Not all unit cells have a cubic structure. Take for example the below image wherein the unit cell takes the shape of a parallelepipe and has lengths a, b, c and angles a, B, y. This particular unit cell has an atom arrangement where it has one atom at each corner, one central atom at each of the bases, one atom at the center of the unit cell, and one atom at the center of each of the edge lengths across length c. Given a density of 26.57 g/cm³, calculate the length of edge c in angstroms of a theoretical element Ro giv the following unit cell dimensions in angstroms and degrees: a = 10.85A b = 7.56A y = 45° Atomic Mass: Ro: 50.639 g/mol C a + b + c a a = ß = 90° ± y 9. a
Not all unit cells have a cubic structure. Take for example the below image wherein the unit cell takes the shape of a parallelepipe and has lengths a, b, c and angles a, B, y. This particular unit cell has an atom arrangement where it has one atom at each corner, one central atom at each of the bases, one atom at the center of the unit cell, and one atom at the center of each of the edge lengths across length c. Given a density of 26.57 g/cm³, calculate the length of edge c in angstroms of a theoretical element Ro giv the following unit cell dimensions in angstroms and degrees: a = 10.85A b = 7.56A y = 45° Atomic Mass: Ro: 50.639 g/mol C a + b + c a a = ß = 90° ± y 9. a
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:Not all unit cells have a cubic structure. Take for example the below image wherein the unit cell takes the shape of a parallelepiped
and has lengths a, b, c and angles a, B, y. This particular unit cell has an atom arrangement where it has one atom at each corner,
one central atom at each of the bases, one atom at the center of the unit cell, and one atom at the center of each of the edge
lengths across length c. Given a density of 26.57 g/cm3, calculate the length of edge c in angstroms of a theoretical element Ro given
the following unit cell dimensions in angstroms and degrees:
a = 10.85A
b = 7.56A
y = 45°
Atomic Mass:
Ro: 50.639 g/mol
C
a + b + c
a = ß = 90° ±Y
9.
а
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