what is the criteria to select a proper reducing agent
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A reducing agent (also called a reductant or reducer) is an element (such as calcium) or compound that loses (or "donates") an electron to another chemical species in a redox chemical reaction. Since the reducing agent is losing electrons, it is said to have been oxidized.
If any chemical is an electron donor (reducing agent), another must be an electron recipient (oxidizing agent). A reducing agent is oxidized because it loses electrons in the redox reaction.
Thus, reducers (reducing agents) "reduce" (or, seen another way, are "oxidized" by) oxidizers (oxidizing agents), and oxidizers "oxidize" (that is, are "reduced" by) reducers.
In their pre-reaction states, reducers have more electrons (that is, they are by themselves reduced) and oxidizers have fewer electrons (that is, they are by themselves oxidized). A reducing agent typically is in one of its lower possible oxidation states and is known as the electron donor. Examples of reducing agents include the earth metals, formic acid, and sulfitecompounds.
For example, consider the overall reaction for aerobic cellular respiration:
C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)
The oxygen (O2) is being reduced, so it is the oxidizing agent. The glucose (C6H12O6) is being oxidized, so it is the reducing agent.
In organic chemistry, reduction more specifically refers to the addition of hydrogen to a molecule, though the aforementioned definition still applies. For example, benzeneis reduced to cyclohexane in the presence of a platinum catalyst:
C6H6 + 3 H2 → C6H12
If any chemical is an electron donor (reducing agent), another must be an electron recipient (oxidizing agent). A reducing agent is oxidized because it loses electrons in the redox reaction.
Thus, reducers (reducing agents) "reduce" (or, seen another way, are "oxidized" by) oxidizers (oxidizing agents), and oxidizers "oxidize" (that is, are "reduced" by) reducers.
In their pre-reaction states, reducers have more electrons (that is, they are by themselves reduced) and oxidizers have fewer electrons (that is, they are by themselves oxidized). A reducing agent typically is in one of its lower possible oxidation states and is known as the electron donor. Examples of reducing agents include the earth metals, formic acid, and sulfitecompounds.
For example, consider the overall reaction for aerobic cellular respiration:
C6H12O6(s) + 6O2(g) → 6CO2(g) + 6H2O(l)
The oxygen (O2) is being reduced, so it is the oxidizing agent. The glucose (C6H12O6) is being oxidized, so it is the reducing agent.
In organic chemistry, reduction more specifically refers to the addition of hydrogen to a molecule, though the aforementioned definition still applies. For example, benzeneis reduced to cyclohexane in the presence of a platinum catalyst:
C6H6 + 3 H2 → C6H12
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It must loose an electron
Can be oxidized to greater oxidation state
Example KMnO4 is a good reducing agent as it can be oxidized to +7 oxidation state
Can be oxidized to greater oxidation state
Example KMnO4 is a good reducing agent as it can be oxidized to +7 oxidation state
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