Read the information below carefully, and answer the questions:

d$-$Block metal compounds are often intense colored due to the electronic $\text{'}d-d\text{'}$

transitions. That's why $C{u}^{2+}$ compounds are blue.

When $C{u}^{2+}$ are complexed with

$N{H}_3$ to form $Cu(N{H}_3{)}_4^{2+},$ the

energy of the $3d$ orbitals are split,

the energy diagram is shown on

the right.

What is the eiectron

configuration of $Cu$

What is the electron configuration of $C{u}^{2+}$

What is the $3$d electron for $C{u}^{2+}$ in its ground state when it is complexed with

$N{H}_3($fill in the electrons in the table on the right$)$