cl2(g)
Calculate the percentage composition of the following.
(a)
49.
(b)
What volume at STP is occupied by each of the following?
(a)
48.
64.8 L of Xe(g)
How many atoms are contained in each of the following?
(a)
47.
0.0861 mol of HCl
Find the mass, in grams, of each of the following.
(a)
46.
(b)
How many atoms are contained in the following.
(a)
45.
24.8 mol of NH3
Calculate the number of moles in the following gases at STP.
(a)
44.
REVIEW SHEET
NaHCO3
(b)
CuSO4•5H2O
Calculate the percentage composition of the bold species in each of the following.
(a)
Cr(NO3)6Cl3•H2O
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(b)
Al2(SO4)3•18H2O
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CHEMISTRY 11
50.
Find the empirical formula for the following compounds.
(a)
51.
REVIEW SHEET
12.6% Li, 29.2% S, 58.2% O
(b)
38.8% Fe, 16.7% C, 44.5% O
A gas has the empirical formula CH2. If 0.550 L of the gas at STP has a mass of 3.44 g,
what is the molecular formula?
52.
A sample of gas is analyzed and found to contain 33.0% Si and 67.0% F. If the gas has a
density of 7.60 g/L at STP, what is the molecular formula?
53.
Calculate the molar concentration of the following solutions.
54.
55.
(a)
0.578 mol of NaCl in 52.0 mL of solution
(b)
50.0 g of Fe(NO3)3 in 150.0 mL of solution
Calculate the mass of solute needed to make the following solutions.
(a)
125.0 mL of 0.0750 M KOH, from solid KOH
(b)
500.0 mL of 0.120 M FeCl3, from solid FeCl3•6H2O
What is the concentration of the solution that results when 250.0 mL of water is added to
550.0 mL of 3.50 M NaOH?
56.
If 500.0 mL of 0.100 M LiOH is boiled down to 200.0 mL, what is the concentration?
57.
What is the resulting concentration when 500.0 mL of 0.250 M NaCl is mixed with
250.0 mL of 0.450 M NaCl and the mixture is boiled down to 400.0 mL?
58.
If 250.0 mL of solution A containing 28.0 g of LiOH is mixed with 500.0 mL of
solution B containing 56.0 g of LiOH and the resulting solution is boiled down to
600.0 mL, what is the concentration?
Unit VI Chemical Reactions
59.
How can you tell that a chemical reaction has occurred?
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CHEMISTRY 11
REVIEW SHEET
60.
What is the Law of Conservation of Mass?
61.
How can you tell that a chemical equation is balanced?
3. Balance the following chemical reactions:
62.
A.
___ Si4H10 + ___ O2  ___ SiO2 + ___ H2O
B.
___ Ca3(PO4)2 + ___ SiO2 + ___ C  ___ CaSiO3 + ___ CO + ___ P4
C.
___ C3H7N2O7 + ___ O2  ___ CO2 + ___ H2O + ___ N2
Write and balance the following word equations:
A.
Aluminum + Copper (II) sulphate  Aluminum sulphate + Copper
__________________________________________________________________
B.
Magnesium nitride + Water  Magnesium hydroxide + Ammonia (NH3)
__________________________________________________________________
C.
Calcium hydroxide + Ammonium chloride  Ammonia + Calcium chloride +
Water
__________________________________________________________________
63.
Complete and balance the following reactions and classify each equation as one of:
synthesis, decomposition, single replacement, double replacement, neutralization or
combustion.
A.
___ HF + ___ Fe(OH)3  ____________________________________________
B.
___ FeCl2 + ___ K2S  ______________________________________________
C.
___ Al + ___ S8  __________________________________________________
D.
___ N2O  _______________________________________________________
E.
___ C3H6OS2 + ___ O2  ____________________________________________
F.
___ Mg + ___ HCl  _______________________________________________
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CHEMISTRY 11
64.
65.
REVIEW SHEET
Define the terms:
A.
Exothermic
B.
