electronic configuration of elempents
Answers
Explanation:
here are some electronic configuration of elements
Explanation:
Electron Configuration Formula for Chemical Elements
Electron configuration or electronic structure of the periodic table elements holds the key to the chemical world in physical and chemical science. Therefore, the chemical properties like oxidizing reducing properties, oxidation number, ionization energy, electron affinity, calculation of shielding effect, the polarity of chemical bonds, etc. are better understood by the electronic configuration formula of elements. A chemical reaction is the change of electron configuration of reactant and product atoms. Hence the organic and inorganic chemical reactions better understood by the electronic structure of chemicals elements. To find the electron configuration first we find the energy of an electron in s, p, d, and f orbitals or sub-levels, for example, 3s orbital has lower energy than 3p orbitals which again lower energy than 3d level. The modern periodic table classification bases on electron configuration and chemical properties to form s, p, d, and f block in the periodic table.
Energy Levels of Electron Orbitals
But difficult for readers to remember the energy levels diagram for many electronic structures. Therefore, the trivial way but most convenient way to remember these energy levels provides in online colleges and schools courses by below this orbital diagram
The different electron orbitals originating from the same energy levels are written in the horizontal dimensions.
Now inclined parallel lines are drawn through the orbitals according to the above picture. Filling up the different orbitals by the number of electrons will follow these lines.
Therefore, according to above digram structure, filling up energy levels with electron particle constructued the following ordering of electronic orbitals
1S < 2S < 2P < 3S < 3P < 4S < 3d < 4P < 5S < 4d < 5P < 6S < 4f < 5d < 6P < 7S < 5f…
Formula for Filling Orbitals and Electronic Configuration
The filling up of orbitals with electron around the nucleus of an atom takes place according to the certain formula which is given below,
The maximum number of electrons in the main quantum shell = 2n2, where n = principal quantum number.
The maximum number of the electron in sub-shell like s, p, d, and f orbitals = 2(2l+1), where l = 0, 1, 2, 3 for s, p, d, f orbitals. Therefore, s, p, d, f energy levels have a maximum of 2, 6, 10, 14 electrons respectively.
German scientist Aufbau express building up a principle for electron filling up the process in different orbitals of an atom. Hence according to this principle, the electrons are filled up in order of energy. Therefore, the orbitals with the lowest energy filled up first while the highest energy orbital filled up in the end.
The electron will tend to form maximum spin. Therefore, electrons with similar spin occupied first.
According to Hund’s rule, electrons are filling in the orbital with maximum spin multiplicity.
Spin pairing occurs only when vacant orbitals of similar energy are not available for occupation.