IP Chemistry Upper Sec 08: Patterns in the Periodic Table
26 Nov 2025, 00:00 Z
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These notes align with SEAB GCE O-Level Chemistry (6092) content used in IP programmes (exams from 2026).
Status: SEAB O-Level Chemistry 6092 syllabus (exams from 2026) checked 2025-11-30 - scope unchanged; remains the reference for this note.
What you must know
- Elements arranged by increasing proton number; period number = number of shells, group number = valence electrons → common ion charge and metallic vs non-metallic character.
- Across a period: metallic to non-metallic; basic oxides → amphoteric → acidic; ionic → giant covalent → simple molecular structures.
- Group 1: soft, low density, mp decreases down group; react with water to form hydroxide + hydrogen (fizzing, floats, lilac flame for K). Down the group reactivity increases.
- Group 17: coloured diatomic molecules (F₂ pale yellow gas, Cl₂ greenish-yellow gas, Br₂ red-brown liquid, I₂ purple solid); reactivity decreases down group; halogen displacement reactions follow reactivity.
- Group 18: full valence shell → very unreactive; uses for inert atmosphere (argon in lamps, helium in balloons).
- Transition elements: higher mp/density than Group 1, variable oxidation states, coloured compounds/ions, good catalysts (Fe in Haber, Ni in hydrogenation).
- Reactivity series: K, Na, Ca, Mg, Al, Zn, Fe, Pb, H, Cu, Ag; predict reactions with water/steam/acid, displacement, reduction of oxides, thermal stability of carbonates (Group 1 most stable).
- Rusting of iron requires oxygen + water; accelerated by salts/acids. Prevention: barrier (paint/oil/plastic), galvanising, sacrificial protection (Mg/Zn).
Detailed notes
- Across a period: increasing nuclear charge with similar shielding → atomic radius decreases, ionisation energy generally rises; metallic to non-metallic character decreases; oxides shift basic → amphoteric → acidic. Structures: metals (Na–Al) metallic, Si giant covalent, P/S/Cl simple molecular, Ar monoatomic.
- Period 3 oxide/chloride behaviour:
