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Class 10 Metals and Non-metals: cheat sheet
CBSE Science. Properties of metals and non-metals, the reactivity series, how ionic compounds form, and how metals are extracted and protected.
Key ideas
- Metals are usually lustrous, malleable, ductile and good conductors. Exceptions: mercury is a liquid, sodium and potassium are soft, and graphite (a non-metal) conducts.
- Metal oxides are basic; non-metal oxides are acidic; aluminium oxide and zinc oxide are amphoteric (they react with acids and bases).
- A more reactive metal displaces a less reactive one from a solution of its salt.
- Metals above hydrogen in the reactivity series give hydrogen with dilute acids; copper, silver and gold do not.
- Metals give electrons to non-metals to form ionic compounds, which have high melting points and conduct when molten or dissolved, but not as solids.
- Extraction: sulphide ores are roasted and carbonate ores calcined to give oxides, which are reduced (by carbon, or by electrolysis for very reactive metals).
- Rusting of iron needs both air and water; it is prevented by painting, oiling, galvanising (a zinc coat) or making alloys.
Remember
| Reactivity series (most to least) | K, Na, Ca, Mg, Al, Zn, Fe, Pb, [H], Cu, Hg, Ag, Au |
| Ionic bond | Na → Na⁺ + e⁻; Cl + e⁻ → Cl⁻; together NaCl |
| Metal + water | 2Na + 2H₂O → 2NaOH + H₂ |
Watch out
- Expecting copper to react with dilute hydrochloric acid (it is below hydrogen).
- Saying ionic solids conduct electricity (only when molten or in solution).
- Calling every metal oxide basic: Al₂O₃ and ZnO are amphoteric.
Worked example
Strips of aluminium are placed in solutions of copper sulphate, lead nitrate, silver nitrate. In which will a reaction take place? Write balanced equations for the reactions.
Working: aluminium displaces only metals below it in the series
Answer: copper sulphate: 2Al + 3CuSO₄ → Al₂(SO₄)₃ + 3Cu; lead nitrate: 2Al + 3Pb(NO₃)₂ → 2Al(NO₃)₃ + 3Pb; silver nitrate: Al + 3AgNO₃ → Al(NO₃)₃ + 3Ag
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