Question

Match List I with List II and Select the correct answer using the codes given below the lists:

$\begin{array}{cc}\text{List 1}& \text{List 2}\\ \text{Complex Ions}& \text{Magnetic Moment}\\ & \text{Bohr magneton}\\ a.\left[Fe\right(CN{)}_6{]}^{-4}& 1.1.73\\ b.\left[Ti\right(H_{2}O{)}_6{]}^{3+}& 2.5.93\\ c.\left[Cr\right(H_{2}O{)}_6{]}^{3+}& 3.0.00\\ d.Ni(H_{2}O{)}_6{]}^{2+}& 4.2.83\\ e.[Fe{F}_6{]}^{-3}& 5.3.88\end{array}$

Codes :

• A. A B C D E
  (a) 1 2 3 4 5
• B. A B C D E
  3 1 5 4 2
• C. A B C D E
  2 3 4 5 1
• D. A B C D E
  4 5 1 2 3

Answer 1

The correct option is B A B C D E

3 1 5 4 2
A B C D E
3 1 5 4 2

$\left[Fe\right(CN{)}_6{]}^{-4}$ has no unpaired electrons. Hence the magnetic moment is given by $\sqrt{\left(n\right)(n+2)}$. Here $n$ is the number of unpaired electrons of the central metal ion.

Likewise, in each case, we will have to evaluate the number of unpaired electrons; this is based on a number of concepts including ligand field strengths and pairing energy and CFSE.