Question

Which elements among the following does form $P\pi - P\pi$ multiple bonds?
A. Arsenic
B. Nitrogen
C. Phosphorus
D. Antimony

Answer 1

Hint- Because of its small size and being strongly electro-negative, nitrogen can shape $P\pi - P\pi $ several connections with itself and with others. Just 1s electrons remain in the internal nitrogen centre. Among unbundled internal core electrons, there is no repulsion. Thus, p orbitals connect quickly to form pi bonds.

Complete step-by-step answer:
Among the above options, only Nitrogen forms $P\pi - P\pi $ multiple bonds
When Diatomic, $N \equiv N$, one bond is Sigma, with the other two bonds being $P\pi - P\pi $.
Sigma Bond: a covalent bond that arises from a molecular orbital creation by the atomic orbital overlap end-to - end, and is labelled with the symbol $\sigma $.
Pi bond: a covalent bond that is created by a side-by - side overlapping of atomic orbitals on the plane perpendicular to the line that links the nuclei of the atoms, which is represented by the symbol $\pi $.
When there is a correlation between two atoms, where the atom has a vacant orbit and the atom has a lone electron pair, so the pair of electrons is donated to the vacant orbit. The bonding is then labelled p-p or p-d, based on the orbital to which the pair is donated. The name of d(pi)-d(pi) bonding when the two orbitals are d. These bonds are often referred to as back-bonding bonds.
Hence, option B is the correct option.

Note: Many group 15 elements do not create several $P\pi - P\pi $ bonds owing to a repulsion between unbonded inner nuclei and size electrons. Among tiny nitrogen atoms there is no other repulsion because they have just $1{s^2}$. Throughout their inner centre, electrons quickly merge their p orbitals through $P\pi - P\pi $ multiple bonds.