SCH 3U – Chemistry 11 - Exam Review
Answer all questions on lined paper using a pencil or pen, not typed. Use GRASP for problem solving,
include units, and consider significant digits. This review is a good sample of questions covered in this
unit. It is by no means the only topics/problem types that you should know. Consider making a problem
types list for each unit summarizing each of the problem types seen in this course as well as the formulas
you need to memorize. Also summarize your notes for the theory concepts.
Unit #1 – Matter and Bonding
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How many significant digits are in the following: a) 1.00 b) 0.0987 c) 900 d) 308.009
Compare accuracy and precision.
Give the chemical notation for nitrogen.
Describe Modern Atomic Theory
What do the group 17 elements have in common in terms of their electrons?
Define and give the trends for a) Atomic radius, b) Ionization energy c) Electron affinity, and d) Electronegativity
Compare 5 properties of ionic and covalent compounds
What type of bond (ionic, polar covalent, non-polar covalent) will the following form: a) CaCl2 b) CO c) Br2
Identify whether each of the following are polar or non-polar molecules, explain your reasoning and include a VSEPR
diagram a) CO2 b) NH3 c) H2
10. Natural neon contains three isotopes: Ne-20, Ne-21, and Ne-22. In a sample, 90.92% of the atoms are Ne-20, 0.26% of the
atoms are Ne-21, and 8.82% of the atoms are Ne-22. Calculate the average atomic mass of neon.
11. Complete the following for each of the molecules listed below: a) Draw the Lewis Structure b) Draw and name the VSEPR
structure c) determine if Polar or Non-polar 1) CO2 2) CH4 3) H2O 4) NH3 5) N2
Unit #2 – Nomenclature/Chemical Reactions
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Give the formula/name of the following: a) magnesium chloride b) FeCl 2 c) cuprous fluoride d) diphosphorus
pentasulphide e) BaCO32- f) copper (II) hydroxide g) iron (II) sulfite h) chromium(III) nitrate nonahydrate i) potassium
thiosulphate j) hydrofluoric acid k) H3PO4 l) CuSO4.5H2O l) sulfurous acid
Balancing reactions: p. 118 # 9 c, d , p. 156 # 34
Provide an example of a synthesis, decomposition, and combustion reaction.
p. 127 # 21 f, g, h
Activity series: p. 131 # 24 a, b, d, e, 23
Predicting double displacement reactions: p. 140 # 2 a, b, c (consider solubilities and neutralization reactions)
p. 141 # 4
Unit #3 – Chemical Quantities
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Define a mole.
How many molecules are in a) 99.00 grams of zinc b) 9.0 x 10 -3 mg of lead?
What is the mass of 0.89 moles of hydrogen gas?
Percentage composition: p. 201 # 2 p. 204 # 6
Empirical formula: p. 209 # 10 p. 211 #15
Molecular formula: p. 218 # 20
Formulas of Hydrates: p. 225 # 25 p. 228 # 7
The combustion (reacting with oxygen) of propane (C3H8 (g)) produces liquid water and carbon dioxide. Write the balanced
chemical reaction and answer the following questions a) if 10.0 g of propane reacts with excess oxygen, what mass of
water will be produced b) if 4.5 g of propane reacts with 3.0 g of oxygen, what mass of carbon dioxide will be produced?
9. Another limiting reactant problem: p. 259 # 6
10. How many atoms of oxygen are in 1.87 g of aluminum carbonate?
11. Percentage yield: p. 262 # 31, 32
Unit #4 – Solutions and Solubility
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Define the following: solution, solvent, solute, miscible, immiscible, saturated solution, unsaturated solution, super
saturated solution.
Describe three factors that affect the RATE of dissolving
Describe the dissolving process.
Describe why salts commonly dissolve in water.
Describe why polar molecules dissolve in water.
Explain “like dissolves like”
What factors determine the solubility of solutes.
What is the mass of 13 mL water? What is the mass of 1.2 L of water?
m/m %, v/v %, ppm, and ppb: p. 308 # 9 p. 310 # 11 p. 15
What is the concentration of a 200 mL solution with 4.8 g of NaCl?
What mass of aluminum is in a 45 mL 1.0 x 10-2 mol/L solution of aluminum sulphate?
A 1350 mL solution contains 3.00 x 1024 ions of potassium. What mass is potassium carbonate was originally dissolved in
the solution?
Diluting solutions: p. 324 # 3, 5
Solubility chart: p. 335 # 3
Predicting a precipitate: p. 339 # 4 i, j, k, l
Describe the technique of qualitative analysis.
Net ionic equations: p. 347 # 2
Limiting reactant: p. 355 # 12, 13
p. 356 # 7
Compare four observable properties of acids and bases.
Define a) an Arrhenius acid and base b) a Bronsted-Lowry acid and base (which theory is more current?)
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Identify the acid base conjugate pairs in HF(aq) + H2O(l)
3O (aq) + F (aq)
What is the conjugate acid of NH3?
Define a strong acid and weak acid. Give an example of each.
Define a strong and weak base (careful, this one is not as simple as #24). Give and example of each.
What is the pH of a) 0.97 mol/L HBr b) 0.065 mol/L of NaOH
Define the following: indicator, end point, equivalence point
Titration problems: p. 398 # 13
Unit #6 – Gases
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Compare the forces between and motion of particles of a) solids b) liquids c) gases
What are the assumptions of KMT?
Define pressure
Convert the following to kPa a) 700 torr b) 1.15 atm c) 15.0 psi d) 100 000 Pa
Define STP and SATP
Define the following Laws: a) Boyle’s b) Charles’ c) Gay-Lussac’s d) Combined gas e) Dalton’s law of partial pressure
f) Avogadro’s g) Ideal gas
p. 435 # 6
Describe the Kelvin scale and define absolute zero.
What is the Kelvin temperature equivalent to 35 °C?
p. 446 # 8, 9
p. 450 # 15
p. 451 # 2
p. 457 # 21
A bubble of methane gas, CH4, is released from a deep bog. The temperature at the bottom of the bog is 12ºC with a
pressure of 375 kPa. If the bubble has a volume of 475 mL at the bottom, what will the new volume be, just underneath the
surface of the bog water level, if the outside temperature is 35ºC and the pressure is 99.5 kPa?
p. 460 # 25
What is the pressure reading on a scuba tank if the tank is filled with N 2 gas at a partial pressure of 115 atm and O2 gas at a
partial pressure of 30 atm?
What amount of oxygen, in mass, is available for a combustion reaction in a volume of 12.5 L at STP?
How do real gasses behave that is different from KMT?
p. 488 # 13, 14
Density of gases: p. p. 493 # 16, 17
21. Molar masses and gases: p. 500 # 20, 21
22. Ammonia is produced by the reaction of nitrogen and hydrogen gas (called the Haber process). If 12.0 L of nitrogen gas
reacts with hydrogen gas at the same temp. and pressure, what volume of ammonia will be produced?
23. p. 506 # 30, 31
24. p. 511 # 35, 36