Q. No.Match the following:
Choose the correct answer from the options given below:
1. A-I, B-III, C-IV, D-II
2. A-III, B-IV, C-I, D-II
3. A-IV, B-I, C-III, D-II
4. A-III, B-I, C-IV, D-II
| List I (Complex/ ion) |
List II (Shape/geometry) |
||
| A. | \([Pt(Cl_2)(NH_3)_2]\) | I. | Octahedral |
| B. | \([Co(NH_3)_6]Cl_3\) | II. | Trigonal bipyramidal |
| C. | \([NiCl_4]^{2-}\) | III. | Square planar |
| D. | \([Fe(CO)_5]\) | IV. | Tetrahedral |
Choose the correct answer from the options given below:
1. A-I, B-III, C-IV, D-II
2. A-III, B-IV, C-I, D-II
3. A-IV, B-I, C-III, D-II
4. A-III, B-I, C-IV, D-II
Subtopic: VBT, CFT & their Limitations |
62%
Level 2: 60%+
NEET - 2026
Please attempt this question first.
Hints
Please attempt this question first.
According to crystal field theory, the correct order of ligands with respect to their decreasing order of field strength is:
| 1. | Cl- > NH3 > H2O > CO |
| 2. | CO > NH3 > H2O > Cl- |
| 3. | CO > H2O > NH3 > Cl- |
| 4. | Cl- > H2O > NH3 > CO |
Subtopic: Ligands | VBT, CFT & their Limitations |
67%
Level 2: 60%+
NEET - 2026
Please attempt this question first.
Hints
Please attempt this question first.
Which of the following are paramagnetic?
Choose the correct answer from the options given below:
| A. | \(\left[{NiCl}_4\right]^{2-}\) | B. | \(Ni(CO)_4\) |
| C. | \(\left[{Ni}({CN})_4\right]^{2-}\) | D. | \(\left[{Ni}\left({H}_2 {O}\right)_6\right]^{2+}\) |
| E. | \({Ni}\left({PPh}_3\right)_4\) | ||
| 1. | A and D only | 2. | A, D and E only |
| 3. | A and C only | 4. | B and E only |
Subtopic: VBT, CFT & their Limitations |
Level 3: 35%-60%
NEET - 2025
Please attempt this question first.
Hints
Please attempt this question first.
The correct order of the wavelength of light absorbed by the following complexes is.
Choose the correct answer from the options given below:
| A. | \(\left[\mathrm{Co}\left(\mathrm{NH}_3\right)_6\right]^{3+} \) | B. | \(\left[\mathrm{Co}(\mathrm{CN})_6\right]^{3-} \) |
| C. | \(\left[\mathrm{Cu}\left(\mathrm{H}_2 \mathrm{O}\right)_4\right]^{2+} \) | D. | \(\left[\mathrm{Ti}\left(\mathrm{H}_2 \mathrm{O}\right)_6\right]^{3+}\) |
| 1. | C < D < A < B | 2. | C < A < D < B |
| 3. | B < D < A < C | 4. | B < A < D < C |
Subtopic: VBT, CFT & their Limitations |
53%
Level 3: 35%-60%
NEET - 2025
Please attempt this question first.
Hints
Please attempt this question first.
Given below are two statements :
In the light of the above statements, choose the correct answer from the options given below:
1. Both Statement I and Statement II are False.
2. Statement I is True and Statement II is False.
3. Statement I is False but Statement II is True.
4. Both Statement I and Statement II are True.
| Statement I : | Both \(\left[\text{Co}\left(\text{NH}_3\right)_6\right]^{3+}\) and \(\left[\text{CoF}_6\right]^{3-}\) Complexes are octahedral but differ in their magnetic behaviour. |
| Statement II : | \(\left[\text{Co}\left(\text{NH}_3\right)_6\right]^{3+}\) is diamagnetic whereas \(\left[\text{CoF}_6\right]^{3-}\) is paramagnetic. |
1. Both Statement I and Statement II are False.
2. Statement I is True and Statement II is False.
3. Statement I is False but Statement II is True.
4. Both Statement I and Statement II are True.
Subtopic: VBT, CFT & their Limitations |
74%
Level 2: 60%+
NEET - 2024
Hints
The correct 'spin only' magnetic moments of \([\text{CoF}_6]^{3-}\) and \(\left[\mathrm{Co}\left(\mathrm{C}_2 \mathrm{O}_4\right)_3\right]^{3-}\) respectively, are:
| 1. | 0 BM and 4.9 BM | 2. | 0 BM and 0 BM |
| 3. | 4.9 BM and 0 BM | 4. | 4.9 BM and 4.9 BM |
Subtopic: VBT, CFT & their Limitations |
70%
Level 2: 60%+
NEET - 2024
Hints
Match the complex ions in List-I with their corresponding hybridization in List-II.
