The correct answer is a) 2<\/strong>.<\/p>\n\n\n\n To determine how many electrons are in the outermost energy level of the Al\u00b3\u207a<\/strong> ion, let’s break it down step by step.<\/p>\n\n\n\n Therefore, the Al\u00b3\u207a ion has 2 electrons<\/strong> in its outermost energy level.<\/p>\n\n\n\n How many electrons are in the outermost energy level of the Al3+ ion in its ground state? a) 2 b) 3 c) 6 d) 8 The Correct Answer and Explanation is: The correct answer is a) 2. Explanation: To determine how many electrons are in the outermost energy level of the Al\u00b3\u207a ion, let’s break […]<\/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-239821","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/239821","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=239821"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/239821\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=239821"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=239821"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=239821"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Explanation:<\/h3>\n\n\n\n
\n
Aluminum (Al) has an atomic number of 13, which means it has 13 protons in the nucleus and, in its neutral state, 13 electrons. The electron configuration for a neutral Al atom is:
Al:\u00a01s2\u20092s2\u20092p6\u20093s2\u20093p1\\text{Al: } 1s^2 \\, 2s^2 \\, 2p^6 \\, 3s^2 \\, 3p^1Al:\u00a01s22s22p63s23p1
This means aluminum has 2 electrons in the first energy level (1s), 8 electrons in the second energy level (2s and 2p), and 3 electrons in the third energy level (3s and 3p).<\/li>\n\n\n\n
When aluminum forms an Al\u00b3\u207a ion, it loses 3 electrons. This happens because aluminum tends to lose electrons to achieve a stable electron configuration, similar to the nearest noble gas (in this case, neon).
The electron configuration of Al\u00b3\u207a<\/strong> is obtained by removing 3 electrons from the neutral aluminum atom:
Al\u00b3\u207a:\u00a01s2\u20092s2\u20092p6\\text{Al\u00b3\u207a: } 1s^2 \\, 2s^2 \\, 2p^6Al\u00b3\u207a:\u00a01s22s22p6
After the loss of 3 electrons, the electron configuration of the Al\u00b3\u207a ion is identical to that of neon (Ne), which has 10 electrons.<\/li>\n\n\n\n
In the Al\u00b3\u207a ion, the outermost energy level is the second energy level (n=2), as the third energy level (n=3) is now empty after the loss of the 3 electrons.
The second energy level (n=2) contains 8 electrons in the 2s and 2p orbitals, but the outermost electrons are in the 2p subshell, which holds 2 electrons<\/strong>.<\/li>\n<\/ol>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-72.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"