1. IMF and water/phase changes LT 1. Which of the following substances would be expected to have the highest melting point? a. NaCl b. H 2 O c. CH 3 OH d. Ne

2. IMF and water/phase changes LT 2. In a closed container when the rate of condensation equals the rate of evaporation for a liquid, this special situation is called: a. physical pressures b. equal states c. physical equilibrium d. none of the above

3. Energy requirements for phase changes LT 3. How much heat is required to melt 50.0 g of ice at 0°C? (The molar heat of fusion for water is 6.02 kJ/mol) a. 301 kJ b. 16.7 kJ c. 12.0 kJ d. 5.02 kJ

4. IMF and water/phase changes LT 4. If you increase the pressure above a liquid, its boiling point will: a. decrease b. increase c. remain the same d. depends on the identity of the liquid

5. IMF and water/phase changes LT 5. The escape of vapor molecules with sufficiently high energy from the surface of a liquid is called a. condensation b. evaporation c. boiling d. sublimation

6. IMF and water/phase changes LT 6. Which of the following statements is INCORRECT? a. the boiling point is the temperature at which the vapor pressure of the liquid equals the atmospheric pressure b. once a substance has begun to boil the temperature of the liquid will remain constant c. evaporation is the same thing as boiling d. if the pressure is changed a substance can be made to boil at a different temperature than its normal boiling point

7. 7. Which of the following substances would be expected to have the lowest boiling point? a. MgCl 2 b. C 12 H 22 O 11 c. H 2 O d. CS 2

8. 8. Which substance has the highest vapor pressure? a. CH 4 b. KCl c. H 2 S d. H 2 O

9. 9. Which of the following should have the lowest boiling point? a. Na 2 S b. HF c. NH 3 d. N 2

10. Identify the major attractive force in each of the following five molecules. 10-14

11. 10. Na 2 S a. dipole-dipole b. London dispersion c. ionic d. hydrogen bonding

12. 11. HF a. dipole-dipole b. London dispersion c. ionic d. hydrogen bonding

13. 12. N 2 a. dipole-dipole b. London dispersion c. ionic d. hydrogen bonding

14. 13. NH 3 a. dipole-dipole b. London dispersion c. ionic d. hydrogen bonding

15. 14. H 2 S a. dipole-dipole b. London dispersion c. ionic d. hydrogen bonding

16. 15. Calculate the quantity of energy required to change 3.00 mol of liquid water to steam at 100°C. The molar heat of vaporization of water is 40.6 kJ/mol. a. 40.6 kJ b. 13.5 kJ c. 122 kJ d. 300 kJ

17. 16. Calculate the quantity of energy required to change 26.5 g of liquid water to steam at 100°C. The molar heat of vaporization of water is 40.6 kJ/mol. a. 1.08 x 10 3 kJ b. 59.8 kJ c. 1.53 kJ d. 27.6 kJ

18. 17. The specific heat capacity of liquid water is 4.18 kJ/g °C. Calculate the quantity of energy required to heat 1.00 g of water from 26.5°C to 83.7°C. a. 239 J b. 57.2 J c. 13.7 J d. 350. J

19. 18. The molar heat of fusion of water is 6.02 kJ/mol. Calculate the energy required to melt 46.8 g of water. a. 282 kJ b. 2.32 kJ c. 6.02 kJ d. none of these

20. 19. The specific heat capacity of liquid water is 4.18 kJ/g °C. Calculate the quantity of energy required to heat 10.0 g of water from 26.5°C to 83.7°C. a. 837 J b. 572 J c. 239 J d. 2.39 x 10 3 J

21. 20. The molar heat of fusion of water is 6.02 kJ/mol. Calculate the energy required to melt 3.00 mol of ice. a. 6.02 kJ/mol b. 12.0 kJ/mol c. 18.1 kJ/mol d. 2.01 kJ/mol

22. 21. The molar heat of fusion of water is 6.02 kJ/mol. Calculate the energy required to melt 14.0 g of water. a. 6.02 kJ b. 4.68 kJ c. 84.3 kJ d. 7.74 kJ

23. 22. Which of the following processes must exist in equilibrium with the evaporation process when a measurement of vapor pressure is made? a. fusion b. vaporization c. sublimation d. condensation

24. 23. As the temperature of a liquid increases, the vapor pressure of the liquid generally a. increases b. decreases c. stays the same d. depends on the type of intermolecular forces

25. 24. As the atmospheric pressure around a liquid decreases, the boiling temperature of the liquid a. increases b. decreases c. stays the same d. may increase or decrease depending on the liquid

26. 25. Which of the following has the highest melting temperature? a. H 2 O b. CO 2 c. S 8 d. MgF 2

27. 26. Name the type of crystalline solid formed by potassium bromide. a. molecular solid b. atomic solid c. ionic solid d. amorphous solid

28. 27. Name the type of crystalline solid formed by copper. a. molecular solid b. atomic solid c. ionic solid d. amorphous solid

29. 28. Name the type of crystalline solid formed by SiO 2. a. molecular solid b. atomic solid c. ionic solid d. amorphous solid