SCH 4C PRACTICE EXAM
NAME:____________________
This practice exam is organized in way that is similar to the actual exam. Read each
question carefully and try to refer to your review sheets and formula sheet as you do these
questions. Good Luck!
ACTUAL
SECTION
PRACTICE
QUESTIONS
MARKS
QUESTIONS
MARKS
PART A – MULTIPLE CHOICE
25
/25
25
/25
PART B - SHORT ANSWER
10
/46
9
/37
PART C – PROBLEM SOLVING
6
/22
5
/23
TOTAL
/93
/85
PART A: Multiple Choice
1.
Which of the following is considered a pure substance?
A. tap water
B.
glucose (C6H12O6)
C. air (N2, O2, Ar)
D.
vinegar (5% acetic acid solution)
2.
Which of the following is an example of chemical change?
A.
boiling water
B.
rusting of iron
C.
heating copper metal
D.
dissolving alcohol in water
3.
Compared to an electron, a proton has:
A.
the same charge and about the same mass.
B.
the same charge but a much greater mass.
C.
the opposite charge and much less mass.
D.
the opposite charge and a much greater mass.
4.
The nucleus of the isotope hydrogen-3 ( 31H) is composed of:
A.
one proton and no neutrons.
B. one proton and two neutrons.
C. one proton and three electrons.
D. one neutron and two protons.
5.
The number of electrons in a sulfide ion (S2-) is:
A. 16
B. 18
C. 32
D. 34
6.
Which of the following is different in the various isotopes of an element?
I. Mass Number
A. I
C. III
II. Atomic Number
III. Electron number and arrangement
B. II
D. I and II
7.
The number of lone pairs of electrons (unbonded electrons) around carbon in the
molecule ethyne (C2H2) is:
A. 0
B. 1
C. 2
D. 3
8.
Which of the following elements is least likely to react with chlorine to form a
compound?
A. potassium
B. lead
C. argon
D. magnesium
9.
A pair of unequally shared electrons between two non-metal atoms in a molecule is
known as:
(a) a covalent bond
(b) a polar covalent bond
(c) an ionic bond
(d) a dipole
10. Zinc metal reacts with aqueous hydrochloric acid to generate hydrogen gas. What other
metal will react this way?
A. Iron
C. Gold
B. Copper
D. Mercury
11. The concentration of a solution in which 2.34 g of magnesium chloride are present in
2.00L of solution is:
a) 0.0123 mol/L
(b) 0.0246 mol/L
(c) 0.0492 mol/L
(d) 0.0509 mol/L
12. How many moles of pure NaOH must be used to prepare 500 mL of 1.00 mol/L NaOH ?
(a)
0.500 mol
(b)
1.00 mol
(c)
2.00 mol
(d)
50.0 mol
13. What is the percentage of solute by mass in a solution prepared by dissolving 50 g of
KNO3 in 200 g of water?
(a) 20%
(b) 25%
(c) 50%
(d) 75%
14. What type of chemical reaction is represented by the following equation:
Cu(s) + 2 AgNO3(aq) ----> Cu(NO3)2(aq) + 2 Ag(s)
(a) precipitation (double displacement)
(c) (acid-base) neutralization
(b) synthesis
(d) decomposition
15. Which of the following scientists discovered the nucleus of the atom?
(a) Dalton
(b) Rutherford
(c) Bohr
(d) Thomson
16. What is the pH of a 0.01 mol/L HCl solution?
(a) 0.01
(b) 1
(c) 2
(d) 7
(e) 13
17. Acid A has a pH of 3.7, and Acid B has a pH of 0.7
Which one of the following statements is true?
(a) Acid A is three times as strong as Acid B.
(b) Acid B is three times as strong as Acid A.
(c) Acid A is one thousand times as strong as Acid B.
(d) Acid B is one thousand times as strong as Acid A.
18. Which one of the following statements about an acid is INCORRECT?
a) an acid produces hydronium ions in aqueous solution
b) an acid turns blue litmus red
c) an acid neutralizes a base
d) an acid is a substance whose pH is greater than seven
19. In the neutralization reaction between calcium hydroxide and hydrochloric acid the
products are water and:
(a) calcium carbonate
(b) calcium chloride
(c) calcium chlorate
(d) chlorine hydroxide
20. What is the molar mass of Al(NO3)3 (in g/mol) ?
(a) 165.00 (b) 56.99
(c) 213.00 (d) 88.99
(e)184.99
21. According to the equation: 2 C2H2 + 5 O2 ----> 4 CO2 + 2 H2O
the number of moles of CO2 formed from 0.20 mole of C2H2 is:
(a) 0.10
(b) 0.20
(c) 0.40
(d) 4.0
(e) 8.0
22. 3.00 mol of silver contains approximately
(a) 3
(b) 324
(c) 6.0 x 1023
atoms:
(d) 1.8 x 1024
23. In the Periodic Table, the elements are arranged in order of increasing:
(a)
number of neutrons
(d)
density
(b)
number of protons
(e)
ionization energy
(c)
number of valence electrons
24. Benzene can react with fluorine according to the unbalanced chemical equation:
C6H6 + F2 ----> C6F12 + HF
If this equation is balanced, the number of moles of F2 required to react with one mole of
benzene is:
(a) 18
(b) 12
(c) 9
(d) 6
(e) 3
25.
