Topic 4 of 6 · Form 5
Inorganic chemistry
Period 3 trends in atomic radius, ionisation energy, electronegativity, melting point and conductivity; reactions of elements with oxygen, chlorine and water; acid–base nature of oxides and chlorides.
Notes for this topic 1 file, in order
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Periodicity
Period 3 trends in atomic radius, ionisation energy, electronegativity, melting point and conductivity; reactions of elements with oxygen, chlorine and water; acid–base nature of oxides and chlorides.
Group 2
Reactions with water and oxygen; thermal stability of carbonates and nitrates increases down the group (cations polarise anions less); solubility of hydroxides increases and sulfates decreases down the group.
Group 17
Volatility, oxidising power of halogens decreases down the group; reducing power of halide ions increases; reactions with sulfuric acid; tests with silver nitrate and ammonia; disproportionation of chlorine in cold and hot NaOH.
Nitrogen and sulfur
Unreactivity of N₂; ammonia and ammonium ions; NOₓ pollution and catalytic converters; SO₂ and acid rain.
Transition elements
Variable oxidation states, complex ions and ligands (monodentate, bidentate, polydentate), shapes (octahedral, tetrahedral, square planar), isomerism (cis–trans, optical), colour from d-orbital splitting, ligand exchange and stability constants, catalytic behaviour, redox titrations with MnO₄⁻ and Cr₂O₇²⁻.
Worked example: In a titration, 20.0 cm³ of 0.0200 mol dm⁻³ KMnO₄ reacts with Fe²⁺. Find the moles of Fe²⁺.
n(MnO₄⁻) = 4.00 × 10⁻⁴; ratio 1 : 5 → n(Fe²⁺) = 2.00 × 10⁻³ mol
Check yourself
- Why does thermal stability of Group 2 carbonates increase down the group?
- What is a bidentate ligand?
- Give the products when chlorine reacts with cold dilute NaOH.
Show answers
- Larger cations with the same charge have lower charge density and polarise the carbonate ion less.
- A ligand that forms two dative bonds to the central ion (e.g. ethanedioate, 1,2-diaminoethane).
- NaCl, NaClO and H₂O.
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