Question

The type of d-d transition of the electron occurs in \([Ti(H_2O)_6]^{3+}\) is:

• A. \( t_{2g}^2 e_g^1 \rightarrow t_{2g}^3 e_g^0 \)
• B. \( t_{2g}^1 e_g^2 \rightarrow t_{2g}^2 e_g^1 \)
• C. \( t_{2g}^1 e_g^3 \rightarrow t_{2g}^2 e_g^2 \)
• D. \( t_{2g}^1 e_g^2 \rightarrow t_{2g}^2 e_g^0 \)
• E. \( t_{2g}^2 e_g^1 \rightarrow t_{2g}^3 e_g^1 \)

Hint:

In octahedral fields, the \( t_{2g} \) orbitals are lower in energy than the \( e_g \) orbitals, and electron transitions occur between these orbitals.

Answer 1

The Correct Option is C

In \( [Ti(H_2O)_6]^{3+} \), titanium has an oxidation state of +3, which means it has 3 electrons in the 3d orbital. The electron configuration follows the crystal field splitting of the \( d \)-orbitals into two sets: \( t_{2g} \) and \( e_g \). 
The electron transition observed in the octahedral field corresponds to \( t_{2g}^1 e_g^3 \rightarrow t_{2g}^2 e_g^2 \).