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

A physical property is a characteristic of a substance that can be observed or measured. For example, the temperature at which a substance melts.

Electrons are said to be delocalised when they are free to move through the structure of a metal and can carry an electrical current.

Molten is the term used to describe a liquid substance formed by heating solid metals, glass, or rocks.

Metal alloys

Chemistry

Why chemical reactions happen

Metallic structure and properties

Alloys and their properties

Forming ions for ionic bonding

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

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

Negatively charged particle free to move through the metal structure.

A liquid substance formed by heating solid metal, glass or rocks.

A characteristic of a substance that can be observed or measured.

Match the following key terms to their definitions.

A metallic bond is a strong electrostatic force of attraction between the positively charged {{}} and the delocalised electrons in a metal.

True or false? Alloys have a disrupted or irregular lattice structure.

Most alloys are more ductile than pure metals.

Most alloys are less malleable than pure metals.

Alloys and pure metals are both good electrical conductors.

Which of the following statements about pure metals and alloys are correct?

Lithium atoms gain one electron to form lithium ions.

Aluminium ions and lithium ions are the same size.

Aluminium contains more delocalised electrons per ion than lithium.

Aluminium atoms lose three electrons to form aluminium ions.

Aluminium atoms form Al³⁺ ions and lithium atoms form Li⁺ ions. 
Which of the following statements about aluminium and lithium ions are correct?

The melting point of a substance is an example of a {{}} property.

Which of the following diagrams models the arrangement of particles in a metal?

Which of the following are common physical properties of metals?

Ions are arranged in layers that can easily slide over each other.

Ions are surrounded by a 'sea' of delocalised electrons.

Strong electrostatic attraction between ions (+) and electrons (–).

Match the following physical properties of metals with the corresponding reasons for each property.

Metallic structures consist of {{}} surrounded by __________.

Which force of attraction binds together the particles in a giant metallic structure?

they can be hammered into shape without breaking.

the layers of metal ions can easily slide over each other.

Metal alloys

Lesson outcome