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Chapter 4 Stoichiometry of Chemical Reactions 191 Using this oxidation number and the compound’s formula, guideline 4 may then be used to calculate the oxidation number for sulfur: charge on H2 S = 0 = (2 × +1) + (1 × x) x = 0 − (2 × +1) = −2 (b) Guideline 3 suggests the oxidation number for oxygen is −2. Using this oxidation number and the ion’s formula, guideline 4 may then be used to calculate the oxidation number for sulfur: charge on SO3 2− = −2 = (3 × −1) + (1 × x) x = −2 − (3 × −2) = +4 (c) For ionic compounds, it’s convenient to assign oxidation numbers for the cation and anion separately. According to guideline 2, the oxidation number for sodium is +1. Assuming the usual oxidation number for oxygen (−2 per guideline 3), the oxidation number for sulfur is calculated as directed by guideline 4: charge on SO4 2− = −2 = (4 × −2) + (1 × x) x = −2 − (4 × −2) = +6 Check Your Learning Assign oxidation states to the elements whose atoms are underlined in each of the following compounds or ions: (a) KNO3 (b) AlH3 (c) N_H4+ (d) H2P_O4− Answer: (a) N, +5; (b) Al, +3; (c) N, −3; (d) P, +5 Using the oxidation number concept, an all-inclusive definition of redox reaction has been established. Oxidation- reduction (redox) reactions are those in which one or more elements involved undergo a change in oxidation number. (While the vast majority of redox reactions involve changes in oxidation number for two or more elements, a few interesting exceptions to this rule do exist Example 4.6.) Definitions for the complementary processes of this reaction class are correspondingly revised as shown here: oxidation = increase in oxidation number reduction = decrease in oxidation number Returning to the reactions used to introduce this topic, they may now both be identified as redox processes. In the reaction between sodium and chlorine to yield sodium chloride, sodium is oxidized (its oxidation number increases from 0 in Na to +1 in NaCl) and chlorine is reduced (its oxidation number decreases from 0 in Cl2 to −1 in NaCl). In the reaction between molecular hydrogen and chlorine, hydrogen is oxidized (its oxidation number increases from 0 in H2 to +1 in HCl) and chlorine is reduced (its oxidation number decreases from 0 in Cl2 to −1 in HCl). Several subclasses of redox reactions are recognized, including combustion reactions in which the reductant (also called a fuel) and oxidant (often, but not necessarily, molecular oxygen) react vigorously and produce significant amounts of heat, and often light, in the form of a flame. Solid rocket-fuel reactions such as the one depicted in FigurePDF Image | Stoichiometry of Chemical Reactions
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