Tro s Chemistry Chapter 11 Liquids, Solids, and Intermolecular forces Page 1 of 13 Acknowledgements: Key terms, concepts, and skills:
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1 Tro s Chemistry Chapter 11 Liquids, Solids, and Intermolecular forces Page 1 of 13 Acknowledgements: Many of the images are adopted from Tro s textbook, the only purpose of which is to enhance student learning. Key terms, concepts, and skills: Refer to pp Review questions: 2 45 minus 36, 40, Suggested problems:49, 50, 54, 55, 59, 63, 67, 69, 77, 81, 83, 85, 89, 91, 97, 99, 105, 107, 109, & 2 Intermolecular Forces and Physical States The force of attraction between two neighboring molecules or atoms. The magnitude of Intermolecular forces determine whether a pure substance will be solid, liquid or gas meaning their mp, bp, surface tension, viscosity. Intramolecular attractions are covalent in nature involving overlapping of bonding electron clouds. Intermolecular forces are much weaker than intramolecular forces.
2 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 2 of IMF in the Condensed Phases E = const x q 1 x q 2 r Dispersion (London) Force Present in all molecules and atoms due to their electron contents. At any given instant when electron(s) populate a spot of the cloud/orbital, it causes an instantaneous or temporary dipole which can affect the neighboring atom or molecule. Magnitude of dispersion force depends upon how easily the electrons can be moved or polarized, which depends on the size of the cloud. Higher molar mass causes increased dispersion force. Dipole-Dipole Force This force exists in all polar molecules. Their permanent dipoles interact with the dipoles of the neighboring ones. This causes higher mp and bp to polar molecules. (Refer to Example 11.1 and Practice 11.1 for more help and hint.)
3 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 3 of 13 Hydrogen Bonding Another stronger force of attraction. It requires polar molecule with H bonded to F, O, N, atoms of high electronegativity. A δ+ charge and its small size causes H to feel attracted to F, O, and N of the other molecule. (Refer to Example 11.2 and Practice 11.2 for more help and hint.) Ion-Dipole Force This force occurs when an ionic compound is mixed with a polar compound. Important in aqueous solutions of ionic compounds. Cations are surrounded by negative pole of polar solvent and anions are surrounded by positive poles causing what s called solvation. This enhances solubility.
4 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 4 of 13 Q #49 & 50. Determine the kinds of intermolecular forces that are present in each of the following elements or compounds: a. Kr b. NCI 3 c. SiH 4 d. HF e. N 2 f. NH 3 g. CO h. CCI 4 Q54. Arrange the following in order of increasing boiling point. Explain your reasoning. a. H 2 S b. H 2 Se c. H 2 O Q #55. For each pair of compounds, pick the one with the highest boiling point. Explain your reasoning. a. CH 3 OH or CH 3 SH b. CH 3 OCH 3 or CH 3 CH 2 OH c. CH 4 or CH 3 CH 3 Q #59. Which of the following pairs of substances would you expect to form homogeneous solutions when combined? For those that form homogeneous solutions, indicate the type of forces that are involved. a. CCI 4 and H 2 O b. KCI and H 2 O c. Br 2 and CCI 4 d. CH 3 CH 2 OH and H 2 O
5 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 5 of IMF in Surface Tension, Viscosity, Capillary Action Surface Tension Molecules of pure liquids at the surface have higher potential energy than the interior ones. As a result, liquids tend to minimize the surface area making the surface to behave like a skin. It is the energy required to increase the surface area by a unit amount. Water and benzene s surface tension are 72.8 and 28 mj/m 2. Viscosity It is the resistance of a liquid to flow, i.e., preventing one to flow around another. This force depends on the IMF and the shape of the molecule. Capillary Action It is the ability of a liquid to flow against gravity up a narrow tube. It is a combination of cohesive and adhesive forces. Q #63. The structures of two isomers of heptanes are shown below. Which of these two compounds would you expect to have the greater viscosity? Compound A Compound B