Choose the correct answer from the options given below:
1. A-IV, B-III, C-II, D-I
2. A-III, B-I, C-IV, D-II
3. A-I, B-II, C-III, D-IV
4. A-III, B-IV, C-II, D-I
| List -I (Complex ion) |
List -II (Hybridisation) |
||
| A. | \([\mathrm{Ni}(\mathrm{CN})_4]^{2-}\) | I. | \(s p^3 \) |
| B. | \(\mathrm{[CoF_6}]^{3-}\) | II. | \( d^2sp^3 \) |
| C. | \([\mathrm{Co}(\mathrm{C}_2 \mathrm{O}_4)_3 ]^{3-}\) | III. | \(s p^3d^2\) |
| D. | \(\mathrm{[NiCl_4}]^{2-}\) | IV. | \(dsp^2\) |
Choose the correct answer from the options given below:
1. A-IV, B-III, C-II, D-I
2. A-III, B-I, C-IV, D-II
3. A-I, B-II, C-III, D-IV
4. A-III, B-IV, C-II, D-I
Subtopic: VBT, CFT & their Limitations |
82%
Level 1: 80%+
NEET - 2024
Hints
The crystal field stabilisation energy (CFSE) and the 'spin only' magnetic moment of \(\mathrm{[FeF_6]^{3-}}\) ion respectively, are:
1. \(0~\Delta~\text{and}~5.9~\text{BM}\)
2. \(0~\Delta~\text{and}~1.73~\text{BM}\)
3. \(2.0~\Delta~\text{and}~5.9~\text{BM}\)
4. \(2.0~\Delta~\text{and}~1.73~\text{BM}\)
1. \(0~\Delta~\text{and}~5.9~\text{BM}\)
2. \(0~\Delta~\text{and}~1.73~\text{BM}\)
3. \(2.0~\Delta~\text{and}~5.9~\text{BM}\)
4. \(2.0~\Delta~\text{and}~1.73~\text{BM}\)
Subtopic: VBT, CFT & their Limitations |
69%
Level 2: 60%+
NEET - 2024
Hints
The order of energy absorbed, which is responsible for the color of complexes, is:
\((A) \ \left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}(\text { en })_{2}\right]^{2+}\)
\( (B) \ \left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}(\mathrm{en})\right]^{2+} \)\( (C) \ \left[\mathrm{Ni}(\mathrm{en})_{3}\right]^{2+}\)
\((A) \ \left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}(\text { en })_{2}\right]^{2+}\)
\( (B) \ \left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}(\mathrm{en})\right]^{2+} \)\( (C) \ \left[\mathrm{Ni}(\mathrm{en})_{3}\right]^{2+}\)
| 1. | B > A > C | 2. | A > B > C |
| 3. | C > B > A | 4. | C > A > B |
Subtopic: VBT, CFT & their Limitations |
66%
Level 2: 60%+
NEET - 2022
Hints
The correct order of spin-only magnetic moment for the given complexes is:
1. \([Co(H_2O)_6]^{2+} > [MnCl_6]^{3-} > [Fe(CN)_6]^{3-} \)
2. \([Fe(CN)_6]^{3-} >[Co(H_2O)_6]^{2+} > [MnCl_6]^{3-} \)
3. \([MnCl_6]^{3-} >[Fe(CN)_6]^{3-} >[Co(H_2O)_6]^{2+} \)
4. \([MnCl_6]^{3-} > [Co(H_2O_6]^{2+} > [Fe(CN)_6]^{3-} \)
Subtopic: VBT, CFT & their Limitations |
64%
Level 2: 60%+
NEET - 2022
Hints
© 2026 GoodEd Technologies Pvt. Ltd.