a) Gold (Au) has an atomic radius 0.137 nm and a density of 19.32 g/cm. (Atomic weight of 196.97 g/mol) (i) (ii) Determine whether it has an FCC or BCC crystal structure. Compute the packing fraction / atomic packing factor (APF), assuming the atoms to be hard spheres.

a) Gold (Au) has an atomic radius 0.137 nm and a density of 19.32 g/cm. (Atomic weight of 196.97 g/mol) (i) (ii) Determine whether it has an FCC or BCC crystal structure. Compute the packing fraction / atomic packing factor (APF), assuming the atoms to be hard spheres.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

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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Concept explainers

Crystal Lattices and Unit Cell

Consider a crystal. The regular and repeating pattern of constituent particles is the most distinguishing feature of crystalline solids. A crystal lattice is formed when these particles are replaced with representative points. The three-dimensional arrangement of constituent particles is known as a crystal lattice. Unit cell is that the smallest portion of a space lattice which when repeated in several directions, generate the whole lattice. Unit cell is a building block of a lattice. It is the smallest unit of cell.

Question

a) Gold (Au) has an atomic radius 0.137 nm and a density of 19.32 g/cm'.
(Atomic weight of 196.97 g/mol)
Determine whether it has an FCC or BCC crystal structure.
Compute the packing fraction/ atomic packing factor (APF), assuming
the atoms to be hard spheres.
(i)
(ii)
b) Fig. Q4 (b) shows the unit cell of Nickel (II) oxide (NiO) with ionic radii of ry
0.069 nm and ro = 0.140 nm. Calculate the density of NiO. (Avogadro's
Constant = 6.022 x 1025 mol)
%3D
%3D
nickel (II) oxide
Ni

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