Which of the following statements best explains why the titanium complex, [Ti(H₂O)6]4+, is colourless. The water ligands emit all wavelengths of light. There are multiple transitional energies, and all visible wavelengths are absorbed equally. The energy to excite the electron from the T2g orbital to the Eg orbital falls outside the visible spectrum. The transition metal possesses no d-electrons to be excited, therefore all wavelengths are transmitted. When the electrons relax back down in the transition metal, all wavelengths of light are emitted.
Which of the following statements best explains why the titanium complex, [Ti(H₂O)6]4+, is colourless. The water ligands emit all wavelengths of light. There are multiple transitional energies, and all visible wavelengths are absorbed equally. The energy to excite the electron from the T2g orbital to the Eg orbital falls outside the visible spectrum. The transition metal possesses no d-electrons to be excited, therefore all wavelengths are transmitted. When the electrons relax back down in the transition metal, all wavelengths of light are emitted.
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter19: Transitition Metals, Coordination Chemistry And Metallurgy
Section: Chapter Questions
Problem 19.46QE
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![Which of the following statements best explains why the titanium complex,
[Ti(H₂O)6]4+, is colourless.
The water ligands emit all wavelengths of light.
There are multiple transitional energies, and all visible wavelengths are absorbed
equally.
The energy to excite the electron from the T2g orbital to the Eg orbital falls
outside the visible spectrum.
The transition metal possesses no d-electrons to be excited, therefore all
wavelengths are transmitted.
When the electrons relax back down in the transition metal, all wavelengths of
light are emitted.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5854b887-9c69-42b6-8782-5d3a53d46b66%2F7ddb6dbc-dd3f-4724-bab0-8f04d47f18d0%2F0806m8_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Which of the following statements best explains why the titanium complex,
[Ti(H₂O)6]4+, is colourless.
The water ligands emit all wavelengths of light.
There are multiple transitional energies, and all visible wavelengths are absorbed
equally.
The energy to excite the electron from the T2g orbital to the Eg orbital falls
outside the visible spectrum.
The transition metal possesses no d-electrons to be excited, therefore all
wavelengths are transmitted.
When the electrons relax back down in the transition metal, all wavelengths of
light are emitted.
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