1. Chemical Formulas and Compounds Oxidation Numbers

2. Objective List the rules for assigning oxidation numbers Give the oxidation number for each element in the formula of a chemical compound Name binary molecular compounds using oxidation numbers and the Stock system

3. Oxidation Numbers The charges on the ions in an ionic compound reflect the electron distribution of the compound In order to indicate the general distribution of electrons among the bonded atoms in a molecular compound or a polyatomic ion, oxidation numbers are assigned to the atoms composing the compound or ion Unlike ionic charges, oxidation numbers do not have an exact physical meaning: rather, they serve as useful “bookkeeping” devices to help keep track of electrons In general when assigning oxidation numbers, shared electrons are assumed to “belong” to the more electronegative atom in each bond

4. Oxidation Numbers Assigning Oxidation Numbers The atoms in a pure element have an oxidation number of zero Monatomic ions have an oxidation number equal to the charge of the ion The more-electronegative element in a binary compound is assigned a negative number equal to the charge it would have as an anion. Likewise for the less-electronegative element Fluorine has an oxidation number of –1 in all of its compounds because it is the most electronegative element Oxygen usually has an oxidation number of –2 In peroxides, such as H 2 O 2, oxygen’s oxidation number is –1 In compounds with fluorine, such as OF 2, oxygen’s oxidation number is +2

5. Oxidation Numbers Assigning Oxidation Numbers Hydrogen has an oxidation number of +1 in all compounds containing elements that are more electronegative than it; it has an oxidation number of –1 with metals The algebraic sum of the oxidation numbers of all atoms in an neutral compound is equal to zero The algebraic sum of the oxidation numbers of all atoms in a polyatomic ion is equal to the charge of the ion Although rules 1 through 7 apply to covalently bonded atoms, oxidation numbers can also be applied to atoms in ionic compounds similarly

6. Oxidation Numbers Sample Problem Assign oxidation numbers to each atom in the following compounds or ions: UF 6 H 2 SO 4

7. Oxidation Numbers Sample Problem Solution Place known oxidation numbers above the appropriate elements Multiply known oxidation numbers by the appropriate number of atoms and place the totals underneath the corresponding elements The sum of the oxidation numbers must equal zero unless there is a charge associated with the compound Oxidation Numbers +5  2 +5  6

8. Oxidation Numbers Oxidation Numbers for Formulas and Names Many nonmetals can have more than one oxidation number These numbers can sometimes be used in the same manner as ionic charges to determine formulas What is the formula of a binary compound formed between sulfur and oxygen? From the common +4 and +6 oxidation states of sulfur, you could predict that sulfur might form SO 2 or SO 3 Both are known compounds

9. Oxidation Numbers Common Oxidation States of Nonmetals Pg. 235

10. Oxidation Numbers Oxidation Numbers for Formulas and Names Using oxidation numbers, the Stock system, introduced in the previous section for naming ionic compounds, can be used as an alternative to the prefix system for naming binary molecular compounds Prefix systemStock system PCl 3 phosphorus trichloridephosphorus(III) chloride PCl 5 phosphorus pentachloridephosphorus(V) chloride N2ON2Odinitrogen monoxidenitrogen(I) oxide NOnitrogen monoxidenitrogen(II) oxide Mo 2 O 3 dimolybdenum trioxidemolybdenum(III) oxide