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Redox Reactions

Redox Reactions. Objectives: Reduction/Oxidation Oxidation Number Oxidizing and Reducing Reagents. 2M g 2M g 2+ + 4 e -. O 2 + 4 e - 2O 2-. Redox (Oxidation-Reduction) Reaction : Type of electron transfer reaction. One substance gives up electrons;

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Redox Reactions

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  1. Redox Reactions Objectives: • Reduction/Oxidation • Oxidation Number • Oxidizing and Reducing Reagents

  2. 2Mg 2Mg2+ + 4e- O2 + 4e- 2O2- Redox (Oxidation-Reduction) Reaction: Type of electron transfer reaction. One substance gives up electrons; the other accepts electrons. OIL RIG • Oxidation Half-Reaction;Oxidation Involves Loss of electrons • Reduction Half-Reaction;Reduction Involves Gain of electrons Net Redox Rxn; 2Mg + O2 -> 2 Mg+2 + 2 O-2

  3. Oxidation number The charge the atom would have in a molecule (or an ionic compound) if electrons were completely transferred to the more electronegative atom. • Oxidation number equals ionic charge for monoatomic ions in ionic compound CaBr2; Ca = +2, Br = -1 2. Metal ions in Family A have one, positive oxidation number; Group IA metals are +1, IIA metals are +2 Li+, Li = +1; Mg+2, Mg = +2 4.4

  4. Oxidation number,continued The charge the atom would have in a molecule (or an ionic compound) if electrons were completely transferred to the more electronegative atom. 3. The oxidation number of a transition metal ion is positive, but can vary in magnitude. • Nonmetals can have a variety of oxidation numbers,both positive and negative numbers which can vary in magnitude. 5. Free elements (uncombined state) have an oxidation number of zero. Each atom in O2, F2, H2, Cl2, K, Be has the same oxidation number; zero. 4.4

  5. 6. The oxidation number of fluorine is always–1. (unless fluorine is in elemental form, F2) • 7. The sum of the oxidation numbers of all the atoms in a molecule or ion is equal to the charge on the molecule or ion. IF; F= -1; I = +1 8. The oxidation number of hydrogen is +1except when it is bonded to metals in binary compounds. In these cases, its oxidation number is –1or when it’s in elemental form (H2; oxidation # =0). HF; F= -1, H= +1 NaH; Na= +1, H = -1

  6. Oxidation numbers of all the atoms in HCO3- ? 9. The oxidation number of oxygen is usually–2. In H2O2 and O22- it is –1, in elemental form (O2 or O3) it is 0. H2O ; H=+1, O= -2 SO3; O = -2; S = +6 HCO3- O = -2 H = +1 3x(-2) + 1 + ? = -1 C = +4 4.4

  7. Oxidation numbers of all the elements in the following ? IF7 F = -1 7x(-1) + ? = 0 I = +7 K2Cr2O7 NaIO3 O = -2 K = +1 O = -2 Na = +1 3x(-2) + 1 + ? = 0 7x(-2) + 2x(+1) + 2x(?) = 0 I = +5 Cr = +6 4.4

  8. Determination of Oxidizing and Reducing Agents • Determine oxidation # for all atoms in both the reactants and products. • Look at same atom in reactants and products and see if oxidation # increased or decreased. • If oxidation # decreased; substance reduced • If oxidation # increased; substance oxidized

  9. Determination of Oxidizing and Reducing Agents, continued • Oxidizing Agent: Substance that oxidizes the other substance by accepting electrons. It is reduced in reaction. • Reducing Agent: Substance that reduces the other substance by donating electrons. It is oxidized in reaction.

  10. Spontaneous Redox ReactionZn(s) + Cu+2 (aq) -> Cu(s) + Zn+2(aq) Zn Cu time Zn+2 Cu+2

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