Lithium #3 – Li
Group:	1 (alkali group)
Period:	2
Atomic Weight:	6.94
Relative Density:	0.53
Melting point:	180 °C / 357 °F
Boiling point:	1330 °C / 2426 °F

Luthium (Li), from the Greek word for stone, lithos, is the lightest metal, as well as the first alkali on the periodic table. As with other alkali metals, lithium readily reacts with oxygen and water, requiring the pure form to be stored in oil. It also means it doesn’t occur on its own in nature. It does, however, appear in batteries!

Lithium batteries

Lithium (not rechargeable lithium ion) batteries contain a fair amount of the pure metal, whether new or discharged. It is fairly easy to disassemble an AA, but keep in mind that lithium will react with the moisture on your skin and burn you – wear gloves! Double and triple A batteries use iron disulfide as an electrolyte; if lithium and iron disulfide react together in water, it will form hydrogen gas and sulfuric acid as well! Even without that, iron disulfide is the chemical used in fart bombs… enjoy!

Begin by removing the plastic insulation / label. Using side cutters, remove the top (positive) of the battery; there is usually a grove. Remove the inside core. You may need to cut down the side of the casing a bit to avoid it coming out like a fly trap. Keep in mind that the core will heat up quickly if you squish it and allow the lithium and iron disulfide to connect and short circuit.

Unwrap and separate the layers until you have the long lithium strip.

Lithium strip inside a battery

Lithium will fizz vigorously if water contacts it, and tarnish in air. Use a mineral oil soaked paper towel to remove the electrolyte, then place the metal in mineral oil to keep it from reacting. Because of its low density, it will float and will still tarnish over time. Lithium will readily burn with a very bright red flame.

Aside from its usage in batteries, lithium is used as an antidepressant medication, as well as a lubricant.