{"id":260356,"date":"2025-07-19T12:43:08","date_gmt":"2025-07-19T12:43:08","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=260356"},"modified":"2025-07-19T12:43:10","modified_gmt":"2025-07-19T12:43:10","slug":"determine-the-total-number-of-electrons-in-the-d-orbitals-of-an-atom-of-tin-sn-z-50","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/19\/determine-the-total-number-of-electrons-in-the-d-orbitals-of-an-atom-of-tin-sn-z-50\/","title":{"rendered":"Determine the total number of electrons in the d orbitals of an atom of tin, Sn (Z = 50)"},"content":{"rendered":"\n<pre id=\"preorder-ask-header-text\" class=\"wp-block-preformatted\">Determine the total number of electrons in the d orbitals of an atom of tin, Sn (Z = 50).<\/pre>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To determine the total number of electrons in the d orbitals of an atom of tin (Sn), we need to first understand the electron configuration of tin and identify which orbitals are involved.<\/p>\n\n\n\n<p>Tin (Sn) has an atomic number (Z) of 50, meaning it has 50 electrons in a neutral state. The electron configuration of an atom describes how these electrons are distributed across different orbitals, from the lowest energy to the highest.<\/p>\n\n\n\n<p>For tin (Sn), the electron configuration is:<br>Sn:[Kr]4d105s25p2\\text{Sn} : [Kr] 4d^{10} 5s^{2} 5p^{2}<\/p>\n\n\n\n<p>This configuration shows that tin has a filled 4d subshell with 10 electrons, two electrons in the 5s subshell, and two electrons in the 5p subshell.<\/p>\n\n\n\n<p>Now, focusing on the d orbitals: The 4d orbitals are filled with 10 electrons. Since each d orbital can hold a maximum of 10 electrons (with five orbitals available in the d subshell), tin&#8217;s 4d subshell is fully occupied.<\/p>\n\n\n\n<p>Thus, the total number of electrons in the d orbitals of tin is <strong>10<\/strong>.<\/p>\n\n\n\n<p>In summary, when determining the number of electrons in the d orbitals of an atom, it is essential to look at the electron configuration and specifically focus on the d subshells. For tin, the 4d subshell holds 10 electrons, making the total number of electrons in the d orbitals equal to 10.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Determine the total number of electrons in the d orbitals of an atom of tin, Sn (Z = 50). The correct answer and explanation is: To determine the total number of electrons in the d orbitals of an atom of tin (Sn), we need to first understand the electron configuration of tin and identify which [&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-260356","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/260356","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=260356"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/260356\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=260356"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=260356"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=260356"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}