CHEM 111 Lecture Notes - Lecture 31: Atomic Orbital
21 Dec 2015
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Chem111 lecture 31 theories of chemical bonding. Allene: the hybridization on the central carbon is sp and that on the outer carbons in sp2. The hch planes at each end are at right angles to each other; so a molecule of allene is not flat. The lewis structure has alternate single and double bonds, but all bonds are equivalent. Don"t need the idea of hybrid structures; bond order is more obvious. Pi bond formation involving d electrons: arsenate, aso4. The three negative charges add another three electrons to the valence electron count. The sigma bonds are formed by the overlap of unhybridized p orbitals on o with sp3 hybrid orbitals on arsenic. Arsenic contributes four electrons to the hybrid orbitals and puts one into an empty 4d orbital, which overlaps with an unhybridized p orbital on each o. The pictures represent effects of rotation about single (sigma) bonds.
