Question

Which of the following orbitals will not form sigma bond after overlapping?

• A. $\text{s}$-orbital and $\text{s}$-orbital
• B. $\text{s}$-orbital and ${\text{p}}_z$-orbital
• C. ${\text{p}}_z$-orbital and ${\text{p}}_z$-orbital
• D. ${\text{p}}_x$-orbital and ${\text{p}}_y$-orbital

Answer 1

The correct option is D ${\text{p}}_x$-orbital and ${\text{p}}_y$-orbital

$S$ and $P_z$ orbitals are along the axis, they able to form the sigma bond while $P_x$ and $P_y$ orbitals are lateral, so they can form only $Pi$ bond.

Examples of $p-p$ overlapping:- $C{l}_2,B{r}_2,I_2$,

The correct option is [D].