A galvanic cell, also known as a voltaic cell, is an electrochemical cell that converts the chemical energy of spontaneous redox reactions into electrical energy. It is named after the scientists Luigi Galvani and Alessandro Volta, respectively. Galvanic cells consist of two half-cells, each with a metallic electrode dipped into an electrolyte. The two half-cells are connected to a voltmeter and a switch externally with the help of metallic wires. When the switch is set on, due to the potential difference, electrons flow from the negative electrode to the positive electrode. The electrode where oxidation takes place is called the anode, and the electrode where reduction takes place is called the cathode. Galvanic cells involve spontaneous electrochemical reactions in which the half-reactions are separated so that current can flow through an external wire/17%3A_Electrochemistry/17.2%3A_Galvanic_Cells). The beaker on one side of the cell is called a half-cell and contains a solution of a metal salt with a piece of metal partially submerged in the solution/17%3A_Electrochemistry/17.2%3A_Galvanic_Cells). The metal is an electrode, and it is undergoing oxidation, making it the anode/17%3A_Electrochemistry/17.2%3A_Galvanic_Cells). The other half-cell contains a solution of a different metal salt with a piece of metal partially submerged in the solution/17%3A_Electrochemistry/17.2%3A_Galvanic_Cells). This metal is an electrode, and it is undergoing reduction, making it the cathode/17%3A_Electrochemistry/17.2%3A_Galvanic_Cells). The two half-cells are separated by a salt bridge, which allows ions to flow between the two half-cells to maintain electrical neutrality/17%3A_Electrochemistry/17.2%3A_Galvanic_Cells). The cell notation is used to describe galvanic cells, which provides information about the various species involved in the reaction/17%3A_Electrochemistry/17.2%3A_Galvanic_Cells). The notation works for other types of cells as well/17%3A_Electrochemistry/17.2%3A_Galvanic_Cells). Galvanic cells are used to supply electrical current through a redox reaction to the transfer of electrons.