{"id":2426,"date":"2024-02-01T23:39:15","date_gmt":"2024-02-01T17:39:15","guid":{"rendered":"https:\/\/valenceelectrons.com\/?p=2426"},"modified":"2024-04-28T00:11:11","modified_gmt":"2024-04-27T18:11:11","slug":"boron-electron-configuration","status":"publish","type":"post","link":"https:\/\/valenceelectrons.com\/boron-electron-configuration\/","title":{"rendered":"Electron Configuration for Boron (B, B3+ ion)"},"content":{"rendered":"\n<p>Boron is the 5th element in the periodic table and its symbol is \u2018B\u2019. In this article, I have discussed in detail how to easily write the complete electron configuration of boron.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">What is the electron configuration of boron?<\/h2>\n\n\n\n<p>The total number of&nbsp;<a href=\"https:\/\/valenceelectrons.com\/boron-protons-neutrons-electrons\/\">electrons in boron<\/a>&nbsp;is five. These electrons are arranged according to specific rules in different orbitals.<\/p>\n\n\n\n<p>The arrangement of electrons in boron in specific rules in different orbits and orbitals is called the&nbsp;<a href=\"https:\/\/valenceelectrons.com\/electron-configuration\/\">electron configuration<\/a>&nbsp;of boron.<\/p>\n\n\n\n<p>The electron configuration of boron is [<a href=\"https:\/\/valenceelectrons.com\/helium-electron-configuration\/\">He<\/a>] 2s<sup>2<\/sup> 2p<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 (Bohr principle)<\/li>\n\n\n\n<li>Electron configuration through orbital (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=\"1137\" height=\"598\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/06\/Boron-B-atom-electron-configuration.jpg\" alt=\"Boron atom electron configuration\" class=\"wp-image-4356\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/06\/Boron-B-atom-electron-configuration.jpg 1137w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/06\/Boron-B-atom-electron-configuration-768x404.jpg 768w\" sizes=\"(max-width: 1137px) 100vw, 1137px\" \/><figcaption class=\"wp-element-caption\">Boron (B) 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=\"boron-b-electron-configuration-through-orbit\">Electron configuration of boron 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 orbits (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 electron holding capacity of the K orbit is 2n<sup>2<\/sup>&nbsp;= 2 \u00d7 1<sup>2<\/sup>&nbsp;= 2 electrons.<\/li>\n\n\n\n<li>For L orbit, n = 2.<br>The electron holding capacity of the L orbit is 2n<sup>2<\/sup>&nbsp;= 2 \u00d7 2<sup>2<\/sup>&nbsp;= 8 electrons.<\/li>\n\n\n\n<li>n=3 for M orbit.<br>The maximum electron holding capacity in the M orbit is 2n<sup>2<\/sup>&nbsp;= 2 \u00d7 3<sup>2&nbsp;<\/sup>= 18 electrons.<\/li>\n\n\n\n<li>n=4 for N orbit.<br>The maximum electron holding capacity in the N orbit is 2n<sup>2<\/sup>&nbsp;= 2 \u00d7 4<sup>2<\/sup>&nbsp;= 32 electrons.<\/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&nbsp;atomic number of boron&nbsp;is 5. That is, the number of electrons in boron is 5. Therefore, a boron atom will have two electrons in the first shell and three in the 2nd shell.<\/p>\n\n\n\n<p>Therefore, the order of the number of electrons in each shell of the boron(B) atom is 2, 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&nbsp;<a href=\"https:\/\/valenceelectrons.com\/electron-configuration-of-all-elements\/\">electron configuration of all the elements<\/a>&nbsp;can be done through the orbital diagram.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"electron-configuration-of-boron-b-atom-through-orbital\">Electron configuration of boron 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. The first two electrons of boron enter the 1s orbital.<\/p>\n\n\n\n<p>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 remaining one electron enters the 2p orbital.&nbsp;Therefore, the boron complete electron configuration will be 1s<sup>2<\/sup>&nbsp;2s<sup>2<\/sup>&nbsp;2p<sup>1<\/sup>.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"1278\" height=\"800\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2023\/03\/Boron-electron-configuration.jpg\" alt=\"Boron electron configuration\" class=\"wp-image-6025\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2023\/03\/Boron-electron-configuration.jpg 1278w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2023\/03\/Boron-electron-configuration-768x481.jpg 768w\" sizes=\"(max-width: 1278px) 100vw, 1278px\" \/><figcaption class=\"wp-element-caption\">Boron 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> The unabbreviated electron configuration of boron is [He] 2s<sup>2<\/sup> 2p<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=\"boron-b-excited-state-electron-configuration\">Electron configuration of boron in the excited state<\/h2>\n\n\n\n<p>Atoms can jump from one orbital to another in an excited state. This is called quantum jump. The ground state electron configuration of boron is 1s<sup>2<\/sup>&nbsp;2s<sup>2<\/sup>&nbsp;2p<sup>1<\/sup>.