Metallic Character
Summary: Metallic character describes how readily an element loses electrons to form positive ions. It decreases across a period (left to right) and increases down a group. Metals are on the left of the Periodic Table; non-metals on the right. Tags: igcse chemistry definition periodic-table Created: 2026-07-14 Last Updated: 2026-07-23
Metallic character refers to the extent to which an element exhibits the properties characteristic of metals — specifically, the tendency to lose electrons and form positive ions (cations).
Trend Across a Period (Left to Right)
Metallic character decreases from left to right across a period:
- Elements on the left readily lose electrons → strong metallic character
- Elements on the right tend to gain or share electrons → non-metallic character
Period 3 example: Na (most metallic) → Mg → Al → Si → P → S → Cl → Ar (non-metallic)
The transition from metallic to non-metallic character across a period is due to:
- Increasing nuclear charge (more protons)
- Electrons held more tightly
- Harder to lose electrons → less metallic
Trend Down a Group (Top to Bottom)
Metallic character increases down a group:
- Atomic radius increases → outer electrons further from nucleus
- More electron shielding from inner shells
- Electrons are held less tightly → easier to lose → more metallic
Example — Group 14: Carbon (non-metal) → Silicon (metalloid) → Germanium (metalloid) → Tin (metal) → Lead (metal)
Properties Related to Metallic Character
| Property | High Metallic Character | Low Metallic Character (Non-Metallic) |
|---|---|---|
| Oxide type | Basic | Acidic |
| Electrical conductivity | Good conductor | Poor conductor (insulator) |
| Ion formed | Positive (cation) | Negative (anion) |
| Bonding type | Metallic / ionic | Covalent |
| Appearance | Shiny, lustrous | Dull (except carbon/graphite) |
| Malleability | Malleable and ductile | Brittle (if solid) |
Amphoteric Oxides — The Borderline
Elements at the borderline between metallic and non-metallic character (e.g. aluminium, zinc) form amphoteric oxides that react with both acids and bases:
- Al₂O₃ — reacts with HCl and with NaOH
- ZnO — reacts with HCl and with NaOH
Key Facts
- Metallic character decreases across a period (left → right)
- Metallic character increases down a group (top → bottom)
- Related to how easily an element loses electrons to form positive ions
- High metallic character → basic oxides
- Low metallic character → acidic oxides
- Borderline → amphoteric oxides (Al₂O₃, ZnO)
See Also
This is a key term definition page — part of the IGCSE Chemistry (0620/0971) keyword glossary.