Identify the weak field ligand from the following.

Write down the number of $3d$ electrons in each of the following ions:
$Ti^{2+}, V^{2+}, Cr^{3+}, Mn^{2+}, Fe^{2+}, Fe^{3+}, Co^{2+}, Ni^{2+}$ and $Cu^{2+}$
Indicate how you would expect the five $3d$ orbitals to be occupied for these hydrated ions (octahedral).

The metal $d-$orbitals that directly face the ligands in $K_3[Co(CN)_6]$ are:

Identify the correct trend given below.
(Atomic No. $= Ti : 22, Cr : 24$ and $Mo : 42$)

Low spin complex of $d^6$ cation in an octahedral field will have the following energy:
($\Delta_o =$ crystal field splitting energy in an octahedral field,$P =$ Electron pairing energy)

What is the electronic arrangement of a metal atom/ion in an octahedral complex with a $d^4$ configuration,if $\Delta_o < \text{pairing energy}$?