Chem102A VSEPR_Hybrid

Chem102A - 4 1 5 trigonal bipyramid see-saw(SF 4 sp 3 d AB 3 E 2 3 2 5 trigonal bipyramid T-shape(ClF 3 sp 3 d AB 2 E 3 2 3 5 trigonal bipyramid

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C102A VSEPR and Hybrid Orbital Summary Molecule a or ion Bonded atoms Lone pairs Steric number Electron pair geometry Molecular geometry (example) Hybrid Orbitals A. Molecules without lone pairs of electrons on central atom: AB 2 2 0 2 linear linear (C 2 H 2 ) sp AB 3 3 0 3 trigonal planar trigonal planar (BF 3 ) sp 2 AB 4 4 0 4 tetrahedral tetrahedral (CH 4 ) sp 3 AB 5 5 0 5 trigonal bipyramid trigonal bipyramid (PF 5 ) sp 3 d AB 6 6 0 6 octahedral octahedral (SF 6 ) sp 3 d 2 B. Molecules with lone pairs of electrons on central atom: AB 2 E 2 1 3 trigonal planar bent (SO 2 ,O 3 ) sp 2 AB 3 E 3 1 4 tetrahedral trigonal pyramid (NH 3 ) sp 3 AB 2 E 2 2 2 4 tetrahedral bent (H 2 O) sp 3 AB4E
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Unformatted text preview: 4 1 5 trigonal bipyramid see-saw (SF 4 ) sp 3 d AB 3 E 2 3 2 5 trigonal bipyramid T-shape (ClF 3 ) sp 3 d AB 2 E 3 2 3 5 trigonal bipyramid linear (XeF 2 ) sp 3 d AB 5 E 5 1 6 octahedral square pyramid (IF 5 ) sp 3 d 2 AB 4 E 2 4 2 6 octahedral square planar (XeF 4 ) sp 3 d 2 a A = central atom; B = atom bonded to central atom; E = lone pair of electrons on central atom b Steric number = number of bonded atoms + number of lone pairs of electrons on central atom Basic VSEPR Shapes (from left to right: linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral)...
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This note was uploaded on 03/17/2010 for the course CHEM chem102 taught by Professor Adamlist during the Spring '10 term at Vanderbilt.

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