{"id":170592,"date":"2024-11-19T21:36:08","date_gmt":"2024-11-19T21:36:08","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=170592"},"modified":"2024-11-19T21:36:10","modified_gmt":"2024-11-19T21:36:10","slug":"which-electron-configuration-violates-hunds-rule","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/19\/which-electron-configuration-violates-hunds-rule\/","title":{"rendered":"Which electron configuration violates Hund’s rule"},"content":{"rendered":"\n

Which electron configuration violates Hund’s rule?
A) [He]2s2 2px2 2py2 2pz1
B) [He]2s2 2px2 2py1 2pz2
C) [He]2s2 2px1 2py2 2pz2
D) [He]2s2 2px2 2py2
E) [He]2s2 2px1 2py1 2pz2<\/p>\n\n\n\n

The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n

The correct answer is B) [He]2s\u00b2 2px\u00b2 2py\u00b9 2pz\u00b2<\/strong>.<\/p>\n\n\n\n

Explanation:<\/h3>\n\n\n\n

Hund’s Rule<\/strong> states that when electrons occupy degenerate orbitals (orbitals with the same energy level, such as the three p orbitals: 2px, 2py, and 2pz), electrons will fill them singly<\/strong> before pairing up. Additionally, they will have parallel spins, meaning electrons in these degenerate orbitals will first occupy them in a way that maximizes the number of unpaired electrons.<\/p>\n\n\n\n

Let’s analyze each option:<\/p>\n\n\n\n

    \n
  1. Option A: [He]2s\u00b2 2px\u00b2 2py\u00b2 2pz\u00b9<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • Here, the electrons are distributed across the 2p orbitals: 2px and 2py each have 2 electrons, and 2pz has 1 electron.<\/li>\n\n\n\n
    • This configuration does not violate Hund’s Rule<\/strong>, as the electrons in the 2px and 2py orbitals are paired, and there is no conflict with unpaired electrons in the 2pz orbital.<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Option B: [He]2s\u00b2 2px\u00b2 2py\u00b9 2pz\u00b2<\/strong><\/li>\n<\/ol>\n\n\n\n
          \n
        • In this configuration, the 2px and 2pz orbitals are paired, but the 2py orbital has only one electron.<\/li>\n\n\n\n
        • This violates Hund’s Rule<\/strong> because according to Hund’s Rule, the electrons in the 2px, 2py, and 2pz orbitals should first occupy the orbitals singly before pairing up. In this case, the electron in 2py should have been placed into the 2pz orbital first to follow Hund’s Rule of maximizing unpaired electrons.<\/li>\n<\/ul>\n\n\n\n
            \n
          1. Option C: [He]2s\u00b2 2px\u00b9 2py\u00b2 2pz\u00b2<\/strong><\/li>\n<\/ol>\n\n\n\n
              \n
            • This configuration is valid according to Hund’s Rule. Electrons in the 2px, 2py, and 2pz orbitals are all placed singly in their respective orbitals first, before pairing occurs.<\/li>\n<\/ul>\n\n\n\n
                \n
              1. Option D: [He]2s\u00b2 2px\u00b2 2py\u00b2<\/strong><\/li>\n<\/ol>\n\n\n\n
                  \n
                • This configuration does not involve the 2pz orbital, so it does not violate Hund’s Rule. It simply shows the 2px and 2py orbitals fully paired.<\/li>\n<\/ul>\n\n\n\n
                    \n
                  1. Option E: [He]2s\u00b2 2px\u00b9 2py\u00b9 2pz\u00b2<\/strong><\/li>\n<\/ol>\n\n\n\n
                      \n
                    • Here, the electrons are distributed across the three p orbitals (2px, 2py, and 2pz), with each orbital having one electron. This adheres to Hund’s Rule because the electrons are occupying the orbitals singly and in parallel spins.<\/li>\n<\/ul>\n\n\n\n

                      Thus, Option B<\/strong> violates Hund’s Rule because it pairs electrons in the 2px and 2pz orbitals before filling all orbitals singly.<\/p>\n","protected":false},"excerpt":{"rendered":"

                      Which electron configuration violates Hund’s rule?A) [He]2s2 2px2 2py2 2pz1B) [He]2s2 2px2 2py1 2pz2C) [He]2s2 2px1 2py2 2pz2D) [He]2s2 2px2 2py2E) [He]2s2 2px1 2py1 2pz2 The Correct Answer and Explanation is : The correct answer is B) [He]2s\u00b2 2px\u00b2 2py\u00b9 2pz\u00b2. Explanation: Hund’s Rule states that when electrons occupy degenerate orbitals (orbitals with the same […]<\/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-170592","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/170592","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=170592"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/170592\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=170592"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=170592"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=170592"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}