Textbook Question
Draw a crystal field energy-level diagram for the 3d orbitals of titanium in [Ti(H2O)6]3+]. Indicate the crystal field splitting, and explain why is [Ti(H2O)6]3+] colored.
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24. Transition Metals and Coordination Compounds
Crystal Field Theory: Octahedral Complexes
Multiple Choice
Which d electron count can exhibit both high-spin and low-spin states in an octahedral complex?
A
d^4
B
d^5
C
d^8
D
d^6
Verified step by step guidance1
Understand that in octahedral complexes, the d electron configuration can influence whether the complex exhibits high-spin or low-spin states, depending on the ligand field strength and electron pairing energy.
Recall that high-spin and low-spin states occur due to the competition between the crystal field splitting energy (\( \Delta_0 \)) and the electron pairing energy (P). If \( \Delta_0 < P \), electrons occupy higher energy orbitals to remain unpaired (high-spin). If \( \Delta_0 > P \), electrons pair up in lower energy orbitals (low-spin).
Analyze each d electron count option to see if it can have both high-spin and low-spin configurations in an octahedral field:
- For \( d^4 \), both high-spin and low-spin states are possible but less common compared to \( d^6 \).
- For \( d^5 \), high-spin is more common, but low-spin can occur with strong field ligands.
- For \( d^8 \), usually low-spin is favored due to electron pairing in lower orbitals.
- For \( d^6 \), it is well-known that both high-spin and low-spin states are commonly observed depending on ligand strength.
Conclude that the \( d^6 \) electron configuration is the classic example where both high-spin and low-spin states are exhibited in octahedral complexes, making it the correct answer.
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