Most elements are METALS — they are found on the left and in the centre of the periodic table.
Typical physical properties of metals:
GOOD CONDUCTORS of electricity and heat — delocalised electrons carry charge and energy.
HIGH MELTING AND BOILING POINTS — strong metallic bonds.
SHINY (lustrous) appearance when cut or polished.
MALLEABLE — can be hammered into sheets without breaking.
DUCTILE — can be drawn into wires.
SOLID at room temperature — except mercury (Hg), which is a liquid.
HIGH DENSITY in most cases.
Chemical properties of metals:
FORM POSITIVE IONS — lose outer electrons in reactions.
REACT with oxygen to form METAL OXIDES (these are BASIC — they neutralise acids).
Many react with water and acids to produce hydrogen gas.
Properties of Non-metals
NON-METALS are found on the right side of the periodic table.
Typical physical properties of non-metals:
POOR CONDUCTORS of electricity (except graphite and graphene).
LOW MELTING AND BOILING POINTS — weak forces between molecules.
BRITTLE when solid — cannot be bent or drawn into wires.
Low density generally.
Many are GASES at room temperature (O₂, N₂, Cl₂, H₂, etc.).
Some are SOLIDS (carbon, sulfur, phosphorus, iodine).
Bromine (Br₂) is a liquid at room temperature.
Chemical properties of non-metals:
FORM NEGATIVE IONS — gain electrons (or share in covalent bonds).
REACT with oxygen to form NON-METAL OXIDES (these are ACIDIC — they dissolve in water to form acids).
Key Differences — Metals vs Non-metals
A useful comparison table:
Electrical conductivity:
METAL: Good conductor (delocalised electrons).
NON-METAL: Poor conductor (no free electrons) — EXCEPT graphite.
Melting/boiling point:
METAL: Generally high — strong metallic bonds.
NON-METAL: Generally low — weak intermolecular forces.
Malleability/ductility:
METAL: Malleable and ductile.
NON-METAL: Brittle.
Ion formation:
METAL: Forms POSITIVE ions (loses electrons).
NON-METAL: Forms NEGATIVE ions (gains electrons).
Oxide type:
METAL: Basic oxides (e.g. MgO, Fe₂O₃).
NON-METAL: Acidic oxides (e.g. CO₂, SO₂, NO₂).
Some elements (like silicon) are METALLOIDS — they have properties between metals and non-metals. Silicon conducts electricity but is brittle — it is a semiconductor, used in electronics.
⚠️ Common Mistake
Graphite and graphene are non-metals that conduct electricity — they are exceptions. Most non-metals do not conduct, but graphite has delocalised electrons between its layers. Don't say 'all non-metals don't conduct' — say 'non-metals generally don't conduct, except graphite and graphene'.
📌 Key Note
Metals: good conductors, high melting points, malleable, ductile, form positive ions, basic oxides. Non-metals: poor conductors (except graphite), low melting points, brittle, form negative ions, acidic oxides. Metallic character decreases across a period and increases down a group.
🎯 Matching Activity — Metal or Non-metal Property?
Sort each property into metals or non-metals. — drag the symbols on the right to match the component names on the left.
Metal
Drop here
Non-metal
Drop here
Metal
Drop here
Non-metal
Drop here
Metal
Drop here
Non-metal
Drop here
Forms acidic oxides — e.g. CO₂ dissolves in water to form carbonic acid
Malleable — can be hammered into sheets without shattering
Poor conductor of electricity — no free electrons (except graphite)
Forms positive ions by losing electrons in reactions
Good conductor of electricity — delocalised electrons carry charge
Brittle solid — shatters when struck
🎯 Test Yourself
Question 1 of 2
1. Why are metals good conductors of electricity?
2. Sulfur dioxide (SO₂) dissolves in water to form an acidic solution. Is sulfur a metal or non-metal?
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