{"id":14,"date":"2020-04-08T14:55:02","date_gmt":"2020-04-08T14:55:02","guid":{"rendered":"https:\/\/thechemicalelements.com\/?page_id=14"},"modified":"2023-08-16T11:31:44","modified_gmt":"2023-08-16T11:31:44","slug":"lithium","status":"publish","type":"post","link":"https:\/\/thechemicalelements.com\/lithium\/","title":{"rendered":"Lithium (Li)"},"content":{"rendered":"\n

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Lithium is a chemical element with atomic number 3 in the periodic table. This chemical element is a mixture of lithium-6 and lithium-7, both stable isotopes. Lithium is the first metal element<\/a> classified according to Mendeleev\u2019s system of elements and it occurs in an abundance of 0.002% of Earth’s crust.\u00a0<\/span><\/p>\n\n\n\n

As a member of the alkali metals family<\/a> of periodic table elements, lithium has one valence electron and can form numerous compounds and reactions with other chemical elements. Its most important application is in the treatment of bipolar disorder.<\/span><\/p>\n\n\n\n

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Chemical and Physical Properties of Lithium<\/span><\/h3>\n\n\n\n

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Property<\/strong><\/td>Value<\/strong><\/td><\/tr>
Symbol<\/td>Li<\/td><\/tr>
Name<\/td>Lithium<\/td><\/tr>
Atomic number<\/td>3<\/td><\/tr>
Atomic weight (mass)<\/td>6.941 g.mol-1<\/td><\/tr>
Uses<\/td>Batteries, certain kinds of glass and ceramics, lubricants<\/td><\/tr>
Description<\/td>Hard, brittle, steel-gray metal. Lightest rigid metal. Sweet but deadly taste.<\/td><\/tr>
Group<\/td>1(IA) Alkali Metal<\/a><\/td><\/tr>
Period<\/td>2<\/td><\/tr>
Color<\/td>Silvery-white with a pearly luster<\/td><\/tr>
Physical state<\/td>Solid at room temperature<\/td><\/tr>
Half-life<\/td>From less than 10 nanoseconds to 839.4 milliseconds<\/td><\/tr>
Electronegativity<\/td>0.98<\/td><\/tr>
Density<\/td>0.53 g.cm-3 at 20\u00b0C<\/td><\/tr>
Melting point<\/td>453.69\u00b0C<\/td><\/tr>
Boiling point<\/td>1619.16\u00b0C<\/td><\/tr>
Van der Waals radius<\/td>0.145 nm<\/td><\/tr>
Ionic radius<\/td>0.76 (+1) \u00c5<\/td><\/tr>
Isotopes<\/td>10 (2 stable isotopes)<\/td><\/tr>
Most characteristic isotope<\/td>7Li<\/td><\/tr>
Electronic shell<\/td>[He] 2s1<\/td><\/tr>
The energy of the first ionization<\/td>520.1 kJ.mol-1<\/td><\/tr>
Crystal Structure<\/td>Cubic: Body centered<\/td><\/tr>
Covalent Radius<\/td>1.23 \u00c5<\/td><\/tr>
Atomic Radius<\/td>2.05 \u00c5<\/td><\/tr>
Atomic Volume<\/td>13.10 cm\u00b3\/mol<\/td><\/tr>
Name Origin<\/td>Greek: lithos (stone)<\/td><\/tr>
Discovery date<\/td>1817, by Johann Arfwedson<\/td><\/tr>
Location<\/td>Sweden<\/td><\/tr>
Pronunciation<\/td>LITH-i-em<\/td><\/tr>
Oxidation States<\/td>1<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

Lithium is a soft and silver-white alkali metal with the periodic table symbol Li, atomic number 3, atomic mass of 6.941 g.mol-1, and electron configuration X. This actinium<\/a> is ductile and reaches its boiling point at 1342\u00b0C (2448\u00b0F, 1615 K), while its melting point is at 180.50\u00b0C (356.90\u00b0F, 453.65 K). This highly reactive member of the alkali metals family of elements in the periodic table has an electronegativity of 1.0 according to Pauling. The atomic radius according to van der Waals is 0.145 nm.\u00a0<\/span><\/p>\n\n\n\n

The chemical properties of lithium resemble the properties of the alkali metals sodium<\/a> and potassium<\/a>. Lithium shares similar atomic and ionic radii with magnesium<\/a>, which is evident from the oxidation states they adopt, as well as from their oxidation properties. This alkali metal has a monoclinic crystal formation and is highly corrosive.\u00a0<\/span><\/p>\n\n\n\n

Lithium burns with a brilliant white flame and reacts violently when it comes into contact with water, a process that results in hydrogen<\/a> gas and an alkali metal hydroxide solution (lithium hydroxide (LiOH)). Due to its light atomic weight, this chemical substance floats on water. Element 3 of the periodic table is more easily soluble in cold water than in hot water.<\/span><\/p>\n\n\n\n

