A simple cubic cell contains one metal atom with a metallic radius of 100 pm. a. Determine the volume of the atom(s) contained in one unit cell [the volume of a sphere = (4343)πr3]. b. What is the length of one edge of the unit cell? (Hint: there is no empty space between atoms.) c. Calculate the volume of the unit cell.
A simple cubic cell contains one metal atom with a metallic radius of 100 pm. a. Determine the volume of the atom(s) contained in one unit cell [the volume of a sphere = (4343)πr3]. b. What is the length of one edge of the unit cell? (Hint: there is no empty space between atoms.) c. Calculate the volume of the unit cell.
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 60QAP: Aluminum metal crystallizes with a face-centered cubic unit cell. The volume of the cell is 0.0662...
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A simple cubic cell contains one metal atom with a metallic radius of 100 pm.
a. Determine the volume of the atom(s) contained in one unit cell [the volume of a sphere = (4343)πr3].
b. What is the length of one edge of the unit cell? (Hint: there is no empty space between atoms.)
c. Calculate the volume of the unit cell.
d. Determine the packing efficiency for this structure.
e. Use the steps on this Problem to calculate the packing efficiency for a bcc unit cell with a metallic radius of 1.00 Å.
1.00 Å= 10−10 metre, or 0.1 nanometre
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