VSEPR Summary - VSEPR Rules and lone pairs Trigonal...

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Page 1 of 5 VSEPR Rules 1. Draw the Lewis structure for the molecule or ion. 2. Count the total number of regions of electron density (bonding and lone electron pairs) around the central atom. Double and triple bonds count as ONE REGION OF HIGH ELECTRON DENSITY . An unpaired electron counts as ONE REGION OF HIGH ELECTRON DENSITY . For molecules or ions that have resonance structures, you may use any one of the resonance structures. 3. Identify the most stable arrangement of the regions of electron density as ONE of the following: linear trigonal planar tetrahedral trigonal bipyramid octahedral 4. Determine the positions of the atoms based on the types of electron pairs present (i.e., bonding pairs vs. lone pairs). The most stable configuration results when the electron pairs move into positions that minimize repulsion in order of: lp-lp > lp-bp > bp-bp For trigonal bipyramid and octahedral arrangements, there can sometimes be more than one possible arrangement of the bonding and lone pairs: Trigonal bipyramid - place any lone pairs in the plane of the triangle (Equatorial positions). Octahedral - if you have two lone pairs, place them on
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VSEPR Summary - VSEPR Rules and lone pairs Trigonal...

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