Chapter 4
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| elements | oxidation # is zero
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| monatomic ions | oxidation # equals charge on the ion
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| oxygen | oxidation # is -2 on most compounds except peroxides
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| hydrogen | oxidation # is +1 in most compounds, (-1 in metal binary compounds ex CaH2)
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| halogens | oxidation # is -1 in F. Cl, Br, and I is -1 in binary compounds except when the other element is another halogen above it or oxygen
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| Compounds and ions | oxidation # is the sum of numbers in compound=0
sum of numbers in polyatomic ions = charge on ion
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| CO3 2- evolves to | CO2 + H2O
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| SO3 2- evolves to | SO2 + H2O
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| S 2- evolves to | H2S +H2O
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| Group 1A and NH4+ compounds | soluble
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| C2H3O2- and NO3- | soluble
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| Cl- Br- I- | soluble except Ag, Hg, Pb bonded
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| SO4 2- | soluble except Ca, Sr, Ba, Ag, Hg, Pb
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| CO3 2- | insoluble except group 1A and NH4+
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| PO4 3- | insoluble except group 1A and NH4+
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| S 2- | insoluble except group 1A and NH4 +
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| OH- | insoluble except group 1A, Ca, Ba, Sr
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