Transition metals differ from s- and p-block elements in several key ways because of their partially filled d-orbitals. Here’s a explanation:
1. Electron configuration
- Transition metals: Have partially filled d-orbitals in atoms or ions.
- s-block elements: Only have s-orbitals being filled (groups 1 and 2).
- p-block elements: Have p-orbitals being filled (groups 13–18).
2. Oxidation states
- Transition metals: Show variable oxidation states (e.g., Fe²⁺, Fe³⁺).
- s-block elements: Usually show one or two oxidation states.
- p-block elements: Usually show fixed oxidation states, often following the octet rule.
3. Colored compounds
- Transition metals: Form colored compounds due to d-d electron transitions.
- s- and p-block elements: Compounds are usually colorless (except a few exceptions).
4. Magnetic properties
- Transition metals: Can be paramagnetic or diamagnetic depending on unpaired d-electrons.
- s- and p-block elements: Usually diamagnetic because they have all paired electrons.
5. Catalytic activity
- Transition metals: Often act as catalysts due to variable oxidation states and complex formation.
- s- and p-block elements: Rarely act as catalysts.
In short:
Transition metals are d-block elements with variable oxidation states, colored compounds, magnetic properties, and catalytic behavior, unlike s- and p-block elements which generally have fixed oxidation states and lack these properties.