CHM120H5 Lecture Notes - Lecture 37: Orbital Hybridisation, Molecular Geometry

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26 Feb 2018
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# in the case of h2c=ch2 we have two such sp2 hybridized carbon atoms. # two of the hybridized orbitals on each c atom are used to form bond with h atoms. # the third orbital on each carbon atom will the over lap each other to form a carbon-carbon bond. # now the unhybridized p orbital on both c atoms are perfectly oriented so that they can overlap laterally to form a (cid:894)pi(cid:895) bond. # so the two c atoms are linked by a a(cid:374)d a bo(cid:374)d. # the bond angles hch, hcc are 1200. What are the differences between a and a bond. # when there is a sp3 hybridized carbon atom in a molecule it is connected to other atoms by single bonds- sp2- double bond and sp - triple bond. # carbon atom at the centre is linked to the other carbon atoms by double bonds.

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