Lithium

Located at Group 1 and Period 2 of the Periodic Table is the element used in batteries. This is Lithium.

First discovered by Johan August Arfwedson in 1817 and first isolated by William Thomas Brande in 1821.

Johan August Arfwedson

Petalite

Actually, Lithium's ore was first discovered by a Brazilian Chemist José Bonifácio de Andrada e Silva in 1800 while he was in a mine in the island of Utö, located at Sweden. However, Jose wasn't aware of the new element containing in the ore he was holding. So, Jose lost his discovery credit.

Until 1817, Johan August Arfwedson went in detail of analyzing the ore found by José, Petalite. He got very confused when he finally purified the ore. He couldn't identify the remaining 10 percent in the Petalite. He decided to name the missing 10 percent of the element Lithium.

The same result have been founded in the following few ores Johan came through, Spodumene and Lepidolite. The following year, another chemist called Christian Gmelin was the first to observe that the bright red color flame was given by red Lithium salts. However, despite these two discoveries, both chemists still fail to isolate Lithium.

William Thomas Brande

Because Johan and Gmelin wasn't able to produce pure Lithium, many scientists tried too. However, almost none of them succeed. Lithium was isolated only at 1821, which William Thomas Brande isolated Lithium by the electrolysis of Lithium Oxide. This method of electrolysis used by William Thomas Brande is once used by Sir Humphry Davy to isolate Potassium and Sodium. So, because of this, William officially became the first isolator of Lithium, after so many failures.

After Lithium was isolated in 1821, larger quantities of Lithium was produced in 1855, which was also produced through electrolysis of Lithium Chloride. This discovery was made by Robert Bunsen and Augustus Matthiessen. The result of this discovery was used by a German Company in 1923 to produce many Lithium.

Today, Lithium was isolated using the same way Robert Bunsen and Augustus Matthiessen used. They converted Lithium Compounds to Lithium Chloride, which then an electric current passes through molten Lithium Chloride. The electrical current separates the compound into Lithium and Chlorine Gas purely.

Lithium is a quite common element, which ranks as 24th most abundant element on Earth. It is estimated to be 17 - 20 parts per million of Lithium on Earth. The most common ores that contain Lithium are Spodumene, Petalite and Lepidolite.

Spodumene

The world Largest producer of Lithium is United States, Australia, Canada, Zimbabwe, Chile and China. Some mines of Lithium in the U.S are Silver Peak, Nevada, Kings Mountain and Bessemer City, which is located in California.

There is many health benefits for Lithium, which helps reduce the severity and frequency of mental illnesses. Studies about Lithium also states that Lithium also help reduce suicidal risks. Lithium can also prevent future mental illnesses and depressive episodes. However, there are still side effects. Curing mental illnesses can help by eating Lithium, however, the person will get depression. He/ she will get moody for further consuming.

When mental illnesses peoples starts eating Lithium, they will get diarrhea, dizziness, muscle weakness, fatigue and a dazed feeling. These effects will improve if continued use of Lithium is made. However, fine tremor, frequent urination and thirst will occur if continued used.

So, just... try not to be mental, okay?

Atomic Number : 3
Name : Lithium
Latin Name : Lithium
Electrons per shell : [ 2, 1 ]
Discoverer : Johan August Arfwedson ( 1817 )
Isolator : William Thomas Brande ( 1821 )
Element's : Atomic Mass : 6.941 u
                  : Density : 0.534 g/cm³
              : Type : Alkali Metals
Chemical Properties : 

Lithium - 7

• An active element
• Reacts slowly with water
• Reacts with acids, giving off Hydrogen gas
• Doesn't react with oxygen at room temperature
• Reacts above 100 degrees Celsius to form Lithium Oxide
• Combines with Sulfur
• Combines with Hydrogen
• Combines with Nitrogen
• Combines with Halogens
• 14 isotopes : 3 of them are :
      Lithium - 6 : Protons : 3
                         : Neutrons : 3
                         : Protons : 3
     ( Half Life : Stable )
  
      Lithium - 7 : Protons : 3
                         : Neutrons : 4
                         : Protons : 3
     ( Half Life : Stable )
  
      Lithium - 8 : Protons : 3
                         : Neutrons : 5
                         : Protons : 3
     ( Half Life : 839.40 milliseconds )

Physical Properties : 

• Soft
• Silvery colored
• Melting Point : 180.54 degrees Celsius ( 356.97 Fahrenheit )
• Boiling Point : 1335 degrees Celsius ( 2435 Fahrenheit )

How Lithium got its name?

Lithium got its name from the Greek Word ' Lithos ', meaning ' stone '. The name was given by Lithium's discoverer, Johann Arfvedson.

Uses

Lithium's most common use in our daily cellphones, which is called Lithium - Ion batteries. Lithium was used because it is highly reactive that Lithium readily loses its outermost electron, making Lithium easy to get current flowing through a battery. Second, Lithium is also much lighter than any other metals that are used in batteries, such as lead. This properties is important because small objects such as phones and cars require many batteries. Lithium is light enough, so, Lithium is used.

Lithium - Ion Batteries

Lithium is also used to treat mental depression people. The symptoms of Mental depression are hyperactivity, rushed speech, poor judgment, reduced need to sleep, aggression and anger. If any of your friends or relatives have this symptoms mentioned above, kindly consult a Mental Doctor at a Mental Hospital to cure your Mental Friend or Mental Relative.

Anyway, Lithium is also alloyed with Carbon and Oxygen to form Lithium Carbonate. This alloy can make glass stronger. Some example of this type of glass is the glass used in labs,Tupperware and many other glass products. The glass is called Pyrex.

Besides, a alloy called Lithium Stearate is also added to Petroleum for making of thick lubricating grease. This grease is used in many industrial applications because it doesn't break down at high temperatures. This grease is very special. This grease doesn't even harden when cooled, doesn't even react with water or even oxygen in the air. This makes this grease applicable in military, industrial, automotive, aircraft and even marine purposes!

Mark 50 torpedo

THIS IS THE END OF LITHIUM

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