4.3 Oxidation Reduction Reactions
PRE-HEALTH PREP
Oxidation-Reduction Reaction (Redox Reactions) - A reaction in which the oxidation states (charges) of atoms change from reactants to products
2Na(s) + Cl2(g) ➔ 2NaCl(s)
Oxidation is the loss of electrons
Reduction is the gain of electrons
(OIL)
(RIG)
(LEO)
(GER)
| DETERMINING OXIDATION STATES | |
|---|---|
| 1 | Atoms in their elemental form are in the zero oxidation state. |
| 2 | Monatomic ions in ionic compounds get their typical ionic charge. |
| 3 | Atoms in Molecular Compounds and Polyatomic Ions Oxygen -2 except in peroxide O22- Hydrogen +1 (when bonded with any nonmetals) Fluorine -1 always Halogens -1 except when bonded to Oxygen |
| 4 | The oxidation numbers sum to zero for a compound or to the overall charge of a polyatomic ion. |
Determine oxidation states for all elements in the following:
Na O2 NaCl NaHCO3
CO2 H2O2 SO42-
Which of the following are oxidation-reduction reactions?
2Mg(s) + O2(g) ➔ 2MgO(s)
CaCO3(s) ➔ CaO(s) + CO2(g)
AgNO3(aq) + HCl(aq) ➔ AgCl(s) + HNO3(aq)
2AgNO3(aq) + Cu(s) ➔ Cu(NO3)2 + 2Ag(s)
Single Displacement Reactions
Which of the following reactions are spontaneous?
Mg(s) + 2HCl(aq) ➔ MgCl2(aq) + H2(g)
Cu(s) + Zn(NO3)2(aq) ➔ Cu(NO3)2(aq) + Zn(s)
Mn(s) + Ni2+(aq) ➔ Mn2+(aq) + Ni(s)
