1. General Chemistry Principles & Modern Applications 9 th Edition Petrucci/Harwood/Herring/Madura Chapter 12 Liquids, Solids and Intermolecular Forces Dr. Travis D. Fridgen Memorial University of Newfoundland © 2007 Pearson Education

2. Which row do you think has the correct heats of vaporization associated with the compound (in its liquid form)? 1.3.410.42.80.5 All values are in kJ mol -1. 3.410.42.80.52. 3.410.42.80.53.

3. Which row do you think has the correct heats of vaporization associated with the compound (in its liquid form)? 1.3.410.42.80.5 All values are in kJ mol -1. 3.410.42.80.52. 3.410.42.80.53.

4. number of molecules kinetic energy AB 1.Compound A has a higher vapor pressure than compound B. 2.More energy is required to vaporize 1 mole of A than one mole of B. The lines marked A and B represent the point where each of the molecules for two different liquids (A and B) have enough kinetic energy to escape into the gas phase. Which of the following statements is correct? 3.On average, at a given temperature, B has more kinetic energy than A. 4.On average, at a given temperature, A has more kinetic energy than B. 5.The intermolecular forces between molecules of A are stronger than those between molecules of B.

5. number of molecules kinetic energy AB 1.Compound A has a higher vapor pressure than compound B. 2.More energy is required to vaporize 1 mole of A than one mole of B. The lines marked A and B represent the point where each of the molecules for two different liquids (A and B) have enough kinetic energy to escape into the gas phase. Which of the following statements is correct? 3.On average, at a given temperature, B has more kinetic energy than A. 4.On average, at a given temperature, A has more kinetic energy than B. 5.The intermolecular forces between molecules of A are stronger than those between molecules of B.

6. number of molecules kinetic energy ABThe lines marked A and B represent the point where each of the molecules for two different liquids (A and B) have enough kinetic energy to escape into the gas phase. Choose the incorrect statement, 1. There would be more A than B molecules in the gas phase. 2.There are stronger intermolecular forces between molecules of A than molecules of B. 3.Increasing the temperature would result in more molecules of both A and B in the gas phase.

7. number of molecules kinetic energy ABThe lines marked A and B represent the point where each of the molecules for two different liquids (A and B) have enough kinetic energy to escape into the gas phase. Choose the incorrect statement, 1. There would be more A than B molecules in the gas phase. 2.There are stronger intermolecular forces between molecules of A than molecules of B. 3.Increasing the temperature would result in more molecules of both A and B in the gas phase.

8. A B D C 5. s g l g s 4. s l g l s 3. g s l g 2. s l g s 1. l s g l To the right is the phase diagram for iodine. Which of the following transitions occur when the temperature and pressure conditions are changed from A to B to C to D?

9. A B D C 5. s g l g s 4. s l g l s 3. g s l g 2. s l g s 1. l s g l To the right is the phase diagram for iodine. Which of the following transitions occur when the temperature and pressure conditions are changed from A to B to C to D?

10. ethane T boil = 185 K butane T boil = 273 K Butane has a much higher melting point than ethane because (choose the best answer) 1. butane is heavier than ethane. 2.butane has more electrons and is therefore more polarizable than ethane. 3.butane has more hydrogens and therefore can make more hydrogen bonds than ethane. 4.butane is more polar than ethane and therefore has stronger dipole-dipole interactions. 5.butane has more protons than ethane.

11. ethane T boil = 185 K butane T boil = 273 K Butane has a much higher melting point than ethane because (choose the best answer) 1. butane is heavier than ethane. 2.butane has more electrons and is therefore more polarizable than ethane. 3.butane has more hydrogens and therefore can make more hydrogen bonds than ethane. 4.butane is more polar than ethane and therefore has stronger dipole-dipole interactions. 5.butane has more protons than ethane.

12. T boil = -269 o C T boil = -246 o C T boil = -186 o C T boil = -153 o C The boiling points of some rare gases are provided to the right. This trend in boiling points is best explained with reference to 1. the masses of the atoms. 2. the polarizabilities of the atoms. 3. the dipole moment of the atoms. 4. the number of neutrons in the nuclei of the atoms. 5. the trend in melting points of the solid rare gases.

13. T boil = -269 o C T boil = -246 o C T boil = -186 o C T boil = -153 o C The boiling points of some rare gases are provided to the right. This trend in boiling points is best explained with reference to 1. the masses of the atoms. 2. the polarizabilities of the atoms. 3. the dipole moment of the atoms. 4. the number of neutrons in the nuclei of the atoms. 5. the trend in melting points of the solid rare gases.

14. Two C 3 H 6 O isomers, acetone and methoxy ethene are shown below. Being isomers, the molar masses and the number of electrons are equal. Their boiling points, however, are quite different. The best reason for the difference in boiling points is? acetone T boil = 330 K methoxy ethene T boil = 279 K 1. Methoxy ethane is much more polarizable. 2.Acetone molecules can participate in hydrogen bonding with one another. 3.Methoxy ethane molecules can participate in hydrogen bonding with one another. 4. Acetone has a higher dipole moment. 5. Methoxy methane has a higher dipole moment.

15. Two C 3 H 6 O isomers, acetone and methoxy ethene are shown below. Being isomers, the molar masses and the number of electrons are equal. Their boiling points, however, are quite different. The best reason for the difference in boiling points is? acetone T boil = 330 K methoxy ethene T boil = 279 K 1. Methoxy ethane is much more polarizable. 2.Acetone molecules can participate in hydrogen bonding with one another. 3.Methoxy ethane molecules can participate in hydrogen bonding with one another. 4. Acetone has a higher dipole moment. 5. Methoxy methane has a higher dipole moment.

