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You are watching: Write the electron configuration for the na+ ion, which has ten electrons.

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electronic configuration, also called electronic structure, the setup of electrons in power levels about an atom nucleus. According to the older shell atomic model, electron occupy number of levels indigenous the first shell nearest the nucleus, K, v the saturday shell, Q, the furthest from the nucleus. In regards to a an ext refined, quantum-mechanical model, the KQ shells room subdivided into a collection of orbitals (see orbital), every of which can be occupied by no an ext than a pair the electrons. The table below lists the number of orbitals accessible in every of the very first four shells.

The electronic configuration of an atom in the shell atomic model might be expressed by denote the number of electrons in every shell start with the first. For example, salt (atomic number 11) has its 11 electrons dispersed in the an initial three shells as follows: the K and also L shells are fully filled, v 2 and also 8 electrons respectively, while the M covering is only partially filled through one electron.


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The digital configuration of an atom in the quantum-mechanical design is stated by listing the occupied orbitals, in stimulate of filling, with the number of electrons in every orbital shown by superscript. In this notation, the electronic configuration the sodium would certainly be 1s22s22p63s1, spread in the orbitals together 2-8-1. Often, a shorthand technique is used that lists only those electron in excess of the noble gas configuration immediately preceding the atom in the periodic table. Because that example, sodium has actually one 3s electron in overfill of the noble gas neon (chemical price Ne, atomic number 10), and so that shorthand notation is 3s1.

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Elements in the same group in the routine table have similar electronic configurations. Because that example, the elements lithium, sodium, potassium, rubidium, cesium, and also francium (the alkali steels of group I) every have digital configurations reflecting one electron in the outermost (most loosely bound) s orbital. This so-called valence electron is responsible because that the comparable chemical properties shared by the above-mentioned alkali aspects in team I: bright metallic lustre, high reactivity, and good thermal conductivity.