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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, additionally called electronic structure, the setup of electron in power levels about an atom nucleus. Follow to the older shell atomic model, electrons occupy numerous levels native the first shell nearest the nucleus, K, through the saturday shell, Q, the furthest from the nucleus. In terms of a more refined, quantum-mechanical model, the KQ shells are subdivided into a collection of orbitals (see orbital), each of which can be inhabited by no much more than a pair of electrons. The table below lists the number of orbitals available in every of the very first four shells.

The electronic configuration of an atom in the shell atomic model may be express by indicating the variety of electrons in every shell beginning with the first. For example, sodium (atomic number 11) has its 11 electrons distributed in the very first three shells together follows: the K and also L shells are fully filled, v 2 and also 8 electron respectively, while the M covering is just partially filled through one electron.


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The electronic configuration of an atom in the quantum-mechanical model is proclaimed by listing the inhabited orbitals, in bespeak of filling, through the number of electrons in each orbital indicated by superscript. In this notation, the digital configuration the sodium would be 1s22s22p63s1, dispersed in the orbitals together 2-8-1. Often, a shorthand method is supplied that lists only those electron in overfill of the noble gas configuration instantly preceding the atom in the regular table. Because that example, sodium has one 3s electron in overabundance of the noble gas neon (chemical prize Ne, atomic number 10), and also so that is shorthand notation is 3s1.

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Elements in the same group in the regular table have comparable electronic configurations. Because that example, the aspects lithium, sodium, potassium, rubidium, cesium, and also francium (the alkali steels of group I) every have digital configurations mirroring 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.