16. 1-propanol glycerol Propanol is a relatively volatile liquid while glycerol is a very viscous liquid much like syrup. The difference in the viscosity of these liquids is best explained by 1.the fact that glycerol is much heavier than 1-propanol. 2.the fact that glycerol is a more polar molecule than 1-propanol. 3.the fact that glycerol can form more hydrogen bonds than 1-propanol. 4.the higher polarizability of 1-propanol. 5.the higher polarizability of glycerol.

17. 1-propanol glycerol Propanol is a relatively volatile liquid while glycerol is a very viscous liquid much like syrup. The difference in the viscosity of these liquids is best explained by 1.the fact that glycerol is much heavier than 1-propanol. 2.the fact that glycerol is a more polar molecule than 1-propanol. 3.the fact that glycerol can form more hydrogen bonds than 1-propanol. 4.the higher polarizability of 1-propanol. 5.the higher polarizability of glycerol.

18. Which process would you expect to require the most energy? 1.The conversion of 1 mole of solid ethanol to 1 mole of liquid ethanol. 2. The conversion of 1 mole of solid chloroethane to 1 mole of liquid chloroethane. 3. The conversion of 1 mole of solid ethane to 1 mole of liquid ethane. 5.The conversion of 1 mole of liquid chloroethane to 1 mole of gaseous chloroethane. 4.The conversion of 1 mole of liquid ethanol to 1 mole of gaseous ethanol.

19. Which process would you expect to require the most energy? 1.The conversion of 1 mole of solid ethanol to 1 mole of liquid ethanol. 2.The conversion of 1 mole of solid chloroethane to 1 mole of liquid chloroethane. 3.The conversion of 1 mole of solid ethane to 1 mole of liquid ethane. 5.The conversion of 1 mole of liquid chloroethane to 1 mole of gaseous chloroethane. 4.The conversion of 1 mole of liquid ethanol to 1 mole of gaseous ethanol.

20. 370 K313 K True or false. At 370 K the vapor pressure of benzene is the greatest of the three substances shown and Toluene has the lowest, whereas at 313 K benzene still has the higher vapor pressure but water has the lowest. 1. True 2. False

21. 370 K313 K True or false. At 370 K the vapor pressure of benzene is the greatest of the three substances shown and Toluene has the lowest, whereas at 313 K benzene still has the higher vapor pressure but water has the lowest. 1. True 2. False

22. To the left is a cartoon diagram of a particular unit cell. How many atoms would there be in 1 mole of these unit cells? 1. 6.022 x 10 23 atoms. 2. 4 moles of atoms 3. 2 x (6.022 x 10 23 ) atoms. 4. 4 x (6.022 x 10 23 ) atoms. 5. 1.875 moles

23. To the left is a cartoon diagram of a particular unit cell. How many atoms would there be in 1 mole of these unit cells? 1. 6.022 x 10 23 atoms. 2. 4 moles of atoms 3. 2 x (6.022 x 10 23 ) atoms. 4. 4 x (6.022 x 10 23 ) atoms. 5. 1.875 moles

24. 444 pm512 pm 627 pm If Ba were to solidify with the crystal structures to the right, the edge lengths would be as given below sccbccfcc This means that the bcc and fcc unit cells have volumes which are roughly 1.5 and 3 times as large, respectively, as the scc unit cell. Which of the following statements is best, 5. The density of the scc unit cell is larger because the mass is larger. 1. The density of the fcc unit cell is larger because the volume is larger. 2. The density of the fcc unit cell is smaller because the volume is larger. 3. The density of the scc unit is larger because the volume is smaller. 4. The density of the fcc unit cell is larger because the mass is larger.

25. 444 pm512 pm 627 pm If Ba were to solidify with the crystal structures to the right, the edge lengths would be as given below sccbccfcc This means that the bcc and fcc unit cells have volumes which are roughly 1.5 and 3 times as large, respectively, as the scc unit cell. Which of the following statements is best, 5. The density of the scc unit cell is larger because the mass is larger. 1. The density of the fcc unit cell is larger because the volume is larger. 2. The density of the fcc unit cell is smaller because the volume is larger. 3. The density of the scc unit is larger because the volume is smaller. 4. The density of the fcc unit cell is larger because the mass is larger.

26. Which of the following would you expect to have the largest lattice energy? 1. MgCl 2 2. MgBr 2 3. NaBr 4. CaCl 2 5. CaBr 2 Δ lattice H° αcation charge x anion charge cation radius + anion radius

27. Which of the following would you expect to have the largest lattice energy? 1. MgCl 2 2. MgBr 2 3. NaBr 4. CaCl 2 5. CaBr 2 Δ lattice H° αcation charge x anion charge cation radius + anion radius

28. Which of the following ionic compounds would you expect to require more energy to decompose to gaseous ions than CaS(s)? 1. NaF(s) 2. SrS(s) 3. AlN(s) 4. MgBr 2 (s) 5. SrSe(s)

29. Which of the following ionic compounds would you expect to require more energy to decompose to gaseous ions than CaS(s)? 1. NaF(s) 2. SrS(s) 3. AlN(s) 4. MgBr 2 (s) 5. SrSe(s)

30. Which of the following ionic compounds would you expect to have the lowest boiling point? 1. KF 2. BeO 3. BN 4. KBr 5. NaCl

31. Which of the following ionic compounds would you expect to have the lowest boiling point? 1. KF 2. BeO 3. BN 4. KBr 5. NaCl