{"id":228574,"date":"2025-06-07T11:59:55","date_gmt":"2025-06-07T11:59:55","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=228574"},"modified":"2025-06-07T11:59:57","modified_gmt":"2025-06-07T11:59:57","slug":"fill-in-the-orbital-energy-diagram-for-the-oxide-ion-2p-5-2s-1s","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/07\/fill-in-the-orbital-energy-diagram-for-the-oxide-ion-2p-5-2s-1s\/","title":{"rendered":"Fill in the orbital energy diagram for the oxide ion. 2p (5 2s 1s"},"content":{"rendered":"\n

Fill in the orbital energy diagram for the oxide ion. 2p (5 2s 1s<\/p>\n\n\n\n

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

\ud83e\uddea Correct Orbital Diagram for O\u00b2\u207b (Oxide Ion):<\/strong><\/h3>\n\n\n\n

Orbitals (in increasing energy):<\/p>\n\n\n\n

makefileCopyEdit1s: \u2191\u2193  \n2s: \u2191\u2193  \n2p: \u2191\u2193 \u2191\u2193 \u2191\u2193  \n<\/code><\/pre>\n\n\n\n
    \n
  • 1s orbital<\/strong> \u2192 2 electrons (\u2191\u2193)<\/li>\n\n\n\n
  • 2s orbital<\/strong> \u2192 2 electrons (\u2191\u2193)<\/li>\n\n\n\n
  • 2p orbitals<\/strong> \u2192 6 electrons (\u2191\u2193 \u2191\u2193 \u2191\u2193)<\/li>\n<\/ul>\n\n\n\n
    \u2705 Total electrons = 10<\/strong><\/p>\n\n\n\n
    \n\n\n\n
    \ud83d\udd0d Explanation<\/h3>\n\n\n\n
    The oxide ion (O\u00b2\u207b) is formed when a neutral oxygen atom gains two electrons. A neutral oxygen atom (O)<\/strong> has an atomic number of 8, meaning it has 8 electrons. When it gains two more electrons to form O\u00b2\u207b, it ends up with 10 electrons total<\/strong>, just like a neon (Ne)<\/strong> atom, making it isoelectronic<\/strong> with Ne.<\/p>\n\n\n\n
    Electrons fill orbitals in order of increasing energy<\/strong>, following the Aufbau principle<\/strong>, Pauli exclusion principle<\/strong>, and Hund\u2019s rule<\/strong>:<\/p>\n\n\n\n
      \n
    1. 1s orbital<\/strong> is the lowest in energy and holds 2 electrons<\/strong> (\u2191\u2193).<\/li>\n\n\n\n
    2. 2s orbital<\/strong> comes next and holds 2 electrons<\/strong> (\u2191\u2193).<\/li>\n\n\n\n
    3. 2p orbitals<\/strong> (px, py, pz) are degenerate (equal in energy). The remaining 6 electrons<\/strong> are placed in these:\n
        \n
      • According to Hund\u2019s Rule<\/strong>, each p orbital gets one electron before any gets paired.<\/li>\n\n\n\n
      • Then the electrons are paired up, completing the 2p subshell: \u2191\u2193 \u2191\u2193 \u2191\u2193<\/strong>.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n
        Thus, the electron configuration of the oxide ion is:<\/p>\n\n\n\n
        \ud83d\udc49 1s\u00b2 2s\u00b2 2p\u2076<\/strong><\/p>\n\n\n\n
        This completely fills the n = 2 shell<\/strong>, making O\u00b2\u207b a stable ion<\/strong> with a full valence shell, like the noble gas neon.<\/p>\n\n\n\n
        The orbital diagram represents this electron filling visually, with arrows indicating spin. The stability of O\u00b2\u207b comes from its full outer shell, explaining why oxygen tends to gain two electrons in chemical reactions.<\/p>\n\n\n\n
        \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"
        Fill in the orbital energy diagram for the oxide ion. 2p (5 2s 1s The Correct Answer and Explanation is: \ud83e\uddea Correct Orbital Diagram for O\u00b2\u207b (Oxide Ion): Orbitals (in increasing energy): makefileCopyEdit1s: \u2191\u2193 2s: \u2191\u2193 2p: \u2191\u2193 \u2191\u2193 \u2191\u2193 \u2705 Total electrons = 10 \ud83d\udd0d Explanation The oxide ion (O\u00b2\u207b) is formed when a […]<\/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-228574","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/228574","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=228574"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/228574\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=228574"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=228574"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=228574"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}