electron configuration of all the elements<\/a> can be done through orbital diagrams.<\/p>\n\n\n\nElectron configuration of aluminum through orbital<\/h2>\n\n\n\n Atomic energy shells are subdivided into sub-energy levels. These sub-energy levels are also called orbital. The most probable region of electron rotation around the nucleus is called the orbital.<\/p>\n\n\n\n
The sub-energy levels depend on the azimuthal quantum number. It is expressed by \u2018l\u2019. The value of \u2018l\u2019 is from 0 to (n \u2013 1). The sub-energy levels are known as s, p, d, and f.<\/p>\n\n\n\nOrbit Number<\/strong><\/td>Value of \u2018l\u2019<\/strong><\/td>Number of subshells<\/strong><\/td>Number of orbital<\/strong><\/td>Subshell name<\/strong><\/td>Electrons holding capacity<\/strong><\/td>Electron configuration<\/strong><\/td><\/tr>1<\/td> 0<\/td> 1<\/td> 1<\/td> 1s<\/td> 2<\/td> 1s2<\/sup><\/td><\/tr>2<\/td> 0 2<\/td> 1 2s 2 2s2<\/sup> 2p6<\/sup><\/td><\/tr>3<\/td> 0 3<\/td> 1 3s 2 3s2<\/sup> 3p6<\/sup> 3d10<\/sup><\/td><\/tr>4<\/td> 0 4<\/td> 1 4s 2 4s2<\/sup> 4p6<\/sup> 4d10<\/sup> 4f14<\/sup><\/td><\/tr><\/tbody><\/table>Orbital number of the subshell<\/figcaption><\/figure>\n\n\n\nFor example,<\/p>\n\n\n\n
\nIf n = 1, If n = 2, If n = 3, If n = 4, If n = 5,Therefore, l = 0,1,2,3,4. The number of sub-shells will be 5 but 4s, 4p, 4d, and 4f in these four subshells it is possible to arrange the electrons of all the elements of the periodic table.<\/p>\n\n\n\nSub-shell name<\/strong><\/td>Name source<\/strong><\/td>Value of \u2018l\u2019<\/strong><\/td>Value of \u2018m\u2019Number of orbital (2l+1)<\/strong><\/td>Electrons holding capacitys<\/td> Sharp<\/td> 0<\/td> 0<\/td> 1<\/td> 2<\/td><\/tr> p<\/td> Principal<\/td> 1<\/td> \u22121, 0, +1<\/td> 3<\/td> 6<\/td><\/tr> d<\/td> Diffuse<\/td> 2<\/td> \u22122, \u22121, 0, +1, +2<\/td> 5<\/td> 10<\/td><\/tr> f<\/td> Fundamental<\/td> 3<\/td> \u22123, \u22122, \u22121, 0, +1, +2, +3<\/td> 7<\/td> 14<\/td><\/tr><\/tbody><\/table>Number of electrons in the orbital<\/figcaption><\/figure>\n\n\n\nThe orbital number of the s-subshell is one, three in the p-subshell, five in the d-subshell, and seven in the f-subshell. Each orbital can have a maximum of two electrons.<\/p>\n\n\n\n
The sub-energy level \u2018s\u2019 can hold a maximum of two electrons, \u2018p\u2019 can hold a maximum of six electrons, \u2018d\u2019 can hold a maximum of ten electrons, and \u2018f\u2019 can hold a maximum of fourteen electrons.<\/p>\n\n\n
\n
Electron configuration via Aufbau principle<\/figcaption><\/figure><\/div>\n\n\nAufbau is a German word, which means building up. The main proponents of this principle are scientists Niels Bohr and Pauli. The Aufbau method is to do electron configuration through the sub-energy level.<\/p>\n\n\n\n
The Aufbau principle is that the electrons present in the atom will first complete the lowest energy orbital and then gradually continue to complete the higher energy orbital.<\/p>\n\n\n\n
The energy of an orbital is calculated from the value of the principal quantum number \u2018n\u2019 and the azimuthal quantum number \u2018l\u2019. The orbital for which the value of (n + l) is lower is the low energy orbital and the electron will enter that orbital first.<\/p>\n\n\n\nOrbital<\/strong><\/td>Orbit (n)<\/strong><\/td>Azimuthal quantum number (l)<\/strong><\/td>Orbital energy (n + l)<\/strong><\/td><\/tr>3d<\/td> 3<\/td> 2<\/td> 5<\/td><\/tr> 4s<\/td> 4<\/td> 0<\/td> 4<\/td><\/tr><\/tbody><\/table>Energy of orbital<\/figcaption><\/figure>\n\n\n\nHere, the energy of 4s orbital is less than that of 3d. So, the electron will enter the 4s orbital first and enter the 3d orbital when the 4s orbital is full. The method of entering electrons into orbitals through the Aufbau principle is 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d.<\/p>\n\n\n\n
The first two electrons of aluminum enter the 1s orbital. The s-orbital can have a maximum of two electrons. Therefore, the next two electrons enter the 2s orbital.<\/p>\n\n\n\n
The p-orbital can have a maximum of six electrons. So, the next six electrons enter the 2p orbital. The second orbit is now full. So, the remaining electrons will enter the third orbit.<\/p>\n\n\n\n
Then two electrons will enter the 3s orbital of the third orbit and the remaining one electron will be in the 3p orbital. Therefore, the aluminum full electron configuration will be 1s2<\/sup> 2s2<\/sup> 2p6<\/sup> 3s2<\/sup> 3p1<\/sup>.<\/p>\n\n\n\n
Electron Configuration for Aluminum<\/figcaption><\/figure><\/div>\n\n\n\nNote:<\/strong> The unabbreviated electron configuration of aluminum is [Ne] 3s2<\/sup> 3p1<\/sup>. When writing an electron configuration, you have to write serially.<\/p>\n<\/blockquote>\n\n\n\nVideo for Aluminum Electron Configuration<\/h2>\n\n\n\n
![\"Aluminum](\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/12\/AluminumAl-atom-electron-configurationBohr-model.jpg\")
![\"position](\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/Position-of-aluminumAl-in-the-periodic-table-1024x509.jpg\")
![\"Electron](\"https:\/\/i0.wp.com\/valenceelectrons.com\/wp-content\/uploads\/2021\/12\/Electron-configuration-via-Aufbau-principal.jpg?resize=774%2C452&ssl=1\")
![\"Electron](\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2023\/03\/Electron-Configuration-for-Aluminum.jpg\")