Study Guide for Chemistry: The Central Science
14th Edition
ISBN: 9780134554075
Author: Theodore E. Brown, H. Eugene LeMay, Bruce E. Bursten, Catherine Murphy, Patrick Woodward, Matthew E. Stoltzfus, James C. Hill
Publisher: PEARSON
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Chapter 12, Problem 21E
Two patterns of packing for two different circles of the same size are shown here. For each structure
- Draw the two-dimensional unit cell;
- Determine the angle between the lattice vectors , and determine whether the lattice vectors are of the same length or of different lengths; and
- Determine the type of two-dimensional lattice (from Figure 12.4).
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Chapter 12 Solutions
Study Guide for Chemistry: The Central Science
Ch. 12.3 - Consider the two-dimensional square lattice of...Ch. 12.3 - Prob. 12.1.2PECh. 12.5 - Given the ionic radii and molar masses of Sc3+...Ch. 12.5 - Prob. 12.2.2PECh. 12.7 - Prob. 12.3.1PECh. 12.7 - Prob. 12.3.2PECh. 12.7 - Prob. 12.4.1PECh. 12.7 - Prob. 12.4.2PECh. 12 - Prob. 1DECh. 12 - Prob. 1E
Ch. 12 - Prob. 2ECh. 12 - Prob. 3ECh. 12 - Prob. 4ECh. 12 - Prob. 5ECh. 12 - Prob. 6ECh. 12 - Prob. 7ECh. 12 - Prob. 8ECh. 12 - Prob. 9ECh. 12 - Prob. 10ECh. 12 - 12.11 Covalent bonding occurs in both molecular...Ch. 12 - Prob. 12ECh. 12 - 12.13 What kinds of attractive forces exist...Ch. 12 - Prob. 14ECh. 12 - Prob. 15ECh. 12 - Prob. 16ECh. 12 - Prob. 17ECh. 12 - Prob. 18ECh. 12 - Prob. 19ECh. 12 - Amorphous silica, SiO2, has a density of about...Ch. 12 - Two patterns of packing for two different circles...Ch. 12 - Prob. 22ECh. 12 - Prob. 23ECh. 12 - Prob. 24ECh. 12 - Which of the three-dimensional primitive lattices...Ch. 12 - Prob. 26ECh. 12 - 12.27 What is the minimum number of atoms that...Ch. 12 - 12.28 What is the minimum number of atoms that...Ch. 12 - Prob. 29ECh. 12 - Prob. 30ECh. 12 - Prob. 31ECh. 12 - Prob. 32ECh. 12 - Prob. 33ECh. 12 - Prob. 34ECh. 12 - Prob. 35ECh. 12 - Prob. 36ECh. 12 - Prob. 37ECh. 12 - Prob. 38ECh. 12 - Prob. 39ECh. 12 - Prob. 40ECh. 12 - Prob. 41ECh. 12 - Prob. 42ECh. 12 - Prob. 43ECh. 12 - Prob. 44ECh. 12 - Prob. 45ECh. 12 - Prob. 46ECh. 12 - Prob. 47ECh. 12 - Prob. 48ECh. 12 - Prob. 49ECh. 12 - Prob. 50ECh. 12 - Prob. 51ECh. 12 - Prob. 52ECh. 12 - 12.53 Which would you expect to be the more...Ch. 12 - 12.54 Which of the following statements does not...Ch. 12 - Prob. 55ECh. 12 - Prob. 56ECh. 12 - Prob. 57ECh. 12 - Prob. 58ECh. 12 - Prob. 59ECh. 12 - Prob. 60ECh. 12 - 12.61 A particular form of cinnabar (HgS) adopts...Ch. 12 - At room temperature and pressure RbI crystallizes...Ch. 12 - Prob. 63ECh. 12 - Prob. 64ECh. 12 - The coordination number for Mg2+ ion is usually...Ch. 12 - Prob. 66ECh. 12 - Prob. 67ECh. 12 - Prob. 68ECh. 12 - Prob. 69ECh. 12 - Prob. 70ECh. 12 - Prob. 71ECh. 12 - Prob. 72ECh. 12 - Prob. 73ECh. 12 - Prob. 74ECh. 12 - Prob. 75ECh. 12 - Prob. 76ECh. 12 - Prob. 77ECh. 12 - Prob. 78ECh. 12 - Prob. 79ECh. 12 - Prob. 80ECh. 12 - Prob. 81ECh. 12 - Prob. 82ECh. 12 - Prob. 83ECh. 12 - Prob. 84ECh. 12 - Prob. 85ECh. 12 - 12.86 Write a balanced chemical equation for the...Ch. 12 - Prob. 87ECh. 12 - Prob. 88ECh. 12 - Prob. 89ECh. 12 - Prob. 90ECh. 12 - Prob. 91ECh. 12 - Prob. 92ECh. 12 - Prob. 93ECh. 12 - Prob. 94ECh. 12 - Explain why “bands” may not be the most accurate...Ch. 12 - Prob. 96ECh. 12 - Prob. 97ECh. 12 - Prob. 98ECh. 12 - Prob. 99ECh. 12 - An ideal quantum dot for use in TVs does not...Ch. 12 - Prob. 101ECh. 12 - Prob. 102ECh. 12 - Prob. 103AECh. 12 - Prob. 104AECh. 12 - Prob. 105AECh. 12 - Pure iron crystallizes in a body-centered cubic...Ch. 12 - Prob. 107AECh. 12 - Prob. 108AECh. 12 - Prob. 109AECh. 12 - What type of latticeprimitive cubic, body-centered...Ch. 12 - Prob. 111AECh. 12 - Prob. 112AECh. 12 - Prob. 113AECh. 12 - Energy bands are considered continuous due to the...Ch. 12 - Prob. 115AECh. 12 - Prob. 116AECh. 12 - Prob. 117AECh. 12 - Prob. 118AECh. 12 - Prob. 119AECh. 12 - Prob. 120AECh. 12 - Prob. 121AECh. 12 - Prob. 122AECh. 12 - Prob. 123AECh. 12 - The karat scale used to describe gold alloys is...Ch. 12 - 12.125 Spinel is a mineral that contains 37.9% AI,...Ch. 12 - Prob. 126IECh. 12 - Prob. 127IECh. 12 - Prob. 128IECh. 12 - Prob. 129IECh. 12 - Silicon has the diamond structure with a unit cell...Ch. 12 - Prob. 131IECh. 12 - Prob. 132IE
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- Outline a two-dimensional unit cell for the pattern shown here. If the black squares are labeled A and the white squares are B, what is the simplest formula for a compound based on this pattern?arrow_forwardDescribe the unit cell of lithium (see Figure).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_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_forwardLithium hydride (LiH) has the sodium chloride structure, and the length of the edge of the unit cell is 4.086 108 cm. Calculate the density of this solid.arrow_forwardThe unit cell for nickel arsenide is shown below. What is the formula of this compound?arrow_forward
- 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_forwardMnO 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_forwardThe free space in a metal may be found by subtracting the volume of the atoms in a unit cell from the volume of the cell. Calculate the percentage of free space in each of the three cubic lattices if all atoms in each are of equal size and touch their nearest neighbors. Which of these structures represents the most efficient packing? That is, which packs with the least amount of unused space?arrow_forward
- Calculate 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_forwardIn an FCC structure, the atoms are found on the corners of the cubic unit cell and at the center of each face. The unit cell has an edge whose length is the distance from the center of one corner atom to the center of another corner atom on the same edge. The atoms on the diagonal of any face are touching. One of the faces of the unit cell is shown below in the following: a. Show the distance dO on the sketch. Draw the boundaries of the unit cell. b. What is the relationship between the length of the face diagonal and the radius of the atoms in the cell? Face diagonal = ______________ c. How is the radius of the atoms related to dO? r= ______________ d. Silver metal crystals have an FCC structure. The unit cell edge in silver is 0.4086nm long. What is the radius of a silver atom? ______________nmarrow_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_forward
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