Reduction-oxidation also referred to as redox and is defined as all the chemical reactions where by the oxidation numbers of atoms are changed. The term redox has two concepts, the reduction and oxidation concept. Reduction refers to the decrease in the oxidation number while oxidation is the increase in oxidation number. This process is understood well when one recognizes the chemical reaction that leads either increase or decrease in oxidation number of an atom or atoms (Jerome, Peter, 2007). This involves taking note on the rules for passing on oxidation numbers.
Oxidation number is the charge that would be there in an atom if the compound was made of ions. For an example, assuming that CH4 has C4- and H ions, then the oxidation number of the hydrogen and the carbon atoms would be 1 and -4. Howeve,r it does not matter whether these compounds have ions or not since this oxidation number refers to the charge an atom would contain if it was ionic.
To reflect this process chemically, we consider how electrons are transferred by the reductant to the oxidant. Therefore, the redundant that gives the electrons is therefore said to be oxidized while the oxidant gains electrons and is be reduced. The pair of a reducing and oxidizing agent involved in any reaction process is referred as redox pair (Jerome, Peter, 2007).
A good example of this redox reaction is between fluorine and hydrogen
H2 F2 2 HF
This can be broken into two half- reaction process and expressed in the equations below
Reduction reaction is expressed as F2 2 e 2 F.
Oxidation reaction is expressed as H2 2 H 2 e
There is no net alteration in charge in a reduction oxidation reaction so the surplus electrons in the oxidation reaction must be equivalent to the number of electrons extreme by the reduction reaction. Hydrogen fluoride is formed when ions come together and the equation is expressed below
H2 F2 2 H 2 F 2 HF
Oxidation number is the charge that would be there in an atom if the compound was made of ions. For an example, assuming that CH4 has C4- and H ions, then the oxidation number of the hydrogen and the carbon atoms would be 1 and -4. Howeve,r it does not matter whether these compounds have ions or not since this oxidation number refers to the charge an atom would contain if it was ionic.
To reflect this process chemically, we consider how electrons are transferred by the reductant to the oxidant. Therefore, the redundant that gives the electrons is therefore said to be oxidized while the oxidant gains electrons and is be reduced. The pair of a reducing and oxidizing agent involved in any reaction process is referred as redox pair (Jerome, Peter, 2007).
A good example of this redox reaction is between fluorine and hydrogen
H2 F2 2 HF
This can be broken into two half- reaction process and expressed in the equations below
Reduction reaction is expressed as F2 2 e 2 F.
Oxidation reaction is expressed as H2 2 H 2 e
There is no net alteration in charge in a reduction oxidation reaction so the surplus electrons in the oxidation reaction must be equivalent to the number of electrons extreme by the reduction reaction. Hydrogen fluoride is formed when ions come together and the equation is expressed below
H2 F2 2 H 2 F 2 HF
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