PP Presentation

OXIDATION-REDUCTION REACTIONS

Cu (s) + 2 AgNO3 (aq) ® Cu(NO3)2 (aq) + 2 Ag(s)

Transfer of electrons:

Cu0 gives 2 electrons to 2 Ag+ to form Cu2+ and 2 Ag0

species that provides electrons …….. called the REDUCING AGENT

species that accepts electrons …….. called the OXIDIZING AGENT

species that loses electrons is said to have been OXIDIZED

species that gains electrons is said to have been REDUCED

Chemists use the concept of OXIDATION NUMBER

to recognize OXIDATION-REDUCTION reactions

Here Cu in Cu (s) O.N. = 0

Cu in Cu(NO3)2 O.N. = +2

Ag in AgNO3 O.N. = +1

Ag in Ag(s) O.N. = 0

(see Fig. 4.17 in Kotz)

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