In which of the following is the O-O bond dis | vedclass

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

Question

(D) To determine the $O-O$ bond distance,we look at the bond order of the species:$1$. $O_2$: Bond order = $2.0$ (Electronic configuration: $\sigma 1s

Vedclass · Accepted Answer

Dioxygen $(O_2)$

Vedclass · Answer

(D) To determine the $O-O$ bond distance,we look at the bond order of the species:$1$. $O_2$: Bond order = $2.0$ (Electronic configuration: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1 = \pi^* 2p_y^1$).$2$. $O_2^-$ (Superoxide): Bond order = $1.5$.$3$. $O_2^{2-}$ (Peroxide): Bond order = $1.0$.Since bond distance is inversely proportional to bond order,the species with the highest bond order will have the minimum bond distance.$O_2$ has the highest bond order $(2.0)$,therefore it has the shortest $O-O$ bond distance.

In which of the following is the $O-O$ bond distance minimum?

Similar Questions

Bond order is a concept in the molecular orbital theory. It depends on the number of electrons in the bonding and antibonding orbitals. Which of the following statements is true about it? The bond order

Which of the following orbitals cannot form a $\pi$-bond as well as a $\delta$-bond?

How are molecular orbitals formed? Explain.

The correct stability order for $N_2$ and its given ions is :-

The bond order in $NO$ is $2.5$ while that in $NO^{+}$ is $3$. Which of the following statements is true for these two species?

Vedclass Test Series

Exam Paper Generator

Online Exam Module