Which of the following underlined carbon atom | vedclass

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(D) To determine the hybridization of a carbon atom,we count the number of $\sigma$ bonds and lone pairs attached to it.$1$. $sp^3$ hybridization: Car

Vedclass · Accepted Answer

$CH_3CH_2\underline{C}N$

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(D) To determine the hybridization of a carbon atom,we count the number of $\sigma$ bonds and lone pairs attached to it.$1$. $sp^3$ hybridization: Carbon is bonded to $4$ atoms (all single bonds,$4\sigma$ bonds).$2$. $sp^2$ hybridization: Carbon is bonded to $3$ atoms (one double bond,$3\sigma$ bonds).$3$. $sp$ hybridization: Carbon is bonded to $2$ atoms (one triple bond or two double bonds,$2\sigma$ bonds).In option $D$,the structure is $CH_3-CH_2-C \equiv N$. The underlined carbon atom is bonded to one nitrogen atom via a triple bond and to one carbon atom via a single bond. Thus,it has $2\sigma$ bonds and $0$ lone pairs,resulting in $sp$ hybridization.

Which of the following underlined carbon atoms possesses $sp$ hybridization?

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Determine the hybridization of the carbon atoms in the following compounds:
$(a)$ $N \equiv C-CH=CH_2$
$(b)$ $HC \equiv C-CH=CH_2$ (Identify the carbon atoms of the single bond $C-C$)
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$(d)$ $H_2C=C=C=CH_2$
$(e)$ Buta$-1,3-$diene (as shown in the figure)

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