Interactive periodic table matching the exact format given in GCSE exams. Click any element for details. Download as PDF for offline revision.
Use the number at the bottom of each element box to calculate relative formula mass (Mr) for compounds.
The group number tells you the number of outer shell electrons (except transition metals).
Group 1 metals get more reactive down the group. Halogens get less reactive down Group 7.
Found in the middle of the table. They have high melting points and can form coloured compounds.
Yes, a periodic table is provided in all GCSE Chemistry exams (AQA, Edexcel, and OCR). The table includes atomic numbers, element symbols, and relative atomic masses. However, you should still be familiar with common elements and their positions to use the table efficiently.
The GCSE periodic table shows: atomic (proton) number, element symbol, and relative atomic mass for each element. The atomic number tells you the number of protons (and electrons in a neutral atom), while the relative atomic mass is used for calculating masses in reactions.
Key groups include: Group 1 (Alkali Metals - Li, Na, K) which are highly reactive, Group 7 (Halogens - F, Cl, Br, I) which are reactive non-metals, and Group 0 (Noble Gases - He, Ne, Ar) which are unreactive. You also need to know about Transition Metals in the middle of the table.
Relative atomic mass (Ar) is shown at the bottom of each element box. To find the relative formula mass (Mr) of a compound, add up the Ar values of all atoms. For example, H₂O has Mr = (2 × 1) + 16 = 18. This is essential for mole calculations and reacting mass problems.
Atomic number is the number of protons in an atom's nucleus and determines which element it is. Mass number is protons plus neutrons. The periodic table shows atomic number and relative atomic mass (a weighted average of isotopes), not mass number.
While the periodic table is given, you should know common element symbols (H, C, N, O, Na, Cl, Fe, Cu, etc.) and the first 20 elements to quickly find them. You don't need to memorise relative atomic masses as these are provided.
Elements in the same group (vertical column) have the same number of outer shell electrons, giving them similar chemical properties. Elements in the same period (horizontal row) have the same number of electron shells. This pattern was discovered by Mendeleev.
Transition metals (middle of the table) have special properties: high melting points, high density, can form coloured compounds, can act as catalysts, and can have variable oxidation states. Common examples include iron, copper, and zinc.
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