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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

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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-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.

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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.