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Which of the following statements best explains why the titanium complex, [Ti(H₂O)614+, is colourless. The energy to excite the electron from the T2g orbital to the Eg orbital falls outside the visible spectrum. There are multiple transitional energies, and all visible wavelengths are absorbed equally. When the electrons relax back down in the transition metal, all wavelengths of light are emitted. The transition metal possesses no d-electrons to be excited, therefore all wavelengths are transmitted. The water ligands emit all wavelengths of light.

Which of the following statements best explains why the titanium complex, [Ti(H₂O)614+, is colourless. The energy to excite the electron from the T2g orbital to the Eg orbital falls outside the visible spectrum. There are multiple transitional energies, and all visible wavelengths are absorbed equally. When the electrons relax back down in the transition metal, all wavelengths of light are emitted. The transition metal possesses no d-electrons to be excited, therefore all wavelengths are transmitted. The water ligands emit all wavelengths of light.

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter8: Bonding In Transition Metal Compounds And Coordination Complexes
Section: Chapter Questions
Problem 33P
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Which of the following statements best explains why the titanium complex, [Ti(H₂O)614+, is colourless. The energy to excite the electron from the T2g orbital to the Eg orbital falls outside the visible spectrum. There are multiple transitional energies, and all visible wavelengths are absorbed equally. When the electrons relax back down in the transition metal, all wavelengths of light are emitted. The transition metal possesses no d-electrons to be excited, therefore all wavelengths are transmitted. The water ligands emit all wavelengths of light.
Transcribed Image Text:Which of the following statements best explains why the titanium complex, [Ti(H₂O)614+, is colourless. The energy to excite the electron from the T2g orbital to the Eg orbital falls outside the visible spectrum. There are multiple transitional energies, and all visible wavelengths are absorbed equally. When the electrons relax back down in the transition metal, all wavelengths of light are emitted. The transition metal possesses no d-electrons to be excited, therefore all wavelengths are transmitted. The water ligands emit all wavelengths of light.
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