Metallic Bonding

Theory · read, then commit

Metallic bonding occurs in metals and alloys — a regular lattice of positive metal ions surrounded by a shared sea of delocalised electrons.

1Metal atoms release their outer electrons, which become delocalised — free to move through the whole structure.

2Each atom that lost electrons is now a positive metal ion.

3The positive ions sit in a regular lattice.

4The delocalised electrons move freely between and around the ions — the 'sea of electrons'.

5Strong electrostatic attraction between the positive ions and the electron sea holds the metal together — this IS the metallic bond.

Checkpoint · quick check

Describe the structure of a metal according to the metallic bonding model.

⚠️ Common Mistake

Students often say the metallic bond is an attraction between neighbouring metal atoms. It is not between atoms: the metal atoms lose their outer electrons to become positive ions, and the bond is the strong electrostatic attraction between those positive ions and the surrounding sea of delocalised electrons. That electron sea is also why metals bend rather than shatter — the layers of ions can slide while the sea holds everything together.

🌡️High melting & boiling point

Strong forces between the many positive ions and the electron sea take a lot of energy to overcome.

⚡Conducts electricity

Delocalised electrons are free to move and carry charge through the structure.

🔥Conducts heat

The same delocalised electrons transfer thermal energy rapidly through the metal.

🔨Malleable & ductile

Layers of ions slide and the electron sea re-surrounds them, so metals bend and draw into wires without breaking.

Checkpoint · quick check

Explain why metals are good conductors of electricity.

🧱Example — why alloys are harder

In a pure metal every ion is the same size, so layers slide easily → soft.

An alloy mixes in different-sized atoms that disrupt the regular lattice.

The layers can no longer slide as easily → the alloy is harder and stronger (steel, bronze, brass).

Retrieval · Metallic Property — Structural Explanation

Test yourself · 10 questions, exam order

0 of 10 answered

Warm-up · 2 questions

Explain why steel is harder than pure iron.

Explain why metals are malleable (can be hammered into shape).

Exam standard · 4 questions

Explain why metals have high melting points.

Name the particles that are free to move in a metal.

State what is meant by an alloy.

Identify a pair of properties of metals that both result from metallic bonding.

Stretch · 4 questions

State the charge on the metal ions in the metallic bonding model.

Identify why alloys are generally harder than the pure metals they are made from.

State why metals can conduct electricity when solid, unlike ionic compounds.

Identify a correct pairing of a common alloy with the main metal it is made from.

Key note · cover it, say it, check it

Revision card · 5 steps Metallic Bonding

01Metallic bonding: positive metal ions in a lattice + sea of delocalised electrons.
02High MP/BP (strong electrostatic forces).
03Conducts electricity and heat (delocalised electrons move freely).
04Malleable/ductile (layers slide, electron sea remains).
05Alloys harder — different sized atoms disrupt regular lattice.

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