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Balancing Oxidation-Reduction Reactions Any reaction involving the transfer of electrons is an oxidation-reduction (or redox) reaction Definitions: Oxidation is the loss of electrons. Reduction is the gain of electrons. Oxidation cannot take place without reduction. During a redox reaction, the oxidation numbers of reactants will change. For any equation to be balanced: 1. The number of atoms of each type on the left side of the arrow must equal the number of atoms of each type to the right of the arrow. 2. The total charges of all the ions on the left side of the arrow must equal the total charges of all the ions to the right of the arrow. Balancing Oxidation-Reduction Reactions: 2. Write ‘bare bones’ half reactions. Include only the atom, ion or element that changes oxidation number. Cr+6 + 3e- Cr+3 C+3 C+4 + 1e- Remember that each half reaction must also be balanced for charge. The total charges on the left must equal the total charges on the right. Redox Stoichiometry Calculations involving concentrations and redox reactions are quite common. Many ores containing metals are analyzed using redox titrations. Since many compounds change color as they are oxidized or reduced, one of the reactants may serve as the indicator in the titration.Redox Stoichiometry The concentration of iron(II) can be determined by titration with bromate ion, in acid. The products are iron(III) ion and the bromide ion. What is the concentration of iron(II) ion if 31.50 mL of 0.105M potassium bromate is required to completely react with 10.00 mL of the iron solution. Redox Stoichiometry The concentration of iron(II) can be determined by titration with bromate ion, in acid. The products are iron(III) ion and the bromide ion. 1. Write the balanced chemical reaction. Fe2+(aq) + BrO31-(aq) Fe3+(aq) + Br1-(aq) Balancing Oxidation-Reduction Reactions: Assign oxidation numbers to every atom in the reaction. Cr2O72- + C2O42- Cr3+ + COAn oxidation-reduction (redox) reaction is a type of chemical reaction that involves a transfer of electrons between two species. An oxidation-reduction reaction is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron. Redox reactions are common and vital to some of the basic functions of life, including photosynthesis, respiration, combustion, and corrosion or rusting. Rules for Assigning Oxidation States The oxidation state (OS) of an element corresponds to the number of electrons, e-, that an atom loses, gains, or appears to use when joining with other atoms in compounds. In determining the oxidation state of an atom, there are seven guidelines to follow: The oxidation state of an individual atom is 0. The total oxidation state of all atoms in: a neutral species is 0 and in an ion is equal to the ion charge. Group 1 metals have an oxidation state of +1 and Group 2 an oxidation state of +2 The oxidation state of fluorine is -1 in com
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