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Electron Configuration and Orbital Diagram

8. 17 Cl

   Orbital Diagram :

   ↑↓      ↑↓     ↑↓  ↑↓  ↑↓     ↑↓     ↑↓  ↑↓  ↑_

    1     2            2          3        3

   Electron Configuration

    1  2  2  3  3  

    or  [Ne] 3  3

9. 20 Ca

   Orbital Diagram :

    ↑↓      ↑↓     ↑↓  ↑↓  ↑↓     ↑↓     ↑↓  ↑↓  ↑↓     ↑↓

     1     2            2          3          3           4

   Electron Configuration

    1  2  2  3 3 4  

    or  [Ar] 4

10. 35 Br

     Orbital Diagram :

↑↓     ↑↓     ↑↓  ↑↓  ↑↓     ↑↓     ↑↓  ↑↓  ↑↓     ↑↓    ↑↓  ↑↓  ↑↓  ↑↓  ↑↓   ↑↓  ↑↓  ↑

1     2            2          3          3           4                3                     4

Electron Configuration

1 2 2  3  3 4  3  4    

or    [Ar]  4  3  4

Explanation:

The electron configuration tells us how the electrons are distributed in the atomic orbitals. It specifically tells us how electrons are arranged around the nucleus or the orbitals around the nucleus. There is a standard and correct order by which electrons occupy the orbitals. Electrons start to fill up orbitals of lower energies first. The order of the filling up of orbitals follows the order below:

1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p

The s orbital can hold a maximum of 2 electrons, p orbital can hold up to 6 electrons, d can hold up to 10 electrons, and the f orbital holds a maximum of 14 electrons. The number of electrons the subshell holds is written as superscript.

In writing the electron configuration, elements with large atomic numbers, the standard notation often has lengthy electron configurations. For these cases, another way to write the electron configuration is by having an abbreviated or condensed notation. This may be used instead of the standard notation. In the abbreviated notation, the noble gas which has completely filled subshells is replaced with the symbol of that noble gas in square brackets followed by the remaining orbitals filled.

An orbital filling diagram is a more visual way to represent the arrangement of all the electrons in a particular atom. Electrons are indicated by arrows. An arrow pointing upwards indicates one spin direction, while a downward pointing arrow indicates the other direction. It follows Hund's rule which states that orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron and that each of the single electrons must have the same spin.

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