{"id":4048,"date":"2023-03-18T00:34:46","date_gmt":"2023-03-17T18:34:46","guid":{"rendered":"https:\/\/valenceelectrons.com\/?p=4048"},"modified":"2023-11-08T18:26:39","modified_gmt":"2023-11-08T12:26:39","slug":"iron-electron-configuration","status":"publish","type":"post","link":"https:\/\/valenceelectrons.com\/iron-electron-configuration\/","title":{"rendered":"Electron Configuration for Iron (Fe and Fe2+, Fe3+ ions)"},"content":{"rendered":"\n<p>Iron is the 26th element in the periodic table and its symbol is \u2018Fe\u2019. In this article, I have discussed in detail how to easily write the complete electron configuration of iron.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">What is the electron configuration of iron?<\/h2>\n\n\n\n<p>The total number of&nbsp;<a href=\"https:\/\/valenceelectrons.com\/iron-protons-neutrons-electrons\/\">electrons in iron<\/a>&nbsp;is twenty-six. These electrons are arranged according to specific rules in different orbitals.<\/p>\n\n\n\n<p>The arrangement of electrons in iron in specific rules in different orbits and orbitals is called the&nbsp;<a href=\"https:\/\/valenceelectrons.com\/electron-configuration\/\">electron configuration<\/a>&nbsp;of iron.<\/p>\n\n\n\n<p>The electron configuration of iron is [<a href=\"https:\/\/valenceelectrons.com\/argon-electron-configuration\/\">Ar<\/a>] 3d<sup>6<\/sup>&nbsp;4s<sup>2<\/sup>,&nbsp;if the electron arrangement is through orbitals. Electron configuration can be done in two ways.<\/p>\n\n\n\n<ul>\n<li>Electron configuration through orbit&nbsp;(Bohr principle)<\/li>\n\n\n\n<li>Electron configuration through orbital&nbsp;(Aufbau principle)<\/li>\n<\/ul>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"797\" height=\"473\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/01\/IronFe-atom-electron-configurationBohr-model.jpg\" alt=\"Iron atom electron configuration\" class=\"wp-image-4070\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/01\/IronFe-atom-electron-configurationBohr-model.jpg 797w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/01\/IronFe-atom-electron-configurationBohr-model-300x178.jpg 300w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/01\/IronFe-atom-electron-configurationBohr-model-768x456.jpg 768w\" sizes=\"(max-width: 797px) 100vw, 797px\" \/><figcaption class=\"wp-element-caption\">Iron(Fe) atom electron configuration(Bohr model)<\/figcaption><\/figure><\/div>\n\n\n<p>Electron configuration through orbitals follows different principles. For example Aufbau principle, Hund\u2019s principle, and Pauli\u2019s exclusion principle.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"iron-fe-electron-configuration-through-orbit\">Iron atom electron configuration through orbit<\/h2>\n\n\n\n<p>Scientist Niels Bohr was the first to give an idea of the atom\u2019s orbit. He provided a model of the atom in 1913. The complete idea of the orbit is given there.<\/p>\n\n\n\n<p>The <a href=\"https:\/\/valenceelectrons.com\/how-to-find-protons-neutrons-and-electrons\/\">electrons of the atom<\/a> revolve around the nucleus in a certain circular path. These circular paths are called orbit(shell). These orbits are expressed by n. [n = 1,2,3,4 . . . The serial number of the orbit]<\/p>\n\n\n\n<p>K is the name of the first orbit, L is the second, M is the third, and N is the name of the fourth orbit. The electron holding capacity of each orbit is 2n<sup>2<\/sup>.