SCH3U MOCK EXAM
KNOWLEDGE
1. When a chlorine atom becomes a chloride ion the:
a. Ion has the same diameter as the atom
d. Nucleus becomes larger
b. Ion has a smaller diameter than the atom
e. Nucleus becomes smaller
c. Ion has a larger diameter than the atom
2. The number of moles of hydrogen required to completely react with 2.0 mol of Fe3O4 in the chemical reaction
Fe3O4 + 4H2 → 3Fe + 4H2O is:
a. 4
b. 6
c. 8 d. 12
The next three questions deal with the identification and characterization of three elements which we shall call X,
Y, and Z. The elements have successive atomic numbers each increasing by one in the order given. Atoms of
element Z form stable ions with the formula Z+.
3. Which element has the highest ionization energy?
a. X b. Y c. Z
4. Which of the following statements is FALSE concerning elements X, Y, and Z?
a. A neutral atom of element Y would have one more electron than a neutral atom of element X, but one less
electron than a neutral atom of element Z.
b. Element X could be a halogen.
c. Elements X, Y, and Z would all be in the same chemical family of the periodic table.
d. Elements X, Y, and Z could be those elements with atomic numbers 9, 10, and 11 respectively.
5. Which of the following statements is FALSE concerning the elements X, Y, Z and their ions?
a. The ions X- and Z+ would have the same number of electrons as neutral atoms of element Y.
b. Atoms of element Y would react with atoms of either elements X or Z.
c. Element X would form a compound with hydrogen with the formula HX.
d. Element Z would form a compound with chlorine with the formula ZCl.
e. Elements X and Z would react to form a compound with the formula ZX.
6. During a chemical reaction which of the following statements is true?
a. When one of the products of reaction is a gas, the mass of the reactants will be greater than that of the products.
b. When one of the products is a precipitate, the mass of the products will be greater than that of the reactants.
c. The mass of the products is not dependent on the mass of the reactants.
d. The mass of the products equals the mass of the reactants.
7. Which of the following principles of conservation apply in all chemical reactions having a balanced equation?
1. conservation of volume
2. conservation of the number of molecules
3. conservation of the number of atoms
4. conservation of mass
a. 1 – 2 – 3
b. 2 – 3 – 4
c. 3 – 4 only d. 1 – 2 only
8. Which of the following equations is not balanced?
a. P4 + 5 O2 → 2 P2O5
d. PbS + 4 H2O2 → PbSO4 + 4 H2O
b. 2 NCl3 → N2 + Cl3
c. 2 H2O + 2 K2O2 → O2 + 4 KOH
9. Which one of the following reactions is not likely?
a. Na → Na + + ec. Ba → Ba2+ + 2e+
b. F → F + e
d. Cl + e- → Cl -
10. How many electrons are there in a sulphide ion, S2- ?
a. 14 b. 15 c. 16 d. 17 e. 18
11. A bromide ion will have a charge of:
a. +1 b. +2 c. +3 d. –1 e. –2
12. An atom of iron 5626Fe has:
a. 26 protons, 26 electrons, 30 neutrons
b. 30 protons, 30 electrons, 26 neutrons
c. 30 protons, 26 electrons, 26 neutrons
d. 26 protons, 26 electrons, 56 neutrons
e. 26 protons, 30 electrons, 30 neutrons
13. How many electrons are in the outer (highest) energy level of a 3919K ion?
a. 3 b. 5
c. 6 d. 7 e. 8
14. Zinc + hydrochloric acid produces:
a. hydrogen and zinc hydroxide
d. chlorine and zinc hydride
b. hydrogen and zinc chloride
e. chlorine and zinc hydroxide
c. hydrogen and zinc nitrate
15. Experimentally, a strong acid differs from a weak acid in :
a. concentration b. solubility c. electrical conductivity d. its reaction with litmus paper
16. Which of the following 1.0 mol /L solutions will be the poorest conductor of electricity?
a. hydrochloric acid b. acetic acid c. sodium hydroxide d. sodium chloride
17. The boiling point of O2 is - 183ºC, and its freezing point is - 219ºC. Within 50 K of absolute zero, oxygen is a :
a. gas b. liquid c. solid d. solution
18. Which one of the following statements is true?
a. a decrease in pressure on a gas causes a decrease in volume
b. absolute zero is - 273 K
c. an increase in the pressure of a gas could be due to a decrease in the number of molecules
d. in a mixture of gases, the one with the most molecules exerts the most pressure.
