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Unformatted text preview: elements) in terms of the overlap of sp , sp 2 , and sp 3 to form (sigma) bonds, also the overlap with hydrogen 1s orbitals to form sigma bonds, and the sidewise overlap of unhybridized p orbitals to form (pi) bonds. 5. Describe a double bond as one sigma and one pi bond and a triple bond as one sigma and two pi bonds. Explain why a pi bond is weaker than a sigma bond. Label a carbon-carbon double bond as stronger than, but less than twice as strong as, a carbon-carbon single bond. Label a carbon-carbon triple bond as stronger than a carbon-carbon double bond, but less than three times as strong as a carbon-carbon single bond. 6. Label the hybridization of atoms and propose plausible bonding schemes from Lewis structures or from experimental information about molecules (that is, bond lengths, bond angles, geometries, and so on)....
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- Spring '08