OxidationNumberRules

OxidationNumberRules - -, H-(H-when bonded to metals) 7A...

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Section 4.4 Oxidation # Rules: 1. Elements in their elemental form have an oxidation number of 0. Examples: Na(s), Al(s), H2(g), O2(g), N2(g), Cl2(g), P4(s), S8(s), Fe(s) 2. Monoatomic ions have oxidation numbers equal to their charge. Examples: s 1 : +1: H +1 , Li +1 , Na +1 , K +1 (H + when bonded to nonmetals) 1A s 2 : +2: Be +2 , Mg +2 , Ca +2 2A s 2 p 1 : +3: B +3 , Al +3 , Ga +3 3A s 2 p 2 : +4: C +4 , Si +4 , Ge +4 4A -1: F - , Cl - , Br - , I
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Unformatted text preview: -, H-(H-when bonded to metals) 7A -2: O-2 (+ 3 others) 6A -3: N-3 (+ 6 others) 5A 3. The sum of the oxidation numbers in a compound = 0. H 2 O K 2 Cr 2 O 7 Ox# +1 -2 +1 +6 -2 # atoms 2 1 2 2 7 2 - 2 = 0 2 + 12 - 14 = 0 4. For ions: The sum of the oxidation numbers = the net charge SO 3 2-Cr 2 O 7 2-Ox# +4 -2 +6 -2 # atoms 1 3 2 7 6 - 6 = -2 12 - 14 = -2...
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