Endothermic
Classify the following is exothermic or endothermic:
A.
2Na + 2H2O  2NaOH + H2 + 283 kJ
B.
KClO3 + 41.4 kJ  K+ + ClO3–
C.
C2H6 + O2  CO2 + H2O
D.
12CO2 + 11H2O  C12H22O11 + 12O2
∆H = – 3718 kJ
∆H = +5638 kJ
Unit VII Stoichiometry
66.
What are limiting and excess reactants?
67.
Consider the reaction: 4C4H9SO2 + 25O2  16CO2 + 18H2O + 4SO2
68.
A.
How many oxygen molecules react with 20 molecules of C4H9SO2?
B.
How many moles of C4H9SO2 are required to produce 100 moles of water?
C.
What mass of SO2 is formed when 50.0 g of C4H9SO2 is reacted?
A 25.0 mL sample of Al(OH)3 is titrated with 67.8 mL of 0.450 M HCl according to the
reaction
Al(OH)3 + 3HCl  AlCl3 + 3H2O
What is the concentration of the original Al(OH)3 solution?
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CHEMISTRY 11
69.
REVIEW SHEET
What mass of CS2 is produced when 25.8 g of C are reacted with 54.2 g of SO2 according
to the equation
5C + 2SO2  CS2 + 4CO
70.
A.
What mass of CS2 is produced?
B.
What mass of the excess reactant will be left over?
Consider the reaction
K2Cr2O7 + 6NaI + 7H2SO4  Cr2(SO4)3 + 3I2 + 7H2O + 3Na2SO4 + K2SO4
A 35.0 g sample of pure K2Cr2O7 produces 9.67 g of H2O. What is the percentage yield?
Unit VIII Atoms, Periodic Table, and Bonding
71.
Which model of the atom is described by the following:
A.
Dense positively charged nucleus with electrons orbiting like planets around the
sun.
B.
Correctly predicts the spectrum of hydrogen.
C.
Plum pudding model.
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CHEMISTRY 11
D.
72.
REVIEW SHEET
Atoms are like small spherical balls of matter.
Fill in the following table:
SYMBOL
PROTONS
NEUTRON
ELECTRONS
Rh
107
Pd2+
123
73.
74.
75.
Sb3–
93
89
50
46
Write the electron configurations for the following:
(a)
Mo
(b)
Bi
(c)
Bk
(d)
Ag+
(e)
As3–
(f)
Pb4+
State the chemical family or group to which each of the following elements belongs.
(a)
silver
(d)
xenon
(g)
silicon
(b)
calcium
(e)
potassium
(h)
promethium
(c)
iodine
(f)
californium
(i)
tungsten
Consider the two atoms Sn and I.
(a)
Which atom has the larger atomic radius?
(b)
Which atom has the larger ionization energy?
(c)
Which atom has more shells?
(d)
How many valence electrons each atom have?
(e)
What is the valence of each atom?
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CHEMISTRY 11
(f)
76.
Na and O
(b)
H and C
(c)
N and F
Which member of each following pair would you expect to have the higher melting
point?
(a)
78.
Which atom has a greater electrostatic attraction between its nucleus and
outermost electrons?
Which of the following pairs would you expect to form ionic bonds and which would you
expect to form covalent bonds?
(a)
77.
REVIEW SHEET
MgO and CsCl
(b)
LiF and BeO
(c)
MgS and BaS
(c)
PF5
Predict the shape of the following molecules.
(a)
NCl3
(b)
H2O
Unit X Organic Chemistry
79.
Name the following compounds:
A.
C—C—C—C—C—C—C—C
|
C—C—C—C
B.
C—C
|
C—C  C—C—C—C—C—C
|
|
C—C—C
C—C
__________________________________
__________________________________
C.
D.
Br F
C—C—C
| |
|
C—C—C—C—C—C—C—C
|
|
|
Br
F
C—C
F F
| |
C—C  C—C—C—C—C—C
|
F
__________________________________
__________________________________
E.
F.
