Redox Reactions

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Classical oxidation is the combination of an element or substance with oxygen. Examples: 1. C(s) + O₂(g) → CO₂(g) (carbon oxidation) 2. 2Mg(s) + O₂(g) → 2MgO(s) (magnesium oxidation) This definition l…

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Oxidizing Agent (Oxidant): A substance that causes oxidation of another species while itself undergoing reduction. It accepts electrons. Reducing Agent (Reductant): A substance that causes reduction …

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Modern Definitions: Oxidation: Loss of electrons by a species Example: Mg → Mg²⁺ + 2e⁻ Reduction: Gain of electrons by a species Example: Cu²⁺ + 2e⁻ → Cu Redox Reaction: Simultaneous occurrence of …

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Oxidation Number: The number of electrical charges an atom carries in a compound, assuming complete electron transfer in covalent bonds. Importance: 1. Helps identify redox reactions involving covale…

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Rule 1: Oxidation number of atoms in free state = 0 Example: H₂, O₂, Cl₂, Ca all have O.N. = 0 Rule 2: O.N. of atom in monoatomic ion = its charge Example: Na⁺ has O.N. = +1, Cl⁻ has O.N. = -1 Rule …

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Rule 5: O.N. of fluorine = -1 always; other halogens usually -1 in halides Example: HF (F = -1), NaCl (Cl = -1) Rule 6: Sum of O.N. in neutral molecule = 0 Example: In CO₂: C + 2(O) = 0, so C = +4 R…

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Given: K₂Cr₂O₇ Step 1: Assign known oxidation numbers K = +1 (alkali metal) O = -2 (standard rule) Step 2: Apply rule for neutral molecule Sum of all O.N. = 0 2(K) + 2(Cr) + 7(O) = 0 2(+1) + 2(Cr) +…

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Stock Notation: A system of representing oxidation states using Roman numerals in parentheses after the chemical symbol, named after Alfred Stock. Examples: 1. AuCl → Au(I)Cl (gold with +1 oxidation …