{"id":230125,"date":"2025-06-08T20:24:10","date_gmt":"2025-06-08T20:24:10","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=230125"},"modified":"2025-06-08T20:24:12","modified_gmt":"2025-06-08T20:24:12","slug":"write-orbital-diagrams-for-each-ion-and-determine-if-the-ion-is-diamagnetic-or-paramagnetic-a-cd2-b-au-c-mo3-d-zr2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/08\/write-orbital-diagrams-for-each-ion-and-determine-if-the-ion-is-diamagnetic-or-paramagnetic-a-cd2-b-au-c-mo3-d-zr2\/","title":{"rendered":"Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic. a. Cd2+ b. Au+ c. Mo3+ d. Zr2+"},"content":{"rendered":"\n<p>Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic. a. Cd2+ b. Au+ c. Mo3+ d. Zr2+<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>Here&#8217;s the correct <strong>orbital diagrams<\/strong> and <strong>magnetic properties<\/strong> for each ion:<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>a. Cd\u00b2\u207a (Cadmium ion)<\/strong><\/h3>\n\n\n\n<p><strong>Atomic number of Cd<\/strong> = 48<br><strong>Electron configuration of Cd<\/strong> = [Kr] 4d\u00b9\u2070 5s\u00b2<br><strong>Cd\u00b2\u207a<\/strong> loses two electrons \u2192 <strong>[Kr] 4d\u00b9\u2070<\/strong><\/p>\n\n\n\n<p><strong>Orbital diagram (Cd\u00b2\u207a):<\/strong><\/p>\n\n\n\n<pre class=\"wp-block-preformatted\">makefileCopyEdit<code>4d: \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193\n<\/code><\/pre>\n\n\n\n<p><strong>All electrons are paired<\/strong> \u2192 <strong>Diamagnetic<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>b. Au\u207a (Gold(I) ion)<\/strong><\/h3>\n\n\n\n<p><strong>Atomic number of Au<\/strong> = 79<br><strong>Electron configuration of Au<\/strong> = [Xe] 4f\u00b9\u2074 5d\u00b9\u2070 6s\u00b9<br><strong>Au\u207a<\/strong> loses one electron \u2192 <strong>[Xe] 4f\u00b9\u2074 5d\u00b9\u2070<\/strong><\/p>\n\n\n\n<p><strong>Orbital diagram (Au\u207a):<\/strong><\/p>\n\n\n\n<pre class=\"wp-block-preformatted\">makefileCopyEdit<code>5d: \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193\n<\/code><\/pre>\n\n\n\n<p><strong>All electrons are paired<\/strong> \u2192 <strong>Diamagnetic<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>c. Mo\u00b3\u207a (Molybdenum(III) ion)<\/strong><\/h3>\n\n\n\n<p><strong>Atomic number of Mo<\/strong> = 42<br><strong>Electron configuration of Mo<\/strong> = [Kr] 4d\u2075 5s\u00b9<br><strong>Mo\u00b3\u207a<\/strong> loses 3 electrons \u2192 [Kr] 4d\u00b3<\/p>\n\n\n\n<p><strong>Orbital diagram (Mo\u00b3\u207a):<\/strong><\/p>\n\n\n\n<pre class=\"wp-block-preformatted\">makefileCopyEdit<code>4d: \u2191 \u2191 \u2191 _ _\n<\/code><\/pre>\n\n\n\n<p><strong>3 unpaired electrons<\/strong> \u2192 <strong>Paramagnetic<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>d. Zr\u00b2\u207a (Zirconium(II) ion)<\/strong><\/h3>\n\n\n\n<p><strong>Atomic number of Zr<\/strong> = 40<br><strong>Electron configuration of Zr<\/strong> = [Kr] 4d\u00b2 5s\u00b2<br><strong>Zr\u00b2\u207a<\/strong> loses two electrons \u2192 [Kr] 4d\u00b2<\/p>\n\n\n\n<p><strong>Orbital diagram (Zr\u00b2\u207a):<\/strong><\/p>\n\n\n\n<pre class=\"wp-block-preformatted\">makefileCopyEdit<code>4d: \u2191 \u2191 _ _ _\n<\/code><\/pre>\n\n\n\n<p><strong>2 unpaired electrons<\/strong> \u2192 <strong>Paramagnetic<\/strong><\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Explanation<\/strong><\/h3>\n\n\n\n<p>The magnetic properties of an ion\u2014whether it&#8217;s diamagnetic or paramagnetic\u2014depend on the presence of <strong>unpaired electrons<\/strong>. <strong>Diamagnetic substances<\/strong> have <strong>all electrons paired<\/strong> and are <strong>not attracted to a magnetic field<\/strong>, while <strong>paramagnetic substances<\/strong> have <strong>unpaired electrons<\/strong> and are <strong>attracted to a magnetic field<\/strong>.<\/p>\n\n\n\n<p>We begin by determining the <strong>ground-state electron configuration<\/strong> of the <strong>neutral atom<\/strong> and then remove electrons according to ionization (typically starting from the outermost s orbital, then d).<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>For <strong>Cd\u00b2\u207a<\/strong>, cadmium loses two electrons from its 5s orbital, resulting in a completely filled 4d subshell (4d\u00b9\u2070). Since all electrons are paired, Cd\u00b2\u207a is <strong>diamagnetic<\/strong>.<\/li>\n\n\n\n<li>For <strong>Au\u207a<\/strong>, gold loses its single 6s electron, leaving a filled 5d subshell (5d\u00b9\u2070). This full set of paired electrons also makes Au\u207a <strong>diamagnetic<\/strong>.<\/li>\n\n\n\n<li>For <strong>Mo\u00b3\u207a<\/strong>, molybdenum normally has 4d\u20755s\u00b9, and upon losing three electrons, we are left with a 4d\u00b3 configuration. These three electrons each occupy separate orbitals due to Hund\u2019s rule, leading to <strong>three unpaired electrons<\/strong>, making it <strong>paramagnetic<\/strong>.<\/li>\n\n\n\n<li>For <strong>Zr\u00b2\u207a<\/strong>, zirconium (4d\u00b2 5s\u00b2) loses the two 5s electrons, resulting in a 4d\u00b2 configuration. These two d electrons are unpaired, so Zr\u00b2\u207a is also <strong>paramagnetic<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>Understanding these magnetic properties is essential in chemistry and materials science, as they influence how substances interact with magnetic fields and can be used in technologies like MRI or spintronic devices.<\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/06\/learnexams-banner7-367.jpeg\" alt=\"\" class=\"wp-image-230126\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic. a. Cd2+ b. Au+ c. Mo3+ d. Zr2+ The Correct Answer and Explanation is: Here&#8217;s the correct orbital diagrams and magnetic properties for each ion: a. Cd\u00b2\u207a (Cadmium ion) Atomic number of Cd = 48Electron configuration of Cd = [Kr] [&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-230125","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230125","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=230125"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230125\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=230125"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=230125"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=230125"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}