Question: (a) Draw Lewis structures for ethane (C2H6), ethylene (C2H4), and acetylene (C2H2). (b) What is the hybridization of the carbon atoms in each molecule? (c)

(a) Draw Lewis structures for ethane (C2H6), ethylene (C2H4), and acetylene (C2H2).
(b) What is the hybridization of the carbon atoms in each molecule?
(c) Predict which molecules, if any, are planar.
(d) How many σ and π bonds are there in each molecule?
(e) Suppose that silicon could form molecules that are precisely the analogs of ethane, ethylene, and acetylene. How would you describe the bonding about Si in terms of hydrid orbitals? Silicon does not readily form some of the analogous compounds containing π bonds. Why might this be the case?

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