14.1 Oxidation-Reduction Reactions and Assigning Oxidation Numbers
Oxidation – loss of electrons
Reduction – gain of electrons
LEO
GER
OIL
RIG
Oxidizing Agent (Oxidant) – species that is reduced
Reducing Agent (Reductant) – species that is oxidized
2Na(s) + Cl2(g) → 2NaCl(s)
| Rules for Determining Oxidation States |
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| 1) Elements in their elemental form are in the zero oxidation state. Rules 2-6 are for Compounds 2) Group 1 metals are +1 and Group 2 metals are +2. 3) Hydrogen is +1 except when bonded to a metal only (when it’s –1). 4) Transition elements must be determined from anion’s charge (except Al=+3, Zn=+2, Cd=+2, Ag=+1) 5) The most electronegative elements get their typical oxidation state. 6) The last element not assigned balances the charge of the compound/ion. |
Determine the oxidation states of all elements in the following:
Cl2 O2 O3
MgCl2 H2O2 N2O4
KO2 NaHCO3 NaN3
Cu(NO3)2