Oxidation involve loss of electrons and reduction involve gain of electrons.
Silver cations are reduced.
Silver (Ag) for apex
Your reaction is AgNO3 + Na ==> NaNO3 + AgIn this reaction Ag goes from 1+ to zero, so it has been reduced. Na goes from zero to 1+ so it has been oxidized.
Silver (Ag)
A disproportionation reaction is one in which a species has been both oxidised and reduced (that is, the oxidation state of the related species found in the products has increased in one instance, and decreased in another, in relation to that of the species found in the reactants). The classic example of disproportionation is the reaction between chlorine gas and dilute sodium hydroxide, although there are many others: Cl2 + 2NaOH --> H2O + NaCl + NaClO The oxidation state of chlorine is 0 in the reactants, but has decreased to -1 in NaCl AND has increased to +1 in sodium chlorate, NaClO.
The reactant that reduces another atom
Silver cations are reduced.
Sodium (Na) has been reduced.
Silver (Ag) for apex
Your reaction is AgNO3 + Na ==> NaNO3 + AgIn this reaction Ag goes from 1+ to zero, so it has been reduced. Na goes from zero to 1+ so it has been oxidized.
Silver (Ag)
Silver (Ag)
oxidized. when fad reacts to fadh2 it is said to be reduced
It is an easily reversible chemical reaction known as a redox reaction.The blue color is due to blue color is due to I2+ cation. The iodine has been oxidized by an oxidizing agent. It can be reduced back to I2 in the reverse reaction.
A chlorine atom gains an electron when it becomes an ion. This means it has been reduced because there is a decrease in oxidation state from 0 to -1.
Well it has less electrons than it had before. That is the definition of oxidation. The loss of electrons is oxidation. The gain of electrons is reduction.
A disproportionation reaction is one in which a species has been both oxidised and reduced (that is, the oxidation state of the related species found in the products has increased in one instance, and decreased in another, in relation to that of the species found in the reactants). The classic example of disproportionation is the reaction between chlorine gas and dilute sodium hydroxide, although there are many others: Cl2 + 2NaOH --> H2O + NaCl + NaClO The oxidation state of chlorine is 0 in the reactants, but has decreased to -1 in NaCl AND has increased to +1 in sodium chlorate, NaClO.