Science 10H 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. Metric System
a) List all prefixes, base units and derived units, along with their values.
See tables in your notes.
b) How many g are there in 0.62 kg ?
0.62 kg x 1000 g = 620 g
1 kg
c) How many L are there in 145 mL ?
145 mL x 1 L = 0.145 L
1000 mL
d) How many nm are there in 2.11 x 10-6 km ?
2.11 x 10-6 km x 1012 nm = 2.11 x 106 nm
1 km
e) How many m3 in 14 km3 ?
14 km3 x (1000 m)3 = 1.4 x 1010 m3
(1 km)3
f) The speed of light is 3.00 x 108 m/s. How far will light travel in 12 days ?
3.00 x 108 m x 60 s x 60 min x 24 h x 12 d = 3.11 x 1014 m
s min h d
g) An oil tanker ran aground and spilled its cargo of 240 000 barrels of oil. If a barrel of oil
contains 42 gallons and a gallon contains 4.0 L, how many litres will the spill contain ? If the oil
spreads into a slick 1 mm thick, what will be the area of the oil slick in square kilometres ?
2.4 x 105 barrels x 42 gal x 4.0 L = 4.0 x 107 L of oil
barrel gal
4.00 x 107 L x 1000 mL = 4.00 x 1010 mL = 4.00 x 1010 cm3
1 L
4.00 x 1010 cm3 x (10 mm)3 = 4.00 x 1013 mm3
(1 cm)3
Area = volume = 4.00 x 1013 mm3 = 4 x 1013 mm2
thickness 1 mm
4 x 1013 mm2 x (1 km)2 = 40 km2
(106 mm)2
h) The annual production of sodium hydroxide in the United States in 1999 was 23.2 billion pounds.
i) How many grams of sodium hydroxide were produced in that year?
23.2 billion pounds = 2.32 x 1010 lb. x 1 kg = 1.05 x 1010 kg NaOH
2.2046 lb
1.05 x 1010 kg NaOH x 103 g = 1.05 x 1013 g NaOH
1 kg
ii) The density of sodium hydroxide is 2.130 g/cm3. How may cubic kilometers were
produced?
1.05 x 1013 g NaOH x 1 cm3 x (1 km)3 = 4.94 x 10-3 km3
2.130 g (105 cm)3
i) A quarter has a mass of 5.67 g and is approximately 1.55 mm thick.
i) How many quarters would have to be stacked to reach the height of the Peace Tower in Ottawa, 92.0 m?
1 quarter x 103 mm x 92.0 m = 5.94 x 104 quarters
1.55 mm 1 m
ii) How much would the stack weigh?
5.94 x 104 quarters x 5.67 g = 3.37 x 105 g
1 quarter
iii) How much money would the stack contain?
5.94 x 104 quarters x $1.00 = $1.48 x 104 ($14 800)
4 quarters
iv) The Canadian total debt is about 4 trillion dollars. How many of these stacks of quarters would be required to pay this debt?
$4 trillion = $4 x 1012 x 1 stack = 3 x 108 stacks of quarters
$1.48 x 104 (300 million)
3. Significant Digits
a) Perform the following additions and subtractions:
i) 22.26 g + 19.1 g 41.4 g iv) 2500 L - 155 L 2300 L
ii) 100.1 L + 0.025 L 100.1 L v) 1.236 mol - 0.33 mol 0.91 mol
iii) 8.21 mL + 2.79 mL 11.00 mL vi) 19 mol - 18.75 mol 0 mol
b) Perform the following multiplications and divisions
i) 233 g / 15.36 g/mol 15.2 mol iv) 13.1 mol x 44.01 g/mol 577 g
ii) 1.59 mol / 0.12 L 13 mol/L v) 22 L x 2.145 mol/L 47 mol
iii) 16 g x (1 kg / 1000 g) 0.016 kg vi) 100 g / 18.02 g/mol 5 mol
4. Graphing
a) Make a graph of the following data. Use graph paper and include all the components of a good graph. Put volume on the x-axis. Draw a best-fit line. Calculate the slope. What does the slope of this line represent? Identify the element of which these blocks were made.
volume of a block (cm3) mass of the block (g)
2.0 5.5
4.0 10.7
6.0 16.2
8.0 21.5
10.0 26.8
15.0 40.5
25.0 68.0
b) Make a graph of the following data. Use graph paper and include all the components of a good graph. Put distance on the x-axis. Draw a best-fit line.
distance from planet (km) Gravity (N)
0 9.8
100 9.5
150 9.4
200 9.2
300 8.9
500 8.4
1000 7.3
5000 3.1
10000 1.5
c) Measurements were taken of small cylinders of an unknown metal:
Radius of Circular End (mm) Length (cm) Mass (g)
4.0 1.55 15.06
4.0 2.65 25.75
4.0 4.00 38.87
4.6 3.15 40.47
4.6 4.50 57.82
4.6 5.80 74.52
i) Calculate the volume of each cylinder.
