Chapter 9, Problem 57b
(b) What is the hybridization of the carbon atoms in each molecule?
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(c) Which is generally stronger, a s bond or a p bond? Explain.
(d) Can two s orbitals combine to form a p bond? Explain.
(b) Imagine that you could hold two atoms that are bonded together, twist them, and not change the bond length. Would it be easier to twist (rotate) around a single s bond or around a double 1s plus p2 bond, or would they be the same?
Propylene, C3H6, is a gas that is used to form the important polymer called polypropylene. Its Lewis structure is (a) What is the total number of valence electrons in the propylene molecule?
Benzaldehyde, C7H6O, is a fragrant substance responsible for the aroma of almonds. Its Lewis structure is
(a) What is the hybridization at each of the carbon atoms of the molecule?
Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is
(c) How many of the valence electrons are used to make s bonds in the molecule?