C—C—C—C
|
Br
\
C—C—C—C—C—C
/
—C—C—C—C
\
C—C—C
__________________________________
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|
Br
__________________________________
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CHEMISTRY 11
80.
81.
82.
REVIEW SHEET
Draw the following compounds (draw carbon skeletons only).
A.
2,2,4,4–tetramethylheptane
B.
3,4–diethyl–3–methyl–1–heptyne
Draw the following compounds (draw carbon skeletons only).
A.
1,3–dipropylcyclopentane
B.
1,1,1–trifluoro–2–methylpentane
Draw the following compounds
A.
3–methyl–1–hexanol
REVIEW FOR FINAL EXAMINATION
B.
1, 2,4–trimethyl benzene
15
CHEMISTRY 11
83.
REVIEW SHEET
Name the following geometric isomers (remember to include cis or trans as appropriate)
A.
C—C—C
C—C
\
/
C=C
/
\
C
C—C—C
__________________________________
84.
B.
C—C—C
\
C=C
C—C
/
\
|
C
C—C—C—C
__________________________________
(A) Name the functional groups:
Carboxyllic acid
Ester
Aromatic ring
Halide
Alcohol
Aldehyde
Ketone
Ether
Amine
Amide
A.
C–C–C–C–C–C–O–C–C
B.
O
||
/
C
\
C–C–C
________________________________
________________________________
C.
D.
F–C–C = C–C–C–C–F
|
C
F
C
|
|
C–C–C–C–C–C–CO–C–C
|
|
C
C
________________________________
________________________________
E.
F.
–CHO
C
C
O
|
|
||
C–C–C–C–C–C–C–C–C
|
|
C
C–C–C
________________________________
________________________________
G.
H.
C–C–C–C–C–COO–C
REVIEW FOR FINAL EXAMINATION
C–C–C–C–C–C–C–NH2
|
|
NH2 NH2
16
CHEMISTRY 11
REVIEW SHEET
________________________________
________________________________
I.
J
F
|
C–C–C–C–C–C–C–COOH
|
|
F
C
________________________________
REVIEW FOR FINAL EXAMINATION
OH
|
|
C
|
C
________________________________
17
CHEMISTRY 11
ANSWERS TO REVIEW SHEET
Answers
1.
An old barometer hanging on the wall of a mountain hut has a reading of 25.5 inches of
mercury. If 1 inch of mercury equals 0.0334 atm (atmoshperes) and 1 atm = 101.3 kPa
and 1 kPa = 7.50 torr. What is the pressure reading of the barometer in torr? 647 torr
2.
If sugar is $9.80 for 10 kg, what is the cost of: (a) 90.0 kg of sugar? $88.20 (b) 6.00
tonnes of sugar (recall 1 tonne = 1000 kg)? $5.88E3
QUANTITY
WRITTEN UNIT
UNIT SYMBOL
length
Metre
M
mass
g
g
time
Second
S
amount of substance
Mole
Mol
volume
Litre
L
WRITTEN PREFIX AND UNIT
PREFIX AND UNIT SYMBOLS
EXPONENTIAL EQUIVALENTS
1.3 kilograms
1.3 kg
103
1.25 micromoles
1.25 µmol
1.25 E -6
7.25 megatonnes
7.25 Mt
7.25 x 106 t
37.5 millimoles
37.5 mmol
37.5E-3 mol
38.3 dekametres
38.3dam
38.3 E1 m
93.5 centilitres
93.5 cL
93.5 E-2 L
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CHEMISTRY 11
3.
ANSWERS TO REVIEW SHEET
Convert the following:
(a)
2.25 mL into L
(c)
2.25E-3L
4.
3125 ML into kL
(e)
25 cm/µs into km/s
3.125E6 kL
2.5 E 2 km/s
If 1 L of granite has a mass of 5.50 kg,
(a)
what is the mass of 7.00 L of granite? 38.5 kg
(b)
what is the volume occupied by 22 kg of granite? 4L
5.