<\/p>\n\n\n\n<p>We already know that the p-sub shell 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. In the boron ground-state electron configuration, an electron of the 3p orbital is located in the p<sub>x<\/sub>&nbsp;orbital.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"851\" height=\"315\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/06\/Boron-B-excited-state-electron-configuration-and-orbital-diagram-1.jpg\" alt=\"Boron excited state electron configuration and orbital diagram\" class=\"wp-image-4357\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/06\/Boron-B-excited-state-electron-configuration-and-orbital-diagram-1.jpg 851w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/06\/Boron-B-excited-state-electron-configuration-and-orbital-diagram-1-768x284.jpg 768w\" sizes=\"(max-width: 851px) 100vw, 851px\" \/><figcaption class=\"wp-element-caption\">Boron excited state electron configuration and orbital diagram<\/figcaption><\/figure><\/div>\n\n\n<p>Then correct electron configuration of boron in the ground state will be 1s<sup>2<\/sup>&nbsp;2s<sup>2<\/sup>&nbsp;2p<sub>x<\/sub><sup>1<\/sup>. When the boron atom is excited, then the boron atom absorbs energy. As a result, an electron in the 2s orbital jumps to the 2p<sub>y<\/sub>&nbsp;orbital.<\/p>\n\n\n\n<p>So, the electron configuration of boron(B*) in the excited state will be 1s<sup>2<\/sup>&nbsp;2s<sup>1<\/sup>&nbsp;2p<sub>x<\/sub><sup>1<\/sup>&nbsp;2p<sub>y<\/sub><sup>1<\/sup>. The valency of an element is determined by electron configuration in the excited state. Here, boron has three unpaired electrons. Therefore, the valency of boron is 3.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"electron-configuration-of-boron-ion-b3\">Boron ion(B<sup>3+<\/sup>) electron configuration<\/h2>\n\n\n\n<p>After the electron configuration, the last shell of the boron atom has three electrons. Therefore, the&nbsp;<a href=\"https:\/\/valenceelectrons.com\/valence-electrons-of-boron\/\">valence electrons&nbsp;of boron<\/a> 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 boron atom donates three electrons of the last shell to turn into a boron ion(B<sup>3+<\/sup>).<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"1198\" height=\"628\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Protons-and-electrons-for-the-boron-ion.jpg\" alt=\"charge of boron\" class=\"wp-image-4847\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Protons-and-electrons-for-the-boron-ion.jpg 1198w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Protons-and-electrons-for-the-boron-ion-768x403.jpg 768w\" sizes=\"(max-width: 1198px) 100vw, 1198px\" \/><figcaption class=\"wp-element-caption\">Charge of boron<\/figcaption><\/figure><\/div>\n\n\n<p>The elements that form bonds by donating electrons are called cation. Boron leaves three electrons and turns into a positive ion. Therefore, boron is a cation element.&nbsp;<\/p>\n\n\n\n<p class=\"has-text-align-center\">B   &#8211;   3e<sup>&#8211;<\/sup>    \u2192   B<sup>3+<\/sup><\/p>\n\n\n\n<p>Here, the electron configuration of boron ion(B<sup>3+<\/sup>) is 1s<sup>2<\/sup>. This electron configuration shows that the boron ion(B<sup>3+<\/sup>) acquired the&nbsp;<a href=\"https:\/\/valenceelectrons.com\/helium-electron-configuration\/\">electron configuration of helium<\/a>&nbsp;and it achieves a stable electron configuration.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"determination-of-group-and-period-through-electron-configuration\">Determine the group and period of boron through the electron configuration<\/h2>\n\n\n\n<p>The last orbit of an element is the period of that element. The electron configuration of the boron atom shows that the last orbit of the boron atom is 2. So, the period of boron is 2.<\/p>\n\n\n\n<p>On the other hand, the number of electrons present in the last orbit of an element is the number of groups in that element. But in the case of p-block elements, group diagnosis is different.