KF is an ionic solid with a cubic crystal structure. Use the information below to answer the following question. K: Z = 19, most common valence = 1+, ionic radius = 0.138 nm, A = 39.10 g/mol = 19.00 g/mol 0.133 nm, A %3D F:Z = 9, most common valence = 1-, ionic radius What is the coordination number for K in KF? O A. 6 ОВ. 8 О С.4 O D. 12

KF is an ionic solid with a cubic crystal structure. Use the information below to answer the following question. K: Z = 19, most common valence = 1+, ionic radius = 0.138 nm, A = 39.10 g/mol = 19.00 g/mol 0.133 nm, A %3D F:Z = 9, most common valence = 1-, ionic radius What is the coordination number for K in KF? O A. 6 ОВ. 8 О С.4 O D. 12

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter9: Liquids And Solids

Section: Chapter Questions

Problem 76QAP: Iron crystallizes in a body-centered unit cell. Its atomic radius is 0.124 nm. Its density is 7.86...

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8.48 Why must the vapor pressure of a substance be measured only after dynamic equilibrium is established?
8.87 Use the vapor pressure curves illustrated here to answer the questions that follow. (a) What is the vapor pressure of ethanol (C2H5OH) at 60°C? (b) Considering only carbon disulfide (CS2) and ethanol, which has the stranger intermolecular forces in the liquid state? (c) At what temperature does heptane (C7H16) have a vapor pressure of 500 mm Hg? (d) What are the approximate normal boiling pains of each of the three substances? (e) At a pressure of 400 mm Hg and a temperature of 70°C, is each substance a liquid, a gas, or a mixture of liquid and gas?
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.
A common prank on college campuses is to switch the salt and sugar on dining hall tables, which is usually easy because the substances look so much alike. Yet, despite the similarity in their appearance, these two substances differ greatly in their properties, since one is a molecular solid and the other is an ionic solid. How do the properties differ and why?
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)?
Iron crystallizes in a body-centered unit cell. Its atomic radius is 0.124 nm. Its density is 7.86 g/cm3. Using this information, estimate Avogadro's number.
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Equilibrium vapor pressures of benzene, C6H6, at various temperatures are given in the table. (a) What is the normal boiling point of benzene? (b) Plot these data so that you have a graph resembling the one in Figure 11.12. At what temperature does the liquid have an equilibrium vapor pressure of 250 mm Hg? At what temperature is the vapor pressure 650 mm Hg? (c) Calculate the molar enthalpy of vaporization for benzene using the ClausiusClapeyron equation.
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).