CHEM 130 Lecture Notes - Lecture 29: Valence Bond Theory, Trigonal Planar Molecular Geometry, Vsepr Theory

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26 May 2016

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Chem 130: general chemistry: macroscopic investigations and reaction principles - An approximate theory to explain the electron pair or covalent bond by quantum mechanics. According to the theory, a bond forms between two atoms when two conditions are met. An orbital on one atom comes to occupy a portion of the same region of space as an orbital on the other atom. Strength of the bond depends on the amount of overlap. The total number of electrons in both orbitals is no more than two. They cannot contain more than two electrons because a given region of space can hold only two electrons with opposite spin. Orbitals used to describe the bonding that are obtained by taking combinations of atomic orbitals of the isolated atom. Steps to obtain the bonding description about any atom in a molecule. Write the lewis electron-dot formula of the molecule.

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Use valence bond theory to describe the bonding and geometry in theSeF4 molecule.

A. The central atom is Se, which has five electron groups around it(four bonding pairs and one nonbonding/lone pair). Theelectron-group geometry is trigonal bipyramidal (and the moleculargeometry is see-saw). To facilitate this geometry, the Se atom'sorbitals are hybridized as sp3d orbitals. Four of these hybridorbitals contain one of Se's 6 valence electrons each, and thesehybrid orbitals overlap with unhybridized p orbitals of the four Fatoms. The fifth hybrid orbital of Se contains a lone pair ofelectrons. There are 4 sigma bonds and 0 pi bonds in thismolecule.
B. The central atom is Se, which has six electron groups around it.The electron-group geometry is octahedral. To facilitate thisgeometry, the Se atom's orbitals are hybridized as sp3d2 orbitals.Four of these hybrid orbitals contain one of Se's 6 valenceelectrons each, and these hybrid orbitals overlap with unhybridizedp orbitals of the four F atoms. The fifth and sixth hybrid orbitalsof Se contain lone pairs of electrons. There are 4 sigma bonds and0 pi bonds in this molecule.
C. The central atom is Se, which has four electron groups aroundit. The electron-group geometry is tetrahedral. To facilitate thisgeometry, the Se atom's orbitals are hybridized as sp3 orbitals.These hybrid orbitals overlap with unhybridized p orbitals of thefour F atoms. There are 4 sigma bonds and 0 pi bonds in thismolecule.
D. The central atom is Se, which has four electron groups aroundit, two single bonds and two double bonds. The electron-groupgeometry is tetrahedral. To facilitate this geometry, the Se atom'sorbitals are hybridized as sp3 orbitals. These hybrid orbitalscontain one electron each of Se's 6 valence electrons, and thesehybrid orbitals overlap with unhybridized p orbitals of the four Fatoms. The final 2 electrons of Se's 6 valence electrons reside inunhybridized p orbitals, which overlap with unhybridized p orbitalsof the F atoms. There are 4 sigma bonds and 2 pi bonds in thismolecule.

CHEM 130 Lecture Notes - Lecture 29: Valence Bond Theory, Trigonal Planar Molecular Geometry, Vsepr Theory

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