Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
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Textbook Question
Chapter 11, Problem 77RQ
Determining the Structure of Solids
What relationship is there between a crystal lattice and its unit cell?
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Chapter 11 Solutions
Chemistry: The Molecular Nature of Matter
Ch. 11 - Prob. 1PECh. 11 - List the following in order of their boiling...Ch. 11 - Propylamine and trimethylamine have the same...Ch. 11 - People living in arid, dry, regions can cool their...Ch. 11 - Use the kinetic molecular theory to explain why...Ch. 11 - Considering Figure 11.24, in which direction...Ch. 11 - Suppose a liquid is in equilibrium with its vapor...Ch. 11 - The Dead Sea is approximately 1300 ft below sea...Ch. 11 - The atmospheric pressure at the summit of Mt....Ch. 11 - Benzene has a boiling point of 80.1C, and a...
Ch. 11 - Steam can cause more severe bums than water, even...Ch. 11 - The equilibrium line from point B to D in Figure...Ch. 11 - What phase changes will occur if water at 20C and...Ch. 11 - Prob. 14PECh. 11 - Use Le Chtelier's principle to predict how a...Ch. 11 - Prob. 16PECh. 11 - At 0.00C, hexane, C6H14, has a vapor pressure of...Ch. 11 - Prob. 18PECh. 11 - Chromium crystallizes in a body-centered cubic...Ch. 11 - What is the ratio of the ions in the unit cell of...Ch. 11 - Polonium is the only metal known to crystallize in...Ch. 11 - Use the data in the previous Practice Exercise to...Ch. 11 - Stearic acid is an organic acid that has a chain...Ch. 11 - Boron nitride, which has the empirical formula BN,...Ch. 11 - Crystals of elemental sulfur are easily crushed...Ch. 11 - 11.1 Why are the intermolecular attractive forces...Ch. 11 - Compare the behavior of gases, liquids, and solids...Ch. 11 - Prob. 3RQCh. 11 - Why do intermolecular attractions weaken as the...Ch. 11 - Prob. 5RQCh. 11 - Define polarizability. How does this property...Ch. 11 - Prob. 7RQCh. 11 - 11.8 Which nonmetals, besides hydrogen, are...Ch. 11 - Prob. 9RQCh. 11 - Which would give a stronger iondipole interaction...Ch. 11 - Prob. 11RQCh. 11 - Prob. 12RQCh. 11 - Intermolecular Forces and Physical...Ch. 11 - Prob. 14RQCh. 11 - Intermolecular Forces and Physical Properties Name...Ch. 11 - Prob. 16RQCh. 11 - Prob. 17RQCh. 11 - Prob. 18RQCh. 11 - Prob. 19RQCh. 11 - Prob. 20RQCh. 11 - Intermolecular Forces and Physical...Ch. 11 - Prob. 22RQCh. 11 - Prob. 23RQCh. 11 - Prob. 24RQCh. 11 - Prob. 25RQCh. 11 - Prob. 26RQCh. 11 - Prob. 27RQCh. 11 - Prob. 28RQCh. 11 - Prob. 29RQCh. 11 - Changes of State and Dynamic Equilibrium What...Ch. 11 - Prob. 31RQCh. 11 - Changes of State and Dynamic Equilibrium
11.32 Why...Ch. 11 - Changes of State and Dynamic Equilibrium
11.33...Ch. 11 - Changes of State and Dynamic Equilibrium
11.34....Ch. 11 - Prob. 35RQCh. 11 - Prob. 36RQCh. 11 - Vapor Pressures of Liquids and Solids
11.37...Ch. 11 - Prob. 38RQCh. 11 - Vapor Pressures of Liquids and Solids 11.39 What...Ch. 11 - Vapor Pressures of Liquids and Solids Why does...Ch. 11 - Vapor Pressures of Liquids and Solids Why do we...Ch. 11 - Prob. 42RQCh. 11 - Boiling Points of Liquids Why does the boiling...Ch. 11 - Boiling Points of Liquids Mt. Kilimanjaro in...Ch. 11 - Boiling Points of Liquids
11.45. When liquid...Ch. 11 - Prob. 46RQCh. 11 - Boiling Points of Liquids Butane, C4H10, has a...Ch. 11 - Boiling Points of Liquids
11.48. Why does have a...Ch. 11 - Boiling Points of Liquids An HF bond is more polar...Ch. 11 - Energy and Changes of State The following is a...Ch. 11 - Energy and Changes of State
11.51 Why is larger...Ch. 11 - Energy and Changes of State Would the heat of...Ch. 11 - Energy and Changes of State Hurricanes can travel...Ch. 11 - Energy and Changes of State Ethanol (grain...Ch. 11 - Energy and Changes of State A burn caused by steam...Ch. 11 - Energy and Changes of State
