Question

Match List-I with List-II and select the correct option.

• A. A-II, B-IV, C-I, D-III
• B. A-IV, B-I, C-II, D-III
• C. A-I, B-II, C-IV, D-III
• D. A-IV, B-II, C-I, D-III

Hint:

When determining the hybridization and magnetic moment, focus on the ligand geometry and the central metal's oxidation state. Use these to determine the appropriate geometry (tetrahedral, square planar, or octahedral) and calculate the number of unpaired electrons for the magnetic moment.

Answer 1

The Correct Option is D

Step 1: Analyze the given complexes and their coordination geometry
\([NiCl_4]^{2-}\) is a tetrahedral complex, typically exhibiting \(sp^3\) hybridization.
It also has a magnetic moment of 3.87 BM.

\([Ni(CN_4)]^{2-}\) is a square planar complex, usually exhibiting \(dsp^2\) hybridization.
It shows no unpaired electrons, so the magnetic moment is 0 BM.

\([CoCl_4]^{2-}\) is an octahedral complex, usually with \(sp^3d^2\) hybridization.
Its magnetic moment is 2.82 BM.

\([Ni(H_2O)_6]^{2+}\) is a tetrahedral complex, exhibiting \(sp^3\) hybridization and a magnetic moment of 2.82 BM.

Step 2: Match the complexes with their characteristics 
A.
\([NiCl_4]^{2-}\) matches with IV.
\(sp^3\), tetrahedral, 3.87 BM.
B.
\([Ni(CN_4)]^{2-}\) matches with II.
\(dsp^2\), square planar, 0 BM.
C.
\([CoCl_4]^{2-}\) matches with I.
\(sp^3d^2\), octahedral, 2.82 BM.
D.
\([Ni(H_2O)_6]^{2+}\) matches with III.
\(sp^3\), tetrahedral, 2.82 BM.