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Chemistry 20 Review
1.
Lab Safety.
a)
What is the WHMIS symbol for a flammable substance?
b)
What is the household symbol which means "the contents of the container are
flammable"?
c)
What is the symbol for a radioactive substance?
d)
What are the three WHMIS symbols which warn of poisons, and what is the
difference between them?
Class D, Division 1 - Poisonous and infectious material. Acute toxin; immediate
and serious toxic effects.
Class D, Division 2 - Poisonous and infectious material. Chronic toxin; other toxic
effects; may cause cancer or other diseases because of long term exposure
Class D, Division 3 - Poisonous and infectious material. Biohazard; may cause
infections and other effects
2.
3.
Metric System
a)
List all prefixes, base units and derived units, along with their values.
b)
How many g are there in 0.62 kg ?
620 g
c)
How many L are there in 145 mL ?
0.145 L
d)
How many nm are there in 2.11 x 10-6 km ?
2.11 x 106 nm
Significant Digits
a)
b)
Perform the following additions and subtractions:
i)
22.26 g + 19.1 g
41.4 g
ii)
100.1 L + 0.025 L
100.1 L
iii)
8.21 mL + 2.79 mL
11.00 mL
iv)
2500 L - 155 L
2300 L
v)
1.236 mol - 0.33 mol
0.91 mol
vi)
19 mol - 18.75 mol
0 mol
Perform the following multiplications and divisions
i)
233 g / 15.36 g/mol
15.2 mol
ii)
1.59 mol / 0.12 L
13 mol/L
iii)
16 g x (1 kg / 1000 g)
0.016 kg
iv)
13.1 mol x 44.01 g/mol
v)
22 L x 2.145 mol/L
47 mol
vi)
100 g / 18.02 g/mol
6 mol
577 g
4.
Nomenclature
a)
Give the formulas for the following substances:
i)
ii)
iii)
iv)
v)
vi)
vii)
viii)
ix)
x)
b)
magnesium hydroxide
sodium hydrogen carbonate
aluminum oxide
calcium oxide hexahydrate
phosphorus pentaoxide
iron (III) phosphate
hexane
ethanol
2-methyl-2-pentene
benzene
Give the name for the following compounds:
i) NaCl
ii) NH3
iii) CaSO4
iv) N2O4
v) C2H2
vi) Ca(OH)2 ·5H2O
vii) MnO2
viii) CO2
ix) NH4NO3
x) C8H18
c)
Mg(OH)2
NaHCO3
Al2O3
CaO  6 H2O
PO5
FePO4
C6H14
C2H5OH
C6H12
C6H6
sodium chloride
ammonia
calcium sulfate
dinitrogen tetraoxide
ethyne
calcium hydroxide pentahydrate
manganese (IV) oxide
carbon dioxide
ammonium nitrate
octane
Draw the structure of each of the following molecules:
i)
nonane
H H H H H H H H H
H C C C C C C C C C H
H H H H H H H H H
ii)
2-hexene
iii)
propyne
iv)
2,3-dimethyl pentane
v)
2-methyl-3-ethylheptane
vi)
cyclobutane
vii)
toluene
viii)
2,2,3-trifluoro-3-hexen-5-ol
5
5.
The Mole
a)
Determine the molar mass of
(i) NaOH
(ii) Cu(NO3)2
(iii) SnCl4
(iv) C2H5OH
(v) O2
(vi) Mg(OH)2  9 H2O
b)
Calculate the number of moles in
(i) 65.0 grams of Ag
(ii) 423 g of N
(iii) 325 grams of Sn
c)
149 g
4.1 g
(119 mol) 7.2 x 103 g
Calculate the concentration of the following
(i)
(ii)
(iii)
(iv)
e)
0.603 mol
30.2 mol
2.74 mol
Calculate the mass of
(i) 2.35 moles of Cu atoms
(ii) 0.17 moles of Mg atoms
(iii) 2.5 x 103 mol of chlorine gas
d)
40.00 g/mol
187.56 g/mol
260.49 g/mol
46.08 g/mol
32.00 g/mol
220.51 g/mol
0.025
25.00
10.00
55.00
mol of NaCl in 50.0 mL of water
mol of Ca(OH)2 in 15.0 L
g of Mg3(PO4)2 in 500.0 mL
g of C6H11O6 in 355.0 mL
0.50 mol/L
1.67 mol/L
0.07608 mol/L
0.8647 mol/L
Determine the following:
(i)
(ii)
(iii)
(iv)
Moles of CaCO3 in 300.0 mL of 1.5 x 10-4 mol/L solution
4.5 x 10-3 mol
-2
Mass of O2 in 50.00 L of 1.00 x 10 mol/L solution
16.0 g
Volume of 1.30 mol/L solution of CuCl which contains 0.025 mol CuCl.
