{"id":2378,"date":"2024-01-29T23:23:09","date_gmt":"2024-01-29T17:23:09","guid":{"rendered":"https:\/\/valenceelectrons.com\/?p=2378"},"modified":"2024-04-28T00:13:10","modified_gmt":"2024-04-27T18:13:10","slug":"lithium-electron-configuration","status":"publish","type":"post","link":"https:\/\/valenceelectrons.com\/lithium-electron-configuration\/","title":{"rendered":"Electronic Configuration of Lithium (Li, Li+ ion)"},"content":{"rendered":"\n<p>Lithium is the 3rd element in the periodic table and its symbol is &#8216;Li&#8217;. In this article, I have discussed in detail how to easily write the complete electron configuration of lithium. Hopefully, after reading this article, you will know more about this topic.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\">What is the electron configuration for lithium?<\/h2>\n\n\n\n<p>The total number of&nbsp;<a href=\"https:\/\/valenceelectrons.com\/lithium-protons-neutrons-electrons\/\">electrons in lithium<\/a>&nbsp;is three. These electrons are arranged according to specific rules in different orbitals.<\/p>\n\n\n\n<p>The arrangement of electrons in lithium in specific rules in different orbits and orbitals is called the&nbsp;<a href=\"https:\/\/valenceelectrons.com\/electron-configuration\/\">electron configuration<\/a>&nbsp;of lithium.<\/p>\n\n\n\n<p>The electron configuration of lithium is [<a href=\"https:\/\/valenceelectrons.com\/helium-electron-configuration\/\">He<\/a>] 2s<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=\"1200\" height=\"630\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/06\/Lithium-Li-electron-configuration.jpg\" alt=\"Lithium atom electron configuration\" class=\"wp-image-4362\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/06\/Lithium-Li-electron-configuration.jpg 1200w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/06\/Lithium-Li-electron-configuration-768x403.jpg 768w\" sizes=\"(max-width: 1200px) 100vw, 1200px\" \/><figcaption class=\"wp-element-caption\">Lithium(Li) 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=\"lithium-li-electron-configuration-through-orbit\">Electron configuration of Lithium 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 electrons of the atom 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 maximum electron holding capacity in the 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 the 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 the 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 the 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 <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. The atomic number is the number of electrons in that element.<\/p>\n\n\n\n<p>The&nbsp;atomic number of lithium&nbsp;is 3. That is, the number of electrons in lithium is 3. Therefore, a lithium atom will have two electrons in the first shell and one in the 2nd shell.<\/p>\n\n\n\n<p>Therefore, the order of the number of electrons in each shell of the lithium(Li) atom is 2, 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&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-lithium-atom-through-orbital\">Electron configuration of lithium atom 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>Sub-shell 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 lithium enter the 1s orbital.