Topic 7 of 8 · Form 3
The Periodic Table and metals
Elements arranged by proton number; groups have the same number of outer electrons. Metallic character decreases across a period.
Notes for this topic 1 file, in order
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Periodic trends
Elements arranged by proton number; groups have the same number of outer electrons. Metallic character decreases across a period.
- Group I: reactivity increases down the group; reactions with water.
- Group VII: colour darkens and reactivity decreases down the group; displacement reactions.
- Transition elements: high density and melting point, coloured compounds, variable oxidation states, catalysts.
- Noble gases: unreactive; uses.
Metals
Properties; alloys (brass, stainless steel) and why they are harder; reactivity series (K, Na, Ca, Mg, Al, C, Zn, Fe, H, Cu, Ag, Au); displacement and reactions with water, steam and acids.
Extraction
- Iron in the blast furnace: coke, haematite, limestone; slag formation.
- Aluminium by electrolysis.
- Zinc from zinc blende.
Corrosion
Rusting needs water and oxygen; prevention by barrier methods and sacrificial protection (galvanising).
Exam tip: Predict extraction methods from position in the reactivity series relative to carbon.
Check yourself
- Why are alloys harder than pure metals?
- State two properties of transition elements.
- Why is zinc used to galvanise iron?
Show answers
- Different-sized atoms disrupt the layers, making it harder for them to slide.
- Any two: coloured compounds, variable oxidation states, catalytic activity, high melting points and density.
- It forms a barrier and, being more reactive, corrodes in preference to iron (sacrificial protection).
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