Volume is equal to the area of the end of the cylinder multiplied by the length:
V = lπr2
Radius (mm) Length (cm) Volume (cm3) Mass (g)
4.0 1.55 0.80 15.06
4.0 2.65 1.3 25.75
4.0 4.00 2.0 38.87
4.6 3.15 2.1 40.47
4.6 4.50 3.0 57.82
4.6 5.80 3.9 74.52
ii) Make a graph with volume on the x-axis.
See end of file
iii) Calculate the slope of the line.
Slope = rise = y2 - y1 = 74.52 g - 15.06 g = 19.2 g/cm3 (20 g/cm3)
run x2 - x1 3.9 cm3 - 0.8 cm3
iv) What is the significance of the slope of the graph ? Can you identify the metal ?
The units of grams per cubic centimeter are the units of density, a characteristic physical property. This density corresponds to that of gold.
5. Nomenclature
a) Give the formulas for the following substances:
i) magnesium hydroxide Mg(OH)2 vi) iron (III) phosphate FePO4
ii) sodium hydrogen carbonate NaHCO3 vii) lime CaO
iii) aluminum oxide Al2O3 viii) ethanol C2H5OH
iv) calcium oxide hexahydrate CaO · 6 H2O ix) nitric acid HNO3
v) phosphorus pentaoxide PO5 x) lead (II) sulfate Pb(SO4)2
b) Give the name for the following compounds:
i) NaCl sodium chloride
ii) NH3 ammonia
iii) CaSO4 calcium sulfate
iv) N2O4 dinitrogen tetraoxide
XXX
v) NaH sodium hydride
vi) Ca(OH)2 ·5 H2O calcium hydroxide pentahydrate
vii) MnO2 manganese (IV) oxide
viii) CO2 carbon dioxide
ix) NH4NO3 ammonium nitrate
x) CH3COOH acetic acid
c) Draw the structures for the following:
i) propane v) 2-methyl-3-heptene
ii) phenol vii) 1,1-dichloro-2-methyl-3-pentanol
iii) 2-butyne viii) 1,2-difluoro-3,3-diiodocyclohexane
iv) ethyl propanoate ix) butanamide
v) diethyl ether x) pentanoic acid
d) propene 4-heptanol
1-fluoro-3-chloropentane 3,4-dimethyl-2-pentene
1-hexadecyne propanone
butylamine ethanal
1,1,2-trifluoro-1,2,2-trichloroethane 2-chloro-4-fluorocyclohexene
1-hexyn-6-ol toluene
6. Atomic Theory
a) Describe the nature and role of the proton, neutron, and electron in the atom.
Proton / Neutron / ElectronLocation / 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) List the diatomic elements, as well as the two other polyatomic elements.
H2 N2 O2 F2 Cl2 Br2 I2 At2 S8 P4
c) 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
d) 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) 20 protons, 20 neutrons, 18 electrons
(ii) 33 protons, 40 neutrons, 36 electrons
(iii) atomic number 52, mass number 128, charge 2-
(iv) atomic number 23, mass number 51, charge 5+
(v) mass number 137, 54 electrons, charge 2+
(vi) mass number 227, 86 electrons, charge 3+
(vii) atomic number 79, mass number 196, charge 0
(viii) atomic number 25, mass number 55, 18 electrons
Name / Symbol / # Protons / # Electrons / # Neutrons / Mass Number / Atomic Number / ChargeCalcium / 40Ca2+
20 / 20 / 18 / 20 / 40 / 20 / 2+
Arsenic / 73As3-
33 / 33 / 36 / 40 / 73 / 33 / 3-
Tellurium / 128Te2-
52 / 52 / 54 / 76 / 128 / 52 / 2-
Vanadium / 51V5+
23 / 23 / 18 / 28 / 51 / 23 / 5+
Barium / 137Ba2+
56 / 56 / 54 / 81 / 137 / 56 / 2+
Actinium / 227Ac3+
89 / 89 / 86 / 138 / 227 / 89 / 3+
Gold / 196Au
79 / 79 / 79 / 117 / 196 / 79 / 0
Manganese / 55Mn7+
25 / 25 / 18 / 30 / 55 / 25 / 7+
e) Write the symbols for the following atoms or ions; indicate the type of ion:
i) 13 protons, 10 electrons Al3+ iii) 54 protons, 54 electrons Xe
ii) 80 protons, 78 electrons Hg2+ iv) 34 protons, 36 electrons Se2-
f) Determine the number of protons and neutrons in the following:
i) 238U (ii) 14C (iii) 21Ne (iv) 47Ti
92 6 10 25