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"1280\" height=\"786\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2023\/03\/Lithium-electron-configuration.jpg\" alt=\"Lithium Electron Configuration\" class=\"wp-image-6023\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2023\/03\/Lithium-electron-configuration.jpg 1280w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2023\/03\/Lithium-electron-configuration-768x472.jpg 768w\" sizes=\"(max-width: 1280px) 100vw, 1280px\" \/><figcaption class=\"wp-element-caption\">Lithium Electron Configuration<\/figcaption><\/figure><\/div>\n\n\n<p>The s-orbital can have a maximum of two electrons. Therefore, the remaining one electron enters the 2s orbital.&nbsp;Therefore, the lithium complete electron configuration will be 1s<sup>2<\/sup>&nbsp;2s<sup>1<\/sup>.<\/p>\n\n\n\n<blockquote class=\"wp-block-quote is-layout-flow wp-block-quote-is-layout-flow\">\n<p>Note: The unabbreviated electron configuration of lithium is [He] 2s<sup>1<\/sup>.<\/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 has-text-align-left\" id=\"electron-configuration-of-lithium-ion-li\">Lithium-ion (Li<sup>+<\/sup>) electron configuration<\/h2>\n\n\n\n<p>After the electron configuration, the last shell of the lithium atom has an electron. In this case, the&nbsp;<a href=\"https:\/\/valenceelectrons.com\/valence-electrons-of-lithium\/\">valence electrons&nbsp;of lithium<\/a> are one, and also valency is 1.<\/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. Lithium atom donates an electron of the last shell to turn into a lithium ion(Li<sup>+<\/sup>).<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-full\"><img loading=\"lazy\" decoding=\"async\" width=\"1197\" height=\"628\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Charge-of-a-lithium-atom.jpg\" alt=\"charge of a lithium atom\" class=\"wp-image-4834\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Charge-of-a-lithium-atom.jpg 1197w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2022\/06\/Charge-of-a-lithium-atom-768x403.jpg 768w\" sizes=\"(max-width: 1197px) 100vw, 1197px\" \/><figcaption class=\"wp-element-caption\">Charge of a lithium atom<\/figcaption><\/figure><\/div>\n\n\n<p>The elements that form bonds by donating electrons are called cation. Lithium leaves an electron and turns into a positive ion. Therefore, lithium is a cation element.<\/p>\n\n\n\n<p class=\"has-text-align-center\">Li     &#8211;    e<sup>&#8211;<\/sup>   \u2192    Li<sup>+<\/sup><\/p>\n\n\n\n<p>Here, the electron configuration of lithium ion(Li<sup>+<\/sup>) is 1s<sup>2<\/sup>. This electron configuration shows that the lithium ion(Li<sup>+<\/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-the-electron-configuration\">Determine the group and period of lithium 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 shows that the last shell of the lithium is 2. So, the period of the lithium atom is 2.<\/p>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-large\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"526\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/The-position-of-lithium-in-the-periodic-table-1024x526.jpg\" alt=\"position of lithium in the periodic table\" class=\"wp-image-2703\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/The-position-of-lithium-in-the-periodic-table-1024x526.jpg 1024w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/The-position-of-lithium-in-the-periodic-table-300x154.jpg 300w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/The-position-of-lithium-in-the-periodic-table-768x394.jpg 768w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/The-position-of-lithium-in-the-periodic-table.jpg 1342w\" sizes=\"(max-width: 1024px) 100vw, 1024px\" \/><figcaption class=\"wp-element-caption\">Position of lithium in the periodic table<\/figcaption><\/figure><\/div>\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. An electron exists in the last orbit of the lithium atom.