Given below are two statements:

$$\textbf{Statement I :}$$ Presence of large number of unpaired electrons in transition metal atoms results in higher enthalpies of their atomisation.

$$\textbf{Statement II :}$$ $$d_{xy} = d_{xz} = d_{yz} < d_{x^2-y^2} = d_{z^2}$$ and $$d_{x^2-y^2} = d_{z^2} < d_{xy} = d_{xz} = d_{yz}$$ are the d-orbital splittings in $$[\text{Fe}(\text{H}_2\text{O})_6]^{3+}$$ and $$[\text{Ni}(\text{Cl})_4]^{2-}$$ complex ions respectively.

In the light of the above statements, choose the correct answer from the options given below:

The high enthalpies of atomisation of transition metals are due to the strong metallic bonding arising from the participation of unpaired (d)-electrons. A larger number of unpaired electrons results in stronger interatomic interactions and, consequently, higher enthalpies of atomisation.

Therefore, Statement I is correct.

For the octahedral complex ([Fe(H_2O)_6]^{3+}), crystal field splitting occurs as

$$d_{xy}=d_{xz}=d_{yz}<d_{x^2-y^2}=d_{z^2},$$

i.e.,

$$t_{2g}<e_g.$$

For the tetrahedral complex ([NiCl_4]^{2-}), the splitting order is reversed and is given by

$$d_{x^2-y^2}=d_{z^2}<d_{xy}=d_{xz}=d_{yz},$$

i.e.,

$$e<t_2.$$

Thus, the orbital splitting patterns stated for both complexes are correct according to Crystal Field Theory.

Hence, Statement I is correct and Statement II is also correct.