Sodium (Na) is an important element in biology and chemistry due to it being the most abundant alkali metal on Earth. The most significant property of sodium is its affinity to ionise by dropping the single electron from its outer shell. This property is responsible for sodium’s affinity for dipolar molecules, notably water, with which it reacts violently. In the human body, sodium is used to send nerve impulses, as well as within cells to absorb nutrients through osmosis.

The name sodium derives from soda, the common name for sodium carbonate. The symbol Na is for the latin word natrium, which refers to the sodium mineral natron.

Pure sodium is a soft, lightweight metal that is slightly less dense than water. It readily forms salts, including ordinary table salt.

Sodium can be extracted from lye (sodium hydroxide) through electrolysis or by extreme heat. The lye must be molten to perform electrolysis, so the latter method is easier. Sodium must be stored in oil as it will react with the atmosphere.

Pure sodium hydroxide crystals can be purchased as heavy duty drain cleaners. While some urban hardware stores carry it, you will have better luck at country farm co-op hardware stores.

Begin by crushing your lye into a fine powder. Mix it in a 1:1 with magnesium powder. Place a fuse or sparkler into the powder and ignite it. This will produce an extremely hot thermite reaction, so do this in a large can on spare concrete. cover the reaction immediately to contain the gases and keep the sodium from oxidising. Once it is almost complete, after a few seconds, douse it in mineral oil.

The reaction produces a sodium-magnesium ore. This must be chipped out of the can and ground into a powder to increase its suface area for the next reaction.

In a clean glass flask, cover the powder with dioxane, heat and stir constantly. Dioxane is highly flammable, so this step should not be done over open flame. As the solution boils, globs of sodium will begin to conglomerate. Store these under mineral oil.