oxidation and reduction
STK 1084 Inorganic Chemistry I, LU 3 Oxidation – Reduction Reactions, Prepared By: Dr. Tay Meng Guan,
Faculty of Resource Science and Technology, Universiti Malaysia Sarawak.
LU 3 Oxidation and Reduction Reactions
3.1
Ideas of Oxidation and Reduction
Oxidation of an atom can be occurred in the following conditions:
1. Losing an electron from the orbitals.
e.g.: A
A+ + e-
2. Adding an electronegative element (e.g.: F, Cl, Br, O) to a molecule.
e.g.: A + F
AF
3. Losing hydrogen from the molecule.
e.g.: H2A + B
H2B + A
In opposite, the reduction of an atom can be occurred in the reverse order of the oxidation conditions above.
Basically, the oxidation and reduction is the process of transferring electrons from one atom (or molecule) to another atom, which has a higher electronegativity (or molecule). Oxidation involves a loss of electrons.
Reduction involves a gain of electrons.
Oxidant (or oxidizing agent) is the species to oxidize the other species, indeed the oxidant itself is being reduced because it accepts electron from the other species.
Reductant (or reducing agent) is the species to reduce the other species, indeed the reductant itself is being oxidized because it donates electron to the other species. Consider the following examples:
1.
When sodium reacts with chlorine (in the gas phase), a white crystalline solid, namely sodium chloride is formed.
2Na + Cl2 2NaCl
1|Page
STK 1084 Inorganic Chemistry I, LU 3 Oxidation – Reduction Reactions, Prepared By: Dr. Tay Meng Guan,
Faculty of Resource Science and Technology, Universiti Malaysia Sarawak.
The reaction involves an electron transfers from Na to Cl, where the Na loses one electron to form Na+ and Cl accept one electron to give Cl-. In this case, oxidant is Cl and Na is the reductant.
2.
If an iron plate is placed into a solution of copper(II) sulfate. After a while, the iron plate will be coated with a layer of copper.
Fe(s) + Cu2+(aq)
Faculty of Resource Science and Technology, Universiti Malaysia Sarawak.
LU 3 Oxidation and Reduction Reactions
3.1
Ideas of Oxidation and Reduction
Oxidation of an atom can be occurred in the following conditions:
1. Losing an electron from the orbitals.
e.g.: A
A+ + e-
2. Adding an electronegative element (e.g.: F, Cl, Br, O) to a molecule.
e.g.: A + F
AF
3. Losing hydrogen from the molecule.
e.g.: H2A + B
H2B + A
In opposite, the reduction of an atom can be occurred in the reverse order of the oxidation conditions above.
Basically, the oxidation and reduction is the process of transferring electrons from one atom (or molecule) to another atom, which has a higher electronegativity (or molecule). Oxidation involves a loss of electrons.
Reduction involves a gain of electrons.
Oxidant (or oxidizing agent) is the species to oxidize the other species, indeed the oxidant itself is being reduced because it accepts electron from the other species.
Reductant (or reducing agent) is the species to reduce the other species, indeed the reductant itself is being oxidized because it donates electron to the other species. Consider the following examples:
1.
When sodium reacts with chlorine (in the gas phase), a white crystalline solid, namely sodium chloride is formed.
2Na + Cl2 2NaCl
1|Page
STK 1084 Inorganic Chemistry I, LU 3 Oxidation – Reduction Reactions, Prepared By: Dr. Tay Meng Guan,
Faculty of Resource Science and Technology, Universiti Malaysia Sarawak.
The reaction involves an electron transfers from Na to Cl, where the Na loses one electron to form Na+ and Cl accept one electron to give Cl-. In this case, oxidant is Cl and Na is the reductant.
2.
If an iron plate is placed into a solution of copper(II) sulfate. After a while, the iron plate will be coated with a layer of copper.
Fe(s) + Cu2+(aq)