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How do you account for the indicated mol...

How do you account for the indicated molecular geometry for the following compounds in terms of valence bond theory. `[AuCl_(4)]^(-)` - square-planar, `[Fe(CN)_(6)]^(3-)` - octahedral, `[GaCl_(4)]^(-)` tetrahedral, [`NiCl_4`] tetrahedral

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To account for the molecular geometries of the given compounds in terms of valence bond theory, we will analyze each compound step by step. ### Step 1: Analyze `[AuCl_(4)]^(-)` - Square-planar 1. **Determine the oxidation state of Gold (Au)**: In `[AuCl_(4)]^(-)`, the oxidation state of Au is +3. 2. **Electronic configuration**: The electronic configuration of Au is [Xe] 4f14 5d10 6s1. In the +3 oxidation state, it loses three electrons, resulting in a configuration of 5d8. 3. **Hybridization**: Chloride is a weak field ligand, but due to the high effective nuclear charge of Au, it causes the pairing of electrons. The orbitals involved are one d orbital, one s orbital, and two p orbitals, leading to dsp2 hybridization. 4. **Geometry**: dsp2 hybridization results in a square-planar geometry. ...
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