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-large\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"523\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/Position-of-boron-in-the-periodic-table-1024x523.jpg\" alt=\"Position of boron in the periodic table\" class=\"wp-image-2747\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/Position-of-boron-in-the-periodic-table-1024x523.jpg 1024w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/Position-of-boron-in-the-periodic-table-300x153.jpg 300w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/Position-of-boron-in-the-periodic-table-768x392.jpg 768w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/Position-of-boron-in-the-periodic-table.jpg 1340w\" sizes=\"(max-width: 1024px) 100vw, 1024px\" \/><figcaption class=\"wp-element-caption\">Position of boron in the periodic table<\/figcaption><\/figure><\/div>\n\n\n<p>To determine the group of p-block elements, the group has to be determined by adding 10 to the total number of electrons in the last orbit.<\/p>\n\n\n\n<p>That is, the group number of boron is 3 + 10 = 13. Therefore, we can say that the period of the boron element is 2 and the group is 13.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"determining-the-block-of-boron-by-electron-configuration\">Determine the block of boron through the electron configuration<\/h2>\n\n\n\n<p>If the last electron enters the p-orbital after the electron configuration of the element, then that element is called the p-block element. The electron configuration shows that the last electron of boron enters the p-orbital. Therefore, boron is the p-block element.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"chemical-bonding-of-boron\">Chemical bonding of boron<\/h2>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"covalent-properties-of-boron-atom\">Covalent properties of boron atom<\/h3>\n\n\n\n<p>The element of group-13 is boron(B). The ion of a boron atom is very small. When boron donates three electrons and turns into a B<sup>3+<\/sup> ion, the value of ionic radius is very low. The cation is much smaller than the size of the positive charge of the nucleus.<\/p>\n\n\n\n<p>In this case, especially in the case of BCl<sub>3<\/sub>, the tendency of Cl<sup>&#8211;<\/sup> ion to attract electrons increases. The B\u2013Cl bond creates more polarity. As a result, covalent properties are revealed in ionic bonds.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"ionic-bonds-of-boron\">Ionic bonds of boron<\/h3>\n\n\n\n<p>Boron atoms form ionic bonds by exchanging electrons with chlorine atoms. The electron configuration of the boron indicates that the last orbit of a boron atom has three electrons.<\/p>\n\n\n\n<p>The boron atom wants to be stable like an inert element by leaving three electrons in its last orbit. On the other hand, the last orbit of the <a href=\"https:\/\/valenceelectrons.com\/chlorine-electron-configuration\/\">chlorine atom<\/a> has seven electrons.<\/p>\n\n\n\n<p>The chlorine atom wants to be stable by accepting an electron in its last orbit. So, three electrons in the last orbit of the boron atom donate to the chlorine atom.<\/p>\n\n\n\n<p>Both come to a stable state by donating electrons. One boron atom and three chlorine atoms exchange electrons to form the boron trichloride(BCl<sub>3<\/sub>) compound through ionic bonding.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"reaction-of-oxygen\">Reaction of oxygen<\/h3>\n\n\n\n<p>The element of group-13 is boron. Boron reacts with the <a href=\"https:\/\/valenceelectrons.com\/oxygen-electron-configuration\/\">oxygen atom<\/a> to form oxide compounds.<\/p>\n\n\n\n<p class=\"has-text-align-center\">4B + 3O<sub>2<\/sub>     \u2192    2B<sub>2<\/sub>O<sub>3<\/sub>.<\/p>\n\n\n\n<p>From the top to the bottom of the group, the acidity of the element decreases, and the alkalinity increases. Boron is the first and most important element in group-13. Therefore, the oxide of the boron atom will be acidic. That is, Di-boron trioxide(B<sub>2<\/sub>O<sub>3<\/sub>) is an acidic compound.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"reaction-of-nitrogen\">Reaction of nitrogen<\/h3>\n\n\n\n<p>Boron reacts with the <a href=\"https:\/\/valenceelectrons.com\/nitrogen-electron-configuration\/\">nitrogen atom<\/a> to form nitride compounds.<\/p>\n\n\n\n<p class=\"has-text-align-center\">2B + N<sub>2<\/sub> (heat)     \u2192     2BN<\/p>\n\n\n\n<p>The BN and halide compounds produced are covalent and are hydrolyzed to form hydride compounds.