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# Ch 22sec2

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assigning oxidation numbers

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### Ch 22sec2

1. 1. 22.2 Oxidation Numbers
2. 2. Assigning Oxidation Numbers An “ oxidation number ” is a positive or negative number assigned to an atom to indicate its degree of oxidation or reduction. Generally, a bonded atom’s oxidation number is the charge it would have if the electrons in the bond were assigned to the atom of the more electronegative element
3. 3. Rules for Assigning Oxidation Numbers The oxidation number of any uncombined element is zero. The oxidation number of a monatomic ion equals its charge.
4. 4. Rules for Assigning Oxidation Numbers The oxidation number of oxygen in compounds is -2, except in peroxides, such as H 2 O 2 where it is -1. The oxidation number of hydrogen in compounds is +1, except in metal hydrides, like NaH, where it is -1.
5. 5. Rules for Assigning Oxidation Numbers The sum of the oxidation numbers of the atoms in the compound must equal 0. 2(+1) + (-2) = 0 H O (+2) + 2(-2) + 2(+1) = 0 Ca O H
6. 6. Rules for Assigning Oxidation Numbers The sum of the oxidation numbers in the formula of a polyatomic ion is equal to its ionic charge. X + 3(-2) = -1 N O  X = +5  X = +6 X + 4(-2) = -2 S O
7. 7. Point to note Oxidation numbers are written with the charge first and number second Ex. HCl H oxidation number is +1 Cl oxidation nmber is -1 Ionic charge though is written with the charge after the number: H charge is 1+, Cl charge is 1-
8. 8. Problem: What is the oxidation number of each element in SO 2 Do oxygen first because you know that is -2. x -4 = 0 S O 2, so, S is +4 S=+4 O=-2
9. 9. Reducing Agents and Oxidizing Agents An increase in oxidation number = oxidation A decrease in oxidation number = reduction Sodium is oxidized – it is the reducing agent Chlorine is reduced – it is the oxidizing agent
10. 10. Trends in Oxidation and Reduction Active metals : Lose electrons easily Are easily oxidized Are strong reducing agents Active nonmetals : Gain electrons easily Are easily reduced Are strong oxidizing agents
11. 11. Problem Use oxidation numbers to decide which elements are oxidized and which reduced in the following reaction: C + O 2 ------CO 2 0 0 +4 -2 C + O 2 ------CO 2 Notice C goes from 0 to +4 so it is oxidized ( reducing agent) O goes from 0 to -2,so it is reduced (oxiding agent)