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Latimer Diagrams

Latimer Diagrams. O, S, N Descriptive Chemistry. E  Red ClO4 - + 2 H + + 2 e -  ClO 3 - + H 2 O 1.19 V ClO3 - + 3 H + + 2 e -  HClO 2 + H 2 O 1.21 V HClO2 + 2 H+ + 2 e -  HClO + H 2 O 1.65 V

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Latimer Diagrams

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  1. Latimer Diagrams O, S, N Descriptive Chemistry

  2. ERed ClO4- + 2 H+ + 2 e- ClO3- + H2O 1.19 V ClO3- + 3 H+ + 2 e- HClO2 + H2O 1.21 V HClO2 + 2 H+ + 2 e- HClO + H2O 1.65 V HClO + H+ + e-1/2 Cl2(g) + H2O 1.63 V 1.19 V 1.21 V 1.65 V 1.63 V 1.36 V ClO4- ClO3- HClO2 HOCl  Cl2 Cl- | 1.47 V | Reduction   Oxidation 0.36 V 0.35 V 0.65 V 0.40 V 1.36 V ClO4- ClO3- ClO2- OCl- Cl2 Cl- | 0.88 V |

  3. Acid: 1.19 V 1.21 V 1.65 V 1.63 V 1.36 V ClO4- ClO3- HClO2 HOCl  Cl2 Cl- | 1.47 V | Basic: 0.36 V 0.35 V 0.65 V 0.40 V 1.36 V ClO4- ClO3- ClO2- OCl- Cl2 Cl- | 0.88 V |

  4. 0.36 V 0.35 V 0.65 V 0.40 V 1.36 V ClO4- ClO3- ClO2- OCl- Cl2 Cl- | 0.50 V | 0.88 V |

  5. Disproportionation of H2O2 0.69 V 1.77 V acidic solution: O2 H2O2 H2O 2 H2O2 O2 + 2 H2O E = 1.77 – 0.69 = 1.08 V • H2O2 unstable

  6. Sulfur 0.16 V 0.41 V 0.49 V 0.17 V SO42-SO2(g)S2O32-SH2S | 0.54 V 0.02 V | |S4O62-| Basic solution: -0.94 V -0.57 V -0.75 V -0.00 V -0.09 V SO42-SO32-S2O32-SS42-HS- | -0.66 V | -0.06 V | Thiosulfate, S2O32-, is unstable with respect to disproportionation Thiosulfate is made by boiling S and SO32- in slightly basic solution SO2 and SO32- are good reducing agents S42- polysulfide ions, catenation: formation of chains of identical atoms (esp. C)

  7. Nitrogen Acidic solution: 0.96 V . |0.79 V 1.12 V 1.00 V |1.59 V 1.77 V 0.27 V NO3-NO2(g)HNO2NON2ON2NH4+ |1.25 V | +5 +4 +3 +2 +1 0 -3 NO2, NO unstable with respect to disproportionation 2 NO2(g) + H2O HNO2 + H+ + NO3- Dilute solution — acid rain 3 NO2(g) + H2O NO (g) + 2 HNO3 Synthesis of nitric acid

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