<\/p>\n\n\n\n<figure class=\"wp-block-table\"><table><tbody><tr><td class=\"has-text-align-center\" data-align=\"center\"><strong>Shell Number (n)<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Shell Name<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Electrons Holding Capacity (2n<sup>2<\/sup>)<\/strong><\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">1<\/td><td class=\"has-text-align-center\" data-align=\"center\">K<\/td><td class=\"has-text-align-center\" data-align=\"center\">2<\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">2<\/td><td class=\"has-text-align-center\" data-align=\"center\">L<\/td><td class=\"has-text-align-center\" data-align=\"center\">8<\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">3<\/td><td class=\"has-text-align-center\" data-align=\"center\">M<\/td><td class=\"has-text-align-center\" data-align=\"center\">18<\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">4<\/td><td class=\"has-text-align-center\" data-align=\"center\">N<\/td><td class=\"has-text-align-center\" data-align=\"center\">32<\/td><\/tr><\/tbody><\/table><figcaption class=\"wp-element-caption\">Electron holding capacity of shells<\/figcaption><\/figure>\n\n\n\n<p>For example,<\/p>\n\n\n\n<ol>\n<li>n = 1 for K orbit.<br>The maximum electron holding capacity in K orbit is 2n<sup>2<\/sup>&nbsp;= 2 \u00d7 1<sup>2<\/sup>&nbsp;= 2.<\/li>\n\n\n\n<li>For L orbit, n = 2.<br>The maximum electron holding capacity in L orbit is 2n<sup>2<\/sup>&nbsp;= 2 \u00d7 2<sup>2<\/sup>&nbsp;= 8.<\/li>\n\n\n\n<li>n=3 for M orbit.<br>The maximum electron holding capacity in M orbit is 2n<sup>2<\/sup>&nbsp;= 2 \u00d7 3<sup>2&nbsp;<\/sup>= 18.<\/li>\n\n\n\n<li>n=4 for N orbit.<br>The maximum electron holding capacity in N orbit is 2n<sup>2<\/sup>&nbsp;= 2 \u00d7 4<sup>2<\/sup>&nbsp;= 32.<\/li>\n<\/ol>\n\n\n\n<p>Therefore, the maximum electron holding capacity in the first shell is two, the second shell is eight and the 3rd shell can have a maximum of eighteen electrons.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-large\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"463\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/10\/Position-of-ironFe-in-the-periodic-table-1024x463.jpg\" alt=\"Position of iron(Fe) in the periodic table\" class=\"wp-image-3293\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/10\/Position-of-ironFe-in-the-periodic-table-1024x463.jpg 1024w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/10\/Position-of-ironFe-in-the-periodic-table-300x136.jpg 300w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/10\/Position-of-ironFe-in-the-periodic-table-768x347.jpg 768w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/10\/Position-of-ironFe-in-the-periodic-table.jpg 1288w\" sizes=\"(max-width: 1024px) 100vw, 1024px\" \/><figcaption class=\"wp-element-caption\">Position of iron(Fe) in the periodic table<\/figcaption><\/figure><\/div>\n\n\n<p>The atomic number is the number of electrons in that element. The atomic number of iron is 26. That is, the number of electrons in iron is twenty-six. Therefore, the iron atom will have two electrons in the first shell and eight in the 2nd shell.<\/p>\n\n\n\n<p>According to Bohr\u2019s formula, the third orbit will have sixteen electrons but the third orbit of iron will have fourteen electrons and the remaining two electrons will be in the fourth orbit.<\/p>\n\n\n\n<p>Therefore, the order of the number of electrons in each shell of the iron(Fe) atom is 2, 8, 14, 2. Electrons can be arranged correctly through orbits from elements 1 to 18.<\/p>\n\n\n\n<p>The electron configuration of an element with an atomic number greater than 18 cannot be properly determined according to the Bohr atomic model. The <a href=\"https:\/\/valenceelectrons.com\/electron-configuration-of-all-elements\/\">electron configuration of all the elements<\/a> can be done through the orbital diagram.