Question

The bond between carbon atom (1) and carbon atom (2) in compound
$N\equiv \underset{\left(1\right)}{C}-\underset{\left(2\right)}{C}H=C{H}_2$, involves the hybrid orbitals:

• A. $sp$ and ${sp}^2$
• B. ${sp}^2$ and ${sp}^2$
• C. $sp$ and ${sp}^3$
• D. $sp$ and $sp$

Answer 1

The correct option is A $sp$ and ${sp}^2$

$N\equiv \underset{\left(1\right)}{C}-\underset{\left(2\right)}{C}H=C{H}_2$, involves $sp$ and ${sp}^2$ hybrid orbitals.

Carbon(I) has $2\sigma$ and $2\pi$- bond forming $sp$ hybridization having linear shape.

Carbon(II) has $3\sigma$- and $1\pi$-bond forming $s{p}^2$ hybridization having trigonal planar shape.