A chlorine molecule, Cl2, is formed in this process. Each chloride ion will lose one electron. At the anode, or positive electrode, in this electrolysis cell, two chloride ions will arrive. This is easily remembered using the mnemonic OILRIG, where oxidation is loss and reduction is gain of electrons. The half equation shown here represents a reduction process. At the negative electrode, or cathode, in this cell, a sodium ion gains one electron to become a sodium atom. The anode, or positive electrode, in this cell is made from graphite, and this is where chlorine gas is produced. And as it’s less dense than the molten sodium chloride and calcium chloride in the cell, it floats upwards and out of the cell. The sodium is molten at the temperature of the cell. Sodium is produced at the negative electrodes, or cathodes, in this cell. This mixture melts at about 600 degrees Celsius. To lower the melting point of sodium chloride, it’s mixed with calcium chloride. To extract sodium metal from sodium chloride, the sodium chloride must first be in a molten state. Using sodium chloride as a starting material, sodium metal may be extracted using electrolysis. Sodium reacts with many other elements to form salts. Although common in the Earth’s crust, sodium is never found in nature as a pure metal. The metals in group one are known as the alkali metals. Sodium is a reactive metal found in group one of the periodic table.
EXAMPLE OF SODIUM ELEMENT HOW TO
In this video, we will learn how to describe and explain the properties of the element sodium and its compounds.
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