A student measured the volume of an iron nail to be 0.880 mL and found that the mass
was 6.92 g. What is the density of the iron? 7.86 g/mL
6.
A sample of vegetable oil had a density of 0.916 g/mL. Calculate the mass of 0.250 L of
the oil. 229g
7.
What volume would 2.86 g of silver occupy? The density of silver is 10.5 g/mL..
0.272mL
8.
Write the following numbers in scientific notation:
(a)
23 000, 2.3E4
(c)
21 700 000, 2.17E7
(e)
95 007 000,
9.5007E7
9.
Write the following numbers in decimal notation:
(a)
2.25 x 103, 2250
(c)
3.125 x 10-4,
0.0003125
10.
2.57 x 106
(e)
2 570 000
How many significant figures does each of the following measurements have?
(a)
3218.04 cm 6
(c)
6.84 x 10-4 mmol 3
(e)
2500 s 2
(b)
250.000 mL 6
(d)
9 000 000 µs 1
(f)
5.2500 x 10-6 cg 5
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CHEMISTRY 11
11.
ANSWERS TO REVIEW SHEET
Determine the volumes of the following graduated cylinders:
54.2+/-.1
12.
82+/-1
38.0+/-.5
Determine the reading on the following scales:
15.17+-.01
10.0+-.02
6.40+-.05
15.69+-.01
16.4+-.02
7.60+-.05
13 State the rule for rounding to the correct number of significant figures after multiplying
or dividing numbers. Lowest number for mult and div, only one uncertain column for
add and sub
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CHEMISTRY 11
14.
ANSWERS TO REVIEW SHEET
Perform the indicated operations and the give the answer to the correct number of
significant figures.
(a)
35.8 x 0.12 =4.3
(d)
1750 x (6.7254 x 102)=1.18E6
(b)
128.62 ÷ 9.25=13.9
(e)
(6.1428 x 103) ÷ 0.004810=
1.277E6
15.
In the following mixed calculations perform multiplications and divisions before doing
the additions and subtractions. Keep track of the number of significant figures at each
stage of a calculation.
(a)
65.00 x 0.24000 – 15.78 x 0.148
(d)
=3E2
=13.26
16.
Which of the following statements describe physical properties and which describe
chemical properties?
(a)
glass is transparent P
(d)
copper conducts electricity P
(b)
salt melts at 801°C P
(e)
fumes from ammonia and
(c)
Adding lye to fat makes soap C
hydrochloric acid mix to
produce a white smoke C
17.
18.
Which of the following are intensive properties and which are extensive?
(a)
shape e
(c)
length e
(e)time to dissolve e
(b)
smell i
(d)
colour i
(f)
density i
Briefly describe the characteristics of solids (fixed shape and volume, particles touching
with only vibrations), liquids (fixed volume, particles can slide past one another, and
gases (particles move quickly and are separated by lots of space).
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CHEMISTRY 11
19.
ANSWERS TO REVIEW SHEET
Classify each of the following as one of element, compound, solution, or mechanical
mixture.
20.
21.
(a)
gravel m
(d)
iron e
(g)
orange juice m
(b)
coffee s
(e)
water c
(h)
ammonia c
Classify each of the following as one of an atom, molecule, or ion.
(a)
NH3 m
(c)
Pb a
(e)
SO42- i
(b)
Cr2O72- i
(d)
PCl5 m
(f)
Co a
How can you separate all the components in a mixture containing sand, iron filings,
water, gasoline, red water-soluble dye, and blue water-soluble dye? In pure form the
dyes are powders…magnet (iron), filter (sand), sep funnel (gas), evaporate (water),
chromatography (dyes)
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5
CHEMISTRY 11
22.
ANSWERS TO REVIEW SHEET
Which of the following represents the cooling curve for a pure substance. Explain how
you know.
c cooling and plateus at phase change
23.
Classify each of the following as either a chemical (primarily) or physical change.
(a)
formation of fog p
(d)
rusting nail c
(b)
burning paper c
(e)
dissolving salt into water p
(c)
plant growing c
(f)
filtering sand and water p
24.
