1. A metallic solid ingot has a mass of 14.7 grams. It was loaded into a graduated cylinder containing 40.0 mL or water. Upon addition of the ingot, the volume of the water and the ingot was 41.6 mL. What is the density of the ingot? 2. Assuming the solid ingot in question 1 is polonium (Po, element 84) which packs in a primitive cubic unit cell structure calculate the packing efficiency of the unit cell? Atoms touch along edge. a = 2r C

1. A metallic solid ingot has a mass of 14.7 grams. It was loaded into a graduated cylinder containing 40.0 mL or water. Upon addition of the ingot, the volume of the water and the ingot was 41.6 mL. What is the density of the ingot? 2. Assuming the solid ingot in question 1 is polonium (Po, element 84) which packs in a primitive cubic unit cell structure calculate the packing efficiency of the unit cell? Atoms touch along edge. a = 2r C

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter12: The Solid State

Section: Chapter Questions

Problem 29PS: A diamond unit cell is shown here. Unit cell of diamond (a) How many carbon atoms are in one unit...

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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?
Consider 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?
• describe the arrangement of atoms in the common cubic crystal lattices and calculate the packing efficiency for a lattice.
Aluminum metal crystallizes with a face-centered cubic unit cell. The volume of the cell is 0.0662 nm3. (a) What is the atomic radius of aluminum in cm? (b) What is the volume of a single aluminum atom? (c) What is the density of a single aluminum atom? (d) In face-centered cubic cell packing, the fraction of empty space is 26.0%. When this is factored in, what is the calculated density of aluminum?
The memory metal, nitinol, is an alloy of nickel and titanium. It is called a memory metal because after being deformed, a piece of nitinol wire will return to its original shape. The structure of nitinol consists of a simple cubic array of Ni atoms and an inner penetrating simple cubic array of Ti atoms. In the extended lattice, a Ti atom is found at the center of a cube of Ni atoms; the reverse is also true. a. Describe the unit cell for nitinol. b. What is the empirical formula of nitinol? c. What are the coordination numbers (number of nearest neighbors) of Ni and Ti in nitinol?
A diamond unit cell is shown here. Unit cell of diamond (a) How many carbon atoms are in one unit cell? (b) The unit cell can be considered as a cubic unit cell of C atoms with other C atoms in holes in the lattice. What type of unit cell is this (pc, bcc, fcc)? In what holes are other C atoms located, octahedral or tetrahedral holes?
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 1012 m). (Data taken from J. Emsley, The Elements, Clarendon Press, Oxford, 1998, 3rd edition.)