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(C) The electronic configuration of nitrogen $(N)$ is $1s^2 2s^2 2p^3$ and that of oxygen $(O)$ is $1s^2 2s^2 2p^4$.Statement-$1$: Nitrogen has a half

Vedclass · Accepted Answer

Both statements $1$ and $2$ are correct

Vedclass · Answer

(C) The electronic configuration of nitrogen $(N)$ is $1s^2 2s^2 2p^3$ and that of oxygen $(O)$ is $1s^2 2s^2 2p^4$.Statement-$1$: Nitrogen has a half-filled $2p$ subshell,which makes it very stable. Adding an electron to nitrogen requires energy (endothermic),whereas adding an electron to oxygen is exothermic. Thus,nitrogen has a less negative (lesser) electron gain enthalpy than oxygen. Statement-$1$ is correct.Statement-$2$: Nitrogen has a stable half-filled $2p^3$ configuration,making it harder to remove an electron compared to oxygen,which has a $2p^4$ configuration. Therefore,the ionization enthalpy of nitrogen is higher than that of oxygen,meaning oxygen has a lesser ionization enthalpy than nitrogen. Statement-$2$ is correct.

Choose the correct option regarding the following statements:
Statement-$1$: Nitrogen has lesser electron gain enthalpy than oxygen.
Statement-$2$: Oxygen has lesser ionization enthalpy than nitrogen.

Similar Questions

Identify the incorrect statement from the following:

Which of the following statements is/are correct?

Which of the following order$(s)$ is/are correct?
$(1) Li < Be < B < C$ $(IE_1)$
$(2) Li < Na < K < Rb < Cs$ (Reducing power in gaseous state)
$(3) Li^{+} < Na^{+} < K^{+} < Rb^{+} < Cs^{+}$ (Ionic mobility in aqueous solution)
$(4) S > Se > Te > O$ $(EA)$

The number of the following pairs of elements which exhibit a diagonal relationship is:
$1. B \text{ and } Si$
$2. Be \text{ and } Al$
$3. Li \text{ and } Mg$
$4. Al \text{ and } S$

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Choose the correct option regarding the following statements:Statement-$1$: Nitrogen has lesser electron gain enthalpy than oxygen.Statement-$2$: Oxygen has lesser ionization enthalpy than nitrogen.