{"id":211056,"date":"2025-05-02T15:00:03","date_gmt":"2025-05-02T15:00:03","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=211056"},"modified":"2025-05-02T15:00:06","modified_gmt":"2025-05-02T15:00:06","slug":"the-following-is-a-representation-of-the-orbital-diagram-of-al","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/02\/the-following-is-a-representation-of-the-orbital-diagram-of-al\/","title":{"rendered":"The following is a representation of the orbital diagram of Al"},"content":{"rendered":"\n<p>The following is a representation of the orbital diagram of Al. What are the four quantum numbers of the electron highlighted in the 3s subshell? 1s 2s 2p 3s<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>The four quantum numbers for the <strong>highlighted electron in the 3s subshell of aluminum (Al)<\/strong> are:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Principal quantum number (n):<\/strong> 3<\/li>\n\n\n\n<li><strong>Azimuthal quantum number (\u2113):<\/strong> 0<\/li>\n\n\n\n<li><strong>Magnetic quantum number (m\u2097):<\/strong> 0<\/li>\n\n\n\n<li><strong>Spin quantum number (m\u209b):<\/strong> +\u00bd (or -\u00bd depending on which of the two electrons in the 3s orbital is highlighted)<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation (Approx. 300 Words):<\/strong><\/h3>\n\n\n\n<p>Quantum numbers describe the properties and location of an electron in an atom. Aluminum (Al) has an atomic number of 13, meaning it has 13 electrons in its neutral state. These electrons fill orbitals in the following order:<br><strong>1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u00b9<\/strong><\/p>\n\n\n\n<p>The orbital diagram for aluminum can be represented as:<\/p>\n\n\n\n<pre class=\"wp-block-code\"><code>1s  \u2191\u2193  \n2s  \u2191\u2193  \n2p  \u2191\u2193 \u2191\u2193 \u2191\u2193  \n3s  \u2191\u2193  \n3p  \u2191<\/code><\/pre>\n\n\n\n<p>We are focusing on an electron in the <strong>3s subshell<\/strong>, which has two electrons.<\/p>\n\n\n\n<p>Each electron is characterized by <strong>four quantum numbers<\/strong>:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Principal Quantum Number (n):<\/strong><br>This indicates the main energy level or shell.<br>For the 3s subshell, <strong>n = 3<\/strong>.<\/li>\n\n\n\n<li><strong>Azimuthal Quantum Number (\u2113):<\/strong><br>This defines the subshell or orbital shape.<br>For <strong>s-orbitals<\/strong>, \u2113 = 0.<\/li>\n\n\n\n<li><strong>Magnetic Quantum Number (m\u2097):<\/strong><br>This defines the orientation of the orbital.<br>For \u2113 = 0, the only possible value is <strong>m\u2097 = 0<\/strong>.<\/li>\n\n\n\n<li><strong>Spin Quantum Number (m\u209b):<\/strong><br>This indicates the spin of the electron, which can be either +\u00bd (spin-up) or -\u00bd (spin-down).<br>The 3s orbital contains <strong>two electrons<\/strong>: one with <strong>m\u209b = +\u00bd<\/strong> and one with <strong>m\u209b = -\u00bd<\/strong>.<\/li>\n<\/ol>\n\n\n\n<p>Since the question mentions a &#8220;highlighted&#8221; electron but doesn&#8217;t specify which of the two in the 3s orbital is meant, both spins are possible. If the diagram shows the first (spin-up) electron, the spin is <strong>+\u00bd<\/strong>. If it\u2019s the second, it&#8217;s <strong>-\u00bd<\/strong>.<\/p>\n\n\n\n<p>Therefore, one possible set of quantum numbers for the 3s electron is:<br><strong>(n = 3, \u2113 = 0, m\u2097 = 0, m\u209b = +\u00bd)<\/strong><\/p>\n","protected":false},"excerpt":{"rendered":"<p>The following is a representation of the orbital diagram of Al. What are the four quantum numbers of the electron highlighted in the 3s subshell? 1s 2s 2p 3s The correct answer and explanation is : The four quantum numbers for the highlighted electron in the 3s subshell of aluminum (Al) are: Explanation (Approx. 300 [&hellip;]<\/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-211056","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/211056","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=211056"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/211056\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=211056"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=211056"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=211056"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}