List 4 characteristics of metals. Shiny, ductile, malleable, conductor
25.
List 4 characteristics of nonmetals. Brittle, dull, poor conductor, usually gas
26.
Indicate which terms apply to each species. There is more than one term which applies to
each species.
N (neutral)
C (cation)
A (anion)
M (monatomic)
D (diatomic)
P (polyatomic)
(a)
A, P, SO42-
(c)
C, M, Ba2+
(e)
C, P, N2H5+
(b)
N, P, NH3
(d)
A, D, ClO-
(f)
N, M, Fe
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CHEMISTRY 11
27.
Write the formulae for the following ionic compounds.
(a)
28.
ANSWERS TO REVIEW SHEET
calcium dihydrogen phosphate
(b)
Ca2(H2PO4)2
U(SO4)2
Name the following ionic compounds.
(a)
Ag3PO4
Silver phosphate
29.
diphosphorus trichloride P2Cl3
S4N2 tetrasulphur dinitride
zinc perchlorate hexahydrate
Zn(ClO4)2.6H2O
FeSO4•5H2O
Iron (II) sulphate pentahydrate
34.
(b)
oxygen diiodide OI2
(b)
ClF3 Chlorine trifluoride
(b)
iron (III) sulphate nonhydrate
Fe2(SO4)3.9H2O
Name the following hydrated compounds.
(a)
33.
sodium monohydrogen phosphate
Write the formulae for the following hydrated compounds.
(a)
32.
Na2HPO4
Name the following covalent compounds.
(a)
31.
(b)
Write the formulae for the following covalent compounds.
(a)
30.
uranium (IV) sulphate
(b)
Co3(PO4)2•8H2O
Cobalt (II) phosphate octahydrate
Write the formulae for the following acids.
(a)
sulphuric acid H2SO4
(c)
acetic acid CH3COOH
(b)
nitric acid HNO3
(d)
hydrochloric acid HCl
Name the following acids.
(a)
HF hydrofluoric acid
(c)
H3PO4 phosphoric acid
(b)
H2SO3 sulphurous acid
(d)
HNO2 nitrous acid
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7
CHEMISTRY 11
ANSWERS TO REVIEW SHEET
The Mole Concept
36.
Calculate the molar mass of each of the following.
NCl3
(b)
120.5g/mol
37.
342.3g/mol
Calculate the molar mass of each of the following.
(a)
NiSO4•7H2O
280.8g/mol
38.
4.50 mol of PCl3
619 g
Cr(NO3)3•9H2O
400.0g/mol
(b)
5.64 x 10-5 mol of AuCl3
0.0171 g
Calculate the number of moles in the following.
(a)
85.6 g of CaO
1.53 mol
40.
(b)
Calculate the mass of the following.
(a)
39.
Al2(SO4)3
(c)
(b)
6.48 kg of KMnO4
41.0 mol
Calculate the molar mass of 0.00496 mol sample of cholesterol has a mass of 1.894 g.
382 g/mol
41.
What is STP and what are the experimental conditions of STP? Standard temp (0-oC) and
pressure (101.3 kPa)
42.
Calculate the volume at STP occupied by the following.
(c)
24.8 mol of NH3
556 L
43.
0.0861 mol of HCl
1.93L
Calculate the number of moles in the following gases at STP.
(a)
44.
(c)
64.8 L of Xe(g)= 2.89 mol
(b)
645 mL of SO2(g) = 2.88E-2 mol
How many atoms are contained in the following.
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8
CHEMISTRY 11
(a)
1 molecule of CH3CO2H
8
45.
(b)
2.56 mol of (NH4)3PO4
3.08E25
Find the mass, in grams, of each of the following.
(a)
1 Pb atom
3.44E-22 g
46.
ANSWERS TO REVIEW SHEET
(b)
5.62 x 1018 Fe(OH)3 molecules
9.97E-4 g
How many atoms are contained in each of the following?
