Format-OxNumbers

Format-OxNumbers - Example: NaOH Na = +1 , K 2 SO 4 2 K =...

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RULES FOR ASSIGNING OXIDIZATION NUMBER TO ATOMS IN A COMPOUND 1) The sum of the oxidization numbers of all atoms in a compound MUST EQUAL ZERO or for an ion MUST EQUAL THE ELECTRICAL CHARGE of the ion. Example: CaSO 4 Ca = +2 Example: SO 4 -2 S = +6 S = +6 O = –8 O = – 8 = – 2 * 4 – 2 * 4 = – 2 0 2) The oxidization number of an atom in a free uncombined state is ZERO. Example: Fe = 0, Cd = 0, Al = 0, H 2 = 0 3) The oxidization number of a monoatomic ion is equal to electrical charge on ion. Example: Fe +3 = +3, H +1 = +1, Zn +2 = +2 4) The oxidization number of the IA atoms are always +1 and IIA atoms are always +2 in compounds or polyatomic ions.
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Unformatted text preview: Example: NaOH Na = +1 , K 2 SO 4 2 K = +1 , LiNO 3 Li = +1 Example: Ca(OH) 2 Ca = +2 , BaSO 4 Ba = +2 , Sr(NO 3 ) 2 Sr = +2 5) The oxidization number of halogens (F, Cl, Br, I, At) in binary compounds with more electropositive atoms is 1. Example: NaCl Cl = 1 , RbF F = 1 , CaBr 2 Br = 1 6) The oxidization number of Oxygen is 2 and Hydrogen is +1 with exceptions: a) Oxygen: peroxides = 1, superoxides = , ozonides = 1/3 b) Hydrogen: binary compounds with metal is 1 Example: CaH 2 H = 1 7) Possible oxidization number noted on Periodic Chart....
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This note was uploaded on 07/28/2011 for the course CHM 2045 taught by Professor Eng during the Spring '10 term at UNF.

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