6 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 6 of Vaporization and Vapor Pressure Vaporization Process Energetics of Vaporization When the high energy molecules are lost from the liquid, it lowers the average kinetic energy If energy is not drawn back into the liquid, its temp. will decrease therefore, vaporization is an endothermic process and condensation is an exothermic process Vaporization requires input of energy to overcome the attractions between molecules (Refer to Example 11.3 and Practice 11.3 for more help and hint.) Vapor Pressure and Dynamic Equilibrium
7 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 7 of 13 Vapor Pressure and BP Clausius-Clapeyron Eqn. P H 2 ln = P1 R vap 1 T2 1 T1 (Refer to Example and Practice for more help and hint.) Q #67. Which will evaporate more quickly: 55 ml of water in a beaker with a diameter of 4.5 cm, or 55 ml of water in a dish with a diameter of 12 cm? Will the vapor pressure of the water be different in the two containers? Explain. Q #69. Spilling room-temperature water over your skin on a hot day will cool you down. Spilling vegetable oil (of the same temperature) over your skin on a hot day will not. Explain the difference. Q #77. Ethanol has a heat of vaporization of kj/mol and a normal boiling point of 78.4 C. What is the vapor pressure of ethanol at 15 C?
8 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 8 of 13 Critical Point Unususal Phase 11.6 Sublimation and Fusion Sublimation Fusion 11.7 Heating Curve for Water Q #81. An 8.5-g ice cube is placed into 255 g of water. Calculate the temperature change in the water upon the complete melting of the ice. Assume that all of the energy required to melt the ice comes from the water. Q #83. How much heat (in kj) is required to warm 10.0 g of ice, initially at 10.0 C, to steam at C? The heat capacity of ice is 2.09 J/g. C and that of steam is 2.01 J/g. C.
9 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 9 of Phase Diagram major features Regions Lines Triple Point Critical Point Q #85. Consider the phase diagram on the right. Identify the phases present at points a through g.
10 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 10 of 13 Q #89. The phase diagram for sulfur is shown on the right. The rhombic and monoclinic phases are two solid phases with different structures. a. Below what pressure will solid sulfur sublime? b. Which of the two solid phases of sulfur is most dense? 11.9 Extraordinary Properties of Water Q #91. Water has a high boiling point for its relatively low molar mass. Why? Crystalline Solids X-Ray Crystallography (skip) 11.11Crystalline Solids Basic Unit Cells
11 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 11 of 13 (Refer to Example 11.7 and Practice 11.7 for more help and hint.) Q #97. Determine the number of atoms per unit cell for each of the following metals.
12 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 12 of 13 Q #99. Platinum crystallizes with the face-centered cubic unit cell. The radius of a platinum atom is 139 pm. Calculate the edge length of the unit cell and the density of platinum in g/cm Crystalline Solids Fundamental Types Molecular Solids Ionic Solids
13 Tro s Chemistry / Chapter 11 Chapter 11 Liquids, Solids, and Intermolecular forces 13 of 13 Atomic Solids Metallic solids Q #105. Identify each of the following solids as molecular, ionic, or atomic. a. Ar(s) b. H 2 O(s) c. K 2 O(s) d. Fe(s) Q #107. Which of the following solids has the highest melting point? Why? Ar(s), CCI 4 (s), LiCI (s), CH 3 OH (s) Q #107. Of each pair of solids, which one has the higher melting point and why? a. TiO 2 (s) or HOOH(s) b. CCI 4 (s) or SiCI 4 (s) c. Kr(s) or Xe(s) d. NaCI(s) or CaO(s) Crystalline Solids Band Theory (skip) Cumulative problem Q #128. A sealed flask contains 0.55 g of water at 28 o C. The vapor pressure of water at this temperature is mmhg. What is the minimum volume of the flask in order that no liquid water be present in the flask?
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