<\/p>\n\n\n\n<p>That is, the group number of lithium is 1. Therefore, we can say that the period of the lithium is 2 and the group is 1.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"determining-the-block-of-lithium-by-electron-configuration\">Determine the block of lithium through the electron configuration<\/h2>\n\n\n\n<p>If the last electron enters the s-orbital after the electron configuration of the element, then that element is called the s-block element. The electron configuration shows that the last electron of lithium enters the s-orbital. Therefore, lithium is the s-block element.<\/p>\n\n\n\n<p>The elements in group-1 and 2 are the s-block elements. And helium is the s-block element. There are 14 s-block elements in the 118 elements of the periodic table.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"lithium-is-an-alkali-metal\">Why lithium is an alkali metal?<\/h2>\n\n\n\n<p>The elements in group-1 of the periodic table are alkali metals. Lithium is the element of group number 1 of the periodic table. Therefore, lithium is an alkali metal. (Excluding the only hydrogen)<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"oxidation-and-reduction-properties\">Oxidation and Reduction properties<\/h2>\n\n\n\n<p>The element of group-1 is lithium. Which is an intense reducing element. The lithium atom donates an electron of the s-orbital. And the lithium atom forms the electron structure of the helium element.<\/p>\n\n\n\n<p>The intensity of lithium is so high that lithium atoms reduce the hydrogen to form lithium hydride compounds.<\/p>\n\n\n\n<p class=\"has-text-align-center\">2Li + H<sub>2<\/sub>    \u2192      2LiH<\/p>\n\n\n\n<p>The ionization potential of the alkali metal decreases as it moves from top to bottom within the group of periodic tables. That is, the reduction capacity continues to increase.<\/p>\n\n\n\n<p>As such, lithium is a weak reducing agent and cesium is a severe reducing agent. But lithium is the most powerful reducing agent among alkali metals. The oxidizing potential of lithium atoms is +3.04.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"properties-of-lithium\">Properties of Lithium<\/h2>\n\n\n\n<ul>\n<li>The atomic number of lithium is 3. The atomic number of an element is the number of electrons in that element. Therefore, the number of electrons in lithium is three.<\/li>\n\n\n\n<li>Lithium&#8217;s standard atomic weight is 6.941.<\/li>\n\n\n\n<li>Lithium is an alkali and an intensely negative metal. Its oxides and hydroxides are strong alkalis.<\/li>\n\n\n\n<li>The value of electronegativity of lithium atoms is comparatively much lower. The value of electronegativity of lithium atoms is 0.98.<\/li>\n\n\n\n<li>The covalent radius of the lithium atom is 128 \u00b1 7 pm.<\/li>\n\n\n\n<li>The ionic radius of the lithium atom is 6.0 \u00d7 10 <sup>\u20132<\/sup> nm.<\/li>\n\n\n\n<li>Lithium atom van der Waals radius 182 pm.<\/li>\n\n\n\n<li>Ionization energies of lithium atoms E1 = 520 kj\/mol, E 2 = 7298 kj\/mol, E3 = 11815 kj\/mol.<\/li>\n\n\n\n<li>The oxidation states of lithium atoms are +1.<\/li>\n\n\n\n<li>The volume of lithium atoms is 13.1cc \/ mol.<\/li>\n\n\n\n<li>The melting point of a lithium atom is 180.50 \u00b0 C (453.65 K, 356.90 \u00b0 F). And the boiling point is 1342 C.<\/li>\n\n\n\n<li>The period of the lithium element is 2. And the group is 1.<\/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 lithium atom is 1.<\/li>\n\n\n\n<li>Lithium forms both covalent and ionic bonds.<\/li>\n\n\n\n<li>Lithium is a highly electrically positive element. As a result, the lithium atom is stable and produces ions in the solution.<\/li>\n\n\n\n<li>An electron exists in the last orbit of lithium.