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Assigning Oxidation Numbers

Assigning Oxidation Numbers. For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table. Assigning Oxidation Numbers. For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table. Alkali Metals = +1.

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Assigning Oxidation Numbers

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  1. Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table.

  2. Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table. Alkali Metals = +1

  3. Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table. Alkaline Earth Metals = +2

  4. Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table. Group 13 Boron Group = +3

  5. Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table. Group 15 Nonmetals = -3

  6. Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table. Group 16 Nonmetals = -2

  7. Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table. Halogens = -1

  8. Assigning Oxidation Numbers For ionic compounds, oxidation numbers can be assigned using the expected charges from the periodic table. Transition Metals depend on anion

  9. Ionic Compounds Example: +2 -1 MgCl2

  10. Ionic Compounds Example: -2 +1 Na2O

  11. Ionic Compounds Example: We don’t know iron’s oxidation number from the periodic table since it is a transition metal. ?? -2 Fe2O3

  12. Ionic Compounds But since we know the compound is neutral, the oxidation numbers must add up to zero. Therefore, Fe has a +3 oxidation number in this compound. Example: +3 -2 Fe2O3

  13. Ionic Compounds Example: We don’t know chromium’s oxidation number from the periodic table since it is a transition metal. ?? -2 Cr2O72-

  14. Ionic Compounds But since this ion has a charge of -2, the oxidation numbers must add up to negative two. Therefore the oxidation number of Cr is +6 Example: +6 -2 Cr2O72-

  15. Covalent Compounds Covalent compounds are made of two nonmetals, which from the periodic table are always expected to be negative

  16. Covalent Compounds But since covalent compounds are neutral species, it is not possible for every element to retain its negative oxidation number

  17. Covalent Compounds ONLY THE MORE ELECTRONEGATIVE ELEMENT keeps its negative oxidation number. Other nonmetals must adapt to keep the compound neutral

  18. Electronegativity Trend Increases

  19. Covalent Compounds Example: -2 SO2 Since oxygen is the more electronegative element, it will have its normal oxidation number.

  20. Covalent Compounds Example: +4 -2 SO2 The compound is neutral, so the oxidation number of sulfur will be sufficient to balance out the two oxygen atoms.

  21. Covalent Compounds Example: -1 OF2 Since fluorine is the more electronegative element, it will have its normal oxidation number.

  22. Covalent Compounds Example: +2 -1 OF2 The compound is neutral, so the oxidation number of oxygen will be sufficient to balance out the two fluorine atoms.

  23. Covalent Compounds Example: -2 PO43- Since oxygen is the more electronegative element, it will have its normal oxidation number.

  24. Covalent Compounds Example: +5 -2 PO43- The ion has a charge of negative three, so the oxidation numbers must add up to the total charge of the ion.

  25. Ionic Compounds with Polyatomics Example: +2 CaSO4 This is an ionic compound, so the charge of the metal cation is its oxidation number

  26. Ionic Compounds with Polyatomics Example: +2 CaSO4 The anion is a polyatomic ion, sulfate, and the charge of sulfate is negative two. So the oxidation numbers of sulfur and oxygen must add to -2

  27. Ionic Compounds with Polyatomics Example: +2 -2 CaSO4 Oxygen is the more electronegative of the two, so it keeps its normal oxidation number.

  28. Ionic Compounds with Polyatomics Example: +2 +6 -2 CaSO4 Sulfur and the four oxygen atoms must add to negative two (the charge of the sulfate anion).

  29. Ionic Compounds with Polyatomics Example: Pb(OH)4 This is an ionic compound, so the charge of the metal cation is its oxidation number. But this is a transition metal, so we cannot know it from its position on the periodic table.

  30. Ionic Compounds with Polyatomics Example: +4 Pb(OH)4 But the anion, the hydroxide ion, carries a charge of negative one. All four hydroxides are negative one, but since the compound is neutral, the oxidation number of lead must balance it out.

  31. Ionic Compounds with Polyatomics Example: +4 -2 Pb(OH)4 Within the anion, oxygen is the more electronegative of the two elements, and keeps its normal oxidation number.

  32. Ionic Compounds with Polyatomics Example: +4 -2 +1 Pb(OH)4 Within the hydroxide ion, the oxygen and hydrogen must add to the charge of the ion, -1

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