A conductor is a substance that allows charge or energy to flow through it easily due to the presence of delocalised electrons.

The temperature at which a substance changes from solid state to a liquid state.

A particle that enables electrical conductivity, such as delocalised electrons or free–moving ions.

When a substance's particles separate and spread throughout the particles of a solvent resulting in it no longer being seen.

The ability of a substance to dissolve in a particular solvent creating a solution; how well a solute dissolves in a solvent.

Properties of giant ionic structures

Chemistry

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 measure of how well a material conducts electricity.

A measure of how well a material transfers energy when heated.

Temperature at which a substance changes from solid to a liquid state.

A particle that enables electrical conductivity.

Match the following terms to the correct definitions.

Which of the following ionic substances is not a good electrical conductor?

In a giant ionic structure, there are strong electrostatic forces in all directions between {{}} charged particles.

A large amount of energy is needed to overcome the strong ionic bonds.

Energy is needed to overcome the electrostatic attraction between the ions.

Large amounts of energy are needed to transfer the electrons between the atoms.

Energy is needed to melt the ions to form a liquid.

Why do ionic compounds have high melting and boiling points?

Water molecules are attracted to the ions in the lattice.

The ionic forces of attraction are overcome.

A large amount of energy is needed to break the ionic bonds.

The ionic compound melts when in contact with water.

Why are most ionic compounds soluble in water?

The electrostatic attraction between magnesium ions and oxygen ions is stronger.

Sodium forms ions with a higher charge than magnesium.

Oxygen forms ions with a higher charge than chlorine.

More energy is needed to overcome the bond between sodium and chlorine ions.

Why is the melting point of magnesium oxide, MgO, higher than sodium chloride, NaCl?

The transfer of electrons between atoms to form oppositely charged ions.

The electrostatic force of attraction between oppositely charged ions

The sharing of electrons between atoms to form molecules.

A regular lattice of positive ions in a sea of delocalised electrons. 

Which of the following describes an ionic bond?

Lithium is a metal found in Group 1, Period 2 on the periodic table. What is the charge on a lithium ion?

To achieve a full outer shell of electrons.

To become electrostatically attracted to cations.

Why do non–metal atoms gain electrons to form anions?

A phosphorus atom has 15 electrons in total. How many electrons are there in the outer shell of a phosphorus atom?

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