Lab 6 - Molecular Geometry

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Unformatted text preview: s and bond length www.webassig n.net/ebooks/wsug encheml1/lab_6/manual.html 3/8 4/15/13 Lab 6 - M olecular Geometr y decreases as the bond order increases. (The bond length is the distance between the centers of the two atoms bonded together). Thus, a s ingle bond is longe r than a triple bond, but the triple bond is s tronge r. Note: This general statement applies when comparing the bond order of similarly bonded atoms. However, as noted, the Lewis structure is a two- dimensional representation of the molecule or ion. The two- dimensional diagram does not show us the geometry or shape of the molecule. Over the years, many theories have attempted to explain the shape of covalently bonded substances; one of the simplest is the Vale nce She ll Ele ctron Pair Re puls ion (VSEPR) theory. In most molecules, electrons occur in pairs, either as part of a bond (bonding pair) or as a lone pair; these pairs occupy space around an atom. The theory proposes that these areas or electron regions repel one another. VSEPR theory's main postulate is that the regions around a given atom will arrange themselves to minimize this repulsion by positioning themselves as far...
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This document was uploaded on 01/22/2014.

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