{"id":4382,"date":"2023-03-20T00:25:51","date_gmt":"2023-03-19T18:25:51","guid":{"rendered":"https:\/\/valenceelectrons.com\/?p=4382"},"modified":"2023-10-24T23:12:04","modified_gmt":"2023-10-24T17:12:04","slug":"indium-electron-configuration","status":"publish","type":"post","link":"https:\/\/valenceelectrons.com\/indium-electron-configuration\/","title":{"rendered":"Complete Electron Configuration for Indium (In, In3+)"},"content":{"rendered":"\n<p>Indium is the 49th element in the periodic table and its symbol is \u2018In\u2019. Indium is a post-transition metal element. In this article, I have discussed in detail how to easily write the complete electron configuration of indium.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">What is the electron configuration of indium?<\/h2>\n\n\n\n<p>The total number of&nbsp;electrons in indium&nbsp;is forty-nine. These electrons are arranged according to specific rules in different orbitals.<\/p>\n\n\n\n<p>The arrangement of electrons in indium in specific rules in different orbits and orbitals is called the&nbsp;<a href=\"https:\/\/valenceelectrons.com\/electron-configuration\/\">electron configuration<\/a>&nbsp;of indium.<\/p>\n\n\n\n<p>The electron configuration of indium is [<a href=\"https:\/\/valenceelectrons.com\/krypton-electron-configuration\/\">Kr<\/a>] 4d<sup>10<\/sup>&nbsp;5s<sup>2<\/sup> 5p<sup>1<\/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=\"1200\" height=\"630\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/02\/Indium-atom-electron-configuration.jpg\" alt=\"indium atom\" class=\"wp-image-4414\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/02\/Indium-atom-electron-configuration.jpg 1200w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/02\/Indium-atom-electron-configuration-768x403.jpg 768w\" sizes=\"(max-width: 1200px) 100vw, 1200px\" \/><figcaption class=\"wp-element-caption\">Indium 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=\"indium-in-electron-configuration-through-orbit\">Indium 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<\/a> of the atom 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. The atomic number is the number of electrons in that element.<\/p>\n\n\n\n<p>The atomic number of indium is 49. That is, the number of electrons in indium is forty-nine. Therefore, an indium atom will have two electrons in the first shell, eight in the 2nd orbit, and eighteen electrons in the 3rd shell.<\/p>\n\n\n\n<p>According to Bohr\u2019s formula, the fourth shell will have twenty-one electrons but the fourth shell of indium will have eighteen electrons and the remaining three electrons will be in the fifth shell.<\/p>\n\n\n\n<p>Therefore, the order of the number of electrons in each shell of the indium atom is 2, 8, 18, 18, 3. 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-indium-in-through-orbital\">Electron configuration of indium 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. 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 <a href=\"https:\/\/valenceelectrons.com\/indium-protons-neutrons-electrons\/\">electrons of indium<\/a> 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<p>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<p>Then two electrons will enter the 3s orbital and the next six electrons will be in the 3p orbital of the third orbit. The 3p orbital is now full. So, the next two electrons will enter the 4s orbital and ten electrons will enter the 3d orbital.<\/p>\n\n\n\n<p>The 3d orbital is now full of electrons. So, the next six electrons enter the 4p orbital. Then next two electrons will enter the 5s orbital and the next ten electrons will enter the 4d orbital.<\/p>\n\n\n\n<p>The 4d orbital is now full of electrons. So, the remaining one electron enters the 5p orbital. Therefore, the indium 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>10<\/sup> 4s<sup>2<\/sup> 4p<sup>6<\/sup> 4d<sup>10<\/sup> 5s<sup>2<\/sup> 5p<sup>1<\/sup>.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"1199\" height=\"628\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/02\/Indium-electron-configuration.jpg\" alt=\"indium electron configuration\" class=\"wp-image-5162\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/02\/Indium-electron-configuration.jpg 1199w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/02\/Indium-electron-configuration-768x402.jpg 768w\" sizes=\"(max-width: 1199px) 100vw, 1199px\" \/><figcaption class=\"wp-element-caption\">Indium 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 unabbreviated electron configuration of indium is [Kr] 4d<sup>10<\/sup>&nbsp;5s<sup>2<\/sup> 5p<sup>1<\/sup>. When writing an electron configuration, you have to write serially.<\/p>\n<\/blockquote>\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\" id=\"indium-in-excited-state-electron-configuration\">Indium excited state electron configuration<\/h2>\n\n\n\n<p>Atoms can jump from one orbital to another orbital in an excited state. This is called quantum jump. The ground-state electron configuration of indium is 1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>6<\/sup> 3s<sup>2<\/sup> 3p<sup>6<\/sup> 3d<sup>10<\/sup> 4s<sup>2<\/sup> 4p<sup>6<\/sup> 4d<sup>10<\/sup> 5s<sup>2<\/sup> 5p<sup>1<\/sup>.<\/p>\n\n\n\n<p>In the indium ground-state electron configuration, the last electron of the 5p orbital is located in the 4p<sub>x<\/sub> sub-orbitals. We already know that the p-subshell has three orbitals. The orbitals are p<sub>x<\/sub>, p<sub>y<\/sub>, and p<sub>z<\/sub> and each orbital can have a maximum of two electrons.<\/p>\n\n\n\n<p>So, the correct electron configuration of indium in the ground state will be 1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>6<\/sup> 3s<sup>2<\/sup> 3p<sup>6<\/sup> 3d<sup>10<\/sup> 4s<sup>2<\/sup> 4p<sup>6<\/sup> 4d<sup>10<\/sup> 5s<sup>2<\/sup> 5p<sub>x<\/sub><sup>1<\/sup>. When the indium atom is excited, then the indium atom absorbs energy. As a result, an electron in the 5s orbital jumps to the 5p<sub>y<\/sub> orbital.