Chlorine ion is oxidized at the negative electrode because it gains electrons, which is the process of oxidation. In this case, the chlorine ion loses its extra electron to become a chlorine atom, which is an oxidation process.
The term "anodic" refers to the electrode or region in an electrochemical cell where oxidation occurs. In simple terms, it is the positively charged electrode where electrons are released.
Hydrogen is used as a standard electrode because it has a well-defined standard electrode potential and is easily reversible in its oxidation and reduction reactions. This makes it a reliable reference point for measuring the electrode potentials of other half-reactions in electrochemical cells.
In the compound HF, the oxidation number of hydrogen (H) is +1 and the oxidation number of fluorine (F) is -1. This is because fluorine is more electronegative than hydrogen, so it takes on a -1 oxidation state while hydrogen takes on a +1 oxidation state.
The standard hydrogen electrode (SHE) is a reference electrode used in electrochemistry to measure electrode potential. It consists of a platinum electrode in contact with a solution of hydrogen ions at unit activity and surrounded by hydrogen gas at a pressure of 1 bar. The SHE has an assigned potential of 0 V at all temperatures.
according to me anode should be oxidizing electrode as oxidation reaction takes place on anode
Oxidation takes place at anode and reduction at cathode - yes, it is correct.
The electrode with the highest oxidation potential
The standard hydrogen electrode (abbreviated SHE), is a redox electrode which forms the basis of the thermodynamic scale of oxidation-reduction potentials.
It is called aerobic respiration, oxidation is usage of oxygen .
These reactions are called redox reactions.Isolated reduction/oxidation is not possible.
water, carbon dioxide and oxygen
Oxidation (slow burning of the tobacco)
An oxidation half-reaction
Chlorine ion is oxidized at the negative electrode because it gains electrons, which is the process of oxidation. In this case, the chlorine ion loses its extra electron to become a chlorine atom, which is an oxidation process.
Definition: The standard hydrogen electrode is the standard measurement of electrode potential for the thermodynamic scale of redox potentials.The standard is determined by the potential of a platinum electrode in the redox half reaction2 H+(aq) + 2 e- → H2(g) at 25 °C.The standard hydrogen electrode is often abbreviated SHE.Also Known As: normal hydrogen electrode or NHE
The term "anodic" refers to the electrode or region in an electrochemical cell where oxidation occurs. In simple terms, it is the positively charged electrode where electrons are released.