Find the hybridisation of the C_1,C_2,and C_3 | vedclass

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(A) To determine the hybridisation of carbon atoms,we count the number of sigma $(\sigma)$ bonds and lone pairs (if any) attached to the carbon atom.$

Vedclass · Accepted Answer

$C_1$$sp$$C_2$$sp^2$$C_3$$sp^2$

Vedclass · Answer

(A) To determine the hybridisation of carbon atoms,we count the number of sigma $(\sigma)$ bonds and lone pairs (if any) attached to the carbon atom.$1$. $C_1$ is involved in a triple bond with the terminal carbon and a single bond with $C_2$. It has $2$ sigma bonds and $2$ pi bonds. Thus,it is $sp$ hybridised.$2$. $C_2$ is bonded to $C_1$,$H$,and $C_3$. It has $3$ sigma bonds and $1$ pi bond. Thus,it is $sp^2$ hybridised.$3$. $C_3$ is bonded to $C_2$,$H$,and $CH_2$. It has $3$ sigma bonds and $1$ pi bond. Thus,it is $sp^2$ hybridised.Therefore,the hybridisations are $C_1: sp$,$C_2: sp^2$,$C_3: sp^2$.

Find the hybridisation of the $C_1$,$C_2$,and $C_3$ labelled carbon atoms in the given molecule: $H-C \equiv C_1-C_2H-C_3H=CH_2$

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