Examples of Sulfur - added to give an octet of valence...

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Examples of Sulfur H 2 S Sulfur (2.5) is more electronegative than hydrogen (2.1), thus it has an oxidation number of -2. The hydrogen will have an oxidation number of +1. S 8 This is an elemental form of sulfur, and thus would have an oxidation number of 0. SCl 2 Chlorine (3.0) is more electronegative than sulfur (2.5), thus it has an oxidation number of -1. The sulfur thus has an oxidation number of +2. Na 2 SO 3 Sodium (alkali metal) always has an oxidation number of +1. The oxygen (3.5) is more electronegative than sulfur (2.5), thus the oxygen would have an oxidation number of -2. The sulfur would therefore have an oxidation number of +4. SO 4 2- The oxygen is more electronegative and thus has an oxidation number of -2. The sulfur thus has an oxidation number of +6. Sulfur exhibits a variety of oxidation numbers (-2 to +6) In general the most negative oxidation number corresponds to the number of electrons which must be
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Unformatted text preview: added to give an octet of valence electrons The most positive oxidation number corresponds to a loss of all valence electrons Oxidation Numbers and Nomenclature Compounds of the alkali (oxidation number +1) and alkaline earth metals (oxidation number +2) are typically ionic in nature. Compounds of metals with higher oxidation numbers (e.g. tin +4) tend to form molecular compounds In ionic and covalent molecular compounds usually the less electronegative element is given first . In ionic compounds the names are given which refer to the oxidation (ionic) state In molecular compounds the names are given which refer to the number of molecules present in the compound Ionic Molecular MgH 2 magnesium hydride H 2 S dihydrogen sulfide FeF 2 iron(II) fluoride OF 2 oxygen difluoride Mn 2 O 3 manganese(III) oxide Cl 2 O 3 dichlorine trioxide...
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