Group Trends and Transition Metals
Properties and trends in Groups 1, 7 and 0, displacement reasoning, and the characteristic behaviour of transition metals.
How to study for GCSE Chemistry
Move between particle models, equations, calculations, observations and data; practise the specific required activities and paper structure named by your exam board.
Core concepts
Concept 1
Group 1 metals become more reactive down the group because the outer electron is lost more readily, while Group 7 non-metals become less reactive as gaining an electron becomes harder.
Exam cue: Explain a reactivity trend through electron arrangement, shielding and attraction rather than merely restating it.
Concept 2
Group 0 elements have stable outer shells and low reactivity; their boiling points rise down the group as intermolecular attractions become stronger.
Exam cue: Use relative reactivity to predict whether a displacement reaction occurs.
Concept 3
Transition metals commonly have high densities and melting points, form coloured ions with different charges and act as catalysts, while generally being less reactive than Group 1 metals.
Exam cue: Identify when a property belongs to transition metals generally and when a particular example is required.
Risk pitfalls and guardrails
Reversing the trends in Group 1 and Group 7.
Guardrail: Do not rely on a memorised keyword alone: preserve charges, ratios, units and conditions, and keep single Chemistry separate from Combined Science.
Explaining Group 0 boiling points through chemical reactivity.
Guardrail: Do not rely on a memorised keyword alone: preserve charges, ratios, units and conditions, and keep single Chemistry separate from Combined Science.
Assuming every transition-metal compound has the same colour or ion charge.
Guardrail: Do not rely on a memorised keyword alone: preserve charges, ratios, units and conditions, and keep single Chemistry separate from Combined Science.
Memory anchors
Group 1 trend
Reactivity increases down the group as the outer electron is lost more easily.
Group 7 trend
Reactivity decreases down the group as attracting an extra electron becomes harder.
Halogen displacement
A more reactive halogen displaces a less reactive halide from solution.
Group 0
Full outer shells make the noble gases very unreactive.
Transition metals
Dense metals that often form coloured ions, variable charges and useful catalysts.
Checkpoint rule
Do the check-up only after you can summarize each concept in one sentence and identify one dangerous pitfall from memory.
Knowledge Check (after reading)
Short check-up to confirm understanding of this module.
Check-up Questions
How does Group 1 reactivity change down the group?
Why does potassium react more vigorously with water than lithium?
Answer all questions to submit.
Next step personalized recommendations
Continue learning
Move forward only after this module is stable.
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