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by: Nina Kalkus

VSEPR CHEM-1070-30

Nina Kalkus

GPA 3.8
General Chemistry I
Schmehl, Russell

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About this Document

VSEPR practice and hybrid orbitals
General Chemistry I
Schmehl, Russell
Class Notes
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This 4 page Class Notes was uploaded by Nina Kalkus on Saturday November 28, 2015. The Class Notes belongs to CHEM-1070-30 at Tulane University taught by Schmehl, Russell in Fall 2015. Since its upload, it has received 20 views. For similar materials see General Chemistry I in Chemistry at Tulane University.


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Date Created: 11/28/15
VJ H20 8e H 0 H 2 nb pairs 2 bonding pairs VSEPR H H 1095 degrees Bent geometry 0 atom valence shell 2s2p4 H z Why isn39t this 90 degrees PX2Py1Pz1 H y H atom ls1 X Linus Pauling The Nature of the Chemical Bond The geometries can be obtained using hybrid atomic orbitals Psp al Ps az l px sp hybrids Make sp hybrid of C 1 2s 1 pr z st S PX X 5 Consider HCCH acetylene C 4 valence shell e gt C2H2 10e H CfC H VSEPR each C linear orbitals that directly overlap and form a bond sigma X H Sp PyPy bonding interaction parallel orbitals interaction to form a bond pi y y C C SP SP Ethylene H2CCH2 12e H H CC H H Shape of each carbon trigonal planar S orbital Py PX gt 3 hybrid orbitals 3 sp2 hybrid orbitals Angle between the orbitals is 120 degrees H 2 H Sp sp2 C sp2 sp2 C sz sp2 H H each C 32sp2 Pz Pz orbitals come out of page Methane CH4 8e H H C H VSEPR tetrahedral angles 1095 degrees H C 2s22p2 gt 4 sp3 hybrids H SP3 1095 degrees H SP3 C sp3 sp3 H H XC15 Cl C1 C1 C1 5 XCl bonds gt must have gt 4 orbitals available for bonding For n3 period atomsgt 3s 3p 3d n3 4 5 or 6 atoms with 5 valence shell egt P As Sb Bi Hybrid sigma bonds pi bonds shape sp 2 2 linear sp2 3 l trigonal plane sp3 4 O tetrahedron dsp3 5 O trigonal bipyramid d2 sp3 6 O octahedron Bond requires an orbital


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