{"id":195466,"date":"2025-02-28T09:35:15","date_gmt":"2025-02-28T09:35:15","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=195466"},"modified":"2025-02-28T09:35:17","modified_gmt":"2025-02-28T09:35:17","slug":"create-the-orbital-diagram-for-sodium","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/28\/create-the-orbital-diagram-for-sodium\/","title":{"rendered":"Create the orbital diagram for sodium"},"content":{"rendered":"\n

Create the orbital diagram for sodium.<\/p>\n\n\n\n

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

Orbital Diagram for Sodium (Na)<\/strong><\/h3>\n\n\n\n

Sodium ((Na)) has an atomic number of 11<\/strong>, meaning it has 11 electrons<\/strong>. These electrons are distributed in different energy levels and orbitals following the Aufbau principle<\/strong>, Pauli exclusion principle<\/strong>, and Hund\u2019s rule<\/strong>.<\/p>\n\n\n\n

\n\n\n\n

Step 1: Electron Configuration of Sodium<\/strong><\/h3>\n\n\n\n

The electron configuration of sodium is:
[
1s^2 2s^2 2p^6 3s^1
]
This tells us how electrons fill up orbitals in increasing energy order.<\/p>\n\n\n\n

    \n
  • 1s orbital<\/strong>: Can hold a maximum of 2 electrons<\/strong> \u2192 Filled<\/strong><\/li>\n\n\n\n
  • 2s orbital<\/strong>: Can hold a maximum of 2 electrons<\/strong> \u2192 Filled<\/strong><\/li>\n\n\n\n
  • 2p orbitals<\/strong>: Can hold a maximum of 6 electrons<\/strong> \u2192 Filled<\/strong><\/li>\n\n\n\n
  • 3s orbital<\/strong>: Has only 1 electron<\/strong> (valence electron)<\/li>\n<\/ul>\n\n\n\n
    \n\n\n\n

    Step 2: Orbital Diagram Representation<\/strong><\/h3>\n\n\n\n

    The orbital diagram visually represents electrons in orbitals using arrows<\/strong> (\u2191\u2193) to indicate electron spins.<\/p>\n\n\n\n

      \n
    1. 1s orbital (Lowest energy level)<\/strong> \u2192 Filled<\/strong>: \u2191\u2193<\/strong><\/li>\n\n\n\n
    2. 2s orbital<\/strong> \u2192 Filled<\/strong>: \u2191\u2193<\/strong><\/li>\n\n\n\n
    3. 2p orbitals<\/strong> \u2192 Each of the three p orbitals get one electron first, then the rest pair up<\/strong>: \u2191\u2193 \u2191\u2193 \u2191\u2193<\/strong><\/li>\n\n\n\n
    4. 3s orbital<\/strong> \u2192 One unpaired electron<\/strong>: \u2191<\/strong><\/li>\n<\/ol>\n\n\n\n

      Now, let’s generate the orbital diagram image.<\/p>\n\n\n\n

      \"\"<\/figure>\n\n\n\n

      Explanation of the Orbital Diagram<\/strong><\/h3>\n\n\n\n
        \n
      1. 1s Orbital<\/strong>: The first energy level contains one s-orbital<\/strong>, which is completely filled<\/strong> with two electrons (\u2191\u2193<\/strong>).<\/li>\n\n\n\n
      2. 2s Orbital<\/strong>: The second energy level starts with another s-orbital<\/strong>, which is also completely filled<\/strong> (\u2191\u2193<\/strong>).<\/li>\n\n\n\n
      3. 2p Orbitals<\/strong>: The second energy level also has three p-orbitals<\/strong>, and they are completely filled<\/strong> with six electrons (\u2191\u2193 \u2191\u2193 \u2191\u2193<\/strong>), following Hund\u2019s Rule<\/strong> (electrons occupy empty orbitals first before pairing up).<\/li>\n\n\n\n
      4. 3s Orbital<\/strong>: The third energy level starts with an s-orbital<\/strong>, but it contains only one electron<\/strong> (\u2191<\/strong>), which is the valence electron<\/strong> of sodium.<\/li>\n<\/ol>\n\n\n\n

        Key Takeaways<\/strong><\/h3>\n\n\n\n
          \n
        • Sodium has one unpaired electron in the 3s orbital<\/strong>, making it highly reactive<\/strong>.<\/li>\n\n\n\n
        • The valence electron (3s\u00b9)<\/strong> is responsible for sodium\u2019s chemical properties, especially its tendency to lose this electron to form a Na\u207a ion<\/strong>.<\/li>\n\n\n\n
        • The diagram follows the Aufbau principle<\/strong> (electrons fill lower energy orbitals first), Hund\u2019s rule<\/strong>, and the Pauli exclusion principle<\/strong>.<\/li>\n<\/ul>\n\n\n\n

          This orbital diagram clearly represents how sodium’s 11 electrons<\/strong> are arranged in different orbitals.<\/p>\n","protected":false},"excerpt":{"rendered":"

          Create the orbital diagram for sodium. The Correct Answer and Explanation is : Orbital Diagram for Sodium (Na) Sodium ((Na)) has an atomic number of 11, meaning it has 11 electrons. These electrons are distributed in different energy levels and orbitals following the Aufbau principle, Pauli exclusion principle, and Hund\u2019s rule. Step 1: Electron Configuration […]<\/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-195466","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/195466","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=195466"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/195466\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=195466"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=195466"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=195466"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}