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"electron-configuration-of-iron-fe-through-orbital\">Electron configuration of iron through orbital<\/h2>\n\n\n\n<p>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<p>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\n<figure class=\"wp-block-table\"><table><tbody><tr><td class=\"has-text-align-center\" data-align=\"center\"><strong>Orbit Number<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Value of \u2018l\u2019<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Number of subshells<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Number of orbital<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Subshell name<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Electrons holding capacity<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Electron configuration<\/strong><\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">1<\/td><td class=\"has-text-align-center\" data-align=\"center\">0<\/td><td class=\"has-text-align-center\" data-align=\"center\">1<\/td><td class=\"has-text-align-center\" data-align=\"center\">1<\/td><td class=\"has-text-align-center\" data-align=\"center\">1s<\/td><td class=\"has-text-align-center\" data-align=\"center\">2<\/td><td class=\"has-text-align-center\" data-align=\"center\">1s<sup>2<\/sup><\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">2<\/td><td class=\"has-text-align-center\" data-align=\"center\">0<br>1<\/td><td class=\"has-text-align-center\" data-align=\"center\">2<\/td><td class=\"has-text-align-center\" data-align=\"center\">1<br>3<\/td><td class=\"has-text-align-center\" data-align=\"center\">2s<br>2p<\/td><td class=\"has-text-align-center\" data-align=\"center\">2<br>6<\/td><td class=\"has-text-align-center\" data-align=\"center\">2s<sup>2<\/sup>&nbsp;2p<sup>6<\/sup><\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">3<\/td><td class=\"has-text-align-center\" data-align=\"center\">0<br>1<br>2<\/td><td class=\"has-text-align-center\" data-align=\"center\">3<\/td><td class=\"has-text-align-center\" data-align=\"center\">1<br>3<br>5<\/td><td class=\"has-text-align-center\" data-align=\"center\">3s<br>3p<br>3d<\/td><td class=\"has-text-align-center\" data-align=\"center\">2<br>6<br>10<\/td><td class=\"has-text-align-center\" data-align=\"center\">3s<sup>2<\/sup>&nbsp;3p<sup>6<\/sup>&nbsp;3d<sup>10<\/sup><\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">4<\/td><td class=\"has-text-align-center\" data-align=\"center\">0<br>1<br>2<br>3<\/td><td class=\"has-text-align-center\" data-align=\"center\">4<\/td><td class=\"has-text-align-center\" data-align=\"center\">1<br>3<br>5<br>7<\/td><td class=\"has-text-align-center\" data-align=\"center\">4s<br>4p<br>4d<br>4f<\/td><td class=\"has-text-align-center\" data-align=\"center\">2<br>6<br>10<br>14<\/td><td class=\"has-text-align-center\" data-align=\"center\">4s<sup>2<\/sup>&nbsp;4p<sup>6<\/sup>&nbsp;4d<sup>10<\/sup>&nbsp;4f<sup>14<\/sup><\/td><\/tr><\/tbody><\/table><figcaption class=\"wp-element-caption\">Orbital number of the subshell<\/figcaption><\/figure>\n\n\n\n<p>For example,<\/p>\n\n\n\n<ul>\n<li>If n = 1,<br>(n \u2013 1) = (1\u20131) = 0<br>Therefore, the value of \u2018l\u2019 is 0. So, the sub-energy level is 1s.<\/li>\n\n\n\n<li>If n = 2,<br>(n \u2013 1) = (2\u20131) = 1.<br>Therefore, the value of \u2018l\u2019 is 0, 1. So, the sub-energy levels are 2s, and 2p.<\/li>\n\n\n\n<li>If n = 3,<br>(n \u2013 1) = (3\u20131) = 2.<br>Therefore, the value of \u2018l\u2019 is 0, 1, 2. So, the sub-energy levels are 3s, 3p, and 3d.<\/li>\n\n\n\n<li>If n = 4,<br>(n \u2013 1) = (4\u20131) = 3<br>Therefore, the value of \u2018l\u2019 is 0, 1, 2, 3. So, the sub-energy levels are 4s, 4p, 4d, and 4f.<\/li>\n\n\n\n<li>If n = 5,<br>(n \u2013 1) = (n \u2013 5) = 4.