SCH4U Chemistry – Gr.11 Review – Diagnostic Assessment Name:__________________
Monday, February 17, 2014
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Section I – Multiple Choice (16 x ½ pt. each – 8 points) – Select the best answer for the
following and circle the corresponding letter. There is only one correct answer for each question.
____ 1. The number of valence electrons in a bromine atom is
a. 1
d. 7
b. 3
e. 9
c. 5
____ 2. How many protons, neutrons, and electrons are there in one calcium ion, Ca2+?
a. 17 protons, 39 neutrons, 39 electrons
b. 20 protons, 20 neutrons, 18 electrons
c. 17 protons, 20 neutrons, 20 electrons
d. 20 protons, 19 neutrons, 19 electrons
____
3. What value of electronegativity difference separates ionic versus covalent bonding?
a. 0.2
b. 0.4
c. 1.4
d. 1.7
e. 4.0
____ 4. The correct formula for nitric acid is
a. HNO3(aq)
b. HNO2(aq)
c. NH3(aq)
d.
e.
N2H4(aq)
NH4+
____ 5. The IUPAC name for Na2CO3(s) is
a. sodium(II) carbonate
b. sodium(II) carbonite
c. sodium carbon trioxide
d.
e.
napthium carbonate
sodium carbonate
____
6. The reaction of silver nitrate with zinc would be classified as a
a. combustion reaction
d. decomposition reaction
b. synthesis reaction
e. single displacement reaction
c. double displacement reaction
____ 7. One way to produce oxygen gas is via the decomposition of potassium chlorate, as shown in the equation
KClO3
KCl + O2. When properly balanced, the sum of all the coefficients is
a. 3
d. 10
b. 6
e. 11
c. 7
____ 8. A compound has a molar mass of 170.0 g/mol and an empirical formula of SiF3. The compound's
molecular formula is
a. SiF3
d. Si4F12
b. Si5F15
e. Si3F9
c. Si2F6
____ 9. Determine the number of moles of chlorine, Cl2, that are required to form 2.50 mol of lithium chloride,
LiCl, according to the following equation: 2LiI + Cl2
2LiCl + I2
a. 2.00 mol
d. 1.25 mol
b. 1.75 mol
e. 1.00 mol
c. 1.50 mol
____ 10. Zinc and sulphur react to form zinc sulfide, as shown in the following balanced chemical equation:
Zn + S
ZnS
If 16.00 g of zinc and 16.00 g of sulphur are available for this reaction, the limiting reagent will be
a. zinc
d. both zinc and sulphur
b. sulphur
e. cannot be determined
c. zinc sulfide
____11. Which of the following is a candidate for an empirical formula?
a. C24H44O22
d. C4H8
b. N2O4
e. Na4S2O8
c. CH3OH
____ 12. Which of the following is a spectator ion in the chemical reaction shown by this total ionic equation:
CO3(s) + 2 H+(aq) + 2 Cl (aq)
Ca2+(aq) + 2 Cl (aq) + H2O(l) + CO2(g)?
2+
a. Ca
b. Cl
c. H+
d. CO3
−
−
−
____ 13. How much more acidic is gastric acid (pH = 1.0) than citric acid (pH = 3.0)?
a. 3.0
d. 10000
b. 1000
e. 0.4
c. 100
____ 14. The pH of a polluted sample of rainwater was found to be 2.85. What is the [H3O+(aq)] of the rainwater?
a. 1.41 x 10-2 mol/L
b. 4.55 x 10-1 mol/L
c. 1.41 x 10-3 mol/L
-3
2
d. 4.55 x 10 mol/L
e. 1.41 x 10 mol/L
____
15. How many moles of KClO3 are needed to form 2.8 L of O2, measured at STP, according to the following
reaction: 2KClO3 → 2KCl + 3O2
a. 0.083 mol
d. 0.25 mol
b. 0.17 mol
e. 0.50 mol
c. 0.33 mol
____
16. What volume of a 2.00 mol/L hydrochloric acid solution is required to produce 250.0 mL of a 1.00 mol/L
solution?
a. 125 mL
b. 8.00 L
c. 500 mL
d. 1.25 L
Section II – Short Answer – Please answer the following questions in the space provided. (21 pts.)
1. Determine what type of bond (ionic, non-polar covalent, or polar covalent) would form between
the following elements. (2 pts.)
Na-O
P-H
2. Draw the Lewis dot structures for the following molecular or ionic compounds – (4 pts.)
(b) OH-
(a) C2H4
3. a) Complete the following table – (2 pts.)
Molecular Formula
SF6
CH4
Name of Molecular
Shape
Bond Angle(s)
4. Determine whether the following molecules are polar or non-polar (2 pts.) Explain your reasoning.
NH3
CO2
5. Using the following graph, show the approximate trends for atomic radius for the first twenty
elements (atomic # 1-20) (2 pts.)
6. Name the following chemical compounds. (4 points)
a) Mg(OH)2
b) H3PO3(aq)
c) SO3
d) Fe(NO3)3
7. Write formulae for the following chemical compounds. (4 points)
a) pernitric acid
b) copper (II) sulphate pentahydrate
c) manganese (II) oxide
d) phosphorous pentachloride
8. Write the net ionic equation for the reaction that occurs between a silver nitrate solution and a
magnesium chloride solution. (2 pts.)
Section III – Problem Solving – Please answer the following questions in the space provided. (17 pts.)
1. Convert 0.427 mol of potassium hydroxide into mass (in grams). (3 pts.)
2. The food we eat is degraded, or broken down, in our bodies to provide energy for growth and
function. A general overall equation for this very complex process represents the degradation
of glucose (C6H12O6) to carbon dioxide and water.
C6H12O6 + O2  CO2 + H2O
a) Balance the above chemical equation. (1 pt.)
b) If 1856 g of C6H12O2 reacts with 1425 g of O2 over a certain period (say a pizza and drink),
what is the volume of CO2 produced at STP? (6 pts.)
3. A student performs a TITRATION. To neutralize a 25.0 mL of nitric acid sample,
HNO3, it takes 13.3 mL of a 0.210 mol/L calcium hydroxide solution, Ca(OH)2.
a) Write a balanced equation for the reaction. (2 pts.)
b) Determine the concentration of nitric acid used – show all your work. (4 pts.)
c) What do you use in your titration to help determine when the solution is neutralized?
(be specific) (1 pt.)