|silvery-white (shown floating in oil)
Spectral lines of lithium
|Name, symbol, number||lithium, Li, 3|
|Element category||alkali metal|
|Group, period, block||1, 2, s|
|Standard atomic weight||6.94(1) g·mol−1|
|Electron configuration||[He] 2s1|
|Electrons per shell||2, 1 (Image)|
|Density (near r.t.)||0.534 g·cm−3|
|Liquid density at m.p.||0.512 g·cm−3|
|Melting point||453.69 K, 180.54 °C, 356.97 °F|
|Boiling point||1615 K, 1342 °C, 2448 °F|
3223 K, 67 MPa
|Heat of fusion||3.00 kJ·mol−1|
|Heat of vaporization||147.1 kJ·mol−1|
|Specific heat capacity||(25 °C) 24.860 J·mol−1·K−1|
(strongly basic oxide)
|Electronegativity||0.98 (Pauling scale)|
|Ionization energies||1st: 520.2 kJ·mol−1|
|2nd: 7298.1 kJ·mol−1|
|3rd: 11815.0 kJ·mol−1|
|Atomic radius||152 pm|
|Covalent radius||128±7 pm|
|Van der Waals radius||182 pm|
|Crystal structure||body-centered cubic|
|Electrical resistivity||(20 °C) 92.8 nΩ·m|
|Thermal conductivity||(300 K) 84.8 W·m−1·K−1|
|Thermal expansion||(25 °C) 46 µm·m−1·K−1|
|Speed of sound (thin rod)||(20 °C) 6000 m/s|
|Young's modulus||4.9 GPa|
|Shear modulus||4.2 GPa|
|Bulk modulus||11 GPa|
|CAS registry number||7439-93-2|
|Most stable isotopes|
|Main article: Isotopes of lithium|
Lithium (from Greek lithos 'stone') is a soft, silver-white metal with symbol Li. It is the third chemical element in the periodic table. This means that it has 3 protons in its nucleus and 3 electrons around it. Its atomic number is 3. Its mass number is 6.94. It has two common isotopes, 6Li and 7Li. 7Li is more common. 92.5% of lithium is 7Li. Lithium is a soft silvery metal that is very reactive. It is used in lithium batteries and certain medicines.
Properties[change | edit source]
Physical properties[change | edit source]
Lithium is one of the alkali metals. Lithium is a silvery solid metal (when freshly cut). It is very soft. Thus it can be cut easily with a knife. It melts at a low temperature. It is very light, similar to wood. It is the least dense metal and the least dense element in a solid or liquid state. It can hold more heat than any other solid element. It conducts heat and electricity easily.
Chemical properties[change | edit source]
It will react with water, giving off hydrogen to form a basic solution (lithium hydroxide). Because of this, lithium must be stored in petroleum jelly. Sodium and potassium can be stored in oil but lithium cannot because it is so light. It will just float on the oil and not be protected by it.
Lithium also reacts with halogens. It can react with nitrogen gas to make lithium nitride. It reacts with air to make a black tarnish and then a white powder of lithium hydroxide and lithium carbonate.
Chemical compounds[change | edit source]
See also: Category:Lithium compounds
Lithium forms chemical compounds with only one oxidation state: +1. Most of them are white and unreactive. They make a bright red color when heated in a flame. They are a little toxic. Most of them dissolve in water. Lithium carbonate is less soluble in water than the other alkali metal carbonates like sodium carbonate.
- Lithium carbonate, used in medicine
- Lithium chloride, colorless crystalline solid, red flame when heated
- Lithium hydroxide, strong base, used to remove carbon dioxide in spaceships
- Lithium nitrate, oxidizing agent
- Lithium nitride, strong base
- Lithium oxide, dissolves in water to make lithium hydroxide
- Lithium peroxide, reacts with water to make oxygen
Occurrence[change | edit source]
It does not occur as an element in nature. It only is in the form of lithium compounds. The ocean has a large amount of lithium in it. Certain granites have large amounts of lithium. Most living things have lithium in them. There are some places where much lithium is in the salt. Some silicates have lithium in them.
History[change | edit source]
Lithium (Greek lithos, meaning "stone") was discovered by Johann Arfvedson in 1817. In 1818, Christian Gmelin observed that lithium salts give a bright red color in flame. W.T. Brande and Sir Humphrey Davy later used electrolysis on lithium oxide to isolate the element. Lithium was used first in greases. Then nuclear weapons became a big use of lithium. Lithium was also used to make glass melt easier and make aluminium oxide melt easier in making aluminium. Now lithium is used mainly in batteries.
Preparation[change | edit source]
Uses[change | edit source]
As an element[change | edit source]
Its main use is in batteries. Lithium is used as an anode in the lithium battery. It has more power than batteries with zinc, like alkaline cells. Lithium ion batteries also have lithium in them, though not as an element. It is also used in heat transfer alloys. Lithium is used to make organolithium compounds. They are used for very strong bases.
In chemical compounds[change | edit source]
Lithium compounds are used in some drugs known as mood stabilizers. Lithium niobate is used in radio transmitters in cell phones. Some lithium compounds are also used in ceramics. Lithium chloride can absorb water from other things. Some lithium compounds are used to make soap and grease.
Safety[change | edit source]
Lithium reacts with water, making irritating smoke and heat. It is not as dangerous as the other alkali metals. Lithium hydroxide is very corrosive.
Isotopes[change | edit source]
There are 5 isotopes of Lithium having respectively 2, 3, 4, 5 and 6 neutrons in the nucleus. The most common isotope in nature is 3Li7 which makes up 92.58 % of the total. The second isotope which is widely available is 3Li6 which makes up 7.42 % of the total. The other 3 isotopes exist in very small quantities. The atomic mass of Lithium is 6.939.
Related pages[change | edit source]