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Revision notes on Group 7/17 The Halogens - aspects of oxidation states and redox reactions - for Advanced A/AS Level Inorganic Chemistry
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Advanced Level Inorganic Chemistry Periodic Table Revision Notes Part 9. Group 7/17 The Halogens 9.8 More on selected halogen–halide REDOX reactions A detailed description and explanation of redox reactions involving halogen molecules and halide ions. Oxidation and reduction are described in terms of electron loss/gain and oxidation state increase/decrease. Reactions covered include the reaction between sulfur dioxide/sulfite and halogens, the reaction between chlorate(V) and manganese(IV) oxide, the reaction of chlorine with hot and cold sodium hydroxide, the reaction between aqueous chlorine and potassium iodide solution, The reaction between iodate(V) and iodide ions in acidified aqueous solution, the oxidation of the chloride ion by acidified potassium manganate(VII) and the reduction of acidified dichromate(VI) with iodide ions. PLEASE NOTE KS4 Science GCSE/IGCSE/O Level GROUP 7 HALOGENS NOTES are on a separate webpage
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INORGANIC Part 9 Group 7/17 Halogens sub–index: 9.1 Introduction, trends & Group 7/17 data * 9.2 Halogen displacement reaction and reactivity trend * 9.3 Reactions of halogens with other elements * 9.4 Reaction between halide salts and conc. sulfuric acid * 9.5 Tests for halogens and halide ions * 9.6 Extraction of halogens from natural sources * 9.7 Uses of halogens & compounds * 9.8 Oxidation & Reduction – more on redox reactions of halogens & halide ions * 9.9 Volumetric analysis – titrations involving halogens or halide ions * 9.10 Ozone, CFC's and halogen organic chemistry links * 9.11 Chemical bonding in halogen compounds * 9.12 Miscellaneous aspects of halogen chemistry Advanced Level Inorganic Chemistry Periodic Table Index * Part 1 Periodic Table history * Part 2 Electron configurations, spectroscopy, hydrogen spectrum, ionisation energies * Part 3 Period 1 survey H to He * Part 4 Period 2 survey Li to Ne * Part 5 Period 3 survey Na to Ar * Part 6 Period 4 survey K to Kr and important trends down a group * Part 7 s–block Groups 1/2 Alkali Metals/Alkaline Earth Metals * Part 8 p–block Groups 3/13 to 0/18 * Part 9 Group 7/17 The Halogens * Part 10 3d block elements & Transition Metal Series * Part 11 Group & Series data & periodicity plots * All 11 Parts have their own sub–indexes near the top of the pages 9.8 Oxidation and Reduction – more on redox reactions involving halogens & halide ions See also Revision notes on Inorganic and organic REDOX reactions, oxidation state explained etc.
A more detailed discussion of some halogen–halide ion REDOX reactions See also Revision notes on Inorganic and organic REDOX reactions, oxidation state explained etc. The oxidation of iodide ions by iron(III) ions
The oxidation of iron(II) to iron(III) using chlorine
The reaction between sulphur dioxide/sulphite and halogens
The reaction between chlorate(V) and manganese(IV) oxide
The reaction of chlorine with hot and cold sodium hydroxide
The reaction between aqueous chlorine and potassium iodide solution
The reaction between iodate(V) and iodide ions in acidified aqueous solution
The oxidation of the chloride ion by acidified potassium manganate(VII)
The reduction of acidified dichromate(VI) with iodide ions
See also Revision notes on Inorganic and organic REDOX reactions, oxidation state explained etc. PLEASE NOTE KS4 Science GCSE/IGCSE/O Level GROUP 7 HALOGENS NOTES are on a separate webpage WHAT NEXT? INORGANIC Part 9 Group 7/17 Halogens sub–index: 9.1 Introduction, trends & Group 7/17 data * 9.2 Halogen displacement reaction and reactivity trend * 9.3 Reactions of halogens with other elements * 9.4 Reaction between halide salts and conc. sulfuric acid * 9.5 Tests for halogens and halide ions * 9.6 Extraction of halogens from natural sources * 9.7 Uses of halogens & compounds * 9.8 Oxidation & Reduction – more on redox reactions of halogens & halide ions * 9.9 Volumetric analysis – titrations involving halogens or halide ions * 9.10 Ozone, CFC's and halogen organic chemistry links * 9.11 Chemical bonding in halogen compounds * 9.12 Miscellaneous aspects of halogen chemistry keywords phrases formula oxidation states balanced symbol equations electrode potentials: 2Fe3+(aq) + 2I–(aq) ==> 2Fe2+(aq) + I2(aq/s) Cl2 (EØCl2/Cl– +1.36V) > Fe3+ (EØFe3+/Fe2+ +0.77V) > I2 (EØI2/I– +0.54V) 2Fe2+(aq) + Cl2(aq) ==> 2Fe3+(aq) + 2Cl–(aq) 2FeCl2(s) + Cl2(g) ==> 2FeCl3(s) SO2(aq) + Br2(aq) + 2H2O(l) ==> SO42–(aq) + 2Br–(aq) + 4H+(aq) SO2(aq) + 2H2O(l) ==> SO42–(aq) + 4H+(aq) + 2e– Br2(aq) + 2e– ==> 2Br–(aq) SO32–(aq) + Cl2(aq) + H2O(l) ==> SO42–(aq) + 2Cl–(aq) + 2H+(aq) 3MnO2 + 6OH– + ClO3– ==> 3MnO42– + 3H2O + Cl– 2NaOH(aq) + Cl2(aq) ==> NaCl(aq) + NaClO(aq) + H2O(l) 2OH–(aq) + Cl2(aq) ==> Cl–(aq) + ClO–(aq) + H2O(l) 6NaOH(aq) + 3Cl2(aq) ==> 5NaCl(aq) + NaClO3(aq) + 3H2O(l) 6OH–(aq) + 3Cl2(aq) ==> 5Cl–(aq) + ClO3–(aq) + 3H2O(l) 3NaClO(aq) ==> 2NaCl(aq) + NaClO3(aq) 3ClO–(aq) ==> 2Cl–(aq) + ClO3–(aq) NaClO(aq) + 2HCl(aq) ==> NaCl(aq) + H2O(l) + Cl2(aq/g) ClO–(aq) + Cl–(aq) + 2H+(aq) ==> H2O(l) + Cl2(aq/g) 1/2Cl2(aq) + e– ==> Cl–(aq) (EØ = +1.36 Cl2(aq) + 2e– ==> 2Cl–(aq) Cl2(aq) + 2e– ==> 2Cl–(aq) 1/2I2(aq) + e– ==> I–(aq) (EØ = +0.54V) I2(aq) + 2e– ==> 2I–(aq) IO3–(aq) + 6H+(aq) + 5e– ==> 1/2I2(aq) + 3H2O(l) IO3–(aq) + 6H+(aq) + 5I–(aq) ==> 3I2(aq) + 3H2O(l) MnO4–(aq) + 8H+(aq) + 5e– ==> Mn2+(aq) + 4H2O(l) (EØ = +1.52 2MnO4–(aq) + 16H+(aq) + 10Cl–(aq) ==> 2Mn2+(aq) + 8H2O(l) + 5Cl2(g/aq) Cr2O72–(aq) + 14H+(aq) + 6I–(aq) ==> 2Cr3+(aq) + 3I2(aq) + 7H2O(l) |
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