The Electron configuration of uranium is [Rn] 5f3 6d1 7s2. Uranium is known as a chemical element that belongs to the periodic table of elements. Its atomic number is 92, it belongs to the actinide series and is represented by the chemical symbol U.
It is metallic and has a grayish and silvery tint. It is composed of 92 electrons and 92 protons, with a valence of 6. Its nucleus is composed of 146 to 142 neutrons. Its most abundant isotopes are U235 with 143 electrons and U238 with 146.
Uranium is the element with the greatest atomic weight of all the others found in nature. This element has a density about 70% greater than that of lead, but less than that of tungsten or gold. It has a slight radioactivity. It was discovered in oxide form in 1789 and was named after the planet Uranus, discovered in 1781.
Electron configuration of uranium
With the Electron configuration it is possible to define the structure that the electrons have in the atoms of any element.
Uranium has a complete electron configuration described as 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10 5s2 5p6 4f14 5d10 6s2 6p6 5f3 6d1 7s2, its simplified or abbreviated version is [Rn] 5f3 6d1 7s2.
There are 92 electrons in total for uranium, the breakdown of these is: the first shell is made up of 2 electrons, the second shell houses 8 electrons, the third shell is made up of 18, in the fourth shell there are has 32 electrons, in the fifth there are 21 electrons, the sixth shell has 9 electrons, the seventh and last shell has 2.
The average radius of this element is 175 pm, its Van der Walls radius is equal to 186 pm, its Bohr radius or atomic radius is 156 pm, while its covalent radius is written as 196 ± 7 pm. Uranium is an element that is in period 7 and in group 3 of the periodic table of elements. The atomic mass of uranium is 238.02891 u.
Properties of uranium
- Uranium is located in the actinide series of the periodic table of chemical elements. Actinides are characterized by a higher atomic number, they are not found in nature and their lifespan is short. All isotopes belonging to this group, including uranium, are radioactive.
- Uranium is naturally found in the solid state.
- The appearance of uranium is metallic, silvery and white.
- It is represented by the chemical symbol U and its corresponding atomic number is 92.
- The boiling point of this element is equal to 4131.85 degrees Celsius or degrees Celsius, similar to 4404 degrees Kelvin.
- Uranium has a melting point of 1132.85 degrees Celsius or Celsius which is the same at 1405 Kelvin.
Origin and obtaining of uranium
- As with each of the elements that have atomic weights greater than iron, this element has a natural origin in the explosions that occur in supernovae. The physical process that is determined during the collapse that occurs in a supernova is gravity.
- The extremely high values of gravity which develop in supernovae are at the origin of the captures of neutrons which generate heavier atoms, among which protactinium and uranium.
Be careful with the Uranium configuration
- The proper functioning of the brain, kidneys, heart, liver and other systems can be damaged by exposure to uranium because it is weakly radioactive. Uranium is also a very toxic metal, even if it is found in small quantities.
- Uranium represents reproductive toxicity. The radiological effects are essentially local because alpha radiation, which is the main form of decay of the isotope U238, has a fairly short range and cannot penetrate the skin.
- Uranium compounds (present in their Electron configuration) are generally poorly absorbed by the wall of the lungs and can constitute a radiological hazard for an indefinite period.
- Exposure to uranium and its decay products, particularly radon, poses well-known health threats. Finely divided uranium metal can ignite because small particles can ignite spontaneously in air at room temperature.
- Nuclear power plants do not produce pollution in the atmosphere, but they do generate large amounts of radioactive waste. These residues harm the environment and health, for this reason they must be stored in highly secure areas for a long time, even for millions of years.