0.0192 L
Volume of 6.50 x 10-3 mol/L solution of NaNO3 which contains 15.00 g
NaNO3
27.1 L
6
f)
6.
Determine the following:
(i)
Moles of CO2 in 160 L of gas at STP
7.1 mol
(ii)
Moles of O2 in 2.11 x 108 L of gas at STP 9.42 x 106 mol
(iii)
Volume of 65.2 mol of N2 gas at STP
1460 L
(iv)
Mass of 89.1 L of He gas at STP
3.98 mol, 15.9 g
(v)
Volume of 5.46 g of Ne gas at STP
0.271 mol, 6.06 L
Chemical Equations
i)
Balance the following equations. Use whole numbers only.
a)
ii)
2 Mg +
1 O2 
2 MgO
b)
2 CuS +
3 O2 
2 CuO +
c)
1 (NH4)2S +
d)
1 P2O5 + 1 H2O 
1 Pb(NO3)2 
2 SO2
2 NH4NO3 + 1
2 PO2 + 1
O2 +
PbS
1 H2
Write and balance the following equations.
a)
The complete combustion of butane gas, C 4H10.
2 C4H10 (g) + 13 O2 (g)  8 CO2 (g) + 10 H2O(g)
b)
The synthesis of sulphur dioxide gas from its elements.
1 S8 (s) + 8 O2 (g)  8 SO2 (g)
c)
A solution of silver nitrate reacts with aqueous calcium chloride to
produce aqueous calcium nitrate and a precipitate of silver chloride.
2 AgNO3 (aq) + 1 CaCl2 (aq)  1 Ca(NO3)2 (aq0 + 2 AgCl(s)
d)
When heated, solid calcium carbonate decomposes to form carbon
dioxide gas and solid calcium oxide.
1 CaCO3 (s)  1 CO2 (g) + 1 CaO(s)
7
7.
Gravimetric Stoichiometry
i)
In the cells of our bodies simple sugars (C6H12O6) react with oxygen to form
carbon dioxide and water.
The balanced equation for this reaction is:
1 C6H12O6 (s) + 6 O2 (g)  6 CO2 (g) + 6 H2O(l)
a)
b)
c)
d)
ii)
If a person eats 1802 g of sugar, how many moles of sugar has he or
she eaten ?
10.00 mol
If a person eats 1802 g of sugar, how many moles of water will be
formed ?
mol water/ mol sugar = 6 mol/1mol = x/10 mol
x = 60.00 mol
If a person eats 1802 g of sugar, how many grams of water will be
formed ?
1081 g H2O
If a person eats 1802 g of sugar, what volume of CO2 gas will be
produced at STP ?
1344 L
To make fertilizer methane gas is burned in the presence of nitrogen gas and
oxygen gas to form ammonia gas and carbon dioxide gas.
a)
Write the balanced chemical equation
3 CH4 (g) + 2 N2 (g) + 3 O2 (g)  4 NH3
b)
(g)
+ 3 CO2 (g)
If 460. t of methane is burned, what mass of ammonia gas will be
produced ?
460. t = 4.60 x 108 g , 2.87 x 107 mol CH4, 3.82 x 107 mol NH3 ,
6.51 x 108 g NH3
c)
If 8.23 x 106 L of methane gas at STP is burned, what volume of ammonia gas at
STP will be produced ?
3.67 x 105 mol CH4 , 4.90 x 105 mol NH3 , 1.10 x 107 L NH3
8
8.
Atomic Theory
a)
Describe the nature and role of the proton, neutron, and electron in the atom.
Proton
Neutron
Electron
Location
in the nucleus.
Cannot leave
in the nucleus.
Cannot leave
in orbit about
nucleus. Can be
added to or taken
away from atom
Charge
positive (1+)
neutral (0)
negative (1-)
Mass
large
equal to proton
insignificant
Role in the Atom
- number of protons
determines atomic
number.
