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The pale yellow color of [Mn(H2O)6]2+ is due to
- a)spin forbidden d-d transition
- b)metal to ligand charge transfer
- c)ligand to metal charge transfer
- d)intra ligand excitation
Correct answer is option 'A'. Can you explain this answer?
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The pale yellow color of [Mn(H2O)6]2+ is due toa)spin forbidden d-d tr...
Spin Forbidden d-d Transition
The pale yellow color of [Mn(H2O)6]2+ is due to a spin forbidden d-d transition. This phenomenon occurs when there is a change in the electron configuration of the metal ion in a complex.
Explanation:
Spin Forbidden Transition:
When an electron in a transition metal complex moves from one d orbital to another, it involves a transition in the spin state of the electrons. According to the selection rules of electronic transitions, a change in spin from one state to another is considered spin forbidden. This means that the probability of such a transition occurring is very low.
Transition Metal Complexes:
Transition metal complexes are characterized by the presence of partially filled d orbitals in the central metal ion. These d orbitals can absorb light energy and undergo electronic transitions, resulting in the absorption or emission of light. The energy difference between the d orbitals determines the wavelength of light that is absorbed or emitted.
Pale Yellow Color of [Mn(H2O)6]2+:
In the case of [Mn(H2O)6]2+, the manganese ion (Mn2+) is in a high spin state with five unpaired electrons in its d orbitals. When light is absorbed by the complex, an electron is promoted from one d orbital to another. In this case, the d-d transition involves the promotion of an electron from a lower energy d orbital to a higher energy d orbital.
Spin Forbidden d-d Transition:
The pale yellow color of [Mn(H2O)6]2+ is due to a spin forbidden d-d transition. This means that the transition between the d orbitals involves a change in the spin state of the electrons. According to the selection rules, a transition that involves a change in spin is unlikely to occur, leading to a low probability of absorption of light in this case.
Conclusion:
In summary, the pale yellow color of [Mn(H2O)6]2+ is due to a spin forbidden d-d transition. This transition involves a change in the spin state of the electrons in the d orbitals of the manganese ion. As a result, the absorption of light is limited, leading to a pale yellow color observed for the complex.
The pale yellow color of [Mn(H2O)6]2+ is due to a spin forbidden d-d transition. This phenomenon occurs when there is a change in the electron configuration of the metal ion in a complex.
Explanation:
Spin Forbidden Transition:
When an electron in a transition metal complex moves from one d orbital to another, it involves a transition in the spin state of the electrons. According to the selection rules of electronic transitions, a change in spin from one state to another is considered spin forbidden. This means that the probability of such a transition occurring is very low.
Transition Metal Complexes:
Transition metal complexes are characterized by the presence of partially filled d orbitals in the central metal ion. These d orbitals can absorb light energy and undergo electronic transitions, resulting in the absorption or emission of light. The energy difference between the d orbitals determines the wavelength of light that is absorbed or emitted.
Pale Yellow Color of [Mn(H2O)6]2+:
In the case of [Mn(H2O)6]2+, the manganese ion (Mn2+) is in a high spin state with five unpaired electrons in its d orbitals. When light is absorbed by the complex, an electron is promoted from one d orbital to another. In this case, the d-d transition involves the promotion of an electron from a lower energy d orbital to a higher energy d orbital.
Spin Forbidden d-d Transition:
The pale yellow color of [Mn(H2O)6]2+ is due to a spin forbidden d-d transition. This means that the transition between the d orbitals involves a change in the spin state of the electrons. According to the selection rules, a transition that involves a change in spin is unlikely to occur, leading to a low probability of absorption of light in this case.
Conclusion:
In summary, the pale yellow color of [Mn(H2O)6]2+ is due to a spin forbidden d-d transition. This transition involves a change in the spin state of the electrons in the d orbitals of the manganese ion. As a result, the absorption of light is limited, leading to a pale yellow color observed for the complex.
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The pale yellow color of [Mn(H2O)6]2+ is due toa)spin forbidden d-d transitionb)metal to ligand charge transferc)ligand to metal charge transferd)intra ligand excitationCorrect answer is option 'A'. Can you explain this answer?
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