Also the difference between reduction and the reducing agent??
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Examine the equation below.
Fe + Cl2 --> FeCl2
The Fe atoms LOSE 2 e each to form Fe 2+.
Loss of electrons is OXIDATION
The Cl atoms GAIN 1 e each to form Cl -
Gain of electrons is REDUCTION
The substance which removes the electrons is called the OXIDISING AGENT. In this case that is chlorine.
The substance which gives the electrons is called the REDUCING AGENT. In this case that is iron.
Happy Studies.
Fe + Cl2 --> FeCl2
The Fe atoms LOSE 2 e each to form Fe 2+.
Loss of electrons is OXIDATION
The Cl atoms GAIN 1 e each to form Cl -
Gain of electrons is REDUCTION
The substance which removes the electrons is called the OXIDISING AGENT. In this case that is chlorine.
The substance which gives the electrons is called the REDUCING AGENT. In this case that is iron.
Happy Studies.
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Oxidation refers to the loss of electrons by an entity be it an atom, molecule/compound or ion.
There are substances that can cause other substances to lose their electrons, meaning oxidation is occuring. The substance that causes this is called the oxidizing agent. Oxidation is caused by oxidizing agents. When an oxidizing agent removes electrons, the agent becomes reduced because it is gaining electrons simutaneously (the electrons it took from oxidizing a substance).
The following is an example:
1. H2 + F2 ----> 2HF
2. H2 ---> 2H+ + 2e
3. F2 + 2e ---> 2F-
The first reaction is the overall general reaction. The second and third reactions are the respective half reactions of the first reaction. They show what happens to the H2 & F2. H2 loses 2 electrons becoming oxidized. Since it's giving up it's two electrons to Flourine it is also a reducing agent. F2 gains 2 electrons becoming reduced. It is an oxidizing agent for taking them from the hydrogen.
Hope this helps.
There are substances that can cause other substances to lose their electrons, meaning oxidation is occuring. The substance that causes this is called the oxidizing agent. Oxidation is caused by oxidizing agents. When an oxidizing agent removes electrons, the agent becomes reduced because it is gaining electrons simutaneously (the electrons it took from oxidizing a substance).
The following is an example:
1. H2 + F2 ----> 2HF
2. H2 ---> 2H+ + 2e
3. F2 + 2e ---> 2F-
The first reaction is the overall general reaction. The second and third reactions are the respective half reactions of the first reaction. They show what happens to the H2 & F2. H2 loses 2 electrons becoming oxidized. Since it's giving up it's two electrons to Flourine it is also a reducing agent. F2 gains 2 electrons becoming reduced. It is an oxidizing agent for taking them from the hydrogen.
Hope this helps.