Groups & Periods — GCSE Chemistry Revision
Revise Groups & Periods for GCSE Chemistry. Step-by-step explanation, worked examples, common mistakes and exam-style practice aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP.
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Go to Metals, Non-Metals & Noble GasesWhat is Groups & Periods?
The periodic table is organized into vertical columns called groups and horizontal rows called periods. Elements in the same group share similar chemical properties because they have the same number of electrons in their outermost shell. The period number indicates the number of electron shells an atom has.
Board notes: All exam boards require a detailed knowledge of the properties and trends in Groups 1, 7, and 0. You should be able to describe and explain these trends.
Step-by-step explanationWorked example
Lithium, sodium, and potassium are all in Group 1. They all have one electron in their outer shell, making them highly reactive metals that readily lose one electron to form a +1 ion.
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Common mistakes
- 1Confusing the properties of elements down a group versus across a period. For example, reactivity of alkali metals increases down the group, while reactivity of halogens decreases.
- 2Forgetting the names of the key groups, such as Group 1 (alkali metals), Group 7 (halogens), and Group 0 (noble gases).
- 3Not being able to predict the properties of an element based on its position in a group or period.
Groups & Periods exam questions
Exam-style questions for Groups & Periods with mark-scheme style solutions and timing practice. Aligned to AQA, Edexcel, OCR, WJEC, Eduqas, CCEA, Cambridge International (CIE), SQA, IB, AP specifications.
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Step-by-step method
Step-by-step explanation
4 steps · Worked method for Groups & Periods
Core concept
The periodic table is organized into vertical columns called groups and horizontal rows called periods. Elements in the same group share similar chemical properties because they have the same number o…
Frequently asked questions
What are the trends in properties across a period?
Across a period, elements generally become less metallic and more non-metallic. Atomic size tends to decrease from left to right.
Why are the noble gases in Group 0 unreactive?
Noble gases have a full outer shell of electrons, which is a very stable arrangement. This makes them very unreactive and unwilling to gain, lose, or share electrons.