Catalytic Property

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Transition metals often act as catalysts because they:

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1. **Variable Oxidation States**: Because transition metals can easily shift between oxidation states ($e.g., Fe^{2+}/Fe^{3+}$), they can facilitate redox reactions by acting as electron transfer agents.
2. **Unoccupied d-orbitals**: The presence of empty or partially filled $d$-orbitals allows them to coordinate with reaction intermediates, lowering the activation energy.
3. **Surface Area (Adsorption)**: Metals like Nickel ($Ni$) and Platinum ($Pt$) provide a large surface area for **adsorption**. This increases the concentration of reactants on the catalyst surface and weakens their internal bonds.
4. **Examples**: Iron in the Haber process, $V_2O_5$ in the Contact process.

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Catalytic Property

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