19. Which one of the following is a basic assumption of the kinetic molecular theory?
a. particles are in constant random motion
c. particles travel faster as the temperature decreases
b. particles lose energy with an increase in velocity
d. particles lose energy when the temperature increases
20. What is the correct name of SnSO4?
a. tin (II) sulphite b. tin (IV) sulphite c. stannic sulphite
d. stannic sulphate e. tin (II) sulphate
21. What is the correct name of Pb(OH)2. 6H2O ?
a. Lead (II) hydroxide heptahydrate b. Lead (II) hydroxide hexahydrate
c. Plumbous hydroxide hydrate
d. Lead (IV) hydroxide hydrate
22. Which of the following molecules is a polar molecule?
a. NF3 b. Cl2 c. SeBr2 d. CCI4 e. CO2
23. Which one of the following covalent bonds is the most polar?
a. H– O b. H– N c. H– Cl d. H– H
24.Which of the following is not a subatomic particle?
a. proton
c. electron
b. neutron
d. isotope
e. all of the above
25.Which of the following groups is known for its reactivity?
a. alkali metals
d. metalloids
b. alkali earth metals
e. non-metals
c. transition metals
26.Which of the following is true regarding krypton?
a. has at least one lone electron
b. is reactive under normal conditions
c. has four complete shells of electrons
d. Normally exists as a diatomic molecule.
e. All of the above are true.
27.Which of the following atoms has two lone pairs of electrons?
a. nitrogen
c. beryllium
e. chlorine
b. oxygen
d. carbon
28.A lone pair of electrons is
a. two electrons located close to the nucleus
b. two lone electrons
c. two electrons that are interacting in a unique way so that they can be close to each other
d. two electrons in the outermost shell of an atom
e. none of the above
29.Why are large elements usually radioactive?
a. They are unstable.
b. They are synthetic.
c. They are rarely found in food products.
d. They are used for medical imaging.
e. They have a short half-life.
30.Which of the following is true regarding sodium chloride?
a. has an ionic bond
d. has a molecular bond
b. Electrons leave chlorine.
e. All of the above are true.
c. Sodium becomes negative.
31.Which of the following molecules is known for having one single bond?
a. oxygen
c. nitrogen
e. argon
b. hydrogen
d. carbon dioxide
32.Which of the following molecules is known for having one double bond?
a. oxygen
c. nitrogen
e. argon
b. hydrogen
d. carbon dioxide
33.Which of the following molecules is known for not bonding?
a. oxygen
c. nitrogen
e. argon
b. hydrogen
d. carbon dioxide
34.Ionic compounds have a ___ boiling point since the ___ forces holding them together are strong.
a. low, ionic
d. medium, electron
b. medium, electrostatic
e. low, electron
c. high, electrostatic
35.What do all elements larger than uranium have in common?
a. They are all radioactive.
d. They are all recent discoveries.
b. They are all unstable.
e. All of the above are true.
c. They do not occur naturally.
36.Which of the following explanations outlines a decomposition reaction?
a. a binary compound decomposing into its elements
b. a metal nitrate decomposing into a metal nitrite and oxygen gas
c. a metal hydroxide decomposing into a metal and aqueous hydroxide ions
d. Two of the above explanations are correct.
e. All three of the above explanations are correct.
37.Which halogen(s) can be displaced by fluorine?
a. chlorine
d.
all halogens
b. bromine
e.
None of the halogens can be displaced by fluorine.
c. iodine
38. Which of the following statements is/are true with respect to single displacement reactions?
a. Metals can displace metals.
d None of the above statements are true.
b. Halogens can displace halogens.
e. All of the above statements are true.
c. Some metals can displace hydrogen from acids and water.
39.Which of the following equations can be used to change the mass of a compound to the amount (in moles) of the
compound?
a.
d.
b.
c.
e.
The conversion depends on the compound.
40.Dinitrogen pentoxide decomposes according to the following equation: 2N2O5(g)  4NO2(g) + O2(g)
According to Avogadro’s law, if 6 L of dinitrogen pentoxide decomposed, then the volume of nitrogen dioxide
and oxygen gas produced would be
a. 4 L NO2 , 1 L O2
b. 6 L NO2 , 3 L O2
c. 12 L NO2 , 3 L O2
d. 8 L NO2 , 4 L O2
e. 8 L NO2 , 2 L O2
41. Which of the following is the most common analytical method used to determine how many water molecules
that are attached to the formula unit in a hydrate?
a. reacting with a hydrocarbon to remove the water
b. reacting the water with an acid, and measuring the dilution factor in the acid
c. heating to remove the water and determining the % of mass loss as the hydrate becomes anhydrous
d. electrolysis of the water and measuring the amount of hydrogen and oxygen gases given off
e. The process used depends on the type of ionic substance.
42.Which statement is most correct with respect to the limiting reactant?
a. It is the reactant that is fully consumed during a chemical reaction.
b. It is the reactant that produces least amount (in moles) of product.
c. It is the reactant that produces the least mass of product.
d. Two of the above are correct.
e. All three of the above are correct.
43.A 250 mL sample of gas was initially at a pressure of 101 kPa at 100C. If the volume decreases to 100 mL at
50C, then the new pressure could be calculated by
a.
d.
b.
c.
e.
