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)