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

Question

Which of the following orbitals will not form sigma bond after overlapping? (A) s-orbital and s-orbital (B) s-orbital and pz-orbital (C) pz-orbital and pz-orbital (D) px-orbital and px-orbital

Tardigrade Admin · Accepted Answer

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:- Cl 2, Br 2, I 2,

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

$s$ -orbital and $s$ -orbital

$s$ -orbital and $p_{z}$ -orbital

$p_{z}$ -orbital and $p_{z}$ -orbital

$p_{x}$ -orbital and $p_{x}$ -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 $P i$ bond.
Examples of $p -$ p overlapping:- $C l_{2}, B r_{2}, I_{2}$ ,

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

s-orbital and s-orbital

s-orbital and pz​-orbital

pz​-orbital and pz​-orbital

px​-orbital and px​-orbital

S and Pz​ orbitals are along the axis, they able to form the sigma bond while Px​ and Py​ orbitals are lateral, so they can form only Pi bond. Examples of p− p overlapping:- Cl2​,Br2​,I2​,

$s$ -orbital and $s$ -orbital

$s$ -orbital and $p_{z}$ -orbital

$p_{z}$ -orbital and $p_{z}$ -orbital

$p_{x}$ -orbital and $p_{x}$ -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 $P i$ bond.
Examples of $p -$ p overlapping:- $C l_{2}, B r_{2}, I_{2}$ ,