Which of the following sequences is correct regarding the field strength of ligands as per the spectrochemical series?

What is pairing energy $(P)$? Explain the distribution of $d^n$ ($n=1$ to $10$) electrons in high spin and low spin octahedral complexes.

$\left[ Ti \left( H_{2} O \right)_{6} \right]^{3+}$ 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: $h = 6.626 \times 10^{-34} \, Js$,$c = 3 \times 10^{8} \, ms^{-1}$.

$A$ metal ion $M^{n+}$ having $d^6$ valence electronic configuration combines with three bidentate ligands to form a complex. Assuming crystal field splitting $(\Delta_0) >$ pairing energy,the $d$-orbital electronic configuration would be

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

The total number of unpaired electrons present in the $d^3$, $d^4$ (low spin), $d^5$ (high spin), $d^6$ (high spin), and $d^7$ (low spin) octahedral complex systems is . . . . . . .