(a)
60.5 g of AlCl3= 1.09E24
(b)
84.6 mL of HCl(g) at STP=
4.55E21
47.
What volume at STP is occupied by each of the following?
(a)
8.27 x 1020 molecules of O2(g)
30.1mL
48.
(b)
125.0 g of Cl2(g)
39.4L
Calculate the percentage composition of the following.
(a)
Na (27.4)H (1.2)C (14.3) O3(57.1)
(c)
CuSO4•5H2O
Cu-25.4, S-12.1, O-57.7, H-4.0
49.
Calculate the percentage composition of the bold species in each of the following.
(a)
Cr(NO3)6Cl3•H2O
67.8%
50.
Al2(SO4)3•18H2O
43.3%
Find the empirical formula for the following compounds.
(a)
12.6% Li, 29.2% S, 58.2% O
Li2SO4
51.
(b)
(b)
38.8% Fe, 16.7% C, 44.5% O
FeC2O4
A gas has the empirical formula CH2. If 0.550 L of the gas at STP has a mass of 3.44 g,
what is the molecular formula? C10H20
REVIEW FOR FINAL EXAMINATION
9
CHEMISTRY 11
ANSWERS TO REVIEW SHEET
52.
A sample of gas is analyzed and found to contain 33.0% Si and 67.0% F. If the gas has a
density of 7.60 g/L at STP, what is the molecular formula? Si2F6
53.
Calculate the molar concentration of the following solutions.
54.
55.
(a)
0.578 mol of NaCl in 52.0 mL of solution. 11.1M
(b)
50.0 g of Fe(NO3)3 in 150.0 mL of solution 1.38M
Calculate the mass of solute needed to make the following solutions.
(a)
125.0 mL of 0.0750 M KOH, from solid KOH 0.526g
(b)
500.0 mL of 0.120 M FeCl3, from solid FeCl3•6H2O
What is the concentration of the solution that results when 250.0 mL of water is added to
550.0 mL of 3.50 M NaOH? 2.41M
56.
If 500.0 mL of 0.100 M LiOH is boiled down to 200.0 mL, what is the concentration?
0.25M
57.
What is the resulting concentration when 500.0 mL of 0.250 M NaCl is mixed with
250.0 mL of 0.450 M NaCl and the mixture is boiled down to 400.0 mL?0.594M
58.
If 250.0 mL of solution A containing 28.0 g of LiOH is mixed with 500.0 mL of
solution B containing 56.0 g of LiOH and the resulting solution is boiled down to
600.0 mL, what is the concentration? 5.86M
Unit VI Chemical Reactions
59.
How can you tell that a chemical reaction has occurred?
New properties due to new substances.
(d)
What is the Law of Conservation of Mass?
Mass of products = mass of reactants in a closed reaction
60. How can you tell that a chemical equation is balanced?
a. Equal #s of atoms on each side
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10
CHEMISTRY 11
61.
62.
ANSWERS TO REVIEW SHEET
Balance the following chemical reactions:
A.
2 Si4H10 + 13 O2  8 SiO2 + 10 H2O
B.
2 Ca3(PO4)2 + 6 SiO2 + 10 C  6 CaSiO3 + 10 CO + 1 P4
C.
4C3H7N2O7 + 5 O2  12 CO2 + 14 H2O + 4 N2
Write and balance the following word equations:
A.
Aluminum + Copper (II) sulphate  Aluminum sulphate + Copper
2Al + 3CuSO4  1Al2(SO4)3 + 3Cu
B.
Magnesium nitride + Water  Magnesium hydroxide + Ammonia (NH3)
1Mg3N2 + 6H2O  3Mg(OH)2 + 2NH3
C.
Calcium hydroxide + Ammonium chloride  Ammonia + Calcium chloride +
Water
1Ca(OH)2 + 2NH4Cl  2NH3 + 1CaCl2 + 2H2O
63.
64.
Complete and balance the following reactions and classify each equation as one of:
synthesis, decomposition, single replacement, double replacement, neutralization or
combustion.
