Unit 9. Liquids and Solids
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1 Unit 9. Liquids and Solids Upon successful completion of this unit, the students should be able to: 9.1 List the various intermolecular attractions in liquids and solids (dipole-dipole, London dispersion, hydrogen bond) describe the nature and relative strength of each, and identify which compounds exhibit which intermolecular attraction. 1. Which of the following compounds will exhibit hydrogen bonding? H 2 NNH 2, CH 3 F, HNNH, HOCH 2 CH 2 OH, H 2 CO 2. The forces of attraction between molecules of I 2 are a. dipole-dipole attractions. b. covalent bonds. c. London dispersion forces. d. ion-dipole attractions. e. hydrogen bonds. 3. Draw a picture showing two ammonia (NH 3 ) molecules undergoing hydrogen bonding. Make sure to clearly label where the hydrogen bond is and explain briefly why the bond occurs. 9.2 Predict and explain how intermolecular attractions affect the physical properties of liquids and solids. 1. Which of the following compounds is expected to have the highest boiling point? Explain your choice. a. CH 3 OCH 3 b. CH 3 CH 2 OH c. CH 3 CH 2 CH 2 CH 3 d. CH 3 CH 2 CH 3 e. CH 3 Cl 2. Which of the following compounds would be expected to have the highest vapor pressure? a. CH 3 CH 2 CH 2 F b. CH 3 CH 2 CH 2 OH c. CH 3 CHCH 3 OH d. CH 3 CH 2 COOH e. CH 3 CH 2 CH 2 NH 2 3. Which compound should have the lowest boiling point? a. C 5 H 12 b. C 6 H 14 c. C 7 H 16 d. C 8 H 18 e. C 8 H 16
2 4. Of HF, HCl, HBr, which has the highest boiling point? Explain. 5. True or False. The stronger the attractice forces among molecules of a liquid, the lower the vapor pressur is. 6. True or False. PH 3 has a lower normal boiling point than AsH List the characteristics of molecular, network covalent, ionic and metallic solids. 1. Lithium hydride, LiH, is a: a. polar molecular gas b. nonpolar molecular gas c. covalent network solid d. ionic solid e. metallic solid 2. SiO 2, quartz, is a: a. polar molecular gas b. nonpolar molecular gas c. covalent network solid d. ionic solid e. metallic solid 3. Describe the differences between the structures of the three main allotropes of carbon: diamond, graphite, and buckyball. 4. Which of the following exists as discrete (or separate) molecules? a. potassium b. glass c. quartz d. carborundum, SiC e. hydrogen chloride 5. Describe two properties that would typically distinguish an ionic solid from a molecular solid. 6. Which of the following statements is not consistent with the properties of a molecular solid? a. A compound that conducts electricity when molten. b. A low melting solid. c. A solid formed by the combination of two nonmetallic elements. d. A solid that is a nonconductor of electricity.
3 9.4 Describe the relationship among temperature, vapor pressure, and boiling point. 1. Define boiling point in terms of vapor pressure. 2. If heat is added to ice and liquid water in a closed container and, after the addition of the heat, ice and liquid water remain: a. the vapor pressure of the water will decrease b. the temperature will increase somewhat c. the temperature will decrease somewhat d. the vapor pressure of the water will rise e. the vapor pressure of the water will remain constant 9.5 Define heat of vaporization and heat of fusion and solve related problems. 1. Define heat of fusion. 2. Which of the following liquids has the highest heat of vaporization? a. HF b. CH 4 c. CO d. all the same 3. Explain why the heat of vaporization of a substance generally tends to be much greater than its heat of fusion. 9.6 Differentiate between the terms melting, freezing, boiling, evaporation, condensation, sublimation, and deposition. 1. Consider the following reversible reaction: CS 2 (l) CS 2 (g) The forward and reverse reactions could represent, respectively: a. melting and freezing b. boiling and condensation c. sublimation and deposition d. freezing and melting 2. Define sublimation. 9.7 Draw and interpret a heating/cooling curve for a substance. 1. Draw a heating curve from -20 o C to 75 o C for a substance having a melting point of -9.0 o C and a boiling point of 62 o C. Label on your curve where condensation would occur. 9.8 Describe the nature of a supercooled liquid and a superheated liquid. 1. a. Describe what is meant by a supercooled liquid. b. Show how a supercooled liquid would appear on a heating and cooling curve.
4 9.9 Solve quantitative problems related to heat of fusion and heat of vaporization. 1. The heat of vaporization of water at 373 K is 40.7 kj/mol. Calculate H when 9.00 g of steam condense at 373 K. 2. What quantity of heat (kj) is required to melt 2.0 kg of ice at its melting point? 9.10 Define normal melting point and normal boiling point. 1. Define normal melting point Interpret phase diagrams. Questions 1-3 refer to the following phase diagram: 100 atm P 1 atm
5 1. Which of the following could represent the minimum pressure at which this substance could exist in the liquid phase? a. 1 atm b. 5 atm c. 100 atm d. 150 atm 2. When this substance is heated at normal atmospheric pressure, which of the following can occur: a. melting and boiling b. melting c. boiling d. sublimation 3. Label on the curve where the triple point is Define the terms critical point and triple point as it applies to phase diagrams. 1. Define triple point. Additional Unit 9 Sample Questions: 1. The enthalpy changes for which of the following processes would be expected to be exothermic? 1. Cl(g) + e- Cl - (g) 2. CO 2 (s) CO 2 (g) 3. Na(g) Na + (g) + e- 4. Cl 2 (g) 2Cl(g) a. 1 only b. 3 only c. 1 and 2 only d. 2 and 3 only e. 2, 3, and 4 2. A 50.0 L tank at 25 o C contains 25.0 g of acetone (C 3 H 6 O). Acetone is found in nail polish remover and is a liquid at room temperature (25 o C) and pressure. The vapor pressure of acetone at that temperature is mm Hg. Which of the following is true? Show work to justify your answer. a. The pressure of acetone in the tank is mm Hg. b. The pressure of acetone in the tank is greater than mm Hg. c. There is no liquid acetone left in the tank because is all evaporated. d. The liquid acetone and gaseous acetone are in dynamic equilibrium. e. None of the above.
6 3. Indicate the strongest type of interparticle attractive force that must be broken in each of the following. Choices are in the right column. 1. melt HF a. dipole-dipole attraction b. London dispersion forces 2. melt Li 2 CO 3 c. ionic bond d. covalent bond 3. boil NF 3 e. metallic bond f. hydrogen bond 4. boil CCl 4
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