{"id":4400,"date":"2023-03-23T12:40:45","date_gmt":"2023-03-23T06:40:45","guid":{"rendered":"https:\/\/valenceelectrons.com\/?p=4400"},"modified":"2023-09-08T03:37:29","modified_gmt":"2023-09-07T21:37:29","slug":"dysprosium-electron-configuration","status":"publish","type":"post","link":"https:\/\/valenceelectrons.com\/dysprosium-electron-configuration\/","title":{"rendered":"Complete Electron Configuration for Dysprosium (Dy)"},"content":{"rendered":"\n<p>Dysprosium is the 66th element in the periodic table and its symbol is \u2018Dy\u2019. Dysprosium is a classified lanthanide element. In this article, I have discussed in detail how to easily write the complete electron configuration of dysprosium.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">What is the electron configuration of dysprosium?<\/h2>\n\n\n\n<p>The total number of&nbsp;electrons in dysprosium is sixty-six. These electrons are arranged according to specific rules in different orbitals.<\/p>\n\n\n\n<p>The arrangement of electrons in dysprosium in specific rules in different orbits and orbitals is called the&nbsp;<a href=\"https:\/\/valenceelectrons.com\/electron-configuration\/\">electron configuration<\/a>&nbsp;of dysprosium.<\/p>\n\n\n\n<p>The electron configuration of dysprosium is  [<a href=\"https:\/\/valenceelectrons.com\/xenon-electron-configuration\/\">Xe<\/a>] 4f<sup>10<\/sup>\u00a06s<sup>2<\/sup>,\u00a0if 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\u00a0(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=\"1199\" height=\"630\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/02\/Dysprosium-atom-electron-configuration.jpg\" alt=\"dysprosium atom\" class=\"wp-image-4487\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/02\/Dysprosium-atom-electron-configuration.jpg 1199w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/02\/Dysprosium-atom-electron-configuration-768x404.jpg 768w\" sizes=\"(max-width: 1199px) 100vw, 1199px\" \/><figcaption class=\"wp-element-caption\">Dysprosium 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<h3 class=\"wp-block-heading\" id=\"dysprosium-dy-electron-configuration-through-orbit\">Dysprosium atom electron configuration through orbit<\/h3>\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 electrons 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>\u00a0= 2 \u00d7 3<sup>2\u00a0<\/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>\u00a0= 2 \u00d7 4<sup>2<\/sup>\u00a0= 32.<\/li>\n<\/ol>\n\n\n\n<p>Therefore, the maximum <a href=\"https:\/\/valenceelectrons.com\/how-to-find-protons-neutrons-and-electrons\/\">electron<\/a> 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\n<p>The atomic number is the number of electrons in that element. The atomic number of dysprosium is 66. That is, the number of electrons in dysprosium is sixty-six.<\/p>\n\n\n\n<p>Therefore, a dysprosium 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 thirty-two electrons and six electrons will be in the fifth shell but the fourth shell of dysprosium will have twenty-eight electrons, eight electrons in the fifth shell and the remaining two electrons will be in the sixth shell.<\/p>\n\n\n\n<p>Therefore, the order of the number of electrons in each shell of the dysprosium(Dy) atom is 2, 8, 18, 28, 8, 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<h3 class=\"wp-block-heading\" id=\"electron-configuration-of-dysprosium-dy-through-orbital\">Electron configuration of dysprosium through orbital<\/h3>\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\">Orbital number of the subshell<\/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\/dysprosium-protons-neutrons-electrons\/\">electrons of dysprosium<\/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 ten electrons will enter the 4d orbital and the next eight electrons enter the 5p and 6s orbital. The 6s orbital is now full.<\/p>\n\n\n\n<p>So the remaining ten electrons will enter the 4f orbital. Therefore, the dysprosium complete 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> 4f<sup>10<\/sup> 5s<sup>2<\/sup> 5p<sup>6<\/sup> 6s<sup>2<\/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\/Dysprosium-electron-configuration.jpg\" alt=\"dysprosium electron configuration\" class=\"wp-image-5203\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/02\/Dysprosium-electron-configuration.jpg 1199w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/02\/Dysprosium-electron-configuration-768x402.jpg 768w\" sizes=\"(max-width: 1199px) 100vw, 1199px\" \/><figcaption class=\"wp-element-caption\">Dysprosium 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>\u00a0The unabbreviated electron configuration of dysprosium is [Xe] 4f<sup>10<\/sup>\u00a06s<sup>2<\/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=\"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-1679553547711\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">What is the symbol for dysprosium?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a0The symbol for dysprosium is \u2018Dy\u2019.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679553556155\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">How many electrons does dysprosium have?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a066 electrons.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679553568640\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">How do you write the full electron configuration for dysprosium?<\/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>\u00a04f<sup>10<\/sup>\u00a05s<sup>2<\/sup>\u00a05p<sup>6<\/sup>\u00a06s<sup>2<\/sup>.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679553583936\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">What is the valency of dysprosium?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a0The valency of dysprosium is 3.<\/p>\n\n<\/div>\n<\/li>\n<\/ol>\n<\/div>","protected":false},"excerpt":{"rendered":"<p>Dysprosium is the 66th element in the periodic table and its symbol is \u2018Dy\u2019. Dysprosium is a classified lanthanide element. In this article, I have discussed in detail how to easily write&#8230;<\/p>\n","protected":false},"author":3,"featured_media":5203,"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\/4400"}],"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=4400"}],"version-history":[{"count":0,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/posts\/4400\/revisions"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media\/5203"}],"wp:attachment":[{"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media?parent=4400"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/categories?post=4400"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/tags?post=4400"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}