Arrange the following Cobalt complexes in the order of increasing Crystal Field Stabilization Energy $(CFSE)$ value.
Complexes: $[CoF_{6}]^{3-}, [Co(H_{2}O)_{6}]^{2+}, [Co(NH_{3})_{6}]^{3+}$ and $[Co(en)_{3}]^{3+}$
$A: [CoF_{6}]^{3-}, B: [Co(H_{2}O)_{6}]^{2+}, C: [Co(NH_{3})_{6}]^{3+}, D: [Co(en)_{3}]^{3+}$
Choose the correct option:

The correct statements among $I$ to $III$ are:
$I$. Valence bond theory cannot explain the color exhibited by transition metal complexes.
$II$. Valence bond theory can predict quantitatively the magnetic properties of transition metal complexes.
$III$. Valence bond theory cannot distinguish ligands as weak and strong field ones.

The correct order of the complexes $[Co(NH_3)_5(H_2O)]^{3+}$ $(A)$,$[Co(NH_3)_6]^{3+}$ $(B)$,$[Co(CN)_6]^{3-}$ $(C)$,and $[CoCl(NH_3)_5]^{2+}$ $(D)$ in terms of the wavelength of light absorbed is:

Calculate the Crystal Field Stabilization Energy $(CFSE)$ for a high-spin $d^4$ tetrahedral complex.

Given below are two statements:
Statement $I$: Presence of a large number of unpaired electrons in transition metal atoms results in higher enthalpies of their atomisation.
Statement $II$: $d_{xy} = d_{xz} = d_{yz} < d_{x^2-y^2} = d_{z^2}$ and $d_{x^2-y^2} < d_{xy} = d_{xz} = d_{yz}$ are the $d$-orbital splittings in $[Fe(H_2O)_6]^{3+}$ and $[Ni(Cl)_4]^{2-}$ complex ions respectively.
In the light of the above statements, choose the correct answer from the options given below:

Given below are two statements:
Statement $I$: Among $Zn$, $Mn$, $Sc$ and $Cu$, the energy required to remove the third valence electron is highest for $Zn$ and lowest for $Sc$.
Statement $II$: The correct order of the following complexes in terms of $CFSE$ is $[Co(H_2O)_6]^{2+} < [Co(H_2O)_6]^{3+} < [Co(en)_3]^{3+}$.