{"id":208349,"date":"2025-04-26T13:35:48","date_gmt":"2025-04-26T13:35:48","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=208349"},"modified":"2025-04-26T13:36:18","modified_gmt":"2025-04-26T13:36:18","slug":"write-the-orbital-diagram-for-titanium-and-write-the-electron-configuration","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/04\/26\/write-the-orbital-diagram-for-titanium-and-write-the-electron-configuration\/","title":{"rendered":"Orbital Diagram For Titanium"},"content":{"rendered":"\n

Write The Orbital Diagram For Titanium And Write The Electron Configuration.<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

Orbital Diagram for Titanium (Ti)<\/h3>\n\n\n\n

Titanium has an atomic number of 22, meaning it has 22 electrons. We will fill these electrons into orbitals based on the Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. The electron configuration of titanium and its orbital diagram are as follows:<\/p>\n\n\n\n

Electron Configuration<\/strong>:<\/h4>\n\n\n\n

[ \\text{Ti}: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^2 4s^2 ]<\/p>\n\n\n\n

This configuration tells us the distribution of electrons in titanium’s energy levels:<\/p>\n\n\n\n

    \n
  • 1s^2<\/strong>: 2 electrons in the 1s orbital<\/li>\n\n\n\n
  • 2s^2<\/strong>: 2 electrons in the 2s orbital<\/li>\n\n\n\n
  • 2p^6<\/strong>: 6 electrons in the 2p orbitals<\/li>\n\n\n\n
  • 3s^2<\/strong>: 2 electrons in the 3s orbital<\/li>\n\n\n\n
  • 3p^6<\/strong>: 6 electrons in the 3p orbitals<\/li>\n\n\n\n
  • 3d^2<\/strong>: 2 electrons in the 3d orbitals<\/li>\n\n\n\n
  • 4s^2<\/strong>: 2 electrons in the 4s orbital<\/li>\n<\/ul>\n\n\n\n

    Orbital Diagram<\/strong>:<\/h4>\n\n\n\n

    The orbital diagram for titanium is represented as:<\/p>\n\n\n\n

      \n
    • 1s<\/strong>: \u2191\u2193<\/li>\n\n\n\n
    • 2s<\/strong>: \u2191\u2193<\/li>\n\n\n\n
    • 2p<\/strong>: \u2191\u2193 \u2191\u2193 \u2191\u2193<\/li>\n\n\n\n
    • 3s<\/strong>: \u2191\u2193<\/li>\n\n\n\n
    • 3p<\/strong>: \u2191\u2193 \u2191\u2193 \u2191\u2193<\/li>\n\n\n\n
    • 3d<\/strong>: \u2191\u2193 \u2191<\/li>\n\n\n\n
    • 4s<\/strong>: \u2191\u2193<\/li>\n<\/ul>\n\n\n\n

      In the orbital diagram:<\/p>\n\n\n\n

        \n
      • Each arrow represents an electron, with an up arrow indicating one electron and a down arrow indicating the second electron in a pair.<\/li>\n\n\n\n
      • The orbitals are filled in order of increasing energy, with 4s<\/strong> being filled before 3d<\/strong>.<\/li>\n<\/ul>\n\n\n\n

        Explanation<\/h3>\n\n\n\n

        Titanium\u2019s atomic number is 22, so it has 22 electrons. These electrons are arranged in orbitals of increasing energy: the 1s<\/strong>, 2s<\/strong>, 2p<\/strong>, 3s<\/strong>, 3p<\/strong>, 3d<\/strong>, and 4s<\/strong> orbitals. According to the Aufbau principle<\/strong>, electrons fill lower-energy orbitals first. The Pauli exclusion principle<\/strong> states that each orbital can hold a maximum of two electrons, which must have opposite spins. Hund’s rule<\/strong> states that electrons will occupy degenerate orbitals (orbitals of the same energy) singly before pairing up.<\/p>\n\n\n\n

          \n
        • The 1s<\/strong>, 2s<\/strong>, and 2p<\/strong> orbitals are fully filled with 2, 2, and 6 electrons, respectively.<\/li>\n\n\n\n
        • The 3s<\/strong> and 3p<\/strong> orbitals are also fully occupied with 2 and 6 electrons, respectively.<\/li>\n\n\n\n
        • The 3d<\/strong> orbital, which is at a slightly higher energy level, holds 2 electrons.<\/li>\n\n\n\n
        • Finally, the 4s<\/strong> orbital holds 2 electrons, even though it\u2019s higher in energy than 3d<\/strong>, due to its relative closeness to the 3d<\/strong> orbital in energy.<\/li>\n<\/ul>\n\n\n\n

          Thus, titanium’s electron configuration is stable with two electrons in the 4s orbital and two electrons in the 3d orbital.<\/p>\n","protected":false},"excerpt":{"rendered":"

          Write The Orbital Diagram For Titanium And Write The Electron Configuration. The correct answer and explanation is : Orbital Diagram for Titanium (Ti) Titanium has an atomic number of 22, meaning it has 22 electrons. We will fill these electrons into orbitals based on the Aufbau principle, Hund’s rule, and Pauli’s exclusion principle. The electron […]<\/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-208349","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/208349","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=208349"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/208349\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=208349"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=208349"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=208349"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}