An atom of an element with the same number of protons, but different mass numbers due to different numbers of neutrons.

A subatomic particle found in the nucleus with a relative mass of 1 and a positive charge (+1).

A subatomic particle found in the nucleus with a relative mass of 1 and no charge.

is the total number of protons and neutrons in the nucleus of an atom.

Isotopes

Chemistry

Atomic structure (negligible electron mass)

Developing a model for atoms

Atoms, elements and compounds

Modern periodic table and electron configuration

Using the periodic table: atomic and mass number

Relative formula mass

Development of the periodic table

In the Structure and Bonding unit, pupils will build on their understanding of atomic structure to explore different types of chemical bonding and how these bonds affect the properties of substances.

In the Atoms, Elements and Compounds unit, pupils learned about the differences between atoms, elements, and compounds, as well as their chemical symbols and formulae.

This unit covers the atomic model, relative atomic mass, isotopes, and the structure of the modern periodic table. It explains how atomic structure influences element positioning, properties, and reactivity. The focus is on identifying trends and using models to develop scientific explanations.

Atomic structure and the periodic table

Depiction or discussion of famine, disease, natural disasters.

Depiction or discussion of violence or suffering

subatomic particles with a mass of 1 and a positive charge

total number of protons and neutrons in an atom

atoms of an element with different number of neutrons

subatomic particles with a mass of 1 and no charge

The word 'abundance' is used to show the proportion of atoms of an element which are a particular isotope. It is often shown as a {{}}. 

They are determined from the isotopes of the elements. 

Why do chlorine and copper have relative atomic masses which are not whole numbers i.e. 35.5Cl and 63.5Cu?

Yes, as they have the same number of protons and a different number of neutrons

No, as they have a different number of neutrons

Yes, as they have the same number of electrons

Yes, as they have different number of neutrons

No, as they have the same number of protons and electrons

Will the isotopes of hydrogen H-1, H-2 and H-3 have the same chemical properties? Select the correct answer to explain why or why not.

Match the isotopes to the number of neutrons. Use your periodic table to help.

Many isotopes are radioactive and can be used for medical purposes, however their abundance is very low. Calculate the abundance of Cr-50 when Cr-52 is 84.0%, Cr-53 is 9.5% and Cr-54 is 2.5%.

Which two subatomic particles are present in the nucleus of an atom?

number of protons = atomic number or proton number, for sodium = 11

number of electrons = same as the number of protons, for sodium = 11

mass number = total number of protons + neutrons

number of neutrons = mass number - number of protons, for sodium: 23 - 11 = 12

Order the method for working out the number of the three subatomic particles in an atom of sodium. Start with the number of protons, then work out the number of electrons, then finally neutrons.

Match the atoms with the number of neutrons in their nucleus. Use your periodic table to help.

This is a mistake as they should all be the same.

³⁵Cl has 18 protons and ³⁷Cl has 20 protons.

³⁷Cl has gained two electrons to get a full outer shell.

³⁵Cl has 18 neutrons and ³⁷Cl has 20 protons.

³⁵Cl has 18 neutrons and ³⁷Cl has 20 neutrons.

Chlorine atoms mainly exist as ³⁵Cl and ³⁷Cl. Why are the mass numbers different?

Isotopes

Lesson outcome

Content guidance