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You are watching: Using noble gas notation write the electron configuration for the sodium atom.

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Electronic configuration, likewise called electronic structure, the arrangement of electrons in power levels roughly an atom nucleus. Follow to the older covering atomic model, electron occupy number of levels indigenous the very first shell nearest the nucleus, K, v the saturday shell, Q, the furthest from the nucleus. In terms of a much more refined, quantum-mechanical model, the KQ shells are subdivided into a collection of orbitals (see orbital), every of which have the right to be occupied by no more than a pair of electrons. The table listed below lists the variety of orbitals easily accessible in every of the first four shells.

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


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The digital configuration of an atom in the quantum-mechanical version is stated by listing the populated orbitals, in order of filling, through the variety of electrons in each orbital suggested by superscript. In this notation, the electronic configuration of sodium would be 1s22s22p63s1, spread in the orbitals as 2-8-1. Often, a shorthand method is offered that lists just those electrons in overfill of the noble gas configuration instantly preceding the atom in the regular table. For example, sodium has one 3s electron in overfill of the noble gas neon (chemical price Ne, atomic number 10), and so the shorthand notation is 3s1.

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Elements in the same group in the regular table have similar electronic configurations. For example, the facets lithium, sodium, potassium, rubidium, cesium, and francium (the alkali metals of team I) all have digital configurations reflecting one electron in the outermost (most loose bound) s orbital. This so-called valence electron is responsible for the comparable chemical properties mutual by the above-mentioned alkali facets in team I: shining metallic lustre, high reactivity, and an excellent thermal conductivity.