To determine the number of d electrons in the valence shell of the Mo4+ cation, we need to follow these steps:<\/p>\n\n\n\n
Step 1: Determine the Electron Configuration of Mo<\/h3>\n\n\n\n
Molybdenum (Mo) has an atomic number of 42, meaning its neutral atom has 42 electrons. The electron configuration for a neutral Mo atom is:Mo:[Kr]\u20094d5\u20095s1\\text{Mo}: [Kr]\\, 4d^5\\, 5s^1Mo:[Kr]4d55s1<\/p>\n\n\n\n
This configuration shows that Mo has 5 electrons in the 4d orbital and 1 electron in the 5s orbital.<\/p>\n\n\n\n
Step 2: Determine the Electron Configuration of Mo4+<\/h3>\n\n\n\n
When Mo loses four electrons to form the Mo4+ cation, these electrons will first be removed from the outermost orbitals, which are the 5s and 4d orbitals.<\/p>\n\n\n\n
Thus, Mo4+ will have:Mo4+:[Kr]\u20094d2\\text{Mo}^{4+}: [Kr]\\, 4d^2Mo4+:[Kr]4d2<\/p>\n\n\n\n
This means that Mo4+ has 2 electrons<\/strong> in the 4d orbital.<\/p>\n\n\n\n The 4d subshell can hold up to 10 electrons, but in this case, Mo4+ has only 2 electrons in the 4d orbital. These two electrons will occupy different 4d orbitals to minimize electron-electron repulsion. Since each electron in the 4d orbitals will be unpaired, Mo4+ has 2 unpaired electrons<\/strong>.<\/p>\n\n\n\n This is because the electron configuration of Mo4+ has 2 electrons in the 4d orbitals, and each of these electrons is unpaired.<\/p>\n\n\n\n How many d electrons are in the valence shell of the Mo4+ cation? How many unpaired electron spins The Correct Answer and Explanation is: To determine the number of d electrons in the valence shell of the Mo4+ cation, we need to follow these steps: Step 1: Determine the Electron Configuration of Mo Molybdenum (Mo) […]<\/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-246087","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246087","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=246087"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246087\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246087"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246087"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246087"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Step 3: Determine the Number of Unpaired Electrons<\/h3>\n\n\n\n
Conclusion<\/h3>\n\n\n\n
\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-785.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"