{"id":226621,"date":"2025-06-05T12:07:54","date_gmt":"2025-06-05T12:07:54","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=226621"},"modified":"2025-06-05T12:07:56","modified_gmt":"2025-06-05T12:07:56","slug":"write-orbital-diagrams-for-each-ion-and-determine-if-the-ion-is-diamagnetic-or-paramagnetic","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/05\/write-orbital-diagrams-for-each-ion-and-determine-if-the-ion-is-diamagnetic-or-paramagnetic\/","title":{"rendered":"Write orbital diagrams for each ion and determine if the ion is diamagnetic or paramagnetic."},"content":{"rendered":"\n

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

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

Orbital Diagrams and Magnetic Properties of Ions<\/h3>\n\n\n\n
\n\n\n\n

a. Cd\u00b2\u207a (Cadmium ion)<\/strong><\/h4>\n\n\n\n
    \n
  • Atomic number:<\/strong> 48<\/li>\n\n\n\n
  • Neutral configuration:<\/strong> [Kr] 4d\u00b9\u2070 5s\u00b2<\/li>\n\n\n\n
  • Cd\u00b2\u207a configuration:<\/strong> [Kr] 4d\u00b9\u2070<\/li>\n<\/ul>\n\n\n\n

    Orbital Diagram:<\/strong><\/p>\n\n\n\n

    4d: \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 (10 electrons) \u2013 all paired\n<\/code><\/pre>\n\n\n\n
    Magnetism:<\/strong> Diamagnetic<\/strong>
    Cd\u00b2\u207a has all electrons paired in its 4d subshell, with no unpaired electrons.<\/p>\n\n\n\n
    \n\n\n\n
    b. Au\u207a (Gold(I) ion)<\/strong><\/h4>\n\n\n\n
      \n
    • Atomic number:<\/strong> 79<\/li>\n\n\n\n
    • Neutral configuration:<\/strong> [Xe] 4f\u00b9\u2074 5d\u00b9\u2070 6s\u00b9<\/li>\n\n\n\n
    • Au\u207a configuration:<\/strong> [Xe] 4f\u00b9\u2074 5d\u00b9\u2070<\/li>\n<\/ul>\n\n\n\n
      Orbital Diagram:<\/strong><\/p>\n\n\n\n
      5d: \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2191\u2193 (10 electrons) \u2013 all paired\n<\/code><\/pre>\n\n\n\n
      Magnetism:<\/strong> Diamagnetic<\/strong>
      Au\u207a has a completely filled 5d subshell, hence no unpaired electrons.<\/p>\n\n\n\n
      \n\n\n\n
      c. Mo\u00b3\u207a (Molybdenum(III) ion)<\/strong><\/h4>\n\n\n\n
        \n
      • Atomic number:<\/strong> 42<\/li>\n\n\n\n
      • Neutral configuration:<\/strong> [Kr] 4d\u2075 5s\u00b9<\/li>\n\n\n\n
      • Mo\u00b3\u207a configuration:<\/strong> [Kr] 4d\u00b3<\/li>\n<\/ul>\n\n\n\n
        Orbital Diagram:<\/strong><\/p>\n\n\n\n
        4d: \u2191 \u2191 \u2191 (3 electrons) \u2013 each in separate orbitals\n<\/code><\/pre>\n\n\n\n
        Magnetism:<\/strong> Paramagnetic<\/strong>
        Mo\u00b3\u207a has 3 unpaired electrons in the 4d orbitals, making it paramagnetic.<\/p>\n\n\n\n
        \n\n\n\n
        d. Zr\u00b2\u207a (Zirconium(II) ion)<\/strong><\/h4>\n\n\n\n
          \n
        • Atomic number:<\/strong> 40<\/li>\n\n\n\n
        • Neutral configuration:<\/strong> [Kr] 4d\u00b2 5s\u00b2<\/li>\n\n\n\n
        • Zr\u00b2\u207a configuration:<\/strong> [Kr] 4d\u00b2<\/li>\n<\/ul>\n\n\n\n
          Orbital Diagram:<\/strong><\/p>\n\n\n\n
          4d: \u2191 \u2191 (2 electrons) \u2013 in separate orbitals\n<\/code><\/pre>\n\n\n\n
          Magnetism:<\/strong> Paramagnetic<\/strong>
          Zr\u00b2\u207a has 2 unpaired electrons in the 4d orbitals, so it’s paramagnetic.<\/p>\n\n\n\n
          \n\n\n\n
          Summary and Explanation<\/h3>\n\n\n\n
          Magnetism in ions is determined by the presence of unpaired electrons in their electron configuration. Diamagnetic<\/strong> ions have all electrons paired and are repelled by a magnetic field, whereas paramagnetic<\/strong> ions have unpaired electrons and are attracted to magnetic fields.<\/p>\n\n\n\n
          In Cd\u00b2\u207a<\/strong>, removing two electrons from neutral cadmium removes both 5s electrons, leaving a full 4d\u00b9\u2070 configuration. Since all electrons are paired, it is diamagnetic.<\/p>\n\n\n\n
          Au\u207a<\/strong>, derived from gold, loses the single 6s electron, resulting in a full 5d\u00b9\u2070 shell. Like Cd\u00b2\u207a, this configuration is fully paired and thus diamagnetic.<\/p>\n\n\n\n
          Mo\u00b3\u207a<\/strong>, however, loses three electrons\u2014first from 5s and then from the 4d orbitals\u2014resulting in 4d\u00b3. These three electrons occupy separate orbitals due to Hund\u2019s rule, leading to three unpaired electrons. Thus, Mo\u00b3\u207a is paramagnetic.<\/p>\n\n\n\n
          Zr\u00b2\u207a<\/strong> loses its two 5s electrons, retaining two electrons in the 4d shell. Following Hund\u2019s rule, the electrons occupy separate orbitals, leading to two unpaired electrons, making Zr\u00b2\u207a paramagnetic.<\/p>\n\n\n\n
          This exercise emphasizes the importance of electron configurations, especially in transition metals, where d-orbital electron count dictates magnetic behavior. When determining the configuration of ions, always remove electrons from the outermost (highest n) orbitals first. Understanding how electrons occupy orbitals helps explain not only magnetism but also chemical reactivity and bonding tendencies.<\/p>\n\n\n\n
          \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
          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: Orbital Diagrams and Magnetic Properties of Ions a. Cd\u00b2\u207a (Cadmium ion) Orbital Diagram: Magnetism: DiamagneticCd\u00b2\u207a has all electrons paired in its 4d subshell, with no unpaired […]<\/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-226621","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/226621","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=226621"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/226621\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=226621"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=226621"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=226621"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}