Question

multiple choice 2 points
what two atomic orbitals or hybrid atomic orbitals overlap to form the c - h bond in ethylene?
cp + hs
csp³ + hs
csp² + hs
csp + hs
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Explanation:

Step1: Determine the hybridization of carbon in ethylene

Ethylene (\(C_{2}H_{4}\)) has a double bond between the two carbon atoms. Each carbon atom in ethylene is \(sp^{2}\) hybridized. The \(sp^{2}\) hybridization occurs when one \(s\) orbital and two \(p\) orbitals of the carbon atom mix to form three \(sp^{2}\) hybrid orbitals.

Step2: Analyze the bonding with hydrogen

Hydrogen has only one \(s\) orbital. The \(C - H\) bonds in ethylene are formed by the overlap of the \(sp^{2}\) hybrid orbital of carbon and the \(s\) orbital of hydrogen.

Answer:

C. \(Csp^{2}+Hs\)