Question

Match List-I with List-II and select the correct answer using the codes given below:

List I	List II
(I) $[Fe{F}_6{]}^{3-}$	(A) $1.73BM$
(II) $\left[Ti\right(H_{2}O{)}_6{]}^{3+}$	(B) $5.93BM$
(III) $\left[Cr\right(N{H}_3{)}_6{]}^{3+}$	(C) $0.00BM$
(IV) $\left[Ni\right(H_{2}O{)}_6{]}^{2+}$	(D) $2.83BM$
(V) $\left[Fe\right(CN{)}_6{]}^{4-}$	(E) $3.88BM$

• A. $BACDE$
• B. $BAEDC$
• C. $BCDEA$
• D. $DEABC$

Answer 1

The correct option is D $DEABC$

(i) In $[Fe{F}_6{]}^{3-}$, the central metal ion has the oxidation state of +3. It has $3d^5$ configuration and undergoes $s{p}^3{d}^2$ hybridization. It contains 5 unpaired electrons and has magnetic moment value of 5.91 B.M.

(ii) In $\left[Ti\right(H_{2}O{)}_6{]}^{3+}$, the central metal ion has the oxidation state of +3. It has $3d^1$ configuration and undergoes $d^{2}s{p}^3$ hybridization. It contains 1 unpaired electron and has magnetic moment value of 1.732 B.M.

(iii) In $\left[Cr\right(N{H}_3{)}_6{]}^{3+}$, the central metal ion has the oxidation state of +3. It has $3d^3$ configuration and undergoes $d^{2}s{p}^3$ hybridization. It contains 3 unpaired electrons and has magnetic moment value of 3.88 B.M.

(iv) In $\left[Ni\right(H_{2}O{)}_6{]}^{2+}$, the central metal ion has the oxidation state of +2. It has $3d^8$ configuration and undergoes $s{p}^3{d}^2$ hybridization. It contains 2 unpaired electrons and has magnetic moment value of 2.83 B.M.

(v) In $\left[Fe\right(CN{)}_6{]}^{4-}$, the central metal ion has the oxidation state of +2. It has $3d^6$ configuration and undergoes $d^{2}s{p}^3$ hybridization. It contains 0 unpaired electrons and has magnetic moment value of 0 B.M.