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Quiz yourself on The Periodic TableGet your flashcardsBuild my revision planTrack my progress⚖️ Metals vs Non-metals
Exam questions on every board often ask you to compare metals and non-metals. This table covers all the key contrasts.
| Property | Metals | Non-metals |
|---|---|---|
| Position in periodic table | Left side and centre (majority of elements) | Right side (smaller group) |
| Typical structure | Giant metallic lattice | Simple molecular (usually), or giant covalent (e.g., diamond) |
| Melting / boiling point | Usually high (strong metallic bonding) | Usually low (simple molecules have weak intermolecular forces) |
| Electrical conductivity | Good — delocalised electrons carry charge | Poor — no free electrons (except graphite) |
| Thermal conductivity | Good | Poor (usually) |
| In reactions (electrons) | Lose electrons → form positive ions (e.g., Na⁺, Mg²⁺) | Gain electrons → form negative ions (e.g., Cl⁻, O²⁻) |
| Physical properties | Shiny, malleable, ductile | Brittle in solid form, dull |
| Example elements | Na, Mg, Fe, Cu, Al | C, N, O, Cl, S, P |
Exception to know: Graphite (a form of carbon, a non-metal) conducts electricity because it has delocalised electrons. It is the standard "exception" examiners use in exam questions to test your depth of understanding.
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