A.
3 HF + 1 Fe(OH)3 neut 3H2O + 1FeF3
B.
1 FeCl2 + 1K2S dr 1FeS + 2KCl
C.
16 Al + 3 S8  syn 8Al2S3
D.
2N2O decom 2N2 + 1O2
E.
1C3H6OS2 + ___ O2 combust 3CO2 + 3H2O + 2SO2
F.
1 Mg + 2 HCl s.r. 1MgCl2 + 2H2
Define the terms:
A.
Exothermic
Heat exits the system
B.
Endothermic
Heat enters the system
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11
CHEMISTRY 11
65.
ANSWERS TO REVIEW SHEET
Classify the following is exothermic or endothermic:
A.
2Na + 2H2O  2NaOH + H2 + 283 kJ ex
B.
KClO3 + 41.4 kJ  K+ + ClO3– en
C.
C2H6 + O2  CO2 + H2O
D.
12CO2 + 11H2O  C12H22O11 + 12O2
∆H = – 3718 kJ ex
∆H = +5638 kJ en
Unit VII Stoichiometry
65.
What are limiting (runs out and determines the amount of product) and excess (there is
more than is needed to fully react with the limiting reactant )reactants?
66.
Consider the reaction: 4C4H9SO2 + 25O2  16CO2 + 18H2O + 4SO2
A.
How many oxygen molecules react with 20 molecules of C4H9SO2?
125
B.
How many moles of C4H9SO2 are required to produce 100 moles of water?
22.2
C.
67.
What mass of SO2 is formed when 50.0 g of C4H9SO2 is reacted? 26.5g
A 25.0 mL sample of Al(OH)3 is titrated with 67.8 mL of 0.450 M HCl according to the
reaction
Al(OH)3 + 3HCl  AlCl3 + 3H2O
What is the concentration of the original Al(OH)3 solution? 0.407M
68.
What mass of CS2 is produced when 25.8 g of C are reacted with 54.2 g of SO2 according
to the equation
5C + 2SO2  CS2 + 4CO
A.
What mass of CS2 is produced? 32.2g
B.
What mass of the excess reactant will be left over? 0.4g C
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12
CHEMISTRY 11
69.
ANSWERS TO REVIEW SHEET
Consider the reaction
K2Cr2O7 + 6NaI + 7H2SO4  Cr2(SO4)3 + 3I2 + 7H2O + 3Na2SO4 + K2SO4
A 35.0 g sample of pure K2Cr2O7 produces 9.67 g of H2O. What is the percentage yield?
64.5%
Unit VIII Atoms, Periodic Table, and Bonding
70.
71.
Which model of the atom is described by the following:
A.
Dense positively charged nucleus with electrons orbiting like planets around the
sun. rutherford
B.
Correctly predicts the spectrum of hydrogen. bohr
C.
Plum pudding model. thompson
D.
Atoms are like small spherical balls of matter. Dalton
Fill in the following table:
SYMBOL
PROTONS
NEUTRON
ELECTRONS
Rh
45
58
45
46
61
44
Sb3–
51
72
54
Np4+
93
144
89
50
69
46
107
Pd2+
123
237
119
72.
73.
Sn4+
Write the electron configurations for the following:
(a)
Mo= [Kr]5s24d4
(b)
Bi =[Xe] 6s24f14 5d10 6p3
(c)
Bk=[Rn]7s26d15f8
(d)
Ag+ =[Kr] 5s1 4d9 or 4d10 like copper
(e)
As3–=[Ar]4s23d104p6
(f)
Pb4+= 4f14 5d10
State the chemical family or group to which each of the following elements belongs.
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CHEMISTRY 11
74.
75.
(a)
silver trans
(d)
xenon noble
(g)
silicon rep
(b)
calcium alk earth
(e)
potassium alk met
(h)
promethium lanth
(c)
iodine halo
(f)
californium Act
(i)
tungsten trans
Consider the two atoms Sn and I.
