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Oxidation States

Oxidation States. Assigning oxidation numbers. An “ oxidation number ” is a positive or negative number assigned to an atom to indicate its degree of oxidation or reduction.

kenneth-garza
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Oxidation States

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  1. Oxidation States Assigning oxidation numbers

  2. An “oxidation number” is a positive or negative number assigned to an atom to indicate its degree of oxidation or reduction. • Generally, a bonded atom’s oxidation number is the charge it would have if the electrons in the bond were assigned to the atom of the more electronegative element Assigning Oxidation Numbers

  3. The oxidation number of any uncombined element is zero. • Examples: all atoms in sodium Na, oxygen O2, phosphorus P4, and sulfur S8. Rules for Assigning Oxidation Numbers

  4. Rules for Assigning Oxidation Numbers • The oxidation number of a monatomic ion equals its charge.

  5. The oxidation number of fluorine is ALWAYS -1 • oxygen usually has and oxidation number of-2 • Exceptions: • In peroxides, such as H2O2oxygen has an oxidation number of -1. • In compounds with fluorine, such as OF2, oxygen’s oxidation number is +2. Rules for Assigning Oxidation Numbers

  6. Rules for Assigning Oxidation Numbers • Hydrogen has and oxidation number of +1. Exceptions: In metal hydrides, like NaH, hydrogens oxidation number is -1.

  7. The sum of the oxidation numbers of the atoms in a neutralcompound must equal 0. Rules for Assigning Oxidation Numbers 2(+1) + (-2) = 0 H O (+2) + 2(-2) + 2(+1) = 0 Ca O H

  8. The sum of the oxidation numbers in the formula of a polyatomic ion is equal to its ionic charge. X + 4(-2) = -2 S O X + 3(-2) = -1 N O Rules for Assigning Oxidation Numbers thus X = +5 thus X = +6

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