Lecture_10 - SF4: 5 pairs (4 bonding + 1 lone pairs) AB4E...

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1 ± SF 4 : 5 pairs (4 bonding + 1 lone pairs) ± IF 3 : 5 pairs (3 bonding + 2 lone pairs) AB 4 E Irregular tetrahedron or See-saw AB 3 E 2 T-shaped Lone pairs are always placed in an equatorial position. Axial equatorial ± I 3 : 5 pairs (2 bonding + 3 lone pairs) AB 2 E 3 Linear!
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2 ± BrF 5 : (6 pairs: 5 bonding + 1 lone pairs) ± XeF 4 : (6 pairs: 4 bonding + 2 lone pairs) AB 5 E Square pyramidal AB 4 E 2 Square planar Cis Trans ± AB 3 E 3 (6 pairs: 3 bonding + 3 lone pairs) ± AB 2 E 4 (6 pairs: 2 bonding + 4 lone pairs) T-shaped Linear Special cases : ¾ VSEPR with multiple bonds: each multiple bond is treated as one effective pair. ² NO 3 : ( trigonal planar , bond angle 120 ° ) ² SO 2 : ( V-shaped , bond angle < 120 ° )
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3 ¾ Molecules containing more than one central atom: ¾ Failure of the VSEPR model: In PH 3 (though like NH 3 ), the bond angle is 94 ° and not 107 ° . CH 3 OH Zumdahl Chapter 9 Chemical Bonding: Orbitals 1.Hybridization and the LE Model: Consider the methane molecule CH
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This note was uploaded on 09/07/2010 for the course FAS chem 201 taught by Professor Sultan during the Summer '07 term at American University of Beirut.

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Lecture_10 - SF4: 5 pairs (4 bonding + 1 lone pairs) AB4E...

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