Given below are two statements: Statement I: Nitrogen forms oxides with +1 to +5 oxidation states due to the formation of $\mathrm{p} \pi-\mathrm{p} \pi$ bond with oxygen. Statement II: Nitrogen does not form halides with +5 oxidation state due to the absence of d-orbital in it. In the light of the above statements, choose the correct answer from the options given below:
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Nitrogen's ability to form oxides and halides depends on its electronic configuration and the availability of d-orbitals.
To verify the provided statements, we will evaluate each one:
Statement I: Nitrogen forms oxides with +1 to +5 oxidation states because of the formation of $\mathrm{p} \pi-\mathrm{p} \pi$ bonds with oxygen.
Nitrogen exhibits various oxidation states from +1 to +5 in its oxides, including N2O, NO, N2O3, NO2, and N2O5.
The ability of nitrogen to form multiple bonds with oxygen via $\mathrm{p} \pi-\mathrm{p} \pi$ bonding facilitates the stabilization of these oxidation states.
Consequently, Statement I is \(\text{true}\).
Statement II: Nitrogen does not form halides with a +5 oxidation state owing to the absence of d-orbitals.
Nitrogen, being in the second period, lacks d-orbitals. This deficiency prevents nitrogen from expanding its octet, which is necessary for forming halides in a +5 oxidation state.
This is why nitrogen commonly forms halides such as NF3, where its oxidation state is +3, and not +5.
Therefore, Statement II is also \(\text{true}\).
Conclusion: As both statements are accurate, the correct response is "Both Statement I and Statement II are true."
