In which of the following pairs first species have higher ionisation energy than second?

O_{2}

and

O

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N_{2}

and

N

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O_{2}^{-}

and

O_{2}^{+}

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O_{2}

and

N_{2}

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Solution

The correct option is B $N_{2}$ and $N$
IE depend upon the size and electronic configuration as well.
More electron-rich atom can give electron easily like $O_{2}^{-}$ is less IE than $O_{2}^{+}$ , but in case of ( $N_{2}$ and $N$ ) and ( $O_{2}$ and $O$ ) since size of $N$ is large but electronic configuration is half filled (stable than partial filled).
So, $N_{2}$ has more IE than $N$ .
(electron has more bonding characters in $N_{2}$ than $O_{2}$ )

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Similar questions

$N_{2}$ and $O_{2}$ are converted into monocations, $N_{2}^{+}$ and $O_{2}^{+}$ respectively. Which of the following is wrong ?

N_{2}

O_{2}

N_{2}^{+}

O_{2}^{+}

Using MOT, compare $O_{2}^{+}$ and $O_{2}^{-}$ species and choose the incorrect option

What is the effect of the following processes on the bond order in $N_{2}$ and $O_{2}$ ?

(i). $N_{2} \to N_{2}^{+} + e^{-}$

(ii) $O_{2} \to O_{2}^{+} + e^{-}$

N_{2}

N_{2}^{+}

O_{2}

O_{2}^{+}

N - N

O - O

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