Which of the following statements is incorrec | vedclass

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(D) The electronic configuration of nitrogen $(Z=7)$ is $[He] 2s^2 2p^3$.Nitrogen has only $s$ and $p$ orbitals in its valence shell $(n=2)$. It lacks

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It can increase its covalency by accepting a lone pair.

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(D) The electronic configuration of nitrogen $(Z=7)$ is $[He] 2s^2 2p^3$.Nitrogen has only $s$ and $p$ orbitals in its valence shell $(n=2)$. It lacks $d$-orbitals.Due to the absence of $d$-orbitals,nitrogen cannot expand its octet or increase its covalency beyond $4$ (e.g.,in $NH_4^+$).Therefore,the statement that it can increase its covalency by accepting a lone pair is correct,but it cannot expand its covalency to accommodate more than $4$ bonds.However,the statement 'It can increase its covalency by accepting a lone pair' is generally true for forming coordinate bonds (like in $NH_4^+$),but nitrogen cannot expand its covalency beyond $4$ because it lacks $d$-orbitals.Option $D$ is often considered incorrect in the context of expanding covalency beyond $4$ compared to other elements of the group,but specifically,nitrogen cannot expand its covalency to $5$ or $6$ due to the absence of $d$-orbitals.

Which of the following statements is incorrect for nitrogen?

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