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

$CH_3CH_2\underline{C}N$

Vedclass · Answer

(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?

Similar Questions

What hybrid orbitals are present in the following compound $H_3C - CH = CH - CH_2 - CH_3$?

The hybridisation of the negatively charged carbon atoms in $(1)$ and $(2)$ are:
$(1)$ $CH_3^-$
$(2)$ $H_2C^- - CHO - CH_3$

How many $(i)$ $sp^{2}$ hybridised carbon atoms and $(ii)$ $\pi$ bonds are present in the following compound?

Which of the following carbon atoms is the most electronegative?

Which among the following possesses a $sp$ carbon in its structure?

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