(a)
Which atom has the larger atomic radius? Sn
(b)
Which atom has the larger ionization energy? I
(c)
Which atom has more shells? tie
(d)
How many valence electrons each atom have? Sn 4, I 7
(e)
What is the valence of each atom? Sn 4, I 1
(f)
Which atom has a greater electrostatic attraction between its nucleus and
outermost electrons? I
Which of the following pairs would you expect to form ionic bonds and which would you
expect to form covalent bonds?
(a)
76.
Na and O Ionic
(b)
H and C covalent
(c)
N and F covalent
Which member of each following pair would you expect to have the higher melting
point?
(a)
77.
ANSWERS TO REVIEW SHEET
MgO and CsCl
(b)
LiF and BeO
(c)
MgS and BaS
(c)
PF5 trigonal bipyramid
Predict the shape of the following molecules.
(a)
NCl3 trigonal pyramid
(b)
H2O bent
Unit X Organic Chemistry
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14
CHEMISTRY 11
78.
ANSWERS TO REVIEW SHEET
Name the following compounds:
A.
C—C—C—C—C—C—C—C
|
C—C—C—C
4, 6-diethyl-4-propyl-2-octyne
C.
D.
Br F
C—C—C
| |
|
C—C—C—C—C—C—C—C
|
|
|
Br
F
C—C
C—C—C—C
|
E.
\
C—C—C
1-butyl-3-propylcyclopentane
F F
| |
C—C  C—C—C—C—C—C
|
F
4,5,6-trifluoro-2-octyne
F.
Br
\
C—C—C—C—C—C
/
—C—C—C—C
|
Br
1,5-dibromo-2-butyl-3-hexylbenzene
Draw the following compounds (draw carbon skeletons only).
A.
2,2,4,4–tetramethylheptane
CH3
H3C
B.
CH3
CH3
CH3
80.
C—C
|
C—C  C—C—C—C—C—C
|
|
C—C—C
C—C
5-propylnonane
1,2-dibromo-6-ethyl-2,4-difluoro-4propyloctane
79.
B.
CH3
3,4–diethyl–3–methyl–1–heptyne
Draw the following compounds (draw carbon skeletons only).
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CHEMISTRY 11
A.
ANSWERS TO REVIEW SHEET
1,3–dipropylcyclopentane
H3C
CH3
B.
1,1,1–trifluoro–2–methylpentane
F
CH3
F
F
CH3
81.
Draw the following compounds
A.
3–methyl–1–hexanol
CH3
CH3
H3C
HO
82.
CH3
1, 2,4–trimethyl benzene
CH3
Name the following geometric isomers (remember to include cis or trans as appropriate)
A.
C—C—C
C—C
\
/
C=C
/
\
C
C—C—C
4-ethyl-5-methyl-trans-4-octene
83.
B.
B.
C—C—C
\
C=C
C—C
/
\
|
C
C—C—C—C
7-ethyl-4-methyl-trans-4-nonene
(A) Name the functional groups:
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16
CHEMISTRY 11
ANSWERS TO REVIEW SHEET
Carboxyllic acid
Ester
Aromatic ring
Halide
Alcohol
Aldehyde
Ketone
Ether
Amine
Amide
A.
C–C–C–C–C–C–O–C–C
B.
O
||
/
C
Ether
\
C–C–C
ketone
C.
F–C–C = C–C–C–C–F
|
C
D.
F
C
|
|
C–C–C–C–C–C–CO–C–C
|
|
C
C
Halide
Halide, ketone
E.
F.
–CHO
C
C
O
|
|
||
C–C–C–C–C–C–C–C–C
|
|
C
C–C–C
Aldehyde and aromatic ring
ketone
G.
H.
C–C–C–C–C–COO–C
ester
I.
C–C–C–C–C–C–C–NH2
|
|
NH2 NH2
amine
F
|
C–C–C–C–C–C–C–COOH
|
|
F
C
Carboxylic acid, halide
REVIEW FOR FINAL EXAMINATION
J
OH
|
|
C
|
C
alcohol
17