- gives the identity of
the atom
- with protons
determines the mass
number of the atom;
determines the
isotope
- mediates strong
nuclear force; holds
nucleus together
- with protons
determines atomic
charge
- responsible for
chemical and physical
properties of an
element.
b)
c)
Draw the electron configuration of the following:
(i) Mg
1s22s22p63s13p1 (electron promotion)
(ii) Ag
1s22s22p63s23p64s23d104p65s24d9
(iii) Rn
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p6
(iv) Es
1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p67s25f11
Draw the orbital diagram of the following:
1s
2s
2p
(i) Mg
↑↓
↑↓
↑↓ ↑↓ ↑↓
↑
↑
(ii) Ar
↑↓
↑↓
↑↓ ↑↓ ↑↓
↑↓
↑↓ ↑↓ ↑↓
(iii) Xe
↑↓
↑↓
↑↓ ↑↓ ↑↓
↑↓
↑↓ ↑↓ ↑↓
4s
↑↓
5p
↑↓ ↑↓ ↑↓
3d
↑↓ ↑↓ ↑↓ ↑↓ ↑↓
3s
3p
4p
5s
↑↓ ↑↓ ↑↓
↑↓
4d
↑↓ ↑↓ ↑↓ ↑↓ ↑↓
9
d)
Draw the Lewis diagram for the following:
(i)
(iii)
(v)
(ii)
(iv)
(vi)
e)
(vii)
(viii)
List the diatomic elements, as well as the two other polyatomic elements.
H2 N2 O2 F2 Cl2 Br2 I2 At2 S8 P4
f)
g)
Determine the number of protons and electrons in the following:
(i) Ca2+
20 protons, 18 electrons
(ii) Ar
18 protons, 18 electrons
(iii) P3-
15 protons, 18 electrons
(iv) Mn6+
25 protons, 19 electrons
Make a table that gives the name, the complete symbol (including atomic
number, mass number and charge), number of protons, neutrons and electrons,
mass number, atomic number and charge for each of the following:
(i)
(ii)
(iii)
(iv)
(v)
(vi)
(vii)
(viii)
20 protons, 20 neutrons, 18 electrons
33 protons, 40 neutrons, 36 electrons
atomic number 52, mass number 128, charge 2atomic number 23, mass number 51, charge 5+
mass number 137, 54 electrons, charge 2+
mass number 227, 86 electrons, charge 3+
atomic number 79, mass number 196, charge 0
atomic number 25, mass number 55, 18 electrons
SEE CHART AT END OF REVIEW
h)
Write the symbols for the following atoms or ions; indicate the type of ion:
i) 13 protons, 10 electrons
Al3+ cation
ii) 80 protons, 78 electrons
Hg2+ cation
iii) 54 protons, 54 electrons
Xe atom
iv) 34 protons, 36 electrons
Se2-
anion
10
i)
Determine the number of protons and neutrons in the following:
i)
238
U
92 protons, 146 neutrons
92
ii)
14
iii)
21
6
C
6 protons, 8 neutrons
Ne
10 protons, 11 neutrons
Ti
22 protons, 25 neutrons
10
iv)
47
22
j)
k)
l)
Calculate the wavelength of the following frequencies of light:
(i)
7.5 x 1014 hertz 4.0 x 10-7 m
(ii)
5.2 x 1014 hertz 5.8 x 10-7 m
(iii)
1.15 x 106 Hz
(iv)
6.67 x 1017 Hz 4.50 x 10-10 m
Calculate the frequency of the following wavelengths of light:
-7
(i)
7.0 x 10-7 m
4.3 x 1014 Hz
(ii)
4.7 x 10 m
(iii)
9.1 m
3.3 x 107 Hz
(iv)
9.22 x 10-13 m 3.25 x 1020 Hz
Calculate the energy of the light in j) and k)
j)
k)
m)
2.61 x 102 m
(i)
5.0 x 10-19 J
(ii)
7.62 x 10-28 J
(iii)
3.4 x 10-19 J
(iv)
4.42 x 10-16 J
(i)
2.8 x 10-19 J
(ii)
2.2 x 10-26 J
(iii)
4.2 x 10-19 J
(iv)
2.16 x 10-13 J
Determine the color of the light in j) and k).
j)
k)
(i)
UV / violet
(ii)
green / yellow
(iii)
radio
(iv)
x-rays
(i)
red / infrared
(ii)
blue
(iii)
microwaves
(iv)
gamma rays
6.4 x 1014 Hz
11
Name
Symbol # of
Protons
40
2+
Ca
20
# of
Neutrons
20
# of
Electrons
18
Mass
Number
40
Atomic
Number
20
Charge
Arsenic
73
33
40
36
73
33
3-
Tellurium
128
52
76
54
128
52
2-
Vanadium
51 5+
23
28
18
51
23
5+
Barium
137 2+
B
56
81
54
137
56
2+
Actinium
227
Ac3+
89
138
86
227
89
3+
Gold
196
Au
79
117
79
196
79
0
Manganese
55
Mn7+
25
30
18
55
25
7+
Calcium
20
33
As3-
52
23
V
56
89
79
25
Te2-
2+