Question

In the complex $[(Ni(H_{2}O{)}_2(N{H}_3{)}_4{]}^{2+}$ the number of unpaired electrons is

• A. 0
• B. 1
• C. 3
• D. 2

Answer 1

Answer: (A)

In the complex ${\left[Ni(H2O{)}_2{\left(N{H}_3\right)}_4\right]}^{2+}$ the $Ni$ is in $+2$ oxidation state and there are 8 electrons in $3d$ subshell and since the $N{H}_3$ is a strong field ligand therefore the two unpaired electrons left gets paired up and hence the number of unpaired electrons become o. hence the magnetic moment $\sqrt{n(n+2)}$ where $n$ is the number of unpaired electron comes out to be o. Hence the correct