{"id":188544,"date":"2025-02-07T05:18:11","date_gmt":"2025-02-07T05:18:11","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=188544"},"modified":"2025-02-07T05:18:14","modified_gmt":"2025-02-07T05:18:14","slug":"fill-in-the-atomic-orbital-diagram-for-nitrogen","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/07\/fill-in-the-atomic-orbital-diagram-for-nitrogen\/","title":{"rendered":"Fill In The Atomic Orbital Diagram For Nitrogen"},"content":{"rendered":"\n

Fill In The Atomic Orbital Diagram For Nitrogen. <\/p>\n\n\n\n

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

Answer Bank Energy Construct The Orbital Diagram For Nickel. 1000 Answer Bank <\/p>\n\n\n\n

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

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

It seems I can’t access the images you provided directly. However, I can explain how to construct the atomic orbital diagrams for both nitrogen and nickel.<\/p>\n\n\n\n

Atomic Orbital Diagram for Nitrogen:<\/h3>\n\n\n\n

Nitrogen (atomic number 7) has an electron configuration of 1s\u00b2 2s\u00b2 2p\u00b3. We can draw the orbital diagram by following these steps:<\/p>\n\n\n\n

    \n
  1. 1s Orbital<\/strong>: The 1s orbital can hold up to two electrons, so it will have two arrows (representing electrons) pointing in opposite directions. These electrons are paired because they occupy the lowest energy level first.<\/li>\n\n\n\n
  2. 2s Orbital<\/strong>: The 2s orbital will also hold two electrons, and they will pair up similarly in the orbital.<\/li>\n\n\n\n
  3. 2p Orbitals<\/strong>: There are three 2p orbitals (2px, 2py, and 2pz), and nitrogen has three electrons in this subshell. According to Hund’s rule, each p orbital will receive one electron before any of them pairs up. This means there will be three unpaired electrons in the 2p orbitals, each with parallel spins.<\/li>\n<\/ol>\n\n\n\n

    The diagram should look like this:<\/p>\n\n\n\n

      \n
    • 1s\u00b2 (two electrons paired)<\/li>\n\n\n\n
    • 2s\u00b2 (two electrons paired)<\/li>\n\n\n\n
    • 2p\u00b3 (three unpaired electrons in the 2p orbitals)<\/li>\n<\/ul>\n\n\n\n

      Atomic Orbital Diagram for Nickel:<\/h3>\n\n\n\n

      Nickel (atomic number 28) has the electron configuration 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 3d\u2078 4s\u00b2. Here’s how to represent its orbital diagram:<\/p>\n\n\n\n

        \n
      1. 1s Orbital<\/strong>: Two electrons, paired.<\/li>\n\n\n\n
      2. 2s Orbital<\/strong>: Two electrons, paired.<\/li>\n\n\n\n
      3. 2p Orbitals<\/strong>: Six electrons, three pairs.<\/li>\n\n\n\n
      4. 3s Orbital<\/strong>: Two electrons, paired.<\/li>\n\n\n\n
      5. 3p Orbitals<\/strong>: Six electrons, three pairs.<\/li>\n\n\n\n
      6. 3d Orbitals<\/strong>: Nickel has eight electrons in the 3d subshell, so they will fill up the five 3d orbitals. However, they will fill in a manner such that no more than two electrons are in any one orbital, and some of them will have parallel spins before pairing (following Hund\u2019s rule).<\/li>\n\n\n\n
      7. 4s Orbital<\/strong>: Two electrons, paired.<\/li>\n<\/ol>\n\n\n\n

        So, the diagram for nickel will show filled orbitals with paired electrons in the 1s, 2s, 2p, 3s, and 3p subshells, and eight electrons in the 3d orbitals.<\/p>\n\n\n\n

        These diagrams reflect the arrangement of electrons in the atomic orbitals, which is crucial for understanding the chemical properties and reactivity of the elements.<\/p>\n","protected":false},"excerpt":{"rendered":"

        Fill In The Atomic Orbital Diagram For Nitrogen. Answer Bank Energy Construct The Orbital Diagram For Nickel. 1000 Answer Bank The Correct Answer and Explanation is : It seems I can’t access the images you provided directly. However, I can explain how to construct the atomic orbital diagrams for both nitrogen and nickel. Atomic Orbital […]<\/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-188544","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/188544","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=188544"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/188544\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=188544"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=188544"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=188544"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}