<\/li>\n<\/ul>\n\n\n\n<p>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\n<figure class=\"wp-block-table\"><table><tbody><tr><td class=\"has-text-align-center\" data-align=\"center\"><strong>Subshell name<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Name source<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Value of \u2018l\u2019<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Value of \u2018m\u2019<br>(0 to \u00b1 l)<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Number of orbital (2l+1)<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Electrons holding capacity<br>2(2l+1)<\/strong><\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">s<\/td><td class=\"has-text-align-center\" data-align=\"center\">Sharp<\/td><td class=\"has-text-align-center\" data-align=\"center\">0<\/td><td class=\"has-text-align-center\" data-align=\"center\">0<\/td><td class=\"has-text-align-center\" data-align=\"center\">1<\/td><td class=\"has-text-align-center\" data-align=\"center\">2<\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">p<\/td><td class=\"has-text-align-center\" data-align=\"center\">Principal<\/td><td class=\"has-text-align-center\" data-align=\"center\">1<\/td><td class=\"has-text-align-center\" data-align=\"center\">\u22121, 0, +1<\/td><td class=\"has-text-align-center\" data-align=\"center\">3<\/td><td class=\"has-text-align-center\" data-align=\"center\">6<\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">d<\/td><td class=\"has-text-align-center\" data-align=\"center\">Diffuse<\/td><td class=\"has-text-align-center\" data-align=\"center\">2<\/td><td class=\"has-text-align-center\" data-align=\"center\">\u22122, \u22121, 0, +1, +2<\/td><td class=\"has-text-align-center\" data-align=\"center\">5<\/td><td class=\"has-text-align-center\" data-align=\"center\">10<\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">f<\/td><td class=\"has-text-align-center\" data-align=\"center\">Fundamental<\/td><td class=\"has-text-align-center\" data-align=\"center\">3<\/td><td class=\"has-text-align-center\" data-align=\"center\">\u22123, \u22122, \u22121, 0, +1, +2, +3<\/td><td class=\"has-text-align-center\" data-align=\"center\">7<\/td><td class=\"has-text-align-center\" data-align=\"center\">14<\/td><\/tr><\/tbody><\/table><figcaption class=\"wp-element-caption\">Number of electrons in the orbital<\/figcaption><\/figure>\n\n\n\n<p>The 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<p>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<div class=\"wp-block-image\">\n<figure class=\"aligncenter\"><img loading=\"lazy\" decoding=\"async\" width=\"774\" height=\"452\" src=\"https:\/\/i0.wp.com\/valenceelectrons.com\/wp-content\/uploads\/2021\/12\/Electron-configuration-via-Aufbau-principal.jpg?resize=774%2C452&amp;ssl=1\" alt=\"Electron configuration via Aufbau principal\" class=\"wp-image-3947\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/12\/Electron-configuration-via-Aufbau-principal.jpg 774w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/12\/Electron-configuration-via-Aufbau-principal-300x175.jpg 300w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/12\/Electron-configuration-via-Aufbau-principal-768x448.jpg 768w\" sizes=\"(max-width: 774px) 100vw, 774px\" \/><figcaption class=\"wp-element-caption\">Electron configuration via Aufbau principle<\/figcaption><\/figure><\/div>\n\n\n<p>Aufbau 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<p>The Aufbau principle is that&nbsp;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<p>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\n<figure class=\"wp-block-table\"><table><tbody><tr><td class=\"has-text-align-center\" data-align=\"center\"><strong>Orbital<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Orbit (n)<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Azimuthal quantum number (l)<\/strong><\/td><td class=\"has-text-align-center\" data-align=\"center\"><strong>Orbital energy (n + l)<\/strong><\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">3d<\/td><td class=\"has-text-align-center\" data-align=\"center\">3<\/td><td class=\"has-text-align-center\" data-align=\"center\">2<\/td><td class=\"has-text-align-center\" data-align=\"center\">5<\/td><\/tr><tr><td class=\"has-text-align-center\" data-align=\"center\">4s<\/td><td class=\"has-text-align-center\" data-align=\"center\">4<\/td><td class=\"has-text-align-center\" data-align=\"center\">0<\/td><td class=\"has-text-align-center\" data-align=\"center\">4<\/td><\/tr><\/tbody><\/table><figcaption class=\"wp-element-caption\">Energy of orbital<\/figcaption><\/figure>\n\n\n\n<p>Here, 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.