{"id":4082,"date":"2023-03-18T00:51:41","date_gmt":"2023-03-17T18:51:41","guid":{"rendered":"https:\/\/valenceelectrons.com\/?p=4082"},"modified":"2023-10-26T23:55:53","modified_gmt":"2023-10-26T17:55:53","slug":"copper-electron-configuration","status":"publish","type":"post","link":"https:\/\/valenceelectrons.com\/copper-electron-configuration\/","title":{"rendered":"Electron Configuration for Copper (Cu, Cu+, Cu2+)"},"content":{"rendered":"\n<p>Copper is the 29th element in the periodic table and its symbol is \u2018Cu\u2019. In this article, I have discussed in detail how to easily write the complete electron configuration of copper.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">What is the electron configuration of copper?<\/h2>\n\n\n\n<p>The total number of&nbsp;electrons in copper&nbsp;is twenty-nine. These electrons are arranged according to specific rules in different orbitals.<\/p>\n\n\n\n<p>The arrangement of electrons in copper in specific rules in different orbits and orbitals is called the&nbsp;<a href=\"https:\/\/valenceelectrons.com\/electron-configuration\/\">electron configuration<\/a>&nbsp;of copper.<\/p>\n\n\n\n<p>The electron configuration of copper is [<a href=\"https:\/\/valenceelectrons.com\/argon-electron-configuration\/\">Ar<\/a>] 3d<sup>10<\/sup>&nbsp;4s<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=\"780\" height=\"438\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/01\/CopperCu-atom-electron-configurationBohr-model.jpg\" alt=\"Copper atom electron configuration\" class=\"wp-image-4083\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/01\/CopperCu-atom-electron-configurationBohr-model.jpg 780w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/01\/CopperCu-atom-electron-configurationBohr-model-300x168.jpg 300w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/01\/CopperCu-atom-electron-configurationBohr-model-768x431.jpg 768w\" sizes=\"(max-width: 780px) 100vw, 780px\" \/><figcaption class=\"wp-element-caption\">Copper(Cu) 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=\"copper-cu-electron-configuration-through-orbit\">Copper 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.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-large\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"376\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/11\/Position-of-copperCu-in-the-periodic-table-1024x376.jpg\" alt=\"Position of copper(Cu) in the periodic table\" class=\"wp-image-3331\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/11\/Position-of-copperCu-in-the-periodic-table-1024x376.jpg 1024w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/11\/Position-of-copperCu-in-the-periodic-table-300x110.jpg 300w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/11\/Position-of-copperCu-in-the-periodic-table-768x282.jpg 768w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/11\/Position-of-copperCu-in-the-periodic-table.jpg 1304w\" sizes=\"(max-width: 1024px) 100vw, 1024px\" \/><figcaption class=\"wp-element-caption\">Position of copper(Cu) 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 copper is 29. That is, the number of electrons in copper is twenty-nine.<\/p>\n\n\n\n<p>Therefore, the copper atom will have two electrons in the first shell, eight in the 2nd orbit, eighteen electrons in the 3rd shell, and the remaining one electron will be in the fourth shell.<\/p>\n\n\n\n<p>Therefore, the order of the number of electrons in each shell of the copper(Cu) atom is 2, 8, 18, 1. 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-copper-cu-through-orbital\">Electron configuration of copper 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 <a href=\"https:\/\/valenceelectrons.com\/copper-protons-neutrons-electrons\/\">electrons of copper<\/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 the remaining nine electrons will enter the 3d orbital.<\/p>\n\n\n\n<p>But the orbital wants to be half-filled or full-filled by electrons. Because the atom may be in a more stable state when the orbital is half-filled and full-filled.<\/p>\n\n\n\n<p>Therefore, an electron of 4s orbital completes a full-filled 3d orbital by jumping into a 3d orbital. So, the copper 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>1<\/sup>.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-large\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"429\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/11\/Copper-electron-configuration-1024x429.jpg\" alt=\"copper electron configuration\" class=\"wp-image-3345\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/11\/Copper-electron-configuration-1024x429.jpg 1024w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/11\/Copper-electron-configuration-300x126.jpg 300w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/11\/Copper-electron-configuration-768x322.jpg 768w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/11\/Copper-electron-configuration.jpg 1374w\" sizes=\"(max-width: 1024px) 100vw, 1024px\" \/><figcaption class=\"wp-element-caption\">Copper 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 copper is [Ar] 3d<sup>10<\/sup>&nbsp;4s<sup>1<\/sup>. When writing an electron configuration, you have to write serially.<\/p>\n<\/blockquote>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"copper-ion-cu-cu2-electron-configuration\">Copper ion(Cu<sup>+<\/sup>, Cu<sup>2+<\/sup>) electron configuration<\/h2>\n\n\n\n<p>The ground state electron configuration of copper 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>1<\/sup>. This electron configuration shows that the last shell of copper has an electron and the d-orbital has a total of ten electrons. Therefore, the <a href=\"https:\/\/valenceelectrons.com\/valence-electrons-of-copper\/\">valence electrons of copper<\/a> are one.