We elaborate the uses of Lithium and atomic properties with characteristics. Lithium is a silver / gray white chemical element with an atomic number 3. Its symbol is Li and it belongs to the group of alkalis and its usual state in nature is solid. Lithium is located at position 3 on the periodic table.
On this page you can discover the chemical properties of lithium and information about lithium and other elements on the periodic table such as hydrogen, sodium, beryllium or magnesium. You will also learn what lithium is for and you will know what its uses are through its properties associated with lithium such as its atomic number or the usual state in which lithium can be found.
You will see qualities of lithium such as its melting and boiling point, its magnetic properties or what its chemical symbol is. In addition, here you will find information about its atomic properties such as the distribution of electrons in lithium atoms and other properties.
For some elements, some of this information is unknown. In these cases we show the properties attributed to them.
Among the properties of alkali metals such as lithium, its reaction to water is remarkable. When mixed with water, these elements, including lithium, in some cases emit light and in others, react violently, producing a large amount of energy. Hydrogen and hydroxides are produced from this reaction.
The state of lithium in its natural form is solid (non-magnetic). Lithium is a silver / gray white chemical element and belongs to the group of alkalis. The atomic number for lithium is 3. The chemical symbol for lithium is Li. The melting point of lithium is 453.69 degrees Kelvin or 181.54 degrees Celsius or degrees Celsius. The boiling point of lithium is 1615 degrees Kelvin or 1342.85 degrees Celsius or degrees Celsius.
Uses of lithium
Lithium is a light and highly reactive metal. Lithium is found in the composition of many stars. If you’ve ever wondered what lithium is for , here is a list of its possible uses:
- Lithium can be used as a refrigerant due to its high specific heat.
- Fireworks and red flares can be created from lithium compounds.
- Lithium hydroxide (LiOH) is used to make lithium soaps. These soaps are used to make lubricating greases.
- Lithium is used to create disposable and rechargeable batteries. Some examples of rechargeable batteries that use lithium are the lithium ion battery and the lithium iron phosphate battery .
- Lithium niobate is used to make mobile phones.
- Lithium is used to absorb neutrons in nuclear fusion.
- Lithium combines with other metals (usually aluminum , cadmium , copper, or manganese) to make aircraft parts.
- Lithium hydroxide and lithium peroxide are used to purify the air in submarines and in spacecraft. Lithium peroxide reacts with carbon dioxide to produce oxygen .
- One of the most important uses of lithium is in the treatment of bipolar disorder and depression. Lithium salts (such as lithium carbonate and lithium citrate) are mood stabilizers.
- Lithium can be used in focal lenses for telescopes and common glasses.
- Lithium Chloride and Lithium Bromide are effective desiccant. A desiccant is a substance that keeps something (usually a container) dry by absorbing (or adsorbing) water molecules .
- Lithium, and its hydrides, are used as high-energy additives in rocket boosters.
Atomic properties of lithium
The atomic mass of an element is determined by the total mass of neutrons and protons that can be found in a single atom belonging to this element. As for the position where to find lithium within the periodic table of the elements, lithium is in group 1 and period 2. Lithium has an atomic mass of 7.0160040 u.
The electronic configuration for lithium is [He] 2s1. The electronic configuration of the elements, determines the form in which the electrons are structured in the atoms of an element. The atomic radius or Bohr radius of lithium is 167 pm, its covalent radius is 134 pm, and its Van der Waals radius is 183 pm. Lithium has a total of 2 electrons whose distribution is as follows: In the first layer it has 2 electrons.
Below you can see a table showing the main characteristics of lithium.
|Appearance||silver white / gray|
|Density||535 kg / m3|
|Atomic mass||7.0160040 u|
|Covalent radius||134 pm|
|Van der Waals radio||183 pm|
|Electronic configuration||[He] 2s1|
|Electrons per layer||2|
|Oxidation states||1 (strong base)|
|Crystal structure||body centered cubic|
|Melting point||453.69 K|
|Boiling point||1615 K|
|Heat of fusion||3 kJ / mol|
|Electronegativity||0.98 (Pauling) 1 (Allred and Rochow)|
|Specific heat||3582 J / (K · kg)|
|Electric conductivity||10.8 × 106S / m|
|Thermal conductivity||84.7 W / (Km)|