<\/p>\n\n\n\n<p>Therefore, the electron configuration of indium(In*) in an excited state will be 1s<sup>2<\/sup> 2s<sup>2<\/sup> 2p<sup>6<\/sup> 3s<sup>2<\/sup> 3p<sup>6<\/sup> 3d<sup>10<\/sup> 4s<sup>2<\/sup> 4p<sup>6<\/sup> 4d<sup>10<\/sup> 5s<sup>1<\/sup> 5p<sub>x<\/sub><sup>1<\/sup> 5p<sub>y<\/sub><sup>1<\/sup>. The valency of the element is determined by electron configuration in the excited state. Here, indium has three unpaired electrons. So, the valency of indium is 3.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"indium-ion-in3-electron-configuration\">Indium ion(In<sup>3+<\/sup>) electron configuration<\/h2>\n\n\n\n<p>The electron configuration shows that the last shell of indium has three electrons. Therefore, the <a href=\"https:\/\/valenceelectrons.com\/what-are-valence-electrons\/\">valence electrons<\/a> of indium are three.<\/p>\n\n\n\n<p>The elements that have 1, 2, or 3 electrons in the last shell donate the electrons in the last shell during bond formation. The elements that form bonds by donating electrons is called cation.<\/p>\n\n\n\n<p>The indium atom donates three electrons in the last shell to form an indium ion(In<sup>3+<\/sup>). That is, indium is a cation element.<\/p>\n\n\n\n<p class=\"has-text-align-center\">In   \u2013   3e<sup>\u2013<\/sup>   \u2192   In<sup>3+<\/sup><\/p>\n\n\n\n<p>The electron configuration of indium ion(In<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>10<\/sup> 4s<sup>2<\/sup> 4p<sup>6<\/sup> 4d<sup>10<\/sup>.<\/p>\n\n\n\n<p>This electron configuration shows that the indium ion(In<sup>3+<\/sup>) has four shells and the last shell has eighteen electrons and it achieves a stable electron configuration. Indium atom exhibits +3 oxidation state.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">Video for Electron configuration of indium and indium ion(In<sup>3+<\/sup>)<\/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=\"How to Write the Electron Configuration for Indium (In)\" width=\"720\" height=\"405\" src=\"https:\/\/www.youtube.com\/embed\/NDcjCpoF5r4?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 indium and indium ion(In<sup>3+<\/sup>)<\/figcaption><\/figure>\n\n\n\n<script type=\"application\/ld+json\">{\n  \"@context\": \"http:\/\/schema.org\",\n  \"@type\": \"VideoObject\",\n  \"name\": \"How to Write the Electron Configuration for Indium (In)\",\n  \"description\": \"A step-by-step description of how to write the electron configuration for Indium (In).  In order to write the In electron configuration we first need to know the number of electrons for the In atom (there are 49 electrons).   When we write the configuration, we'll put all 49 electrons in orbitals around the nucleus of the Indium atom.  In this video we'll use the Periodic Table to help us write the notation for Indium .   Note that the Indium electron configuration will be Kr 4d10 5s2 5p1.  \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  Note that when writing the electron configuration for an atom like In, the d orbital is usually written before the s.   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).   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\/NDcjCpoF5r4\/default.jpg\",\n  \"uploadDate\": \"2020-11-16T17:38:03Z\",\n  \"duration\": \"PT2M55S\",\n  \"embedUrl\": \"https:\/\/www.youtube.com\/embed\/NDcjCpoF5r4\",\n  \"interactionCount\": \"17597\"\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-1679250165707\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">What is the symbol for indium?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a0The symbol for indium is \u2018In\u2019.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679250173980\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">How many electrons does indium have?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a049 electrons.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679250187279\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">How do you write the full electron configuration for indium?<\/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>10<\/sup>\u00a04s<sup>2<\/sup>\u00a04p<sup>6<\/sup>\u00a04d<sup>10<\/sup>\u00a05s<sup>2<\/sup> 5p<sup>1<\/sup>.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679250201490\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">How many valence electrons does indium have?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a0Three valence electrons.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679250231260\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">What is the valency of indium?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a0The valency of indium is 3.<\/p>\n\n<\/div>\n<\/li>\n<\/ol>\n<\/div>","protected":false},"excerpt":{"rendered":"<p>Indium is the 49th element in the periodic table and its symbol is \u2018In\u2019. Indium is a post-transition metal element. In this article, I have discussed in detail how to easily write&#8230;<\/p>\n","protected":false},"author":3,"featured_media":5162,"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\/4382"}],"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=4382"}],"version-history":[{"count":0,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/posts\/4382\/revisions"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media\/5162"}],"wp:attachment":[{"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media?parent=4382"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/categories?post=4382"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/tags?post=4382"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}