<\/p>\n\n\n\n<p>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<p>The first two electrons of iron enter the 1s orbital. The s-orbital can have a maximum of two electrons. Therefore, the next two electrons enter the 2s orbital. The p-orbital can have a maximum of six electrons.<\/p>\n\n\n\n<p>So, the next six electrons enter the 2p orbital. The second orbit is now full. So, the remaining electrons will enter the third orbit. Then two electrons will enter the 3s orbital of the third orbit and the next six electrons will be in the 3p orbital.<\/p>\n\n\n\n<p>The 3p orbital is now full. So, the next two electrons will enter the 4s orbital and the remaining six electrons will enter the 3d orbital. Therefore, the iron full electron configuration will be 1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>6<\/sup> 3s<sup>2<\/sup> 3p<sup>6<\/sup> 3d<sup>6<\/sup> 4s<sup>2<\/sup>.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-large\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"486\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/10\/Iron-electron-configuration-1024x486.jpg\" alt=\"iron electron configuration\" class=\"wp-image-3294\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/10\/Iron-electron-configuration-1024x486.jpg 1024w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/10\/Iron-electron-configuration-300x142.jpg 300w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/10\/Iron-electron-configuration-768x364.jpg 768w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/10\/Iron-electron-configuration.jpg 1373w\" sizes=\"(max-width: 1024px) 100vw, 1024px\" \/><figcaption class=\"wp-element-caption\">Iron electron configuration<\/figcaption><\/figure><\/div>\n\n\n<blockquote class=\"wp-block-quote is-layout-flow wp-block-quote-is-layout-flow\">\n<p><strong>Note:<\/strong>&nbsp;The abbreviated electron configuration of iron is [Ar] 3d<sup>6<\/sup>&nbsp;4s<sup>2<\/sup>. When writing an electron configuration, you have to write serially.<\/p>\n<\/blockquote>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"iron-ion-fe2-fe3-electron-configuration\">Iron ion(Fe<sup>2+<\/sup>, Fe<sup>3+<\/sup>) electron configuration<\/h2>\n\n\n\n<p>The ground state electron configuration of iron is 1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>6<\/sup> 3s<sup>2<\/sup> 3p<sup>6<\/sup> 3d<sup>6<\/sup> 4s<sup>2<\/sup>. This electron configuration shows that the last shell of iron has two electrons and the d-orbital has a total of six electrons. Therefore, the <a href=\"https:\/\/valenceelectrons.com\/valence-electrons-of-iron\/\">valence electrons of iron<\/a> are eight.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"1199\" height=\"626\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Charge-of-iron-ion.jpg\" alt=\"charge of iron ion\" class=\"wp-image-4977\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Charge-of-iron-ion.jpg 1199w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Charge-of-iron-ion-768x401.jpg 768w\" sizes=\"(max-width: 1199px) 100vw, 1199px\" \/><figcaption class=\"wp-element-caption\">Atomic number, atomic weight and charge of iron ion<\/figcaption><\/figure><\/div>\n\n\n<p>There are two types of iron ions. The iron atoms exhibit Fe<sup>2+<\/sup> and Fe<sup>3+<\/sup> ions. The iron atom donates two electrons in the 4s orbital to form an iron ion(Fe<sup>2+<\/sup>).<\/p>\n\n\n\n<p class=\"has-text-align-center\">Fe   \u2013   2e<sup>\u2013<\/sup>   \u2192   Fe<sup>2+<\/sup><\/p>\n\n\n\n<p>Here, the electron configuration of iron ion(Fe<sup>2+<\/sup>) is 1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>6<\/sup> 3s<sup>2<\/sup> 3p<sup>6<\/sup> 3d<sup>6<\/sup>. The iron atom donates two electrons in 4s orbital and an electron in 3d orbital to convert iron ion(Fe<sup>3+<\/sup>).