Chemistry: An Atoms First Approach
2nd Edition
ISBN: 9781305079243
Author: Steven S. Zumdahl, Susan A. Zumdahl
Publisher: Cengage Learning
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Chapter 9, Problem 5RQ
What is a lattice? What is a unit cell? Describe a simple cubic unit cell. How many net atoms are contained in a simple cubic unit cell? How is the radius of the atom related to the cube edge length for a simple cubic unit cell? Answer the same questions for the body-centered cubic unit cell and for the face-centered unit cell.
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Chapter 9 Solutions
Chemistry: An Atoms First Approach
Ch. 9 - What are intermolecular forces? How do they differ...Ch. 9 - Define the following terms and describe how each...Ch. 9 - Compare and contrast solids, liquids, and gases.Ch. 9 - Prob. 4RQCh. 9 - What is a lattice? What is a unit cell? Describe a...Ch. 9 - What is closest packing? What is the difference...Ch. 9 - Describe, in general, the structures of ionic...Ch. 9 - Prob. 9RQCh. 9 - Prob. 10RQCh. 9 - Compare and contrast the phase diagrams of water...
Ch. 9 - It is possible to balance a paper clip on the...Ch. 9 - Prob. 2ALQCh. 9 - Prob. 3ALQCh. 9 - Prob. 4ALQCh. 9 - Prob. 5ALQCh. 9 - Prob. 6ALQCh. 9 - Prob. 7ALQCh. 9 - Prob. 8ALQCh. 9 - Prob. 9ALQCh. 9 - Prob. 10ALQCh. 9 - Prob. 11ALQCh. 9 - Prob. 12QCh. 9 - In the diagram below, which lines represent the...Ch. 9 - Prob. 14QCh. 9 - Atoms are assumed to touch in closest packed...Ch. 9 - Define critical temperature and critical pressure....Ch. 9 - Prob. 17QCh. 9 - Prob. 18QCh. 9 - Prob. 19QCh. 9 - Prob. 20QCh. 9 - Prob. 21QCh. 9 - A common response to hearing that the temperature...Ch. 9 - Prob. 23QCh. 9 - Prob. 24QCh. 9 - When wet laundry is hung on a clothesline on a...Ch. 9 - Cake mixes and other packaged foods that require...Ch. 9 - You have three covalent compounds with three very...Ch. 9 - Prob. 28QCh. 9 - Compare and contrast the structures of the...Ch. 9 - Prob. 30QCh. 9 - How could you tell experimentally if TiO2 is an...Ch. 9 - A common prank on college campuses is to switch...Ch. 9 - A plot of In (Pvap) versus 1/T (K) is linear with...Ch. 9 - Prob. 34QCh. 9 - Identify the most important types of interparticle...Ch. 9 - Prob. 36ECh. 9 - Predict which substance in each of the following...Ch. 9 - Consider the compounds CI2, HCI. F2, NaF, and HF....Ch. 9 - Prob. 39ECh. 9 - Consider the following electrostatic potential...Ch. 9 - In each of the following groups of substances,...Ch. 9 - Prob. 42ECh. 9 - The shape of the meniscus of water in a glass tube...Ch. 9 - Prob. 44ECh. 9 - Prob. 45ECh. 9 - Prob. 46ECh. 9 - X rays from a copper X-ray tube ( = 154 pm) were...Ch. 9 - The second-order diffraction (n = 2) for a gold...Ch. 9 - A topaz crystal has an interplanar spacing (d) of...Ch. 9 - X rays of wavelength 2.63 were used to analyze a...Ch. 9 - Prob. 51ECh. 9 - Prob. 52ECh. 9 - Prob. 53ECh. 9 - Iridium (Ir) has a face-centered cubic unit cell...Ch. 9 - You are given a small bar of an unknown metal X....Ch. 9 - A metallic solid with atoms in a face-centered...Ch. 9 - Titanium metal has a body-centered cubic unit...Ch. 9 - Barium has a body-centered cubic structure. If the...Ch. 9 - The radius of gold is 144 pm, and the density is...Ch. 9 - The radius of tungsten is 137 pm and the density...Ch. 9 - What fraction of the total volume of a cubic...Ch. 9 - Iron has a density of 7.86 g/cm3 and crystallizes...Ch. 9 - Prob. 63ECh. 9 - Prob. 64ECh. 9 - Selenium is a semiconductor used in photocopying...Ch. 9 - Prob. 66ECh. 9 - Prob. 67ECh. 9 - Prob. 68ECh. 9 - The structures of some common crystalline...Ch. 9 - The unit cell for nickel arsenide is shown below....Ch. 9 - Cobalt fluoride crystallizes in a closest packed...Ch. 9 - The compounds Na2O, CdS, and ZrI4. all can be...Ch. 9 - What is the formula for the compound that...Ch. 9 - Prob. 74ECh. 9 - A certain metal fluoride crystallizes in such a...Ch. 9 - The structure of manganese fluoride can be...Ch. 9 - The unit cell of MgO is shown below l Does MgO...Ch. 9 - In solid KCl the smallest distance between the...Ch. 9 - The CsCl structure is a simple cubic array of...Ch. 9 - MnO has either the NaCI type structure or the CsCI...Ch. 9 - Prob. 81ECh. 9 - What type of solid will each of the following...Ch. 9 - The memory metal, nitinol, is an alloy of nickel...Ch. 9 - Superalloys have been made of nickel and aluminum....Ch. 9 - Perovskite is a mineral containing calcium,...Ch. 9 - A mineral crystallizes in a cubic closest packed...Ch. 9 - Materials containing the elements Y, Ba, Cu, and O...Ch. 9 - The structures of another class of ceramic,...Ch. 9 - Plot the following data and determine Hvap for...Ch. 9 - From the following data for liquid nitric acid,...Ch. 9 - Prob. 91ECh. 9 - Prob. 92ECh. 9 - Prob. 93ECh. 9 - Diethyl ether (CH3CH2OCH2CH3) was one of the first...Ch. 9 - A substance, X, has the following properties:...Ch. 9 - Use the heating-cooling curve below to answer the...Ch. 9 - The molar heat of fusion of sodium metal