(a)
(b)
(c)
(d)
Based on the solubility rules, which of these substances is insoluble in water?
calcium bromide
copper(II) hydroxide
sodium carbonate
sodium chloride
PART B: Short Answer:
1. Give correct chemical formulae for each of the following: {5 marks}
i) tin (IV) hydroxide
_______________
ii) copper(II) chloride
_______________
iii) calcium nitrate
_______________
iv) sulfur trioxide
_______________
v) aluminium oxide
_______________
2. Give correct chemical name for each of the following: {5 marks}
i) N2O4 (Greek prefix method)
______________________
ii) Pb(ClO3)4 (IUPAC)
______________________
iii) HBr (aq)
______________________
iv) Ca3(PO4)2
______________________
v) FeSO4 (IUPAC)
______________________
2. Balance each of the following equations: {3 marks)
(i)
__BF3 + __H2O  ___HF + ___H3BO3
(ii)
___C2H3Cl + ___O2  ___CO2 + ___ H2O + ___HCl
(iii)
___Al + ___H2SO4 
___Al2(SO4)3 + ___H2
3. Name the types of reactions shown below.
{3 marks}
Equation
2 H2
CH4
Fe
+
Type
O2  2 H2O
+ 2O2
CO2 + 2H2O
+ H2SO4
FeSO4 + H2
4. Using the activity series, predict if a single displacement reaction will occur in each
case. If a reaction occurs, write either the chemical or the word equation. If no
reaction occurs, write NR. {5 marks}
(i)
Solid calcium is added to a solution of hydrochloric acid.
(ii)
A piece of aluminum is placed in an aqueous solution of copper(II) sulfate.
(iii)
A piece of silver metal is placed in sulphuric acid.
5. Write the balanced chemical equation for each of the following: {4 marks}
(i) the precipitation reaction that occurs when aqueous solutions of silver nitrate and sodium
chloride are mixed. (Give state symbols)
(ii) the reaction that occurs when sodium metal is added to water.
6. Draw a Lewis Structure of these inorganic compounds. {5 marks}
a) PCl3
b) Br2
c) H2O
7. Draw the structures of the following organic compounds. {4 marks}
a) 3-hexene
b) 2,3-dimethylpentane
c) cyclobutane
d) propanoic acid
8. Name the following organic compounds. { 3 marks}
a)
b)
c)
9. a) Calculate the number of subatomic particles in this isotope of phosphorus. {1 mark}
32 P
15
protons: _____
neutrons: _____
electrons: ______
b) Draw a Bohr-Rutherford diagram for this atom. {2 marks}
PART C: Problem Solving
1. A chemist needs to create 25 L of a 0.35 mol/L calcium nitrate solution.
a) What is the molar mass of Ca(NO3)2? {1 mark}
b) How many moles of calcium nitrate are required? {2 marks}
c) What mass should the chemist weight out? {2 marks}
2. A certain salt contains 26.58% potassium, 35.35% chromium and 38.07% oxygen. What
is the empirical formula? {5 marks}
3. What will be the concentration of a solution when 25 mL of 12 mol/L HCl is diluted with
water to a final volume of 10 L? {2 marks}
4. Chlorine gas can be prepared by the reaction of manganese(IV) oxide with concentrated
hydrochloric acid. The balanced equation for the reaction is:
MnO2 (s) + 4 HCl (aq)  MnCl2 (aq) + 2 H2O (l) + Cl2 (g)
(a)
How many moles of MnO2 will react with 0.400 mol of HCl according to the above equation?
{1 mark}
(b)
How many grams of MnO2 would you need to react with excess HCl in order to produce
2.22 g of H2O according to the above equation ? {4 marks}
5. In an acid-base titration, a student reacted 0.241 mol/L sulfuric acid with potassium
hydroxide.
a) Complete the balanced equation. {2 marks}
___H2SO4 + ___KOH  ___________ + ___________
b) Based on the following data, determine the concentration of the base. {3 marks}
Volume of acid used: 25.00 mL
Volume of base used: 12.45 mL