<\/p>\n\n\n\n<p class=\"has-text-align-center\">Fe   \u2013   3e<sup>\u2013<\/sup>   \u2192   Fe<sup>3+<\/sup><\/p>\n\n\n\n<p>The electron configuration of iron ion(Fe<sup>3+<\/sup>) is 1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>6<\/sup> 3s<sup>2<\/sup> 3p<sup>6<\/sup> 3d<sup>6<\/sup>. Iron atom exhibit +2 and +3 oxidation states. The oxidation state of the element changes depending on the bond formation.<\/p>\n\n\n\n<div class=\"wp-block-group\"><div class=\"wp-block-group__inner-container is-layout-constrained wp-block-group-is-layout-constrained\"><div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><a href=\"https:\/\/valenceelectrons.com\/electron-configuration-calculator\/\"><img loading=\"lazy\" decoding=\"async\" width=\"1000\" height=\"606\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2023\/03\/Electron-Configuration-Calculator.jpg\" alt=\"Electron Configuration Calculator\" class=\"wp-image-6229\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2023\/03\/Electron-Configuration-Calculator.jpg 1000w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2023\/03\/Electron-Configuration-Calculator-768x465.jpg 768w\" sizes=\"(max-width: 1000px) 100vw, 1000px\" \/><\/a><\/figure><\/div>\n\n\n<blockquote class=\"wp-block-quote is-layout-flow wp-block-quote-is-layout-flow\">\n<p><a href=\"https:\/\/valenceelectrons.com\/electron-configuration-calculator\/\" data-type=\"link\" data-id=\"https:\/\/valenceelectrons.com\/electron-configuration-calculator\/\">Try the Electron Configuration Calculator and get instant results for any element.<\/a><\/p>\n<\/blockquote>\n<\/div><\/div>\n\n\n\n<h2 class=\"wp-block-heading\">Video for Electron Configuration for Fe, Fe2+, and Fe3+ (Iron and Iron Ions)<\/h2>\n\n\n\n<figure class=\"wp-block-embed aligncenter is-type-video is-provider-youtube wp-block-embed-youtube wp-embed-aspect-16-9 wp-has-aspect-ratio\"><div class=\"wp-block-embed__wrapper\">\n<iframe loading=\"lazy\" title=\"Electron Configuration for Fe, Fe2+, and Fe3+  (Iron and Iron Ions)\" width=\"720\" height=\"405\" src=\"https:\/\/www.youtube.com\/embed\/HcXj60cSUX4?feature=oembed\" frameborder=\"0\" allow=\"accelerometer; autoplay; clipboard-write; encrypted-media; gyroscope; picture-in-picture; web-share\" referrerpolicy=\"strict-origin-when-cross-origin\" allowfullscreen><\/iframe>\n<\/div><figcaption class=\"wp-element-caption\">Electron Configuration for Iron and Iron ions(Fe2+, Fe3+)<\/figcaption><\/figure>\n\n\n\n<script type=\"application\/ld+json\">{\n  \"@context\": \"http:\/\/schema.org\",\n  \"@type\": \"VideoObject\",\n  \"name\": \"Electron Configuration for Fe, Fe2+, and Fe3+  (Iron and Iron Ions)\",\n  \"description\": \"To write the configuration for the Iron ions, first we need to write the electron configuration for just Iron (Fe).  We first need to find the number of electrons for the Fe  atom (there are 26 electrons) using the Periodic Table.   When we write the configuration, we'll put all 26 electrons in orbitals around the nucleus of the Iron atom.  In this video we'll use the Periodic Table to help us write the notation for Iron.   Alternatively you can use a chart showing how the orbitals fill (https:\/\/youtu.be\/TjVrcw2sZLs).    Either way,  the Iron electron configuration will be 1s2 2s2 2p6 3s2 3p6 3d6 4s2  Note that when writing the electron configuration for an atom like Fe, the 3d is usually written before the 4s.   Both of the configurations have the correct numbers of electrons in each orbital, it is just a matter of how the electronic configuration notation is written (see below for an explanation why).   