For an electrochemical reduction process,
electrons are
1. taken from solution species at the surface
of the cathode.
2. added to solution species at the surface of
the anode.
3. added to solution species at the surface of
the cathode.
See your previous question.
The correct answer for an electrochemical reduction process is 3. Electrons are added to solution species at the surface of the cathode.
To understand why this is the correct answer, let's start by explaining the different components of an electrochemical cell.
An electrochemical cell consists of two electrodes, namely the cathode and the anode, submerged in an electrolyte solution. The cathode is the electrode where reduction occurs, while the anode is where oxidation takes place.
During an electrochemical reduction process, which is a type of redox (reduction-oxidation) reaction, electrons are transferred from the anode to the cathode. This transfer of electrons is facilitated by the flow of ions in the electrolyte solution.
At the anode, oxidation takes place, and electrons are usually removed from the metal surface of the anode. The anode, therefore, tends to lose mass or corrode during this process.
On the other hand, at the cathode, reduction occurs, and electrons are added to the solution species present at its surface. These solution species can be ions or molecules that gain electrons and are reduced to a lower oxidation state or a different chemical form. This reduction process results in the cathode gaining mass or being deposited with reduced species.
Therefore, the correct statement is that electrons are added to solution species at the surface of the cathode during an electrochemical reduction process.