Redox

Redox

Ion Formation
1. Metals: Are oxidised and form positive ions.
2. Non-Metals: Are reduced and form negative ions.
Oxidation Number Rules
1. Ion: Charge on ion
2. Uncombined Element: 0
3. Combined Oxygen: -2
4. Combined Hydrogen: +1
5. Combined Fluorine: -1
6. If there is a roman numeral after an element name, that element has that oxidation number (e.g. In Iron(II) Chloride, Iron has an oxidation number of 2+).
Reactions
1. Metals+Acids
  1. Metal is oxidised to form positive ion
  2. Hydrogen in acid reduced to form hydrogen gas
  3. Acid+Metal==Salt+H2
2. Half Equations
  1. Show the oxidation or reduction of certain elements during a reaction.
  2. e.g. Mg+Cl2==MgCl2
    1. Mg==Mg(2+)+2[e(-)]
    2. Cl2+2[e(-)]==2[CL(-)]
Definitions
1. Reduction
  1. Gain of electrons
  2. Decrease in oxidation number.
2. Oxidation
  1. Loss of electrons
  2. Increase in oxidation number.

Resource summary

	Created by Thundorz about 10 years ago