Question:
According to crystal field theory, when ligands approach the metal atom or ion in an octahedral field, the orbitals that undergo increase in energy are:
According to crystal field theory, when ligands approach the metal atom or ion in an octahedral field, the orbitals that undergo increase in energy are:
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In octahedral complexes, \(e_g\) orbitals always have higher energy than \(t_{2g}\) due to direct ligand interaction.
Updated On: Jun 20, 2026
- d\(_{xy}\), d\(_{yz}\), d\(_{z^2}\)
- d\(_{yz}\), d\(_{z^2}\)
- d\(_{x^2-y^2}\), d\(_{z^2}\)
- d\(_{xz}\), d\(_{x^2-y^2}\)
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The Correct Option is C
Solution and Explanation
Step 1: Understand octahedral crystal field splitting.
In an octahedral field, ligands approach along the x, y, and z axes. This causes repulsion between ligand electron pairs and metal d-electrons, splitting the five d-orbitals into two energy levels.
Step 2: Identify orbital orientation.
Orbitals aligned directly along axes experience maximum repulsion. These are: \[ d_{x^2-y^2}, \quad d_{z^2} \] They point directly toward ligands placed along axes.
Step 3: Determine energy increase.
Due to strong repulsion with ligands, these orbitals increase in energy and form the \(e_g\) set in octahedral splitting.
Step 4: Lower energy orbitals.
Orbitals lying between axes experience less repulsion: \[ d_{xy}, d_{xz}, d_{yz} \] These form the \(t_{2g}\) set with lower energy.
Step 5: Compare options.
Only option containing orbitals pointing directly along axes corresponds to higher energy set.
Step 6: Final conclusion.
Thus, \(d_{x^2-y^2}\) and \(d_{z^2}\) are the orbitals whose energy increases.
Final Answer: \[ \boxed{d_{x^2-y^2},\ d_{z^2}} \]
In an octahedral field, ligands approach along the x, y, and z axes. This causes repulsion between ligand electron pairs and metal d-electrons, splitting the five d-orbitals into two energy levels.
Step 2: Identify orbital orientation.
Orbitals aligned directly along axes experience maximum repulsion. These are: \[ d_{x^2-y^2}, \quad d_{z^2} \] They point directly toward ligands placed along axes.
Step 3: Determine energy increase.
Due to strong repulsion with ligands, these orbitals increase in energy and form the \(e_g\) set in octahedral splitting.
Step 4: Lower energy orbitals.
Orbitals lying between axes experience less repulsion: \[ d_{xy}, d_{xz}, d_{yz} \] These form the \(t_{2g}\) set with lower energy.
Step 5: Compare options.
Only option containing orbitals pointing directly along axes corresponds to higher energy set.
Step 6: Final conclusion.
Thus, \(d_{x^2-y^2}\) and \(d_{z^2}\) are the orbitals whose energy increases.
Final Answer: \[ \boxed{d_{x^2-y^2},\ d_{z^2}} \]
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