44.Which of the following can be used measure a very small concentration (much less than 1% m/m)?
a. ppm
d. Two of the above can be used.
b. ppb
e. All of (a), (b), and (c) can be used.
c. moles
45.According to the kinetic molecular theory, gas particles have ___________attractive forces and have and exhibit
____________ collisions.
a. negligible, elastic
d. negligible, inelastic
b. large, elastic
e. small, elastic
c. small, inelastic
46.Which of the following conditions will cause a decrease in the pressure of a gas?
I. decreasing the temperature II. decreasing the volume III. removing some amount of the gas
a. I only
b. II only
c. III only
d. I and II
e. I and III
47.Which statement is not true?
a. The average kinetic energies of molecules from samples of different “ideal” gases is the same at the same
temperature.
b. The molecules of an ideal gas are relatively far apart.
c. All molecules of an ideal gas have the same kinetic energy at constant temperature.
d. Molecules of a gas undergo many collisions with each other and the container walls.
e. Molecules of greater mass have a lower average speed than those of less mass at the same temperature.
48.Decreasing the temperature of an ideal gas at constant mass will cause which of the following to decrease
I. molar mass
IV. the average kinetic energy of the gas
II. the volume of the gas
V. the pressure of the gas
III. the density of the gas
a. II, III, and IV
c. I, II, and III
e. II, III, IV, and V
b. III, IV, and V
d. II, IV, and V
49.According to Boyle’s law, which of the following will occur if the pressure on a gas is increased?
a. The volume of gas will increase.
b. The volume of gas will decrease.
c. The amount (in moles) of gas will increase.
d. The temperature of the gas will increase.
e. The temperature of the gas will decrease.
50.Which of the following statements conflicts with the kinetic molecular theory of gases?
a. There are no intermolecular forces between gas particles.
b. Gas particles occupy a negligible volume compared with the volume of their container.
c. The average kinetic energy of the gas particles is proportional to the temperature.
d. Gas particles lose energy only when they collide with the walls of the container.
e. Gas particles are in constant, random motion.
51.Which of the following scientists is credited with discovering the mathematical relationship between the
temperature and pressure of a fixed volume of a gas?
a. Evangelista Torricelli
d. Jacques Charles
b. Galileo Galilei
e. Joseph Louis Gay-Lussac
c. Robert Boyle
52.Which of the following formulas best describes Gay-Lussac’s law?
a.
c.
e. T1V1 = T2V2
b.
d. P1V1 = P2V2
SCH3U MOCK EXAM
PART B: COMMUNICATION, THINKING AND APPLICATION
1. Using the periodic table, explain the following:
a. Why potassium is more reactive than sodium [2]
b. Why noble gases are assigned a value of zero for electronegativity. [2]
c. Why silicon has higher ionization energy than sodium. [2]
d. Why sodium ion is smaller than the sodium atom. [2]
2. For each of the following molecules:
- draw the Lewis structure. (Remember to determine bond type first)
- for compounds with polar bonds, determine if the compound is overall polar.
- name each compound
a. PCl3[3] b. CO2[3] c. NiCl2[3]
3. For the following double displacement reactions:
- give a balanced equation, including states
- write a total ionic equation, including states
- write a net ionic equation, including states
a. lithium hydroxide solution reacts with ammonium chloride solution[3]
b. Lead (II) nitrate solution reacts with sodium iodide solution[3]
c. Sufuric acid reacts with sodium hydroxide solution. [3]
4. a. A compound was found to contain 46.7% N; 53.3% O What is the empirical formula? [4]
b. If the molar mass is 60g/mol, what is the molecular formula? [1]
5. Tin (II) iodide, SnI2, can be prepared by adding a solution of potassium iodide, KI(aq) to a solution of tin
(II) chloride, SnCl2 (aq) . If 2.280 g of SnCl2 were dissolved in 25.0 mL of water and mixed with 10.0 mL of
1.40 mol/ L KI(aq) to precipitate the tin (II) iodide.
a. Write a balanced chemical equation and determine which of the reagents is limiting.[4]
b. Calculate the maximum mass of tin (II) iodide that could be formed[3]
c. If 1.89 g of tin (II)iodide was obtained, determine the percentage yield. [2]
6. A gas occupies 2.00L at 280.0Kand 1.00 atm. What V would it occupy at 300.0K and 3.00 atm. [3]
7. What is the density of SO2, if it exerts a pressure of 750.00 mm Hg at a temperature of 23.5 ºC? [4]
8. Tums, essentially calcium carbonate, CaCO3, on the market are sold as an antacid. A tablet of Tums was
crushed and reacted with hydrochloric acid, HCl(aq). 28.50 mL of 0.200 mol /L hydrochloric acid was
required to completely neutralize one of the Tums tablet.
a. Write a balanced equation for the reaction of the Tums tablet, (CaCO3 (s)) with hydrochloric acid. [3]
b. Determine the mols of hydrochloric acid consumed. [3]
c. Determine the mols of Tums consumed. [2]
d. Determine the mass of the CaCO3(s) in each of the Tums tablet. [2]
9. How much 15.4 mol/L nitric acid is needed so that the dilution results in 150 mL of 0.200 mol/L solution
of the nitric acid. [3]