The Periodic Table: An Interactive Element Explorer
Simulation Description
This simulation is a fully interactive periodic table of all 118 elements, designed for AQA GCSE Chemistry and Physics (atomic structure, chemical properties, reactivity series, and nuclear physics topics). It replaces a static poster with a living reference tool that students can explore, search, filter, and interrogate at any point in a lesson.
The table follows the standard 18-column layout with all seven periods, the transition metal d-block, and the lanthanide and actinide f-block rows below. Each element cell shows the atomic number, symbol, full name, and atomic mass. Every cell is colour-coded by category — ten distinct colours for alkali metals (red), alkaline earth metals (orange), transition metals (amber), post-transition metals (steel blue), metalloids (teal), non-metals (cyan), halogens (violet), noble gases (pink), lanthanides (mint), and actinides (peach) — giving students an immediate visual map of the table’s structure before any text is read.
Clicking any element opens a detailed info panel at the bottom of the screen showing the element’s full name, category badge, atomic number, atomic mass, period, group, physical state at 25°C, electron configuration, and a GCSE-relevant key fact. Electron configurations include all anomalous cases: chromium shows [Ar] 3d⁵ 4s¹ (half-filled d stability), copper shows [Ar] 3d¹⁰ 4s¹ (fully-filled d stability), and palladium shows [Kr] 4d¹⁰ (unique empty 5s). Physical states are correct at 25°C — bromine and mercury are marked as liquids, gallium as solid (its melting point of 29.76°C is above 25°C but the fact card notes it melts in your hand).
The search bar (top-left) filters the table in real time by element name, symbol, or atomic number — dimming non-matching elements while keeping them visible for context. Typing “metal” highlights all metals; typing “26” jumps to iron; typing “he” finds helium.
The filter buttons (bottom strip) instantly highlight metals, non-metals, or metalloids across the entire table, dimming everything else. Students can see at a glance that metals dominate the left and centre, non-metals cluster at the top-right, and the metalloids form a diagonal staircase between them.
The 🏷 Legend toggle reveals the colour key for all ten element categories.
The table scrolls and scales to any screen — cell sizes use clamp() so it fills a 4K projector or a phone without losing legibility. The full ClassAdapt accessibility panel provides high contrast, dyslexia-friendly spacing, reading ruler, and Irlen colour overlays.
Suggested Class Activity
“Patterns in the Periodic Table” — Structure, Properties and Trends Suitable for: GCSE Chemistry Year 9/10 — Atomic structure and the periodic table. 25–30 minutes. Also useful for AQA GCSE Physics — atomic structure and nuclear topics.
Setup (2 min) Display the table on the board. Click hydrogen to show the info panel. Tell students: “Every element in the universe is on this table. By the end of today, you will be able to read it, see its patterns, and explain why it is arranged the way it is.”
Stage 1 — Reading the table (4 min) Ask students to identify from the info panel: “What four pieces of information does every element cell give you?” Target: symbol, name, atomic number, atomic mass. Ask: “What is the atomic number? What does it tell you?” Target: number of protons — unique for every element. Ask: “What pattern do you notice in atomic numbers across any row?” Target: they increase by one from left to right. Mendeleev arranged elements by atomic mass; the modern table uses atomic number.
Stage 2 — Metals, non-metals and metalloids (5 min) Press the Metals filter. Ask: “Where are the metals? Where are the non-metals?” Target: metals left and centre, non-metals top-right. Press Metalloids. Ask: “What do you notice about where the metalloids are?” Target: they form a diagonal staircase between metals and non-metals — a boundary zone. Ask students to name three metalloids from the table (boron, silicon, germanium, arsenic, antimony, tellurium, polonium). Ask: “Silicon is the basis of computer chips. Why might a metalloid be useful for electronics rather than a pure metal or non-metal?” Target: metalloids can act as both conductors and insulators, making them ideal semiconductors.
Stage 3 — Groups and periods (6 min) Click lithium (Li, group 1), then sodium (Na, group 1), then potassium (K, group 1). Ask students to read each fact card and spot what all group 1 elements have in common. Target: all react vigorously with water; all are soft, silvery metals; reactivity increases going down the group. Ask: “What does group 1 tell us about electron configuration?” Target: all have one electron in their outer shell.
Click helium, neon, and argon in turn. Ask: “Why are these called noble gases?” Target: their outer shells are full — they are unreactive and do not form compounds under normal conditions.
Ask: “Fluorine, chlorine, bromine, and iodine are all in group 17. What do they have in common?” Target: seven electrons in their outer shell; they all form singly-charged negative ions; reactivity decreases going down the group.
Stage 4 — Period trends (5 min) Ask students to look at period 3 (Na to Ar) using the filter to isolate it if helpful. Ask: “As you move across period 3 from left to right, what changes?” Target: atomic number increases by one; elements change from reactive metals (Na, Mg) through a transition zone (Al, Si) to reactive non-metals (P, S, Cl) and finish with an unreactive noble gas (Ar). Ask: “What causes this pattern?” Target: each element has one more proton and one more electron, filling the 3s and 3p orbitals across the period. When the outer shell is full, the element is unreactive.
Stage 5 — Finding elements by application (5 min) Search task — students use the search bar to find the following elements from clues, then check their info panel:
| Clue | Element | Key information to find |
|---|---|---|
| “Used in nuclear power stations as fuel” | Uranium | Atomic number, radioactive, actinide |
| “Added to water to prevent tooth decay” | Fluorine | Group 17, halogen, most electronegative |
| “Lightest metal, used in batteries” | Lithium | Group 1, period 2, alkali metal |
| “Found in haemoglobin in your blood” | Iron | Transition metal, group 8, period 4 |
| “Burns with a crimson flame in fireworks” | Strontium | Group 2, alkaline earth metal |
Students record the element’s group and period and write one sentence explaining why its position in the table matches its properties.
Adaptation notes
- For lower-confidence learners: start with the filter buttons rather than asking open questions — let students click and compare before being asked to explain; use the info panel’s category badge as a sentence starter
- For higher ability: ask why transition metals have variable oxidation states (incomplete d orbitals); ask why noble gases have full outer shells but helium only has two electrons (period 1 only has the 1s subshell)
- For SEND learners: the reading ruler supports use of the info panel; the search function removes the need to visually scan 118 cells; the colour coding provides a visual category map that does not require reading text; Irlen overlays are available in six colours for students with visual processing needs