Physical Sciences (Level 3): should I choose it?

What will I learn?

How will I be assessed?

Progression and companion subjects

No complete companion or exclusion review is attached to this profile. Check the official course-entry conditions, language eligibility and your school’s sequence before enrolling. Links between resource hubs show related learning; they do not establish a compulsory prerequisite.

Will I find it hard?

Difficulty depends on your experience, interests, teaching and assessment. These are our reflection prompts, not an official difficulty rating.

• Look at how much data, calculation and graph interpretation appear in the sample for this particular science.
• Can you explain the ideas in your own words as well as recall the terminology?
• Do investigations and evaluating evidence interest you? Check the course’s practical requirements.

Does it scale up or down?

TASC awards and scaled TE scores are distinct. The old requirement for three final-year results was removed from 2025.

Scaling is not a measure of difficulty or a guaranteed bonus. Prioritise content you can engage with and required subjects for courses you are considering.

Try a little of the subject

Properties of atoms and nuclear reactions

The periodic table arranges elements in order of increasing atomic number, Z, which is the number of protons in the nucleus. In a neutral atom the number of electrons equals Z. In the shell model used in this course, the nucleus is surrounded by electrons in distinct energy levels, or shells. The electrons are held near the nucleus by the electrostatic attraction between the positive nucleus and the negative electrons. For elements 1 to 20 the shells fill in a simple pattern: the first shell holds at most 2 electrons, the second holds 8, and the third holds 8 before the fourth shell begins. No s, p, d or f orbital theory is needed. The layout of the table follows directly from this pattern. The period number equals the number of occupied shells, so sodium (2,8,1) is in period 3. The group is linked to the number of outer-shell (valence) electrons: group 1 atoms have one, group 2 atoms have two, group 17 atoms have seven and group 18 atoms have a full outer shell. Elements in the same group therefore have similar chemical behaviour and show gradual changes in physical properties. Atomic radius. Across a period the nuclear charge increases while electrons are added to the same shell, so the outer electrons are pulled closer and the radius decreases: a sodium atom is larger than a chlorine atom. Down a group each new period adds another occupied shell, so the radius increases: lithium is smaller than sodium, which is smaller than potassium. Valency is the number of electrons an atom typically loses, gains or shares when it bonds. Across periods 2 and 3 it rises from 1 (group 1) to 4 (group 14), then falls to 3, 2, 1 and 0 for groups 15 to 18. Ions. Atoms with one to three outer electrons tend to lose them and form positive ions; atoms with five to seven outer electrons ten

Original practice question: An atom has the shell configuration 2,8,7. Which element is it?

This is ATARMAxxing’s original sample learning material. It is not an official assessment task or a prediction of your school’s workload.

Explore the resources

Open the Physical Sciences (Level 3) subject hub and free preview (opens in a new tab)

• Physical Sciences — TCE Level 3 (opens in a new tab)

Core subject information and planning are free. Full study resources are optional.