The paramagnetic nature of oxygen can be expl | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(D) The paramagnetic nature of the oxygen molecule $(O_2)$ is due to the presence of two unpaired electrons in the antibonding $\pi^* 2p_x$ and $\pi^*

Vedclass · Accepted Answer

Molecular orbital concept

Vedclass · Answer

(D) The paramagnetic nature of the oxygen molecule $(O_2)$ is due to the presence of two unpaired electrons in the antibonding $\pi^* 2p_x$ and $\pi^* 2p_y$ molecular orbitals. This behavior cannot be explained by the Lewis structure or the octet rule,which suggest all electrons are paired. The Molecular Orbital Theory $(MOT)$ successfully accounts for this by considering the distribution of electrons in molecular orbitals.

The paramagnetic nature of oxygen can be explained by

Similar Questions

What is the effect of the following processes on the bond order in $N_{2}$ and $O_{2}$?
$(A)$ $N_{2} \to N_{2}^{+} + e^{-}$
$(B)$ $O_{2} \to O_{2}^{+} + e^{-}$

In which pair,or pairs,is the stronger bond found in the first species?
$(a) \ O_2^-, O_2$
$(b) \ N_2, N_2^+$
$(c) \ NO^+, NO^-$

Which of the following species are paramagnetic: $O_2, O_2^-, O_2^{2-}$?

If the sum of bond orders of $O_2^{-}$ and $O_2^{2-}$ is $x$,then bond order of $O_2^{2+}$ will be (in $x$)

Which of the following pairs of species have the same bond order?

Vedclass Test Series

Exam Paper Generator

Online Exam Module