{"id":247826,"date":"2025-07-07T20:09:13","date_gmt":"2025-07-07T20:09:13","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=247826"},"modified":"2025-07-07T20:09:15","modified_gmt":"2025-07-07T20:09:15","slug":"give-the-full-electron-configuration-for-sodium-na-electron-configuration","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/07\/give-the-full-electron-configuration-for-sodium-na-electron-configuration\/","title":{"rendered":"Give the full electron configuration for sodium (Na) electron configuration"},"content":{"rendered":"\n

Give the full electron configuration for sodium (Na) electron configuration: U X2 x2<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

The electron configuration of sodium (Na) is the distribution of its 11 electrons in various orbitals, according to the Aufbau principle, Pauli Exclusion Principle, and Hund’s Rule.<\/p>\n\n\n\n

Sodium (Na) Electron Configuration:<\/h3>\n\n\n\n

The full electron configuration for sodium (Na) is:<\/p>\n\n\n\n

1s\u00b2 2s\u00b2 2p\u2076 3s\u00b9<\/strong><\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n

Sodium (Na) has an atomic number of 11, which means it has 11 electrons. The electron configuration is determined by filling the orbitals in order of increasing energy, as outlined by the Aufbau principle.<\/p>\n\n\n\n

    \n
  1. 1s\u00b2<\/strong>: The first two electrons go into the 1s orbital. This is the lowest energy orbital, and it can hold a maximum of two electrons.<\/li>\n\n\n\n
  2. 2s\u00b2<\/strong>: The next two electrons fill the 2s orbital. The 2s orbital is also a low-energy orbital, and it can hold a maximum of two electrons.<\/li>\n\n\n\n
  3. 2p\u2076<\/strong>: The next six electrons fill the 2p orbital. The 2p orbital can hold a maximum of six electrons, and once it’s full, the remaining electrons must go into higher-energy orbitals.<\/li>\n\n\n\n
  4. 3s\u00b9<\/strong>: The final electron goes into the 3s orbital, which is the next available orbital. Since this is the 11th electron, it occupies the lowest available energy level, which is the 3s orbital.<\/li>\n<\/ol>\n\n\n\n

    This configuration shows that sodium has a stable inner shell with a full 1s, 2s, and 2p orbitals, and a single electron in its outer 3s orbital. This outer electron is loosely bound and is responsible for the chemical reactivity of sodium. Sodium tends to lose this electron easily, forming a Na\u207a ion with a stable electron configuration of 1s\u00b2 2s\u00b2 2p\u2076<\/strong>, similar to the noble gas neon (Ne).<\/p>\n\n\n\n

    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

    Give the full electron configuration for sodium (Na) electron configuration: U X2 x2 The Correct Answer and Explanation is: The electron configuration of sodium (Na) is the distribution of its 11 electrons in various orbitals, according to the Aufbau principle, Pauli Exclusion Principle, and Hund’s Rule. Sodium (Na) Electron Configuration: The full electron configuration for […]<\/p>\n","protected":false},"author":1,"featured_media":0,"comment_status":"closed","ping_status":"closed","sticky":false,"template":"","format":"standard","meta":{"site-sidebar-layout":"default","site-content-layout":"","ast-site-content-layout":"default","site-content-style":"default","site-sidebar-style":"default","ast-global-header-display":"","ast-banner-title-visibility":"","ast-main-header-display":"","ast-hfb-above-header-display":"","ast-hfb-below-header-display":"","ast-hfb-mobile-header-display":"","site-post-title":"","ast-breadcrumbs-content":"","ast-featured-img":"","footer-sml-layout":"","ast-disable-related-posts":"","theme-transparent-header-meta":"","adv-header-id-meta":"","stick-header-meta":"","header-above-stick-meta":"","header-main-stick-meta":"","header-below-stick-meta":"","astra-migrate-meta-layouts":"default","ast-page-background-enabled":"default","ast-page-background-meta":{"desktop":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"ast-content-background-meta":{"desktop":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"tablet":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""},"mobile":{"background-color":"var(--ast-global-color-5)","background-image":"","background-repeat":"repeat","background-position":"center center","background-size":"auto","background-attachment":"scroll","background-type":"","background-media":"","overlay-type":"","overlay-color":"","overlay-opacity":"","overlay-gradient":""}},"footnotes":""},"categories":[25],"tags":[],"class_list":["post-247826","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/247826","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/users\/1"}],"replies":[{"embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/comments?post=247826"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/247826\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=247826"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=247826"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=247826"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}