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Grade 11 Chemistry Review
The following questions highlight the main knowledge and skills from grade 11 chemistry. A good understanding
of the concepts covered in grade 11 chemistry is essential for success in grade 12 chemistry and you may need to
do some independent review of some material if you do not have a clear understanding of the concepts.
1. Use arrows to show the periodic trends for the following properties.
Increasing
Atomic Radius
Increasing
Metal Reactivity
Increasing 1st
Ionization Energy
Increasing
Electronegativity
Increasing
Non-Metal Reactivity
Increasing
Metallic Properties
Increasing
Electron Affinity
2. Rank the following elements in order of increasing 1st Ionization Energy. Explain your choice.
N, Ba, Al, Mg
3. Rank the following elements in order of decreasing 1st Atomic Radius. Explain your choice.
O, F, S, Br
4. Why is the ionic radius of a negative ion larger than the atomic radius of the corresponding neutral atom?
5. Why is the ionic radius of a positive ion smaller than the radius of the corresponding neutral atom?
6. Draw the full electron configuration for the following elements.
A) F
B) Ti
C) Sn
7. Distinguish between an ionic bond, polar covalent bond, pure covalent bond and coordinate covalent
bond.
8. Draw Lewis Dot diagrams for the following compounds.
A) KI
B) CH4
C) CO32-
D) XeF6
9. Determine which of the following molecules contain polar covalent bonds and if the molecules are polar.
A) Br2
C) PCl3
B) SrCl2
D) HF
10. How is it possible for a non-polar molecule to have polar covalent bonds?
11. Distinguish between intramolecular and intermolecular forces. Give examples of each.
12. Explain why polar molecules have higher boiling and melting points than non polar molecules.
13. Why does chloromethane have a higher solubility in water than methane? Draw a diagram to aid in your
explanation.
14. What is the charge on the stable ion formed by the following elements?
A) Na
C) Ba
B) S
D) I
15. Complete the following word equations, identify the type of reaction and write balanced chemical
equations. (BEWARE NOT ALL WILL RESULT IN A REACTION)
A) iron + copper (II) sulphate 
B) potassium bromide + iodine 
C) sodium chlorate 
D) ethane (dicarbon hexahydride) + oxygen 
E) magnesium oxide + carbon dioxide 
F) calcium hydroxide 
G) sulphur trioxide + water 
H) lithium hydroxide + phosphoric acid 
16. Determine the molar mass for the following compounds.
A) Mg(SCN)2
B) SrCl2∙ 4H2O
17. Determine the number of molecules in 45.2 g of calcium carbonate.
18. Determine the number of moles of HCl in 36 mL of a 0.15 M solution.
19. Determine the percent composition of the following compounds.
C) CsHS2O2
A) SO3
B) CuSO3
20. A sample of copper (II) sulphate pentahydrate weighs 6.8 g. What mass of the sample is due to the
water?
21. A compound contains 85.6 % C and 14.4 % H.
A) Determine the empirical formula of the compound.
B) If the molar mass of the compound is 42.1 g/mol, what is the molecular formula of the compound.
22. What is the concentration in % w/v and mol/L of the solution prepared by dissolving 13.6 g of sodium
hydroxide in 450 mL of water?
23. Write an ionic equation for the dissociation of calcium chloride in water.
24. Complete the following table by indicating the products of the double displacement reaction and by
circling any insoluble products.
Reactants
NaCl
MgSO4
PbNO3
Li3PO4
KC2H2O2
BaS
25. Sketch a typical solubility curve for a solid and a gas.
Na2CO3
CaCl2
26. Using an example to help you, distinguish between dissociation and ionization.
27. Lead (II) nitrate reacts with potassium iodide to produce a bright yellow solid. Write a balanced chemical
equation, an ionic equation and a net ionic equation for the reaction. MAKE SURE TO INCLUDE STATES.
28. Distinguish between an Arrhenius acid and a Bronsted-Lowry acid?
29. Give an example of a conjugate acid-base pair.
30. Which of the following could be an amphiprotic substance.
A) H2O
B) SO42C) HCO3-
D) OH-
31. Determine the pH of solutions with the following hydronium concentrations.
A) [H3O+ (aq)] = 2.5 x 10-3
B) [H3O+ (aq)] = 6.76 x 10-5
32. Determine the hydronium concentrations for solutions with the following pHs.
A) pH= 5.60
B) pH= 2.31
C) pH= 12.80
33. Magnesium metal reacts with hydrochloric acid to produce magnesium chloride and hydrogen gas. How
many hydrogen molecules are produced when 60.0 g of hydrochloric acid are reacted with excess
magnesium.
34. Determine the mass of silver chloride (AgCl) produced when 75 mL of a 4.5 M solution of silver nitrate
(AgNO3) reacts with 15 g of sodium chloride (NaCl).
35. When solid iron (II) oxide is heated in the presence of carbon monoxide gas, iron metal and carbon
dioxide gas are produced.
A) Write a balanced chemical equation for the reaction.
B) If 74.20 kg of iron (II) oxide and 40.30 kg of carbon monoxide are reacted, what is the mass of iron
that can be produced.
C) If 48.90 kg of iron metal is actually produced what is the % yield of the reaction?
36. 20.0 mL of 0.20 M NaOH reacts with 25.0 mL of 0.25 M HCl (aq). What mass of sodium chloride would be
produced and what would the pH of the solution be after the reaction was complete?