<\/li>\n\n\n\n<li>The atomic radius of a lithium atom is 152 pm.<\/li>\n\n\n\n<li>Lithium atoms react with hydrogen, oxygen, and halogen to form compounds.<\/li>\n<\/ul>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"ionic-bond-of-lithium\">Ionic bond of lithium<\/h2>\n\n\n\n<p>Lithium atoms form an ionic bond with fluorine atoms through the exchange of electrons. An electron exists in the last orbit of the lithium atom. The lithium atom wants to be more stable by forming one helium atom by eliminating an electron in the last orbit. <\/p>\n\n\n\n<p>On the other hand, The <a href=\"https:\/\/valenceelectrons.com\/fluorine-electron-configuration\/\">electron configuration of fluorine<\/a> atom shows that the seven electrons exist in the last orbit. The fluorine atom wants to be more stable like the <a href=\"https:\/\/valenceelectrons.com\/neon-electron-configuration\/\">neon atom<\/a> by accepting an electron.<\/p>\n\n\n\n<p>The lithium atom donates an electron of its last orbit to the fluorine atom and LiF forms compounds through ionic bonds.<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"lithium-compound-formation\">lithium compound formation<\/h2>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"reaction-of-lithium-with-halogen\">Reaction of lithium with halogen<\/h3>\n\n\n\n<p>Lithium atoms react with halogen to form halide compounds.<br><\/p>\n\n\n\n<ul>\n<li>2Li + F<sub>2<\/sub>     \u2192      2LiF<\/li>\n\n\n\n<li>2Li + Cl<sub>2<\/sub>    \u2192      2LiCl<\/li>\n\n\n\n<li>2Li + Br<sub>2<\/sub>   \u2192      2LiBr<\/li>\n\n\n\n<li>2Li + I<sub>2<\/sub>      \u2192      2LiI<\/li>\n<\/ul>\n\n\n<div class=\"wp-block-image\">\n<figure class=\"aligncenter size-large\"><img loading=\"lazy\" decoding=\"async\" width=\"1024\" height=\"509\" src=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/LiF-bonding-1024x509.jpg\" alt=\"LiF bonding\" class=\"wp-image-2705\" srcset=\"https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/LiF-bonding-1024x509.jpg 1024w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/LiF-bonding-300x149.jpg 300w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/LiF-bonding-768x382.jpg 768w, https:\/\/valenceelectrons.com\/wp-content\/uploads\/2021\/08\/LiF-bonding.jpg 1244w\" sizes=\"(max-width: 1024px) 100vw, 1024px\" \/><figcaption class=\"wp-element-caption\">LiF bonding<\/figcaption><\/figure><\/div>\n\n\n<p>The activity of alkali metals with specific halogens gradually increases from lithium to cesium. That is, Li &lt; Na &lt; K &lt; Rb &lt; Cs. But except for lithium, all other alkali metal halides dissolve very easily in water.<\/p>\n\n\n\n<p>The intense gravitational force between Li<sup>+<\/sup> and F<sup>\u2013<\/sup> ion in the crystal reduces the solubility of LiF. Therefore, LiF is less soluble in water. LiCl, LiBr, and LiI are soluble in organic solvents ethanol, and propanol.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"reaction-of-oxygen\">Reaction of oxygen<\/h3>\n\n\n\n<p>Group-1 elements, such as alkali metals, have a greater ability to bind to oxygen. Lithium (an alkali metal) reacts with controlled amounts of <a href=\"https:\/\/valenceelectrons.com\/oxygen-electron-configuration\/\">oxygen<\/a> to form LiO (oxide) compounds. <\/p>\n\n\n\n<p class=\"has-text-align-center\">4Li (s) + O<sub>2<\/sub> (g) \u2192 2Li<sub>2<\/sub>O (lithium oxide)<br>Heating lithium with excess oxygen produces the compound Li<sub>2<\/sub>O<sub>2<\/sub>.<br>2Li + O<sub>2<\/sub>   \u2192  Li<sub>2<\/sub>O<sub>2<\/sub> (lithium peroxide).