Year 11 Water Practice Quiz 2
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1. Which word describes the salt part of seawater? Multiple Choice: 1 mark each
a) solute.
b) solvate.
c) solvent.
d) solution.
2. Construct Lewis dot diagrams of the following:

Water (H2O)

Nitrogen (N2)

Hydrogen Sulfide (H2S)

Ammonia (NH3)

Hydronium ion (H3O+)
5 marks
3. A solid has a density of 2.5 g/cm3. What will the mass of 12cm3 of the solid be?
1 mark
4. Which of the following is not a reason for the importance of water to life on Earth?
a) Its high heat capacity helps regulate the temperature of the planet.
b) It is a reactant in the photosynthesis reaction.
c) It allows substances to dissolve and move around inside cells.
d) Every animal needs to drink water to stay properly hydrated.
5. Which words describe the giving out and taking in of heat?
2 marks
6. What is the heat capacity of water?
a) 4.18 Cal/g.K.
b) 4.18 J/g.K
c) 418 J/g.K.
d) 6 kJ/g.K
7. Why does water have a higher boiling point than hydrogen sulphide?
a) Water has a higher density.
b) Water often has impurities dissolved in it.
c) The molecular weight of water is greater than that molecular weight of hydrogen sulfide.
d) Hydrogen bonding in water.
8. Write an ionic equation for ammonia dissolving in water.
1 mark
9. Write a net ionic equation of the formation of the precipitate when calcium chloride is mixed with
ammonium carbonate. 1 mark
10. Which statement is true?
a) H2O has a higher boiling point than any other liquid because of its low molecular weight.
b) H2S has a lower boiling point than H2O because of its lack of hydrogen bonding.
c) H2O has a lower boiling point than H2S because of hydrogen bonding.
d) H2S has a similar boiling point than H2O because of hydrogen bonding.
11. Which list contains only polar molecules?
a) Water, ammonia, hydrogen fluoride.
b) Ammonium, water, hydrogen.
c) Biodiesel, kerosene, carbon dioxide
d) Sodium chloride, water, potassium iodide.
12. Name three types of intermolecular forces in order of decreasing strength.
3 marks
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13. Which of the following is a solubility rule?
a) All chlorides are soluble.
b) All ionic substances are soluble in water.
c) Most sulfates are insoluble in water.
d) Most sulfates are soluble in water.
14. Identify the main type of intermolecular forces for each of the following substances.

Ethanol

Hydrogen chloride

Neon
3 marks
15. Soap molecules are long molecules with a polar end and a non-polar end. Which statement is true?
a) The polar end dissolves in both oil and water and the non-polar end does not dissolve.
b) Soap molecules are insoluble.
c) The polar end dissolves in water and the non-polar end dissolves in oil.
d) The water end dissolves in oil and the oil end dissolves in water.
16. Which of the following substances are highly soluble in water?
a) Oxygen, ammonia, carbon dioxide.
b) Salts, alcohols, oxygen.
c) Methanol, lithium bromide, ammonia.
d) Strontium carbonate, barium sulfate, magnesium oxide.
17. Which statement best defines hydrogen bonding?
a) An force of attraction between the hydrogen atoms in a molecule and the unbonded pair of electrons of
an oxygen, nitrogen or fluorine atom of another molecule.
b) An force of attraction between the hydrogen atoms in a molecule and the unbonded pair of electrons of
an oxygen, nitrogen or fluorine atom of the same molecule.
c) A force of repulsion between hydrogen atoms in the same molecule.
d) A force of attraction between hydrogen atoms in different molecules.
18. What is the chemical formula of the precipitate when solutions of calcium chloride and silver (I) nitrate are
mixed?
a) AgCl.
b) KNO3.
c) CaNO3.
d) KCl.
19. Write an equation for the reaction between barium nitrate and ammonium sulfate solutions. Show all states.
2 marks
20. How is molarity defined?
a) The number of moles of solvent per litre of solution.
b) The number of moles of solute per litre of solution.
c) The mass of solute per litre of solution.
d) The number of moles of solute per litre of solvent.
21. What is the molarity of 265ml of solution containing 18g of calcium chloride?
2 marks
22. How much heat is required to raise the temperature of 10kg of water from 305K to 400K?
2 marks
23. What is the volume of a 280ml of 0.6M Ba(NO3)2 solution diluted to 0.5M?
2 marks
24. If one calorie is defined as the amount of heat required to raise the temperature of one gram of water by
one degree Celsius, how many joules is one calorie equal to?
2 marks
25. When would oxygen levels be expected to be lowest in a body of water?
a) Before sunrise because oxygen is used by aquatic life at night but photosynthesis has not yet started.
b) At midday because that is when the warming by the sun is greatest.
c) Oxygen levels do not change because oxygen is highly soluble.
d) Before sunset because that is when the water is warmest.
26. The enthalpy of solution of anhydrous oxalic acid in water at 298.15 K was measured in a calorimeter and
found to be +8853 J·mol-1. Thermodynamically, what type of process is this?
1 mark
27. Hydrogen bromide (HBr) is a linear molecule with no unbonded electron pairs. Explain why hydrogen
bromide is polar.
2 marks
28. Draw potassium bromide dissolved in water.
2 marks
29. Describe the trend in electronegativity across periods.
30. Describe the trend in electronegativity down groups.
31. Describe the electronegativity of group 8 elements.
2 marks
2 marks
2 marks