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(C) The molecular orbital configuration of the $O_2$ molecule ($16$ electrons) is:$[\sigma (1s)^2, \sigma^*(1s)^2, \sigma (2s)^2, \sigma^*(2s)^2, \sig

Vedclass · Accepted Answer

$14$

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(C) The molecular orbital configuration of the $O_2$ molecule ($16$ electrons) is:$[\sigma (1s)^2, \sigma^*(1s)^2, \sigma (2s)^2, \sigma^*(2s)^2, \sigma (2p_z)^2, \pi (2p_x)^2, \pi (2p_y)^2, \pi^*(2p_x)^1, \pi^*(2p_y)^1]$Counting the electrons in the filled orbitals:- $\sigma (1s)^2$: $2$ electrons ($1$ pair)- $\sigma^*(1s)^2$: $2$ electrons ($1$ pair)- $\sigma (2s)^2$: $2$ electrons ($1$ pair)- $\sigma^*(2s)^2$: $2$ electrons ($1$ pair)- $\sigma (2p_z)^2$: $2$ electrons ($1$ pair)- $\pi (2p_x)^2$: $2$ electrons ($1$ pair)- $\pi (2p_y)^2$: $2$ electrons ($1$ pair)Total number of pairs = $7$.Total number of paired electrons = $7 	imes 2 = 14$.

The number of electrons that are paired in an oxygen molecule $(O_2)$ is:

Similar Questions

According to $MO$ theory,which of the following lists ranks the nitrogen species in terms of increasing bond order?

Match the following molecules/ions in List-$I$ with their respective bond orders in List-$II$:
| List-$I$ (Molecules/ions) | List-$II$ (Bond order) |
| :--- | :--- |
| $A. N_2^+$ | $I. 1.0$ |
| $B. CO$ | $II. 1.5$ |
| $C. O_2$ | $III. 2.0$ |
| $D. O_2^-$ | $IV. 2.5$ |
| | $V. 3.0$ |

In dinitrogen tetroxide $(N_2O_4)$,there:

Among the following,the molecule expected to be stabilized by anion formation is

$A$ simplified application of $MO$ theory to the hypothetical molecule $OF$ would give its bond order as:

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