Chapter 8 Solid Materials
Molecular solids are composed of molecu
les or atoms that interact only through
intermolecular interactions. These interacti
ons vary considerably from the weakest
dispersion force in He to fairly strong hy
drogen bonds. Consequently, molecular solids
can be solids, liquids, or gases at room conditions.
Atomic radii can be given as the metallic radius, the covalent radius, or the van der
Waals radius. Metallic radii are deduced from
the distance between metal atoms that are
touching in a metallic solid. Covalent rad
ii are defined from bond lengths because the
length of a covalent bond is the sum of the c
ovalent radii of the bound atoms. The van der
Waals radius is one-half of the van der W
aals distance (distance between two adjacent
molecules in the crystal of an element). The spheres used to represent the atoms in space-filling models are based on their van der Waals radii. Thus, a covalent bond can be represented as the contact of two spheres with ra
dii equal to the covalent radii of the atoms
or as the penetration of two spheres with radii equal to the van der Waals radii.
After studying the material presented in this chapter, you should be able to: 1. identify and define unit cells (Section 8.1); 2. draw the sc, bcc and fcc unit cells (Section 8.2); 3. determine the metallic radius of an atom from
the edge length of the unit cell and cell type
(Section 8.2);
- determine the formula of a substance based on the unit ce
ll occupancy (Section 8.3);
- determine the coordination num
ber of an atom or ion in a crystal lattice (Section 8.4);
- explain packing efficiency and why it is impo
rtant and calculate the densit
y of a solid from its
unit cell dimensions (Section 8.5);
- differentiate between a conductor, a semico
nductor, and an insulator on the basis of their
band structures (Section 8.6);
- determine the distances between ions in a crystal given their ionic radii and the crystal type
(Section 8.7);
- differentiate between the sodium chloride and
cesium chloride structures and explain why
one structure would be preferred ov
er the other (Section 8.7);
10.
distinguish between the following forms of carbon: graphite, diamond, buckyball, and nanotubes (Section 8.8 );
11.
describe the diamond and zinc blende struct
ures adopted by several covalent solids
(Section 8.8);
12.
describe the structure and function
of zeolites and clays (Section 8.8);
13.
define the van der Waal
s distance (Section 8.9);
14.
distinguish between covalent and van der Waals radii and determine a bond length from the covalent radii of the atoms (Section 8.9); and
15.
predict relative melting points fr
om the types of solids (Section 8.10).
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