An ion $M^{2+}$ forms the complexes $[M(H_2O)_6]^{2+}$,$[M(en)_3]^{2+}$,and $[MBr_6]^{4-}$. Match the complex with the appropriate colour.

The correct increasing order for the wavelengths of absorption in the visible region for the complexes of $Co^{3+}$ is:

If the $CFSE$ of $[Ti(H_2O)_6]^{3+}$ is $-96.0 \ kJ / mol$,this complex will absorb maximum at wavelength $........nm$. (nearest integer)
Assume Planck's constant $(h) = 6.4 \times 10^{-34} \ Js$,Speed of light $(c) = 3.0 \times 10^8 \ m / s$ and Avogadro's constant $(N_A) = 6 \times 10^{23} / mol$.

$[Fe(H_2O)_6]^{3+}$ is strongly paramagnetic whereas $[Fe(CN)_6]^{3-}$ is weakly paramagnetic. Explain.

Match the electronic configurations in List-$I$ with appropriate metal complex ions in List-$II$ and choose the correct option.
[Atomic Number: $Fe=26, Mn=25, Co=27$]

List-$I$	List-$II$
$P$. $t_{2g}^6 e_g^0$	$1$. $[Fe(H_2O)_6]^{2+}$
$Q$. $t_{2g}^3 e_g^2$	$2$. $[Mn(H_2O)_6]^{2+}$
$R$. $e^2 t_2^3$	$3$. $[Co(NH_3)_6]^{3+}$
$S$. $t_{2g}^4 e_g^2$	$4$. $[FeCl_4]^{-}$
	$5$. $[CoCl_4]^{2-}$

$\left[ Ti \left( H_{2} O \right)_{6} \right]^{3+}$ absorbs light of wavelength $498 \, nm$ during a $d-d$ transition. The octahedral splitting energy for the above complex is $....... \times 10^{-19} \, J$. (Round off to the Nearest Integer). Given: $h = 6.626 \times 10^{-34} \, Js$,$c = 3 \times 10^{8} \, ms^{-1}$.