<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"reaction-of-hydrogen\">Reaction of hydrogen<\/h3>\n\n\n\n<p>Alkali metals react with dry <a href=\"https:\/\/valenceelectrons.com\/hydrogen-electron-configuration\/\">hydrogen<\/a> at a temperature of about 400 \u00b0 C to form metallic hydrides. However, the lithium atom is different from all other alkali metals. Lithium reacts with hydrogen at a temperature of 800\u00b0C to produce lithium hydride.<\/p>\n\n\n\n<p class=\"has-text-align-center\">2Li + H<sub>2<\/sub>  \u2192    2 LiH.<\/p>\n\n\n\n<p>The reaction activity decreases as it moves from lithium to cesium element. Metal hydride stability tends to decrease from LiH to CsH.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"lithium-oxide\">Lithium oxide<\/h3>\n\n\n\n<p>Lithium reacts with water to produce LiOH.<\/p>\n\n\n\n<p class=\"has-text-align-center\">2Li + 2H<sub>2<\/sub>O   \u2192   2LiOH + H<sub>2<\/sub><\/p>\n\n\n\n<p>Lithium is oxidized by oxygen in the air to produce alkaline Li<sub>2<\/sub>O.<\/p>\n\n\n\n<p class=\"has-text-align-center\">4Li + O<sub>2<\/sub>    \u2192    2Li<sub>2<\/sub>O<\/p>\n\n\n\n<p>Li<sub>2<\/sub>O reacts with water to produce mild alkali LiOH.<\/p>\n\n\n\n<p class=\"has-text-align-center\">Li<sub>2<\/sub>O + H<sub>2<\/sub>O   \u2192    2LiOH<\/p>\n\n\n\n<p>As Li<sub>2<\/sub>O is alkaline, it destroys the acidity of HCl and produces salt and water.<\/p>\n\n\n\n<p class=\"has-text-align-center\">Li<sub>2<\/sub>O + 2HCl    \u2192   2LiCl + H<sub>2<\/sub>O<\/p>\n\n\n\n<h3 class=\"wp-block-heading\" id=\"reaction-of-lithium-with-other-elements\">Reaction of lithium with other elements<\/h3>\n\n\n\n<p>Lithium atoms react with <a href=\"https:\/\/valenceelectrons.com\/sulfur-electron-configuration\/\">sulfur<\/a> and <a href=\"https:\/\/valenceelectrons.com\/phosphorus-electron-configuration\/\">phosphorus<\/a> to form sulfide and phosphide compounds.<\/p>\n\n\n\n<p class=\"has-text-align-center\">16 Li + S<sub>8<\/sub>      \u2192      8Li<sub>2<\/sub>S<br>12Li + P<sub>4 <\/sub>      \u2192      4Li<sub>3<\/sub>P<\/p>\n\n\n\n<p>The alkali metal lithium reacts with <a href=\"https:\/\/valenceelectrons.com\/nitrogen-electron-configuration\/\">nitrogen(N<sub>2<\/sub>)<\/a> at high temperatures to form nitride compounds.<\/p>\n\n\n\n<p class=\"has-text-align-center\">6Li + N<sub>2<\/sub> \u2192 2Li<sub>3<\/sub>N<\/p>\n\n\n\n<h2 class=\"wp-block-heading\" id=\"exceptional-properties-of-lithium-atom\">Exceptional properties of the lithium atom<\/h2>\n\n\n\n<p>In general, elements of the same group have similarities in physical and chemical properties. The elements of group-1 are alkali metals. The elements are lithium(Li), <a href=\"https:\/\/valenceelectrons.com\/sodium-electron-configuration\/\">sodium(Na)<\/a>, <a href=\"https:\/\/valenceelectrons.com\/potassium-electron-configuration\/\">potassium(K)<\/a>, <a href=\"https:\/\/valenceelectrons.com\/rubidium-electron-configuration\/\">rubidium(Rb)<\/a>, <a href=\"https:\/\/valenceelectrons.com\/cesium-electron-configuration\/\">cesium(Cs)<\/a>.<\/p>\n\n\n\n<p>However, the properties of lithium are different from the properties of all the other elements in this group. The elements in group 1 form ionic bonds in halide compounds. However, the halide compounds of the lithium atom have covalent bonds.<\/p>\n\n\n\n<p>For this reason, sodium halide is soluble in water but lithium halide is very slightly soluble in water. LiCl, LiBr, and LiI are soluble in various organic solvents (ethanol, propanol, ether).<\/p>\n\n\n\n<p>Alkali metals react with hydrogen at 400\u00b0 C to form hydride compounds. But lithium atoms form lithium hydride compounds with hydrogen at a temperature of 800\u00b0 C.