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Class 10 · Chapter 3 · Chemistry

Metals and Non‑metals Cheat Sheet

Reactions

Reaction with oxygen (combustion)

2 Mg+OX2→2 MgO\ce{2Mg + O2 -> 2MgO}

Magnesium burns in air with a dazzling white flame to form white magnesium oxide.

Sodium with oxygen

4 Na+OX2→2 NaX2O\ce{4Na + O2 -> 2Na2O}

Sodium is so reactive that it is stored under kerosene to keep it from air and moisture.

Aluminium with oxygen

4 Al+3 OX2→2 AlX2OX3\ce{4Al + 3O2 -> 2Al2O3}

A layer of aluminium oxide protects the metal from further oxidation.

Copper with oxygen

2 Cu+OX2→Δ2 CuO\ce{2Cu + O2 ->[\Delta] 2CuO}

On heating, brown copper is coated with black copper oxide.

Sodium with water

2 Na+2 HX2O→2 NaOH+HX2↑\ce{2Na + 2H2O -> 2NaOH + H2 ^}

The reaction is so vigorous that the hydrogen gas catches fire.

Calcium with water

Ca+2 HX2O→Ca(OH)X2+HX2↑\ce{Ca + 2H2O -> Ca(OH)2 + H2 ^}

Calcium reacts less violently; bubbles of hydrogen stick to the metal.

Iron with steam

3 Fe+4 HX2O→FeX3OX4+4 HX2↑\ce{3Fe + 4H2O -> Fe3O4 + 4H2 ^}

Iron reacts with steam, not with cold or hot water.

Magnesium with dilute acid

Mg+2 HCl→MgClX2+HX2↑\ce{Mg + 2HCl -> MgCl2 + H2 ^}

Metals above hydrogen in the reactivity series displace hydrogen from dilute acids.

Amphoteric oxide with acid

AlX2OX3+6 HCl→2 AlClX3+3 HX2O\ce{Al2O3 + 6HCl -> 2AlCl3 + 3H2O}

Aluminium oxide reacts with both acids and bases, so it is amphoteric.

Amphoteric oxide with base

AlX2OX3+2 NaOH→2 NaAlOX2+HX2O\ce{Al2O3 + 2NaOH -> 2NaAlO2 + H2O}

The same oxide (Al₂O₃) also reacts with a base to give sodium aluminate.

Thermit reaction

FeX2OX3+2 Al→2 Fe+AlX2OX3\ce{Fe2O3 + 2Al -> 2Fe + Al2O3}

Aluminium reduces iron oxide with the release of a large amount of heat; used to join railway tracks.

Displacement of manganese

3 MnOX2+4 Al→3 Mn+2 AlX2OX3\ce{3MnO2 + 4Al -> 3Mn + 2Al2O3}

Aluminium displaces manganese because it is more reactive.

Roasting of zinc sulphide

2 ZnS+3 OX2→2 ZnO+2 SOX2\ce{2ZnS + 3O2 -> 2ZnO + 2SO2}

Sulphide ores are roasted (heated in air) to give the metal oxide.

Calcination of limestone

CaCOX3→ΔCaO+COX2\ce{CaCO3 ->[\Delta] CaO + CO2}

Carbonate ores are calcined (heated strongly) to give the metal oxide.

Reduction of zinc oxide

ZnO+C→Zn+CO\ce{ZnO + C -> Zn + CO}

The metal oxide is reduced to the metal using carbon as the reducing agent.

Extraction of iron (blast furnace)

FeX2OX3+3 CO→2 Fe+3 COX2\ce{Fe2O3 + 3CO -> 2Fe + 3CO2}

Carbon monoxide reduces haematite to give molten iron.

Definitions

Metal
An element that is generally hard, lustrous, malleable, ductile and a good conductor of heat and electricity.
Non-metal
An element that is generally soft, dull, brittle and a poor conductor of heat and electricity.
Malleability
The property of a metal by which it can be beaten into thin sheets.
Ductility
The property of a metal by which it can be drawn into thin wires.
Sonorous
The property of a metal to produce a ringing sound when struck.
Amphoteric oxide
A metal oxide that reacts with both acids and bases; e.g. Al₂O₃, ZnO.
Alloy
A homogeneous mixture of a metal with one or more other metals or non-metals; e.g. brass.
Corrosion
The wearing away of a metal surface by the action of air, moisture or chemicals.
Galvanisation
Coating iron or steel with a thin layer of zinc to prevent rusting.
Anodising
Making a thick, protective oxide layer on aluminium by electrolysis.
Ore
A mineral from which a metal can be extracted profitably.
Gangue
The unwanted impurities such as sand and clay present in an ore.
Roasting
Heating a sulphide ore strongly in the presence of air to convert it into its oxide.
Calcination
Heating a carbonate ore strongly in the absence of air to convert it into its oxide.
Ionic bond
The bond formed by the transfer of electrons from a metal to a non-metal.
Aqua regia
A mixture of 3 parts concentrated HCl and 1 part concentrated HNO₃, which can dissolve gold.

Key Points

  • Physical properties of metals: lustre, malleability, ductility, sonority, good conduction of heat and electricity, high melting and boiling points.
  • Exceptions: mercury is a liquid metal; gallium melts on the palm; graphite (a non-metal) conducts electricity; iodine is lustrous.
  • Reactivity series: K > Na > Ca > Mg > Al > Zn > Fe > Pb > (H) > Cu > Hg > Ag > Au.
  • Metals above hydrogen displace hydrogen from dilute acids; metals below it do not.
  • Ionic compounds have high melting and boiling points, are soluble in water and conduct electricity in molten or aqueous state.
  • Extraction of metals: concentration of ore → roasting/calcination → reduction → refining (electrolytic).
  • Corrosion is prevented by painting, oiling, greasing, galvanisation and anodising.
  • Alloys: brass (Cu + Zn), bronze (Cu + Sn), solder (Pb + Sn), amalgam (metal + Hg); steel is iron with carbon.