Underlined carbon is sp ^3 hybridized in (a) CH3 CH=CH2 (b) CH3 CH2 NH2 (c) CH3 CONH2 (d) CH3 CH

step 1 Hi, in this problem, we are given four structures as A, B, C, and D, in which one carbon atom is

Underlined carbon is sp ^3 hybridized in (a) CH3 CH=CH2 (b)...

Underlined carbon is sp $^{3}$ hybridized in
(a) $\mathrm{CH}_{3} \mathrm{CH}=\underline{\mathrm{CH}}_{2}$
(b) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{2}$
(c) $\mathrm{CH}_{3} \mathrm{CONH}_{2}$
(d) $\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CN}$

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Key Concepts

Carbon Hybridization

Hybridization refers to the mixing of atomic orbitals to form new orbitals that are better oriented for bonding in molecules. In carbon, the most common hybridizations are sp3, sp2, and sp, which lead to tetrahedral, trigonal planar, and linear geometries, respectively. Understanding hybridization is essential for predicting the shape, bond angles, and reactivity of organic molecules.

sp3 Hybridization

sp3 hybridization occurs when one s orbital mixes with three p orbitals, resulting in four equivalent hybrid orbitals arranged in a tetrahedral geometry with bond angles of approximately 109.5°. This type of hybridization is typical for carbon atoms that form single bonds only, which is crucial in differentiating saturated carbons from those involved in multiple bonding.

Analyzing Bonding Environments

Determining the hybridization state of a carbon atom requires examining its bonding environment, including the number and types of bonds (single, double, or triple) and the presence of any lone pairs. Accurate analysis helps in understanding molecular structure, reactivity, and the physical properties of organic compounds.

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