<\/p>\n\n\n\n<p>There are two types of copper ions. The copper atom exhibits Cu<sup>+<\/sup> and Cu<sup>2+<\/sup> ions. The copper atom donates an electron in the 4s orbital to form a copper ion(Cu<sup>+<\/sup>).<\/p>\n\n\n\n<p class=\"has-text-align-center\">Cu   \u2013   e<sup>\u2013<\/sup>   \u2192   Cu<sup>+<\/sup><\/p>\n\n\n\n<p>Here, the electron configuration of copper ion(Cu<sup>+<\/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>. On the other hand, the copper atom donates an electron in the 4s orbital and an electron in the 3d orbital to convert copper ion(Cu<sup>2+<\/sup>).<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"1200\" height=\"628\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Charge-of-copper-ion.jpg\" alt=\"charge of copper ion\" class=\"wp-image-4990\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Charge-of-copper-ion.jpg 1200w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Charge-of-copper-ion-768x402.jpg 768w\" sizes=\"(max-width: 1200px) 100vw, 1200px\" \/><figcaption class=\"wp-element-caption\">Atomic number, atomic weight and charge of copper ion<\/figcaption><\/figure><\/div>\n\n\n<p class=\"has-text-align-center\">Cu   \u2013   2e<sup>\u2013<\/sup>   \u2192   Cu<sup>2+<\/sup><\/p>\n\n\n\n<p>The electron configuration of copper ions(Cu<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>9<\/sup>. Copper atoms exhibit +1 and +2 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 Cu, Cu+, and Cu2+ (Copper and Copper 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 Cu, Cu+, and Cu2+  (Copper and Copper Ions)\" width=\"720\" height=\"405\" src=\"https:\/\/www.youtube.com\/embed\/At3j7r1shxE?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 copper ion(Cu<sup>+<\/sup>, Cu<sup>2+<\/sup>)<\/figcaption><\/figure>\n\n\n\n<script type=\"application\/ld+json\">{\n  \"@context\": \"http:\/\/schema.org\",\n  \"@type\": \"VideoObject\",\n  \"name\": \"Electron Configuration for Cu, Cu+, and Cu2+  (Copper and Copper Ions)\",\n  \"description\": \"To write the configuration for the Copper ions, first we need to write the electron configuration for just Copper (Cu).  We first need to find the number of electrons for the Cu  atom (there are 29 electrons) using the Periodic Table.   When we write the configuration, we'll put all 29 electrons in orbitals around the nucleus of the Copper atom.  In this video we'll start with using the Periodic Table to help us write the notation for Copper.   Alternatively you can use a chart showing how the orbitals fill (https:\/\/youtu.be\/TjVrcw2sZLs).  This would give us the (incorrect) Copper electron configuration of  1s2 2s2 2p6 3s2 3p6 3d9 4s2  ---Copper is an exception! ---  Half-filled and fully filled subshell have got extra stability.    Therefore, one of the 4s2 electrons jumps to the 3d9.  This give us the (correct) configuration of:  1s2 2s2 2p6 3s2 3p6 3d10 4s1   Note that when writing the electron configuration for an atom like Cu, 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 link to an explanation why).    For the Cu+ ion we remove one electron from 4s1 leaving us with:  1s2 2s2 2p6 3s2 3p6 3d10   For the Cu2+ ion we remove a total of three electrons (two from the 4s1 and one form the 3d10) leaving us with   1s2 2s2 2p6 3s2 3p6 3d9   \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\/At3j7r1shxE\/default.jpg\",\n  \"uploadDate\": \"2019-07-08T18:49:49Z\",\n  \"duration\": \"PT3M53S\",\n  \"embedUrl\": \"https:\/\/www.youtube.com\/embed\/At3j7r1shxE\",\n  \"interactionCount\": \"245589\"\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-1679078987758\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">What is the symbol for copper?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a0The symbol for copper is \u2018Cu\u2019.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679078994382\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">How many electrons does copper have?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a029 electrons.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679079007413\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">How do you write the full electron configuration for copper?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong> 1s<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>1<\/sup>.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679079026865\" 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 copper have?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a0One valence electrons.<\/p>\n\n<\/div>\n<\/li>\n<li id=\"faq-question-1679079042075\" class=\"rank-math-list-item\">\n<h3 class=\"rank-math-question \">What is the valency of copper?<\/h3>\n<div class=\"rank-math-answer \">\n\n<p><strong>Ans:<\/strong>\u00a0The valency of copper is 1 and 2.<\/p>\n\n<\/div>\n<\/li>\n<\/ol>\n<\/div>","protected":false},"excerpt":{"rendered":"<p>Copper is the 29th element in the periodic table and its symbol is \u2018Cu\u2019. In this article, I have discussed in detail how to easily write the complete electron configuration of copper&#8230;.<\/p>\n","protected":false},"author":3,"featured_media":3345,"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\/4082"}],"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=4082"}],"version-history":[{"count":0,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/posts\/4082\/revisions"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media\/3345"}],"wp:attachment":[{"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media?parent=4082"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/categories?post=4082"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/tags?post=4082"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}