<br>2Li + H<sub>2<\/sub> (800\u00b0 C) \u2192 2LiH.<\/p>\n\n\n\n<p>The reasons for the exceptional properties of lithium (Li) are-<\/p>\n\n\n\n<ul>\n<li>The small size of Li atom and Li<sup>+<\/sup> ion.<\/li>\n\n\n\n<li>The polarization capacity of Li<sup>+<\/sup> ions is high.<\/li>\n\n\n\n<li>The zero d orbital is missing at the valence level.<\/li>\n\n\n\n<li>Lithium is a high ionic potential element.<\/li>\n<\/ul>\n\n\n\n<p>Due to the exceptional properties of lithium, several distinctions of lithium with other alkali metals have been observed. They are-<\/p>\n\n\n\n<ol>\n<li>Lithium is less active than alkali metals. Its bright color does not fade easily when it comes in contact with air. In the case of other alkali metals, their bright color fades in contact with air.<\/li>\n\n\n\n<li>Lithium (Li) reacts with oxygen to form only monoxide (Li<sub>2<\/sub>O) compounds. But never forms peroxide (Li<sub>2<\/sub>O<sub>2<\/sub>) or superoxide (LiO<sub>2<\/sub>).<\/li>\n\n\n\n<li>Lithium is the only alkali metal that reacts with nitrogen (N<sub>2<\/sub>) to produce Li<sub>3<\/sub>N.<br>6Li + N<sub>2<\/sub>     \u2192    2Li<sub>3<\/sub>N.<br>All other alkali metals do not react with nitrogen (N<sub>2<\/sub>).<\/li>\n\n\n\n<li>When the alkaline metal nitride is heated, it decomposes, and metallic nitride and oxygen are produced.<br>2MNO<sub>3<\/sub>    \u2192    2 MNO<sub>2<\/sub> + O<sub>2<\/sub>. Here, [M = Na, K, Rb]<\/li>\n\n\n\n<li>When lithium nitride is heated, it decomposes and produces lithium monoxide (Li<sub>2<\/sub>O), NO<sub>2<\/sub>, and oxygen (O<sub>2<\/sub>).<br>4LiNO<sub>3<\/sub> (heat) \u2192 2Li<sub>2<\/sub>O + 4NO<sub>2 <\/sub>+ O<sub>2<\/sub><\/li>\n\n\n\n<li>Hydroxides of alkali metals have a strong base. However, lithium hydroxide is a weak base.<\/li>\n\n\n\n<li>Lithium chloride (LiCl) combines with water to form dihydrate compounds. But NaCl, KCl, and CsCl never form hydrate compounds.<\/li>\n<\/ol>\n\n\n\n<h2 class=\"wp-block-heading\">Reference<\/h2>\n\n\n\n<ol>\n<li>&nbsp;<a href=\"https:\/\/www.ciaaw.org\/lithium.htm\" target=\"_blank\" rel=\"noreferrer noopener nofollow\">&#8220;Standard Atomic Weights: Lithium&#8221;<\/a>.&nbsp;<a href=\"https:\/\/en.wikipedia.org\/wiki\/Commission_on_Isotopic_Abundances_and_Atomic_Weights\" target=\"_blank\" rel=\"noreferrer noopener nofollow\">CIAAW<\/a>. 2009.<\/li>\n\n\n\n<li>Weast, Robert (1984).&nbsp;<em>CRC, Handbook of Chemistry and Physics<\/em>. Boca Raton, Florida: Chemical Rubber Company Publishing. pp.&nbsp;E110.&nbsp;ISBN&nbsp;<bdi>0-8493-0464-4<\/bdi>.<\/li>\n<\/ol>\n","protected":false},"excerpt":{"rendered":"<p>Lithium is the 3rd element in the periodic table and its symbol is &#8216;Li&#8217;. In this article, I have discussed in detail how to easily write the complete electron configuration of lithium&#8230;.<\/p>\n","protected":false},"author":3,"featured_media":6023,"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\/2378"}],"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=2378"}],"version-history":[{"count":1,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/posts\/2378\/revisions"}],"predecessor-version":[{"id":6383,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/posts\/2378\/revisions\/6383"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media\/6023"}],"wp:attachment":[{"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/media?parent=2378"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/categories?post=2378"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/valenceelectrons.com\/wp-json\/wp\/v2\/tags?post=2378"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}