11 Lecture 7, January 30, 2008 Section Two: Solid State Chemistry I. Why Solids? A. Features 1. Unique to inorganic chemistry. Extended solids consist of many atoms or ions interacting with each other in a similar manner. In contrast, a molecular solid consists of atoms strongly held together with covalent bonding, but interacting with each other much more weakly through intermolecular forces. 2. Most of the periodic table consists of metals, which exist as solids in their natural state; they have high melting and boiling points. 3. The explanation of the bonding that results in extended solids is different than the VSEPR/molecular bonding theory used to explain covalent bonding in molecules. 4. Sometimes interesting things happen when many atoms are very close to each other (i.e., conduction, semiconductors, band theory, etc.) II. Metallic Solids A. Metallic bonding 1. Atoms with low ∆ H IE are next to each other in the solid; thus, electrons can easily leave one atom and attach to another. However, these atoms typically also have low
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