The electron configuration for the sodium ion (Na\u00b3\u207a) can be derived by first considering the neutral sodium atom and then removing electrons, since Na\u00b3\u207a is a positively charged ion.<\/p>\n\n\n\n
- \n
- Neutral Sodium (Na)<\/strong>: Sodium has an atomic number of 11, which means a neutral sodium atom has 11 electrons. The electron configuration for a neutral sodium atom is: 1s2\u20092s2\u20092p6\u20093s11s^2 \\, 2s^2 \\, 2p^6 \\, 3s^11s22s22p63s1 This represents the distribution of 11 electrons in different orbitals, with the first shell (1s) holding 2 electrons, the second shell (2s and 2p) holding 8 electrons, and the third shell (3s) holding 1 electron.<\/li>\n\n\n\n
- Sodium Ion (Na\u00b3\u207a)<\/strong>: The Na\u00b3\u207a ion is formed by removing 3 electrons from the neutral sodium atom. Since the 3s orbital has the outermost electrons, these are the first to be removed. Therefore, we remove the 1 electron from the 3s orbital. After removing 3 electrons from the neutral sodium atom (2 from the 3s orbital and 1 more), the electron configuration becomes: 1s2\u20092s2\u20092p61s^2 \\, 2s^2 \\, 2p^61s22s22p6 This is the electron configuration for the Na\u00b3\u207a ion, which is the same as that of the noble gas neon (Ne), with a stable, filled shell configuration of 2 electrons in the first shell and 8 electrons in the second shell.<\/li>\n<\/ol>\n\n\n\n
Explanation<\/strong>: When a sodium atom loses 3 electrons to form the Na\u00b3\u207a ion, it reaches the same electron configuration as neon (Ne), which is a stable configuration. This is because neon has a full second shell (2s\u00b2 2p\u2076), and the loss of electrons from the 3rd shell allows sodium to achieve this stable state, resembling the noble gas configuration.<\/p>\n\n\n\n
Thus, the full electron configuration for Na\u00b3\u207a is:1s2\u20092s2\u20092p61s^2 \\, 2s^2 \\, 2p^61s22s22p6<\/p>\n\n\n\n
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<\/figure>\n","protected":false},"excerpt":{"rendered":"What is the full electron configuration for Na ^3+ The Correct Answer and Explanation is: The electron configuration for the sodium ion (Na\u00b3\u207a) can be derived by first considering the neutral sodium atom and then removing electrons, since Na\u00b3\u207a is a positively charged ion. Explanation: When a sodium atom loses 3 electrons to form the […]<\/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-247816","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/247816","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=247816"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/247816\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=247816"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=247816"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=247816"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
- Sodium Ion (Na\u00b3\u207a)<\/strong>: The Na\u00b3\u207a ion is formed by removing 3 electrons from the neutral sodium atom. Since the 3s orbital has the outermost electrons, these are the first to be removed. Therefore, we remove the 1 electron from the 3s orbital. After removing 3 electrons from the neutral sodium atom (2 from the 3s orbital and 1 more), the electron configuration becomes: 1s2\u20092s2\u20092p61s^2 \\, 2s^2 \\, 2p^61s22s22p6 This is the electron configuration for the Na\u00b3\u207a ion, which is the same as that of the noble gas neon (Ne), with a stable, filled shell configuration of 2 electrons in the first shell and 8 electrons in the second shell.<\/li>\n<\/ol>\n\n\n\n