A mixture of two or more elements, where at least one element is a metal.

An alloy of iron that contains specific amounts of carbon and may contain other metals.

A substance that has the ability to break up easily.

Alloys and their properties

Chemistry

Why chemical reactions occur

Metallic structure and properties

Metal alloys

Forming ions for ionic bonding (RAM 1 d.p.)

Giant ionic structures

Determining ionic formulae

Ionic diagrams for binary ionic substances

Properties of giant ionic structures

Forming covalent bonds

Properties of covalent substances

Bonding models

In the Chemistry of Carbon unit, pupils will build on their understanding of chemical bonding to explore the unique properties and bonding of carbon, leading to various natural and synthetic organic compounds.

In the Atomic Structure and the Periodic Table unit, pupils learned about the model of the atom, isotopes, and the arrangement of elements in the periodic table.

This unit explores changes of state, particle kinetics, and energy transfers in relation to chemical bonding, including ionic, covalent, and metallic bonds. It examines carbon's unique bonding properties, leading to organic compounds and materials like diamond, graphite, fullerenes, and graphene.

Structure and bonding

Match the following terms to the correct definition.

Which two metals are found in the alloy bronze?

Steel is more resistant to corrosion than pure iron.

Which of the following statements about steel are correct?

Which of the following are examples of alloys?

A 0.500 kg piece of copper alloy contains 27% aluminium. What mass of aluminium does it contain? Give your answer to three significant figures.

There are different sized ions in the structure.

There are delocalised electrons in the structure.

The bonds between the ions and electrons are weaker.

Why do metal alloys usually have lower melting points than the metals they are made from?

Which of the following best describes an alloy?

Metallic bonding consists of metal ions in a 'sea' of {{}}.

Metal ions are arranged in layers that can slide over one another.

Delocalised electrons are free to move through the metal.

Strong electrostatic attraction between metal ions and delocalised electrons.

Is this statement true or false? Pure metals are generally more malleable than their alloy counterparts.

What is 25% of 50.0? Give your answer to 3 significant figures.

Alloys and their properties

Lesson outcome