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# In vinyl acetylene, $CH\equiv C-CH=C{{H}_{2}}$, the type of overlapping in $({{C}_{2}}\sigma {{C}_{3}})$ bond is:A. $s{{p}^{2}}-sp$B. $sp-s{{p}^{2}}$C. $s{{p}^{3}}-s{{p}^{3}}$D. $s{{p}^{3}}-s{{p}^{2}}$ Verified
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Hint: Take into consideration the number of bonds each carbon is forming and whether they are $\sigma$-bonds or$\pi$-bonds. This will help you determine the hybridization of each carbon atom.

First, let us identify and name the carbon atoms that are asked in the question:
${{C}^{1}}H\equiv {{C}^{2}}-{{C}^{3}}H={{C}^{4}}{{H}_{2}}$
We have to find the hybridization of the two carbons present in the middle.
Consider carbon number 2.
We can see that it is forming 1 $\sigma$-bond and 2 $\pi$-bonds with carbon number 1, and 1 $\sigma$-bond with carbon number 3. It does not form any bonds with a hydrogen atom.
Thus, it has 2 $\sigma$-bonds whose bond pairs we need to consider while calculating the hybridization of the atom. $\pi$-bonds are not considered while calculating the hybridization. As there are only 2 bond pairs involved, 2 hybridized orbitals are required to accommodate them. Thus, the hybridization of this carbon is $sp$.
Consider carbon number 3.
We can see that it is forming 1 $\sigma$-bond with carbon number 2, and 1 $\sigma$-bond and 1 $\pi$-bond with carbon number 4. It also forms 1 $\sigma$-bond with a hydrogen atom.
Now, to calculate the hybridization of this carbon, consider the number of $\sigma$-bonds present. We see that 3 $\sigma$-bonds are present and 3 hybridized orbitals are required to accommodate the 3 bond pairs. Thus, the hybridization of this carbon is $s{{p}^{2}}$.

So, the correct answer is “Option B”.

Note: Please be careful while calculating the number of $\sigma$-bonds that each of the carbon atoms forms with not only other carbon atoms but also the hydrogen atoms since they are not explicitly shown and you might miss them.
Last updated date: 23rd Sep 2023
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