{"id":230881,"date":"2025-06-10T07:32:58","date_gmt":"2025-06-10T07:32:58","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=230881"},"modified":"2025-06-10T07:33:00","modified_gmt":"2025-06-10T07:33:00","slug":"enter-the-orbital-diagram-for-the-ion-cd2cd2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/10\/enter-the-orbital-diagram-for-the-ion-cd2cd2\/","title":{"rendered":"Enter the orbital diagram for the ion Cd2+Cd2+."},"content":{"rendered":"\n
Enter the orbital diagram for the ion Cd2+Cd2+. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. Not all group 2 targets will be filled. Reset Help 1s Group 1 1s 4d Group 1 4d 2s Group 1 2s 4f Group 1 4f 2p Group 1 2p 5s Group 1 5s 3s Group 1 3s 5p Group 1 5p 3p Group 1 3p 5d Group 1 5d 3d Group 1 3d 5f Group 1 5f 4s Group 1 4s \u00e2\u2020\u00bf\u00e2\u2020\u00bf Group 2 upharpoonleft 4p Group 1 4p \u00e2\u2020\u00bf\u00e2\u2021\u201a\u00e2\u2020\u00bf\u00e2\u2021\u201a Group 2 upharpoonleft ! downharpoonright G1G1G1G1G1G1G1G1G1G1G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2 SubmitRequest Answer Part B Enter the orbital diagram for the ion Au+Au+. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. Not all group 2 targets will be filled. Reset Help 1s Group 1 1s 5s Group 1 5s 2s Group 1 2s 5p Group 1 5p 2p Group 1 2p 5d Group 1 5d 3s Group 1 3s 5f Group 1 5f 3p Group 1 3p 6s Group 1 6s 3d Group 1 3d 6p Group 1 6p 4s Group 1 4s 6d Group 1 6d 4p Group 1 4p 6f Group 1 6f 4d Group 1 4d \u00e2\u2020\u00bf\u00e2\u2020\u00bf Group 2 upharpoonleft 4f Group 1 4f \u00e2\u2020\u00bf\u00e2\u2021\u201a\u00e2\u2020\u00bf\u00e2\u2021\u201a Group 2 upharpoonleft ! downharpoonright G1G1G1G1G1G1G1G1G1G1G1G1G1G1G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2 SubmitRequest Answer Part C Construct the orbital diagram for the ion Mo3+Mo3+. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. Not all group 2 targets will be filled. Reset Help 1s Group 1 1s 4d Group 1 4d 2s Group 1 2s 4f Group 1 4f 2p Group 1 2p 5s Group 1 5s 3s Group 1 3s 5p Group 1 5p 3p Group 1 3p 5d Group 1 5d 3d Group 1 3d 5f Group 1 5f 4s Group 1 4s \u00e2\u2020\u00bf\u00e2\u2020\u00bf Group 2 upharpoonleft 4p Group 1 4p \u00e2\u2020\u00bf\u00e2\u2021\u201a\u00e2\u2020\u00bf\u00e2\u2021\u201a Group 2 upharpoonleft ! downharpoonright G1G1G1G1G1G1G1G1G1G1G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2G2<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
Orbital Diagrams and Explanations for Cd\u00b2\u207a, Au\u207a, and Mo\u00b3\u207a<\/strong><\/h3>\n\n\n\n\n\n\n\n
Part A: Cd\u00b2\u207a Ion Orbital Diagram<\/strong><\/h2>\n\n\n\n
Electron configuration of neutral Cd:<\/strong> Cd (Z = 48): [Kr] 4d\u00b9\u2070 5s\u00b2<\/code><\/p>\n\n\n\n
Cd\u00b2\u207a loses 2 electrons<\/strong>, typically from the 5s orbital<\/strong>:<\/p>\n\n\n\n
pgsqlCopyEdit1s \u2191\u2193 2s \u2191\u2193 2p \u2191\u2193\u2191\u2193\u2191\u2193 3s \u2191\u2193 3p \u2191\u2193\u2191\u2193\u2191\u2193 4s \u2191\u2193 3d \u2191\u2193\u2191\u2193\u2191\u2193\u2191\u2193\u2191\u2193\u2191\u2193 4p \u2191\u2193\u2191\u2193\u2191\u2193 \n4d \u2191\u2191\u2191 (3 electrons in separate 4d orbitals, following Hund\u2019s rule) \n(5s is empty)\n<\/code><\/pre>\n\n\n\n\n\n\n\n
Explanation<\/strong><\/h2>\n\n\n\n
Electron configurations and orbital diagrams follow the Aufbau principle<\/strong>, Pauli exclusion principle<\/strong>, and Hund\u2019s rule<\/strong>. These rules govern the order of orbital filling and how electrons are arranged in orbitals.<\/p>\n\n\n\n
Cadmium\u2019s atomic number is 48. In its neutral state, its configuration ends in 5s\u00b2 4d\u00b9\u2070<\/code>. When it becomes Cd\u00b2\u207a, it loses the two 5s<\/strong> electrons first, leaving a full 4d subshell (4d\u00b9\u2070<\/code>). This makes Cd\u00b2\u207a a d\u00b9\u2070<\/strong> system with a stable noble-gas-like configuration and a diamagnetic character (no unpaired electrons).<\/p>\n\n\n\n
Au\u207a (Gold ion):<\/strong><\/h3>\n\n\n\n
Gold (Z = 79) has a filled 5d subshell and one electron in the 6s orbital (6s\u00b9<\/code>). Upon ionization to Au\u207a, it loses that lone 6s electron, resulting in a configuration of 4f\u00b9\u2074 5d\u00b9\u2070<\/code>. This again gives a fully filled d-subshell<\/strong>, contributing to gold\u2019s relative inertness and stability as Au\u207a. The configuration is also diamagnetic.<\/p>\n\n\n\n
Molybdenum (Z = 42) is a special case where electron configuration adjusts for stability: it adopts 5s\u00b9 4d\u2075<\/code> rather than 5s\u00b2 4d\u2074<\/code>. When it becomes Mo\u00b3\u207a, it loses one 5s electron and two 4d electrons, leaving 4d\u00b3<\/code>. According to Hund\u2019s rule, the three 4d electrons will occupy three separate orbitals with parallel spins to minimize electron repulsion, leading to paramagnetism<\/strong> due to three unpaired electrons.<\/p>\n\n\n\n
These diagrams help understand atomic properties like magnetism, chemical behavior, and ion stability.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
Enter the orbital diagram for the ion Cd2+Cd2+. Drag the appropriate labels to their respective targets. Labels can be used once, more than once, or not at all. Not all group 2 targets will be filled. Reset Help 1s Group 1 1s 4d Group 1 4d 2s Group 1 2s 4f Group 1 4f 2p […]<\/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-230881","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230881","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=230881"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230881\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=230881"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=230881"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=230881"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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<\/figure>\n","protected":false},"excerpt":{"rendered":"