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Chapter 10

Chapter 10. Oxidation Numbers With Manganese Ions Demo. Oxidation Number. The oxidation number is the charge on a single atom. Oxidation Number. The oxidation number is the charge on a single atom. Examples: Na + (oxidation number = +1) Clˉ (oxidation number = -1)

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Chapter 10

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  1. Chapter 10 Oxidation Numbers With Manganese Ions Demo

  2. Oxidation Number • The oxidation number is the charge on a single atom.

  3. Oxidation Number • The oxidation number is the charge on a single atom. • Examples: Na+ (oxidation number = +1) Clˉ (oxidation number = -1) Al3+ (oxidation number = +3) O2ˉ (oxidation number = -2)

  4. We can use the periodic table to determine oxidation numbers.

  5. Determining Oxidation Numbers • Metals form positive ions (7+ is the highest positive oxidation number). • Nonmetals tend to form negative ions. • However other than the noble gases which have an oxidation number of zero, and fluoride (F-) which is always a 1-, all other nonmetals could have positive oxidation numbers as well.

  6. We can use the periodic table to “predict” oxidation numbers • If we have the name of the ion a “prediction” is unnecessary. • Potassium ion • Iron (II) • Nitride • We can often predict the range of oxidation numbers of the positive monatomic ions other than groups 1 & 2, Ag, Cd, Zn, and Al.

  7. What common ions can Iron form? Often the electron configuration can help us to understand why certain oxidation numbers form. Fe +2 Fe +3

  8. Most transition metal elements have more than one positive ion. (However +2 is the most common oxidation number for metal ions). Fe +2 Fe +3

  9. What oxidation numbers might we predict for Vanadium? V = [Ar]4s23d3 V2+ = [Ar]3d3 V5+ = [Ar] • This gives the range of possible oxidation numbers for Vandadium (V2+ through V5+)

  10. What oxidation numbers might you predict for Manganese? (Mn)

  11. Mn+2

  12. The most common oxidation number for metal ions 2+ Mn+2

  13. The most common oxidation number for metal ions 2+ Mn+2 Mn +7

  14. Each electron is harder to remove than the one before so sometimes losing electrons can be a gradual process. Mn +4 Mn +5 Mn +6 Mn +3 Mn+2 Mn +7

  15. Electrons do not have to be lost one at a time. The process can be rather random. Mn +4 Mn +6 Mn Mn +2 Mn +7

  16. Demonstration a Mn

  17. Demonstration a Mn

  18. Determining Oxidation Numbers • What is the oxidation number of nitrogen ([He]2s22p3) within a compound? • Would you predict -3? • Could nitrogen have a positive oxidation number? • How about +2 or maybe +5? • The fact is we can only guess as to what the oxidation number of nitrogen is within a compound unless we have some additional information.

  19. Determining Oxidation Numbers • The best way to determine oxidation number of an element is to examine the formula of the compound that the element is in. • We then use some basic rules to help us make a determination as to the oxidation numbers of the elements that make up the compound.

  20. Oxidation Number Rules • The oxidation number of all Group 1 metals (+1), Group 2 metals (+2), Ag+, Zn2+, Cd2+, and Al3+ within compounds is a set value. • Hydrogen (H) has two possible oxidation numbers: • +1 when bonded to a nonmetal • -1 when bonded to a metal • The oxidation number of fluorine (F) is always -1. • In a compound thenonmetalclosest to fluorine is negative. • The sum of the oxidation numbers of all atoms (ions) in a neutral compound = 0. • The sum of the oxidation numbers of all atoms (ions) in a polyatomic ion = charge on the polyatomic ion.

  21. What is the oxidation number of nitrogen? N2O • N2O is nitrogen (I) oxide • Commonly known as “laughing gas”.

  22. Example NaCl

  23. Example BaH2

  24. Example PO33-

  25. Example FePO3

  26. Example Fe3(PO3)2

  27. Homework Ions and Oxidation Numbers Worksheet

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