11.56 Arrange the...Ch. 11 - Prob. 57RQCh. 11 - Phase Diagrams
11.58 Define critical temperature...Ch. 11 - Phase Diagrams What is a supercritical fluid? Why...Ch. 11 - Phase Diagrams
11.60 What phases of a substance...Ch. 11 - Prob. 61RQCh. 11 - Prob. 62RQCh. 11 - Phase Diagrams Sketch a generic phase diagram that...Ch. 11 - Phase Diagrams
11.64 What is the significance of...Ch. 11 - Prob. 65RQCh. 11 - Le Chtelier's Principle and Changes of State State...Ch. 11 - Le Châtelier's Principle and Changes of...Ch. 11 - Le Chtelier's Principle and Changes of State Use...Ch. 11 - Le Chtelier's Principle and Changes of State Use...Ch. 11 - Le Châtelier's Principle and Changes of...Ch. 11 - Determining Heats of Vaporization According to the...Ch. 11 - Determining Heats of Vaporization Why can't...Ch. 11 - Determining Heats of Vaporization Why can any...Ch. 11 - Prob. 74RQCh. 11 - Prob. 75RQCh. 11 - Prob. 76RQCh. 11 - Determining the Structure of Solids What...Ch. 11 - Determining the Structure of Solids
11.78 The...Ch. 11 - The figure below illustrates the way the atoms of...Ch. 11 - Make a sketch of a layer of sodium ions and...Ch. 11 - 11.81 How do the crystal structures of copper and...Ch. 11 - Determining the Structure of Solids
11.82 What...Ch. 11 - Determining the Structure of Solids Only 14...Ch. 11 - Determining the Structure of Solids Write the...Ch. 11 - Determining the Structure of Solids Why cant...Ch. 11 - Prob. 86RQCh. 11 - Crystal Types and Physical Properties
11.87 What...Ch. 11 - Prob. 88RQCh. 11 - Prob. 89RQCh. 11 - Prob. 90RQCh. 11 - Intermolecular Forces and Physical Properties What...Ch. 11 - Intermolecular Forces and Physical Properties What...Ch. 11 - Intermolecular Forces and Physical Properties...Ch. 11 - Prob. 94RQCh. 11 - 11.95 Consider the compounds (chloroform, an...Ch. 11 - 11.96 Carbon dioxide does not liquefy at...Ch. 11 - Prob. 97RQCh. 11 - Prob. 98RQCh. 11 - Prob. 99RQCh. 11 - Prob. 100RQCh. 11 - 11.101 The following are the vapor pressures of...Ch. 11 - 11.102 The boiling points of some common...Ch. 11 - 11.103 Using the information in Problem 11.101,...Ch. 11 - 11.104 Using the information in Problem 11.102,...Ch. 11 - 11.105 What intermolecular forces must the...Ch. 11 - 11.106 What intermolecular attractions will be...Ch. 11 - Energy and Changes of State The molar heat of...Ch. 11 - Energy and Changes of State The molar heat of...Ch. 11 - *11.109 Suppose 45.0 g of water at is added to...Ch. 11 - A cube of solid benzene (C6H6) at its melting...Ch. 11 - Prob. 111RQCh. 11 - Prob. 112RQCh. 11 - Prob. 113RQCh. 11 - Prob. 114RQCh. 11 - Prob. 115RQCh. 11 - Prob. 116RQCh. 11 - Determining Heats of Vaporization
*11.117 Mercury...Ch. 11 - Prob. 118RQCh. 11 - Prob. 119RQCh. 11 - *11.120 If the vapor pressure of ethylene glycol...Ch. 11 - Determining the Structure of Solids
11.121 How...Ch. 11 - 11.122 How many copper atoms are within the...Ch. 11 - The atomic radius of nickel is 1.24 . Nickel...Ch. 11 - 11.124 Silver forms face-centered cubic crystals....Ch. 11 - Potassium ions have a radius of 133 pm, and...Ch. 11 - 11.126 The unit cell edge in sodium chloride has a...Ch. 11 - Prob. 127RQCh. 11 - Prob. 128RQCh. 11 - *11.129 Cesium chloride forms a simple cubic...Ch. 11 - 11.130 Rubidium chloride has the rock salt...Ch. 11 - Prob. 131RQCh. 11 - Crystal Types and Physical Properties Elemental...Ch. 11 - Prob. 133RQCh. 11 - Prob. 134RQCh. 11 - Prob. 135RQCh. 11 - Crystal Types and Physical Properties
