CHE 131 Lecture Notes - Lecture 27: Valence Bond Theory, Sigma Bond, Atomic Orbital

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CHE 131 Full Course Notes
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CHE 131 Full Course Notes
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Sigma pond = overlap of atomic orbital along the internuclear axis. Highest electron density between the two along the bond axis. Pi bond =sidewise overlapping of atomic orbitals. Electron density is present a love and below the inter nucleus axis. Double bond consists of one sigma bond and one pi bond. Triple bond has one sigma bond and two pi bonds. Bonding in covalent compounds cyrus via the overlap of two half-filled orbitals of the bonding atoms. Requires overlap of four orbitals at the c atom with 1s orbitals. Valence bond theory invokes the concept of hybridization to explain this. Can share two electrons together and see a new hybrid. There are two types of covalent bond based on overlaps. Linear, with sigma bond (works well for simple covalent molecules) A hybrid orbitals results from a mixing of different orbitals to form a new hybridized orbital. Use lewis structure and steric number to determine hybridization.

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