is 2.60...Ch. 9 - Prob. 98ECh. 9 - What quantity of energy does it take to convert...Ch. 9 - Consider a 75.0-g sample of H2O(g) at 125C. What...Ch. 9 - An ice cube tray contains enough water at 22.0C to...Ch. 9 - A 0.250-g chunk of sodium metal is cautiously...Ch. 9 - Prob. 103ECh. 9 - Prob. 104ECh. 9 - Prob. 105ECh. 9 - Prob. 106ECh. 9 - Prob. 107ECh. 9 - Consider the following data for xenon: Triple...Ch. 9 - Some of the physical properties of H2O and D2O are...Ch. 9 - Rationalize the following boiling points:Ch. 9 - Prob. 111AECh. 9 - Consider the following enthalpy changes:...Ch. 9 - Prob. 113AECh. 9 - Boron nitride (BN) exists in two forms. The first...Ch. 9 - Prob. 115AECh. 9 - Argon has a cubic closest packed structure as a...Ch. 9 - Prob. 117AECh. 9 - A 20.0-g sample of ice at 10.0C is mixed with...Ch. 9 - In regions with dry climates, evaporative coolers...Ch. 9 - The critical point of NH3 is 132C and 111 atm, and...Ch. 9 - Which of the following compound(s) exhibit only...Ch. 9 - Which of the following statements about...Ch. 9 - Prob. 123CWPCh. 9 - Aluminum has an atomic radius of 143 pm and forms...Ch. 9 - Pyrolusite is a mineral containing manganese ions...Ch. 9 - The structure of the compound K2O is best...Ch. 9 - Prob. 127CWPCh. 9 - Some ice cubes at 0c with a total mass of 403 g...Ch. 9 - The enthalpy of vaporization for acetone is 32.0...Ch. 9 - Prob. 130CWPCh. 9 - When I mole of benzene is vaporized at a constant...Ch. 9 - Prob. 132CPCh. 9 - Using the heats of fusion and vaporization for...Ch. 9 - Prob. 134CPCh. 9 - Consider two different organic compounds, each...Ch. 9 - Prob. 136CPCh. 9 - Prob. 137CPCh. 9 - Prob. 138CPCh. 9 - Prob. 139CPCh. 9 - Prob. 140CPCh. 9 - Mn crystallizes in the same type of cubic unit...Ch. 9 - Prob. 142CPCh. 9 - Some water is placed in a sealed glass container...Ch. 9 - The molar enthalpy of vaporization of water at 373...Ch. 9 - Prob. 145CPCh. 9 - Rubidium chloride has the sodium chloride...Ch. 9 - Prob. 147IPCh. 9 - A metal burns in air at 600c under high pressure...Ch. 9 - Prob. 149IPCh. 9 - General Zod has sold Lex Luthor what Zod claims to...
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- The 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_forwardAn 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_forwardCalculate the percent of volume that is actually occupied by spheres in a body-centered cubic lattice of identical spheres You can do this by first relating the radius of a sphere, r, to the length of an edge of a unit cell, l. (Note that the spheres do not touch along an edge but do touch along a diagonal passing through the body-centered sphere.) Then calculate the volume of a unit cell in terms of r. The volume occupied by spheres equals the number of spheres per unit cell times the volume of a sphere (4r3/3).arrow_forward
- Describe the unit cell of lithium (see Figure).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_forwardCalculate the percent of volume that is actually occupied by spheres in a face-centered cubic lattice of identical spheres. You can do this by first relating the radius of a sphere, r, to the length of an edge of a unit cell, l. (Note that the spheres do not touch along an edge but do touch along the diagonal of a face.) Then calculate the volume of a unit cell in terms of r. The volume occupied by spheres equals the number of spheres per unit cell times the volume of a sphere (4r3/3).arrow_forward
- 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_forwardConsider the three types of cubic units cells. (a) Assuming that the spherical atoms or ions in a primitive cubic unit cell just touch along the cubes edges, calculate the percentage of occupied space within the unit cell. (Recall that the volume of a sphere is (4/3)r3, where r is the radius of the sphere.) (b) Compare the percentage of occupied space in the primitive cell (pc) with the bcc and fcc unit cells. Based on this, will a metal in these three forms have the same or different densities? If different, in which is it most dense? In which is it least dense?arrow_forwardThe structure of manganese fluoride can be described as a simple cubic array of manganese ions with fluoride ions at the center of each edge of the cubic unit cell. What is the charge of the manganese ions in this compound?arrow_forward
- Assume X has a body-centered cubic lattice with all atoms at the lattice points. The edge length of the unit cell is 379.0 pm. The atomic mass of X is 195.0 amu. Calculate the density of X.arrow_forwardCrystalline polonium has a primitive cubic unit cell, lithium has a body-centered cubic unit cell, and calcium has a face-centered cubic unit cell. How many Po atoms belong to one unit cell? How many Li atoms belong to one unit cell? How many Ca atoms belong to one unit cell? Draw each unit cell. Indicate on your drawing what fraction of each atom lies within the unit cell.arrow_forwardIdentify 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_forward
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