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In which of the following pairs are both the ions coloured in aqueous solutions ? [2006] (At. no. : Sc = 21, Ti = 22, Ni = 28, Cu = 29, Co = 27)
- a)Sc3+, Ti3+
- b)Sc3+, Co2+
- c)Ni2+, Cu+
- d)Ni2+, Ti3+
Correct answer is option 'D'. Can you explain this answer?
Verified Answer
In which of the following pairs are both the ions coloured in aqueous ...
Sc3+ : 1s2, 2s2p6, 3s2p6d0, 4s0; no unpaired electron.
Cu+ : 1s2, 2s2p6, 3s2p6d10, 4s0; no unpaired electron.
Ni2+: 1s2, 2s2p6, 3s2p6d8, 4s0; unpaired electron present.
Ti3+ : 1s2, 2s2p6, 2s2p6d1, 4s0; unpaired electron present Co2+ : 1s2, 2s2p6, 3s2p6d7, 4s0; unpaired electron present So from the given option the only correct combination is Ni2+ and Ti3+
Cu+ : 1s2, 2s2p6, 3s2p6d10, 4s0; no unpaired electron.
Ni2+: 1s2, 2s2p6, 3s2p6d8, 4s0; unpaired electron present.
Ti3+ : 1s2, 2s2p6, 2s2p6d1, 4s0; unpaired electron present Co2+ : 1s2, 2s2p6, 3s2p6d7, 4s0; unpaired electron present So from the given option the only correct combination is Ni2+ and Ti3+
Most Upvoted Answer
In which of the following pairs are both the ions coloured in aqueous ...
Explanation:
In order to determine which of the following pairs have both ions colored in aqueous solutions, we need to consider the electronic configurations and the corresponding absorption spectra of the ions.
Sc3+ ion:
The electronic configuration of Sc3+ is 1s2 2s2 2p6 3s2 3p6 3d0 4s0. Since there are no electrons in the d orbitals, Sc3+ does not have any d-d transitions, and therefore it appears colorless in aqueous solutions.
Ti3+ ion:
The electronic configuration of Ti3+ is 1s2 2s2 2p6 3s2 3p6 3d1 4s0. Ti3+ has one electron in the d orbital, which allows for d-d transitions and absorption of certain wavelengths of light. As a result, Ti3+ appears colored in aqueous solutions.
Co2+ ion:
The electronic configuration of Co2+ is 1s2 2s2 2p6 3s2 3p6 3d7 4s0. Co2+ has seven electrons in the d orbitals, which leads to multiple d-d transitions and absorption of different wavelengths of light. As a result, Co2+ appears colored in aqueous solutions.
Ni2+ ion:
The electronic configuration of Ni2+ is 1s2 2s2 2p6 3s2 3p6 3d8 4s0. Ni2+ also has eight electrons in the d orbitals, which leads to multiple d-d transitions and absorption of different wavelengths of light. Therefore, Ni2+ appears colored in aqueous solutions.
Cu2+ ion:
The electronic configuration of Cu2+ is 1s2 2s2 2p6 3s2 3p6 3d9 4s0. Cu2+ has nine electrons in the d orbitals, and because of the extra stability associated with a completely filled d orbital, Cu2+ does not have any d-d transitions. Therefore, Cu2+ appears colorless in aqueous solutions.
Based on the above explanations, we can conclude that the pair Ni2+ and Ti3+ have both ions colored in aqueous solutions.
In order to determine which of the following pairs have both ions colored in aqueous solutions, we need to consider the electronic configurations and the corresponding absorption spectra of the ions.
Sc3+ ion:
The electronic configuration of Sc3+ is 1s2 2s2 2p6 3s2 3p6 3d0 4s0. Since there are no electrons in the d orbitals, Sc3+ does not have any d-d transitions, and therefore it appears colorless in aqueous solutions.
Ti3+ ion:
The electronic configuration of Ti3+ is 1s2 2s2 2p6 3s2 3p6 3d1 4s0. Ti3+ has one electron in the d orbital, which allows for d-d transitions and absorption of certain wavelengths of light. As a result, Ti3+ appears colored in aqueous solutions.
Co2+ ion:
The electronic configuration of Co2+ is 1s2 2s2 2p6 3s2 3p6 3d7 4s0. Co2+ has seven electrons in the d orbitals, which leads to multiple d-d transitions and absorption of different wavelengths of light. As a result, Co2+ appears colored in aqueous solutions.
Ni2+ ion:
The electronic configuration of Ni2+ is 1s2 2s2 2p6 3s2 3p6 3d8 4s0. Ni2+ also has eight electrons in the d orbitals, which leads to multiple d-d transitions and absorption of different wavelengths of light. Therefore, Ni2+ appears colored in aqueous solutions.
Cu2+ ion:
The electronic configuration of Cu2+ is 1s2 2s2 2p6 3s2 3p6 3d9 4s0. Cu2+ has nine electrons in the d orbitals, and because of the extra stability associated with a completely filled d orbital, Cu2+ does not have any d-d transitions. Therefore, Cu2+ appears colorless in aqueous solutions.
Based on the above explanations, we can conclude that the pair Ni2+ and Ti3+ have both ions colored in aqueous solutions.
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In which of the following pairs are both the ions coloured in aqueous solutions ? [2006] (At. no. : Sc = 21, Ti = 22, Ni = 28, Cu = 29, Co = 27)a)Sc3+, Ti3+b)Sc3+, Co2+c)Ni2+, Cu+d)Ni2+, Ti3+Correct answer is option 'D'. Can you explain this answer? for Class 12 2026 is part of Class 12 preparation. The Question and answers have been prepared according to the Class 12 exam syllabus. Information about In which of the following pairs are both the ions coloured in aqueous solutions ? [2006] (At. no. : Sc = 21, Ti = 22, Ni = 28, Cu = 29, Co = 27)a)Sc3+, Ti3+b)Sc3+, Co2+c)Ni2+, Cu+d)Ni2+, Ti3+Correct answer is option 'D'. Can you explain this answer? covers all topics & solutions for Class 12 2026 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for In which of the following pairs are both the ions coloured in aqueous solutions ? [2006] (At. no. : Sc = 21, Ti = 22, Ni = 28, Cu = 29, Co = 27)a)Sc3+, Ti3+b)Sc3+, Co2+c)Ni2+, Cu+d)Ni2+, Ti3+Correct answer is option 'D'. Can you explain this answer?.
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