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190 Chapter 4 Stoichiometry of Chemical Reactions oxidation = reduction = loss of electrons gain of electrons In this reaction, then, sodium is oxidized and chlorine undergoes reduction. Viewed from a more active perspective, sodium functions as a reducing agent (reductant), since it provides electrons to (or reduces) chlorine. Likewise, chlorine functions as an oxidizing agent (oxidant), as it effectively removes electrons from (oxidizes) sodium. reducing agent = species that is oxidized oxidizing agent = species that is reduced Some redox processes, however, do not involve the transfer of electrons. Consider, for example, a reaction similar to the one yielding NaCl: H2(g) + Cl2(g) ⟶ 2HCl(g) The product of this reaction is a covalent compound, so transfer of electrons in the explicit sense is not involved. To clarify the similarity of this reaction to the previous one and permit an unambiguous definition of redox reactions, a property called oxidation number has been defined. The oxidation number (or oxidation state) of an element in a compound is the charge its atoms would possess if the compound was ionic. The following guidelines are used to assign oxidation numbers to each element in a molecule or ion. 1. The oxidation number of an atom in an elemental substance is zero. 2. The oxidation number of a monatomic ion is equal to the ion’s charge. 3. Oxidation numbers for common nonmetals are usually assigned as follows: • Hydrogen: +1 when combined with nonmetals, −1 when combined with metals • Oxygen: −2 in most compounds, sometimes −1 (so-called peroxides, O2 2−), very rarely − 12 (so- called superoxides, O2 −), positive values when combined with F (values vary) • Halogens: −1 for F always, −1 for other halogens except when combined with oxygen or other halogens (positive oxidation numbers in these cases, varying values) 4. The sum of oxidation numbers for all atoms in a molecule or polyatomic ion equals the charge on the molecule or ion. Note: The proper convention for reporting charge is to write the number first, followed by the sign (e.g., 2+), while oxidation number is written with the reversed sequence, sign followed by number (e.g., +2). This convention aims to emphasize the distinction between these two related properties. Example 4.5 Assigning Oxidation Numbers Follow the guidelines in this section of the text to assign oxidation numbers to all the elements in the following species: (a) H2S (b) SO3 2− (c) Na2SO4 Solution (a) According to guideline 1, the oxidation number for H is +1. This content is available for free at http://cnx.org/content/col11760/1.9PDF Image | Stoichiometry of Chemical Reactions
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