The low density and the high thermal and electrical conductivity are some of the main chemical properties that make lithium an ideal component of many metal alloys.<\/span><\/p>\n\n\n\n

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How Was Lithium Discovered?<\/span><\/h2>\n\n\n\n

According to writings that refer to events from the 2nd century AD, lithium was known to the <\/span>ancient civilizations<\/span><\/a> millennia before its discovery as a chemical element.\u00a0<\/span><\/p>\n\n\n\n

In modern times, lithium was discovered in 1817 by the Swedish chemist Johan August Arfvedson (1792-1841). By conducting an experimental analysis at <\/span>J\u00f6ns Jakob Berzelius<\/span><\/a>\u2019 Stockholm laboratory, Arfvedson attempted to confirm his belief that a certain petalite (LiAlSi4O10) sample hides a new metal that was waiting to be discovered. According to his projections, this new element had to be a new alkali metal that was lighter than sodium.\u00a0<\/span><\/p>\n\n\n\n

Because of his hypothesis, Arfvedson used the same method of electrolysis that Sir Humprey Davy employed in 1807 when he discovered sodium. However, the attempt of the Swedish chemist to isolate the new alkali metal with electrolysis from the ore sample obtained from a Swedish iron<\/a> mine was not successful.\u00a0<\/span><\/p>\n\n\n\n

However, Arfvedson\u2019s work was not futile. Although he didn\u2019t succeed in isolating the elemental form of lithium, he did manage to detect the new metal in the minerals spodumene and lepidolite.<\/span><\/p>\n\n\n\n

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The Contribution of William Thomas Brande and Sir Humphry Davy  to the Discovery of Lithium <\/span><\/h3>\n\n\n\n

In 1818, William Thomas Brande and Sir Humphry Davy attempted to finish the chemical trial started by Arfvedson. By using the electrolysis method on lithium oxide, these two chemists finally managed to isolate the pure elemental form of the lithium metal. Upon performing the experiment, Davy observed that the new element emitted a red flame that resembled that of strontium<\/a>. The new metallic substance produced an alkali solution when dissolved in water.<\/span><\/p>\n\n\n\n

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How Did Lithium Get Its Name?<\/span><\/h2>\n\n\n\n

The name of this element originates from the Greek word \u2018<\/span>lithos<\/span><\/i>\u2019, meaning \u2018<\/span>stone<\/span><\/i>\u2019. The reason behind the name is the fact that this alkali metal is obtained from mineral rocks, unlike the other alkali members of its group.<\/span><\/p>\n\n\n\n

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Where Can You Find Lithium?<\/span><\/h2>\n\n\n\n

Despite being one of the three chemical elements (along with hydrogen and helium<\/a>) that were created within the first three minutes of the Universe\u2019s birth – the <\/span>Big Bang<\/span><\/a> –\u00a0 lithium is rarely found free in the Universe. This highly reactive chemical element is present in the human body, the soil, plants, and animals, as well as in numerous compounds. It\u2019s mainly extracted from ores and mineral springs.\u00a0<\/span><\/p>\n\n\n\n

Lepidolite<\/span><\/i> and <\/span>spodumene<\/span><\/i> are the most common mineral forms in which lithium occurs. These two minerals are found in abundance in a special igneous rock deposit, referred to as <\/span>pegmatite<\/span><\/i>. Lithium carbonate may also be recovered from subsurface brines encapsulated in the Earth\u2019s crust.<\/span><\/p>\n\n\n\n

For commercial purposes, lithium is obtained from the minerals petalite (LiAl(Si2O5)2, lepidolite K(Li,Al)3(Al,Si,Rb)4O10(F,OH)2, and spodumene LiAl(SiO3)2. This chemical is produced by the electrolysis of a fused mixture of lithium and potassium chlorides. The largest amounts of lithium come from Chile, Australia, China, Argentina, Russia, Canada, Zimbabwe, Portugal, Brazil, and Bolivia. The richest lithium mineral ore locations in the world can be found in these countries.\u00a0<\/span><\/p>\n\n\n\n

On the other hand, South Dakota, in the United States, is the location of the largest spodumene ore deposits that are used for the extraction of lithium aluminum silicate. In the United States, lithium can also be obtained from the brine pools in Nevada<\/span>.<\/p>\n\n\n\n

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Lithium in Everyday Life<\/span><\/h2>\n\n\n\n

The primary use of lithium compounds, also referred to as <\/span>lithium salts<\/span><\/i>, is in the treatment of some psychiatric conditions and mental illnesses that do not improve from the administration of antidepressants in the therapy of an affected individual.<\/span><\/p>\n\n\n\n

Additionally, numerous lithium compounds have a broad range of applications in various industries. They are used in the following instances:<\/span><\/p>\n\n\n\n