For example, the electron configuration of Oxygen (atomic number 8) is 1s ^2 2s ^2 2p^ 4. Each symbol has a subscript on the right indicating the number of electrons occupied in that subshell. The electron configuration is described by a notation that lists the subshell symbols, one after another. Shells closer to the nucleus have higher binding energy. The electron configuration for an element is the arrangement of electrons in the orbits (or shells) of a neutral atom. Note the crossover ofĮnergies from 1 orbital to another, particularly the fact that 4s has a Other atoms the energy depends on both n and l. Though theĮnergy levels in orbitals of Hydrogen depend only on the value of n, in The energy levels of different orbitals are indicated. The closer an electron is to the nucleus, the lower its energy level and the orbitals fill such that the next added electron will occupy the lowest energy level
As a result, the electrons are held less tightly which has a profound effect on the trends visible throughout the periodic table.
Part of the attractive force of the nucleus is disrupted by the repelling force of the inner electrons and we say they shield the outermost electrons from the nucleus. This phenomenon does not occur in Hydrogen, since it has a single electron but the repulsion of outer electrons by inner ones occurs in all other atoms. Just as the positive nucleus attracts it, the negative charges of its neighbouring electrons repel it. An electron’s energy level is not only determines by its distance from the nucleus but all by the presence of other electrons. Orbitals have varying energy levels with those furthest away from the nucleus having the greatest ones. In all atoms other then hydrogen, electrons in different
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