11.1 36...Ch. 11 - List all of the attractive forces that exist in...Ch. 11 - 11.138 Calculate the mass of water vapor present...Ch. 11 - 11.139 Should acetone molecules be attracted to...Ch. 11 - The following thermochemical equations apply to...Ch. 11 - Melting point is sometimes used as an indication...Ch. 11 - When warm, moist air sweeps in from the ocean and...Ch. 11 - *11.143 Gold crystallizes in a face-centered cubic...Ch. 11 - Gold crystallizes with a face-centered cubic unit...Ch. 11 - Identify the type of unit cell belonging to the...Ch. 11 - Calculate the amount of empty space (in pm3) in...Ch. 11 - Silver has an atomic radius of 144 pm. What would...Ch. 11 - Potassium chloride crystallizes with the rock salt...Ch. 11 - Prob. 149RQCh. 11 - There are 270 Calories in a Hersheys* Milk...Ch. 11 - Prob. 151RQCh. 11 - *11.152 Frecze-drying is a process used to...Ch. 11 - When reporting the vapor pressure for a substance...Ch. 11 - 11.154 Supercritical is used to decaffeinate...Ch. 11 - 11.155 Freshly precipitated crystals are usually...Ch. 11 - 11.156 What are three “everyday” applications of...Ch. 11 - Prob. 157RQCh. 11 - 11.158 Galileo's thermometer is a tube of liquid...Ch. 11 - Use the Clausius-Clapeyron equation to plot the...Ch. 11 - Prob. 160RQCh. 11 - Earlier in this chapter it was noted that the...
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- Identify the kinds of forces that are most important in holding the particles together in a crystalline solid sample of each of the following substances. (a) Kr (b) HF (c) K2O (d) CO2 (e) Zn (f) NH3arrow_forwardSilicon carbide, SiC, is a very hard, high-melting solid. What kind of crystal forces account for these properties?arrow_forwardThe CsCl structure is a simple cubic array of chloride ions with a cesium ion at the center of each cubic array (see Exercise 69). Given that the density of cesium chloride is 3.97 g/cm3, and assuming that the chloride and cesium ions touch along the body diagonal of the cubic unit cell, calculate the distance between the centers of adjacent Cs+ and Cl ions in the solid. Compare this value with the expected distance based on the sizes of the ions. The ionic radius of Cs+ is 169 pm, and the ionic radius of Cl is 181 pm.arrow_forward
- An amorphous solid can sometimes be converted to a crystalline solid by a process called annealing. Annealing consists of heating the substance to a temperature just below the melting point of the crystalline form and then cooling it slowly. Explain why this process helps produce a crystalline solid.arrow_forwardThe structures of some common crystalline substances are shown below. Show that the net composition of each unit cell corresponds to the correct formula of each substance.arrow_forwardArrange the following substances in order of increasing strength of the crystal forces: He, NH3, NO2, NaBr, BaO. Identify the kinds of forces that are most important in holding the particles together in a crystalline solid sample of each of the following substances. (a) H2O (b) C6H6 (c) CaCl2 (d) SiO2 (e) Fearrow_forward
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- MnO has either the NaCI type structure or the CsCI type structure (see Exercise 69). The edge length of the MnO unit cell is 4.47 10-8 cm and the density of MnO is 5.28 g/cm3. a. Does MnO crystallize in the NaCl or the CsCl type structure? b. Assuming that the ionic radius of oxygen is 140. pm, estimate the ionic radius of manganese.arrow_forward(a) Determining an Atom Radius from Lattice Dimensions: Gold has a face-centered unit cell, and its density is 19.32 g/cm3. Calculate the radius of a gold atom. (b) The Structure of Solid Iron: Iron has a density of 7.8740 g/cm3, and the radius of an iron atom is 126 pm. Verify that solid iron has a body-centered cubic unit cell. (Be sure to note that the atoms in a body-centered cubic unit cell touch along the diagonal across the cell. They do not touch along the edges of the cell.) (Hint: The diagonal distance across the unit cell = edge 3.)arrow_forwardA portion of the crystalline lattice for potassium is illustrated below. (a) In what type of unit cell are the K atoms arranged? A portion of the solid-state structure of potassium. (b) If one edge of the potassium unit cell is 533 pm, what is the density of potassium?arrow_forward
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