Analyze Statement I

Statement I says:

Nitrogen forms oxides with $+1$ to $+5$ oxidation states due to the formation of $p\pi$-$p\pi$ bond with oxygen.

Nitrogen shows many oxidation states in its oxides:

• $\mathrm{N_2O}$ : average oxidation state of N = $+1$
• $\mathrm{NO}$ : $+2$
• $\mathrm{N_2O_3}$ : $+3$
• $\mathrm{NO_2}$ / $\mathrm{N_2O_4}$ : $+4$
• $\mathrm{N_2O_5}$ / $\mathrm{HNO_3}$ : $+5$

This wide range is possible because nitrogen forms strong multiple bonds with oxygen through effective $2p\pi$-$2p\pi$ overlap.

Hence, Statement I is true.

Analyze Statement II

Statement II says:

Nitrogen does not form halides with $+5$ oxidation state due to the absence of d-orbital in it.

Nitrogen can form trihalides such as $\mathrm{NF_3,\ NCl_3}$ where N is in $+3$ oxidation state, but it does not form pentahalides like $\mathrm{NCl_5}$.

Reason:

• Nitrogen belongs to the 2nd period.
• Its valence shell contains only $2s$ and $2p$ orbitals.
• It has no vacant d-orbitals in the valence shell, so it cannot expand its octet to accommodate five halogen atoms.

Therefore, Statement II is also true.

Choose the correct option

Since both statements are true, the correct option is:

$\boxed{\text{A}}$

Comparison with stored answer

Stored correct answer = A

My derived answer = A

So, the answer agrees with the stored correct answer.