CEM 141 Exam 3 Study Guide

CEM 141 Exam 3 Study Guide - Exam 3 Study Guide Topics and...

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Topics and Equations Lewis Structures and resonance Multiple Bonds, Strength: triple bond > double bond > single bond Length: triple bond < double bond < single bond Bond order = 1 for a single bond, 2 for a double bond, and 3 for a triple bond Lone pairs: # of valence electrons/8 = number of bonds with a remainder of non-bonding electrons (two non-bonding electrons make up a lone pair) Formal charge: 1) Formal charge = # of valence electrons - # bonds - # non-bonding electrons (from your text) 2) Negative formal charge should be on the more electronegative atom. 3) Formal charge is a way of checking your Lewis Dot structure- you want the lowest formal charges possible and they MUST add up to the charge on your molecule. Polar vs. Non-polar VSEPR: Total Electron Pairs: Lone Pairs: Shape: Hybridization: 2 0 Linear sp 3 0 Trigonal sp 2 1 V-Shape (Bent) 4 0 Tetrahedral sp 3 1 Trigonal Pyramidal 2 V-Shape (Bent) 5 0 Trigonal Bipyramidal sp 3 d 1 Seesaw 2 T-shape 3 Linear 6 0 Octahedral sp 3 d 2 1 Square-Pyramidal 2 Square-Planar Electron Arrangement is the same as the shape with zero lone pairs. Bond Angles for each arrangement.
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This note was uploaded on 03/21/2008 for the course CEM 141 taught by Professor Hunter during the Spring '08 term at Michigan State University.

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CEM 141 Exam 3 Study Guide - Exam 3 Study Guide Topics and...

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