The aluminum metals
In an electrolyte cell with aluminum and gold electrodes, oxidation occurs at the aluminum electrode. Aluminum, being more reactive than gold, donates electrons and is oxidized to form aluminum ions (Al³⁺). The gold electrode, on the other hand, typically acts as the cathode, where reduction occurs as it accepts the electrons released from the aluminum. This movement of electrons generates an electric current in the electrolyte cell.
Two electrodes in electrolyte solutions
Mg(s) Apex baby
In a standard galvanic cell using zinc and aluminum, the zinc metal will act as the anode and the aluminum metal will act as the cathode. Zinc will undergo oxidation at the anode, releasing electrons which flow through the external circuit to the cathode where aluminum will undergo reduction. This flow of electrons creates an electrical current.
The standard cell notation for a galvanic cell involving aluminum and nickel can be represented as: Al | Al³⁺ (aq) || Ni²⁺ (aq) | Ni. In this notation, aluminum (Al) serves as the anode where oxidation occurs, while nickel (Ni) acts as the cathode where reduction takes place. The double vertical line (||) indicates the salt bridge separating the two half-cells.
the nickel metal
The standard cell notation for a galvanic cell with aluminum and gold electrodes is represented as: Al(s) | Al³⁺(aq) || Au³⁺(aq) | Au(s). In this notation, the anode (aluminum) is listed on the left, and the cathode (gold) is on the right. The double vertical line (||) indicates the salt bridge or separation between the two half-cells. The state of each component (solid or aqueous) is also noted.
Al(s) I AI3+(aq) II AI3+ (aq) I Al(s)
In a galvanic cell made with silver and nickel electrodes, the nickel electrode undergoes oxidation as it loses electrons, which travel through the external circuit to the silver electrode where reduction occurs. This flow of electrons generates an electric current in the cell.
the gold metal
In an electrolytic cell with aluminum and gold electrodes, aluminum would be oxidized at the anode. This is because aluminum has a higher tendency to lose electrons compared to gold, making it more likely to undergo oxidation.
In a galvanic cell with silver and nickel electrodes, the nickel electrode will be oxidized. Oxidation occurs at the anode, where electrons are released as nickel atoms lose electrons and form nickel ions. Silver ions from the other electrode will capture these electrons as the reduction reaction occurs at the cathode.
The aluminum metals
In a galvanic cell with silver and nickel electrodes, nickel is oxidized at the anode. During oxidation, nickel atoms lose electrons and become Ni2+ ions, contributing to the flow of electrons in the cell. Silver acts as the cathode where reduction reactions take place.
Two electrodes in electrolyte solutions
aluminum oxidized, zinc reduced
Ni2+(aq) + 2e- Ni(s) and Mg(s) Mg2+(aq) + 2e-