i) 92 protons, 146 neutrons
ii) 6 protons, 8 neutrons
iii) 10 protons, 11 neutrons
iv) 25 protons, 22 neutrons
g) Given the following data calculate the average atomic mass of silver:
Isotope Mass(amu) Abundance (%)
Ag-107 106.90509 51.840
Ag-109 108.90476 48.160
Ave. Mass = (51.840%/100)(106.90509 amu) + (48.160%/100)(108.90476 amu)
= 107.87 amu
h) Given the following data calculate the abundance of each isotope of boron:
Isotope Mass (amu) Abundance (%)
B-10 10.0129 20.00
B-11 11.0093 80.00
Average mass of boron is 10.81 amu
10.81 amu = (x)(10.0129 amu) + (1 - x)(11.0093 amu)
x = 0.2000
7. Heat
Following is a list of the specific heats of several materials (in J/g·°C):
Aluminum 0.90 Lead 0.13 Silver 0.24
Copper 0.39 Magnesium 0.98 Water 4.18
Ethylene glycol 2.20 Methanol 2.50 Water vapour 1.87
Gold 0.13 Oxygen 0.92 Zinc 0.39
Ice 2.06 Paraffin oil 2.10
Iron 0.45 Sand 0.80
a) Calculate the amount of energy, in Joules, required for the following:
i) to heat 150 g of water from 14°C to 36°C 1.4 x 104 J
ii) to cool 16 kg of sand from 45°C to 4.0°C - 5.2 x 105 J
iii) to increase the temperature of 351 g of gold 101°C 4600 J
iv) to decrease the temperature of 89 g paraffin oil 55°C 1.0 x 104 J
b) Calculate the temperature change:
i) if 4.5 kg of aluminum receives 780 J of energy 0.19 °C
ii) if 335 g of iron receives 16 kJ of energy 110 °C
iii) if 78.5 kg of silver loses 14.1 kJ of energy - 0.75 °C
c) Calculate the mass:
i) if 560 J of energy causes the temperature of copper to rise 67°C 21 g
ii) if a loss of 7 kJ of energy causes the temperature of lead to go from 246°C to 182°C
800 g
Following is a list of heats of fusion and vapourization of several substances:
Heat of fusion (J/g) Heat of vapourization (J/g)
water 333 2260
methanol 100 1076
ethanol 109 855
hexane 152 335
toluene 72 363
d) Calculate the heat required:
i) to melt 678 g of hexane 1.03 x 105 J
ii) to freeze 8.1 kg of methanol - 8.10 x 105 J
iii) to boil 780 g of ethanol 6.7 x 105 J
iv) to condense 224 kg of toluene - 8.13 x 107 J
e) Calculate the heat required:
i) to change 569 g of ice at -35.0°C to steam at 172°C
Heat ice: (2.06 J/g °C)(569 g)(0 °C - (-35.0 °C)) = 4.10 x 104 J
Melt ice: (333 J/g)(569 g) = 1.89 x 105 J
Heat water: (4.18 J/g °C)(569 g)(100 °C - 0 °C) = 2.38 x 105 J
Boil water: (2260 J/g)(569 g) = 1.29 x 106 J
Heat steam: (1.87 J/g °C)(569 g)(172 °C - 100 °C) = 7.7 x 104 J
Total: = 1.84 x 106 J
ii) to change 3.55 kg of water at 45°C to ice at -15°C
3.55 kg x 1000 g = 3550 g
1 kg
Cool water: (4.18 J/g °C)(3550 g)(0 °C - 45 °C) = - 6.7 x 105 J
Freeze water: (-333 J/g)(3550 g) = - 1.18 x 106 J
Cool ice: (2.06 J/g °C)(3550 g)((-15 °C) - 0 °C) = - 1.1 x 105 J
Total: = 1.96 x 106 J
8. Light
Speed of light = wavelength x frequency c = λν c = 3.00 x 108 m/s
Energy of light = Planck’s constant x frequency E = hν h = 6.626 x 10-34 J·s
i. Calculate the frequency of each of the following wavelengths of light, and indicate the
‘colour’ of the light:
a) 4.50 x 10-7 m (6.67 x 1014 Hz, blue) (4.42 x 10-19 J)
b) 6.1 x 10-7 m (4.9 x 1014 s-1, orange) (3.3 x 10-19 J)
c) 2.11 x 10-12 m (1.42 x 1020 1/s , gamma rays) (9.42 x 10-14 J)
d) 1.6 x 10-5 m (1.9 x 1013 Hz, infrared) (1.2 x 10-20 J)
ii. Calculate the wavelength of each of the following frequencies, and indicate the ‘colour’
of the light:
a) 4.44 x 1014 Hz (6.76 x 10-7 m, red) (2.94 x 10-19 J)
b) 7.4 x 1014 s-1 (4.1 x 10-7 m, violet) (4.9 x 10-19 J)