{"id":220760,"date":"2025-05-28T18:20:17","date_gmt":"2025-05-28T18:20:17","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=220760"},"modified":"2025-05-28T18:20:19","modified_gmt":"2025-05-28T18:20:19","slug":"show-units-and-working-out-please","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/28\/show-units-and-working-out-please\/","title":{"rendered":"show units and working out please"},"content":{"rendered":"\n

show units and working out please<\/p>\n\n\n\n

\n
    \n
  1. Draw the orbital energy diagram for Cobalt (Co) and circle the valence electrons in the diagram. Pay careful attention to the relative energies of your orbitals, and indicate each orbital using a line or box. Label each subshell, and complete the orbital diagram with the correct number of electrons.<\/li>\n<\/ol>\n<\/blockquote>\n\n\n\n

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

    1. Electron Configuration and Orbital Energy Diagram for Cobalt (Co)<\/strong><\/h3>\n\n\n\n

    Step 1: Determine the number of electrons in Co.<\/strong><\/p>\n\n\n\n

      \n
    • Atomic number of Co = 27<\/strong><\/li>\n\n\n\n
    • Therefore, Co has 27 electrons<\/strong><\/li>\n<\/ul>\n\n\n\n

      Step 2: Write the full electron configuration of Co:<\/strong>
      1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 4s\u00b2 3d\u2077<\/p>\n\n\n\n

        \n
      • Or in noble gas shorthand:
        [Ar] 4s\u00b2 3d\u2077<\/strong><\/li>\n<\/ul>\n\n\n\n

        Step 3: Draw the Orbital Energy Diagram<\/strong><\/p>\n\n\n\n

        Below is the orbital energy diagram with relative energies increasing from bottom to top<\/strong>.
        Each box or line represents one orbital (can hold 2 electrons max with opposite spins \u2191\u2193).<\/p>\n\n\n\n

        Energy \u2191\n\n       3d:  \u2191\u2193  \u2191\u2193  \u2191   \u2191   \u2191        (5 orbitals, 7 electrons)\n       4s:  \u2191\u2193                      (1 orbital, 2 electrons)\n       3p:  \u2191\u2193  \u2191\u2193  \u2191\u2193              (3 orbitals, 6 electrons)\n       3s:  \u2191\u2193                      (1 orbital, 2 electrons)\n       2p:  \u2191\u2193  \u2191\u2193  \u2191\u2193              (3 orbitals, 6 electrons)\n       2s:  \u2191\u2193                      (1 orbital, 2 electrons)\n       1s:  \u2191\u2193                      (1 orbital, 2 electrons)\n<\/code><\/pre>\n\n\n\n
        \ud83d\udc49 Valence electrons<\/strong> (circled in diagram):
        Cobalt is a transition metal<\/strong>, so the valence electrons are in the 4s and 3d orbitals<\/strong>.<\/p>\n\n\n\n
          \n
        • Valence electrons = 4s\u00b2 3d\u2077<\/strong> = 9 valence electrons<\/strong><\/li>\n<\/ul>\n\n\n\n
          \n\n\n\n
          \u2705 Explanation<\/strong><\/h3>\n\n\n\n
          Cobalt (Co), with atomic number 27, has 27 electrons in its neutral atomic state. To determine the orbital energy diagram, we follow the Aufbau principle<\/strong>, which dictates the order of orbital filling based on increasing energy. According to this rule, electrons fill lower-energy orbitals (like 1s) before higher ones (like 3d and 4s).<\/p>\n\n\n\n
          The electron configuration of cobalt is:
          1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 4s\u00b2 3d\u2077<\/strong>, or using noble gas notation: [Ar] 4s\u00b2 3d\u2077<\/strong>.<\/p>\n\n\n\n
          In orbital diagrams, each orbital is represented by a line or box. Each can hold two electrons with opposite spins (\u2191\u2193). We fill these orbitals following Hund\u2019s Rule<\/strong>, which states that electrons fill degenerate orbitals (orbitals of the same energy) singly before pairing up. This explains why the 3d subshell in Co is filled as \u2191\u2193 \u2191\u2193 \u2191 \u2191 \u2191 (total of 7 electrons across 5 orbitals).<\/p>\n\n\n\n
          Importantly, although the 4s orbital is filled before the 3d, the 3d orbitals are lower in energy once they contain electrons<\/strong>, so they are often drawn below or at similar energy to 4s in diagrams of transition metals.<\/p>\n\n\n\n
          Cobalt is a transition metal<\/strong>, meaning its valence electrons include not just those in the outermost s orbital (4s), but also in the partially filled d orbital (3d). So, Co has 9 valence electrons<\/strong>: two from 4s and seven from 3d.<\/p>\n\n\n\n
          These valence electrons are crucial in determining cobalt\u2019s chemical behavior, including bonding, oxidation states, and magnetic properties. For instance, Co commonly exhibits +2 and +3 oxidation states by losing electrons from these orbitals. Understanding its orbital diagram helps explain cobalt\u2019s role in catalysts, alloys, and biological systems like Vitamin B12.<\/p>\n\n\n\n
          \n\n\n\n
          \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
          show units and working out please The Correct Answer and Explanation is: 1. Electron Configuration and Orbital Energy Diagram for Cobalt (Co) Step 1: Determine the number of electrons in Co. Step 2: Write the full electron configuration of Co:1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 4s\u00b2 3d\u2077 Step 3: Draw the Orbital Energy Diagram Below is […]<\/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-220760","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/220760","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=220760"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/220760\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=220760"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=220760"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=220760"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}