{"id":230899,"date":"2025-06-10T07:49:30","date_gmt":"2025-06-10T07:49:30","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=230899"},"modified":"2025-06-10T07:49:32","modified_gmt":"2025-06-10T07:49:32","slug":"write-the-electron-configuration-for-the-following-particles-s-v-cl-al3-fe3","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/10\/write-the-electron-configuration-for-the-following-particles-s-v-cl-al3-fe3\/","title":{"rendered":"Write the electron configuration for the following particles S V Cl Al3+ Fe3+"},"content":{"rendered":"\n

Write the electron configuration for the following particles S V Cl Al3+ Fe3+<\/p>\n\n\n\n

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

Electron Configurations:<\/strong><\/h3>\n\n\n\n
    \n
  1. Sulfur (S):<\/strong>
    Atomic number = 16
    Electron configuration:<\/strong>
    \u2192 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2074<\/strong><\/li>\n\n\n\n
  2. Vanadium (V):<\/strong>
    Atomic number = 23
    Electron configuration:<\/strong>
    \u2192 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 4s\u00b2 3d\u00b3<\/strong><\/li>\n\n\n\n
  3. Chlorine (Cl):<\/strong>
    Atomic number = 17
    Electron configuration:<\/strong>
    \u2192 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2075<\/strong><\/li>\n\n\n\n
  4. Aluminum ion (Al\u00b3\u207a):<\/strong>
    Atomic number = 13
    Neutral Al: 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u00b9
    Remove 3 electrons for Al\u00b3\u207a \u2192 Remove from 3p and 3s
    Electron configuration:<\/strong>
    \u2192 1s\u00b2 2s\u00b2 2p\u2076<\/strong><\/li>\n\n\n\n
  5. Iron ion (Fe\u00b3\u207a):<\/strong>
    Atomic number = 26
    Neutral Fe: 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 4s\u00b2 3d\u2076
    Remove 3 electrons \u2192 2 from 4s, 1 from 3d
    Electron configuration:<\/strong>
    \u2192 1s\u00b2 2s\u00b2 2p\u2076 3s\u00b2 3p\u2076 3d\u2075<\/strong><\/li>\n<\/ol>\n\n\n\n
    \n\n\n\n

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

    Electron configuration represents the distribution of electrons among atomic orbitals. It follows specific rules: Aufbau principle<\/strong> (fill lower energy orbitals first), Pauli exclusion principle<\/strong> (no two electrons in an atom can have the same set of four quantum numbers), and Hund\u2019s rule<\/strong> (maximize unpaired electrons in orbitals of the same energy).<\/p>\n\n\n\n

    For sulfur (S)<\/strong> with 16 electrons, electrons fill the 1s to 3p orbitals in order. The 3p sublevel holds 4 electrons, which aligns with its position in group 16 of the periodic table.<\/p>\n\n\n\n

    Vanadium (V)<\/strong> has 23 electrons. After the 4s orbital is filled, electrons begin filling the 3d orbitals. This explains why vanadium\u2019s configuration includes 3d\u00b3, consistent with its position among transition metals.<\/p>\n\n\n\n

    Chlorine (Cl)<\/strong>, with 17 electrons, fills up to the 3p sublevel. The 3p orbital holds 5 electrons, just one short of a full p-orbital (which holds 6), explaining chlorine\u2019s high reactivity\u2014it tends to gain one electron to achieve a full outer shell.<\/p>\n\n\n\n

    For Al\u00b3\u207a<\/strong>, we remove three electrons from aluminum\u2019s neutral state. Since electrons are lost from higher energy levels first, the two 3s electrons and the single 3p electron are removed, leaving a stable noble gas configuration (same as neon).<\/p>\n\n\n\n

    Fe\u00b3\u207a<\/strong> is more complex because it is a transition metal. Although 4s fills before 3d, electrons are lost from 4s first upon ionization. So, Fe\u00b3\u207a has lost 2 electrons from 4s and one from 3d, resulting in a 3d\u2075 configuration. This half-filled 3d sublevel is relatively stable and common among transition metal ions.<\/p>\n\n\n\n

    Understanding electron configurations is essential for predicting chemical reactivity, bonding behavior, and properties of elements and ions.<\/p>\n\n\n\n

    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

    Write the electron configuration for the following particles S V Cl Al3+ Fe3+ The Correct Answer and Explanation is: Electron Configurations: Explanation Electron configuration represents the distribution of electrons among atomic orbitals. It follows specific rules: Aufbau principle (fill lower energy orbitals first), Pauli exclusion principle (no two electrons in an atom can have the […]<\/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-230899","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230899","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=230899"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/230899\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=230899"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=230899"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=230899"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}