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In which of the following pair both the species have $s p^3$ hybridization?
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Verified Answer
The correct answer is:
$\mathrm{NF}_3, \mathrm{H}_2 \mathrm{O}$
Key concept - Hybridization
\(Z=\frac{1}{2}\left(\text { No. of valence } e^{-} \text {of central atom }+\text { Monovalent atom }+ \text { charge } \right)\)
\(\begin{aligned}
& \text {(1) } \mathrm{H}_2 \mathrm{~S}, B \mathrm{~F}_3 \\
& \mathrm{H}_2 \mathrm{~S}=\frac{1}{2}(8+2)=4 S p^3 \\
& B F_3=\frac{1}{2}(3+3)=3 s p^2
\end{aligned}\)
\(\begin{aligned}
\text {(2) } \operatorname{SiF}_4 & =\frac{1}{2}(4+4)=4 s p^3 \\
B C H_2 & =\frac{1}{2}(2+2)=2 \mathrm{Sp}
\end{aligned}\)
\(\begin{aligned}
\text {(3) } & N f_3=\frac{1}{2}(5+3)=4 s p^3 \\
& H_2 O=\frac{1}{2}(6+2)=4 S p^3
\end{aligned}\)
\(\begin{aligned}
\text {(4) } & N F_3 \\
= & \frac{1}{2}(5+3)=4 s p^3 \\
& B F_3=\frac{1}{2}
\end{aligned}\)
\(Z=\frac{1}{2}\left(\text { No. of valence } e^{-} \text {of central atom }+\text { Monovalent atom }+ \text { charge } \right)\)
\(\begin{aligned}
& \text {(1) } \mathrm{H}_2 \mathrm{~S}, B \mathrm{~F}_3 \\
& \mathrm{H}_2 \mathrm{~S}=\frac{1}{2}(8+2)=4 S p^3 \\
& B F_3=\frac{1}{2}(3+3)=3 s p^2
\end{aligned}\)
\(\begin{aligned}
\text {(2) } \operatorname{SiF}_4 & =\frac{1}{2}(4+4)=4 s p^3 \\
B C H_2 & =\frac{1}{2}(2+2)=2 \mathrm{Sp}
\end{aligned}\)
\(\begin{aligned}
\text {(3) } & N f_3=\frac{1}{2}(5+3)=4 s p^3 \\
& H_2 O=\frac{1}{2}(6+2)=4 S p^3
\end{aligned}\)
\(\begin{aligned}
\text {(4) } & N F_3 \\
= & \frac{1}{2}(5+3)=4 s p^3 \\
& B F_3=\frac{1}{2}
\end{aligned}\)
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