Chemistry & Chemical Reactivity
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ISBN: 9781133949640
Author: John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher: Cengage Learning
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Chapter 12.2, Problem 2CYU
Potassium chloride has the same unit cell as NaCl. Using the ion sizes in Figure 7.11, calculate the density of KCl.
FIGURE 7.11 Relative sizes of some common ions. Rodii are given in picometers (1 pm 1 × 10‒12 m). (Data taken from J. Emsley, The Elements, Clarendon Press, Oxford, 1998, 3rd edition.)
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- 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.arrow_forwardConsider the CsCl unit shown in Figure 9.21. How many Cs+ ions are there per unit cell? How many Cl- ions? (Note that each Cl- ion is shared by eight cubes.)arrow_forwardThe edge length of the unit cell of tantalum metal, Ta, is 330.6 pm; the unit cell is body-centered cubic (one atom at each lattice point). Tantalum has a density of 16.69 g/cm3. What is the mass of a tantalum atom? Use Avogadros number to calculate the atomic mass of tantalum.arrow_forward
- In the LiCl structure shown in Figure 9.21, the chloride ions form a face-centered cubic unit cell 0.513 nm on an edge. The ionic radius of Cl- is 0.181 nm. (a) Along a cell edge, how much space is between the Cl- ions? (b) Would an Na+ ion (r=0.095nm) fit into this space? a K+ ion (r=0.133nm)?arrow_forwardNickel has a face-centered unit cell with all atoms at lattice points and an edge length of 352.4 pm. The density of metallic nickel is 8.91 g/cm3. What is the mass of a nickel atom? From the atomic mass, calculate Avogadros number.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
- CaTiO3, a perovskite, has the structure below. (a) If the density of the solid is 4.10 g/cm3, what is the length of a side of the unit cell? (b) Calculate the radius of the Ti4+ ion in the center of the unit cell. How well does your calculation agree with a literature value of 75 pm? Unit cell of the perovskite CaTiO3 A sample of perovskite, iO3 FIGURE 7.11 Relative sizes of some common ions. Rodii are given in picometers (1 pm 1 1012 m). (Data taken from J. Emsley, The Elements, Clarendon Press, Oxford, 1998, 3rd edition.)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_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
- A unit cell of cesium chloride is illustrated in Figure 12.8. The density of the solid is 3.99 g/cm3, and the radius of the Cl ion is 181 pm. Calculate the radius of the Cs+ ion in the center of the cell. (Assume that the Cs+ ion touches all of the comer Cl ions.)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_forward
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