<\/p>\n\n\n\n<ul>\n<li>BN + 3H<sub>2<\/sub>O    \u2192    B(OH)<sub>3<\/sub> + NH<sub>3<\/sub><\/li>\n\n\n\n<li>BF<sub>3<\/sub> + 3H<sub>2<\/sub>O     \u2192     B(OH)<sub>3<\/sub> + 3HF<\/li>\n\n\n\n<li>BCl<sub>3<\/sub> + 3H<sub>2<\/sub>O    \u2192    B(OH)<sub>3 <\/sub>+ 3HCl<\/li>\n\n\n\n<li>BBr<sub>3<\/sub> + 3H<sub>2<\/sub>O    \u2192    B(OH)<sub>3<\/sub> + 3HBr<\/li>\n\n\n\n<li>BI<sub>3<\/sub> + 3H<sub>2<\/sub>O     \u2192    B(OH)<sub>3<\/sub> + 3HI<\/li>\n<\/ul>\n\n\n\n<p>Boron nitride compounds are produced when boron N<sub>2<\/sub> gas is heated to a temperature of about 900\u00b0C.<\/p>\n\n\n\n<p class=\"has-text-align-center\">2B + N<sub>2<\/sub> (900 \u00b0 C)   \u2192   2BN.<\/p>\n\n\n\n<p>Boron nitride is a very slippery solid element. Boron nitride is a permanent structure composed of numerous layers of boron and nitrogen arranged in a balanced hexagonal shape. Its structure is similar to that of graphite.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"reaction-with-halogen\">Reaction with halogen<\/h3>\n\n\n\n<p>The element of group-13 is boron. Boron atoms react with halogen to form halide compounds.<\/p>\n\n\n\n<ul>\n<li>2B + 3F (heat)    \u2192    2 BF<sub>3<\/sub><\/li>\n\n\n\n<li>2B + 3Cl (heat)    \u2192    2 BCl<sub>3<\/sub><\/li>\n\n\n\n<li>2B + 3Br (heat)   \u2192    2 BBr<sub>3<\/sub><\/li>\n\n\n\n<li>2B + 3I (heat)     \u2192    2 BI<sub>3<\/sub><\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"reaction-with-water\">Reaction with water<\/h3>\n\n\n\n<p>Boron atoms react with water at 100 \u00b0 C to form hydroxide compounds.<\/p>\n\n\n\n<p class=\"has-text-align-center\">2B + 6H<sub>2<\/sub>O (100 \u00b0 C)    \u2192   2B(OH)<sub>3<\/sub> + 3H<sub>2<\/sub><\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"properties-of-boron-b\">Properties of boron atom<\/h2>\n\n\n\n<ul>\n<li>The atomic number of boron is 5. The atomic number of an element is the number of electrons in that element. Therefore, the number of electrons in the boron is five.<\/li>\n\n\n\n<li>The standard atomic weight is [10.806, 10.821]<\/li>\n\n\n\n<li>The period of the boron element is 2 and the group is 13.<\/li>\n\n\n\n<li>The value of electronegativity of boron atoms is 2.04.<\/li>\n\n\n\n<li>The covalent radius of the boron atom is 84\u00b13 pm.<\/li>\n\n\n\n<li>The atomic radius of the boron atom is 87pm.<\/li>\n\n\n\n<li>Boron atom van der Waals radius 192 pm.<\/li>\n\n\n\n<li>Ionization energies of boron atoms 1st: 800.6 kJ\/mol, 2nd: 2427.1 kJ\/mol. 3rd: 3659.7 kJ\/mol.<\/li>\n\n\n\n<li>The oxidation states of boron atoms are +3.<\/li>\n\n\n\n<li>Boron is a p-block element.<\/li>\n\n\n\n<li>The melting point of a boron atom is 2349 K \u200b(2076 \u00b0C, \u200b3769 \u00b0F). And the boiling point is 4200 K \u200b(3927 \u00b0C, \u200b7101 \u00b0F).<\/li>\n\n\n\n<li>The electron addiction value of boron atoms is \u201327kj mol <sup>\u20131<\/sup>.<\/li>\n\n\n\n<li>The number of valency and <a href=\"https:\/\/valenceelectrons.com\/what-are-valence-electrons\/\">valence electrons<\/a> of a boron atom is 3.<\/li>\n\n\n\n<li>Boron forms both covalent and ionic bonds.<\/li>\n\n\n\n<li>The ionic energy (E) of the boron atom is greater than that of the s-block element.<\/li>\n\n\n\n<li>3 electrons exist in the last orbit of the boron.<\/li>\n\n\n\n<li>Boron is used as a semiconductor.<\/li>\n\n\n\n<li>Boron conducts heat and is slightly electrically conductive.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Boron is the 5th element in the periodic table and its symbol is \u2018B\u2019. In this article, I have discussed in detail how to easily write the complete electron configuration of boron&#8230;.<\/p>\n","protected":false},"author":3,"featured_media":6025,"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\/2426"}],"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=2426"}],"version-history":[{"count":1,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/posts\/2426\/revisions"}],"predecessor-version":[{"id":6381,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/posts\/2426\/revisions\/6381"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media\/6025"}],"wp:attachment":[{"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media?parent=2426"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/categories?post=2426"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/tags?post=2426"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}