For the Fe2+ ion we remove two electrons from 4s2 leaving us with:  1s2 2s2 2p6 3s2 3p6 3d6   For the Fe3+ ion we remove a total of three electrons (two from the 4s2 and one form the 3d6) leaving us with   1s2 2s2 2p6 3s2 3p6 3d5  \u2022 Introduction to Writing Electron Configurations: https:\/\/youtu.be\/J-v9_ieCqJI \u2022 Electron Configurations Chart: https:\/\/youtu.be\/TjVrcw2sZLs \u2022 Writing Electron Configs Using only the Periodic Table: https:\/\/youtu.be\/ououF9nHUhk \u2022 Order of d and s Orbital Filling:  https:\/\/eic.rsc.org\/Coature\/the-trouble-with-the-aufbau-principle\/2000133.article  The configuration notation provides an easy way for scientists to write and communicate how electrons are arranged around the nucleus of an atom.  This makes it easier to understand and predict how atoms will interact to form chemical bonds.\",\n  \"thumbnailUrl\": \"https:\/\/i.ytimg.com\/vi\/HcXj60cSUX4\/default.jpg\",\n  \"uploadDate\": \"2019-07-02T21:52:13Z\",\n  \"duration\": \"PT3M38S\",\n  \"embedUrl\": \"https:\/\/www.youtube.com\/embed\/HcXj60cSUX4\",\n  \"interactionCount\": \"263190\"\n}<\/script>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"faqs\">FAQs<\/h2>\n\n\n<div id=\"rank-math-faq\" class=\"rank-math-block\">\n<ol class=\"rank-math-list \">\n<li id=\"faq-question-1679077929124\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">What is the symbol for iron?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a0The symbol for iron is \u2018Fe\u2019.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679077938350\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">How many electrons does iron have?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a026 electrons.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679077950782\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">How do you write the full electron configuration for iron?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a01s<sup>2<\/sup>\u00a02s<sup>2<\/sup>\u00a02p<sup>6<\/sup>\u00a03s<sup>2<\/sup>\u00a03p<sup>6<\/sup>\u00a03d<sup>6<\/sup>\u00a04s<sup>2<\/sup>.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679077992718\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">How many <a href=\"https:\/\/valenceelectrons.com\/what-are-valence-electrons\/\">valence electrons<\/a> does iron have?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a0Eight valence electrons.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679078009670\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">What is the valency of iron?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a0The valency of iron is 2 and 3.<\/p>\n\n<\/div>\n<\/li>\n<\/ol>\n<\/div>","protected":false},"excerpt":{"rendered":"<p>Iron is the 26th element in the periodic table and its symbol is \u2018Fe\u2019. In this article, I have discussed in detail how to easily write the complete electron configuration of iron&#8230;.<\/p>\n","protected":false},"author":3,"featured_media":3294,"comment_status":"open","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"_kad_post_transparent":"","_kad_post_title":"","_kad_post_layout":"","_kad_post_sidebar_id":"","_kad_post_content_style":"","_kad_post_vertical_padding":"","_kad_post_feature":"","_kad_post_feature_position":"","_kad_post_header":false,"_kad_post_footer":false,"footnotes":""},"categories":[3],"tags":[],"_links":{"self":[{"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/posts\/4048"}],"collection":[{"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/users\/3"}],"replies":[{"embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/comments?post=4048"}],"version-history":[{"count":0,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/posts\/4048\/revisions"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media\/3294"}],"wp:attachment":[{"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media?parent=4048"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/categories?post=4048"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/tags?post=4048"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}