Explain d3s hybridization in detail and also compounds which show this. Is d3s hybridization possible? Please explain how.

d3s hybridization is a type of coordinate covalent bonding concept in coordination chemistry involving the mixing of one s orbital and three d orbitals in a central atom to form four equivalent hybrid orbitals. This allows the central atom to bond with ligands in a specific geometry.

In d3s hybridization, the orbitals involved are the s orbital (usually the 4s) and three d orbitals (typically 3dxy, 3dyz, 3dzx). These hybrid orbitals arrange themselves spatially to maximize bonding and minimize repulsion, potentially resulting in square planar or tetrahedral geometries.

This hybridization is observed in complexes where the central atom uses d orbitals from the penultimate shell and s orbital from the outermost shell for bonding, usually found in transition metal complexes with higher oxidation states or special ligand fields.

Examples of compounds showing d3s hybridization include chromium in chromyl chloride (CrO2Cl2) and manganese in potassium manganate (K2MnO4). In these compounds, the central metallic atom forms hybrid orbitals by mixing d and s orbitals to bond with surrounding atoms or ligands efficiently. The hybrid orbitals accommodate bonding electrons and explain molecular shapes and bonding patterns observed experimentally.

The possibility of d3s hybridization arises because transition metals have accessible d orbitals that can mix with s orbitals under appropriate electronic and geometric conditions. The process involves promotion and rearrangement of electrons to allow maximum bonding capacity, making d3s hybridization feasible.