{"id":229280,"date":"2025-06-08T05:07:50","date_gmt":"2025-06-08T05:07:50","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=229280"},"modified":"2025-06-08T05:07:52","modified_gmt":"2025-06-08T05:07:52","slug":"give-the-electron-configurations-for-the-following-ions-p5-p3-sn4-se2-i-and-ni2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/08\/give-the-electron-configurations-for-the-following-ions-p5-p3-sn4-se2-i-and-ni2\/","title":{"rendered":"Give the electron configurations for the following ions: P5+, P3+, Sn4+, Se2+, I+, and Ni2+."},"content":{"rendered":"\n

Give the electron configurations for the following ions: P5+, P3+, Sn4+, Se2+, I+, and Ni2+.<\/p>\n\n\n\n

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

Electron Configurations of Ions<\/strong><\/h3>\n\n\n\n
    \n
  1. P\u2075\u207a (Phosphorus 5+)<\/strong>: [Ne]<\/li>\n\n\n\n
  2. P\u00b3\u207a (Phosphorus 3+)<\/strong>: [Ne] 3s\u00b2<\/li>\n\n\n\n
  3. Sn\u2074\u207a (Tin 4+)<\/strong>: [Kr] 4d\u00b9\u2070<\/li>\n\n\n\n
  4. Se\u00b2\u207a (Selenium 2+)<\/strong>: [Ar] 3d\u00b9\u2070 4s\u00b2 4p\u00b2<\/li>\n\n\n\n
  5. I\u207a (Iodine 1+)<\/strong>: [Kr] 4d\u00b9\u2070 5s\u00b2 5p\u2074<\/li>\n\n\n\n
  6. Ni\u00b2\u207a (Nickel 2+)<\/strong>: [Ar] 3d\u2078<\/li>\n<\/ol>\n\n\n\n
    \n\n\n\n

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

    Electron configuration refers to the arrangement of electrons in an atom or ion. When atoms become ions, they either lose or gain electrons to achieve greater stability, typically aiming for a noble gas configuration. The configurations of cations<\/strong> (positive ions) are formed by removing electrons<\/strong> from the outermost shells, while anions<\/strong> (negative ions) are formed by adding electrons<\/strong> to the outer orbitals.<\/p>\n\n\n\n

      \n
    1. Phosphorus (P)<\/strong> has an atomic number of 15: [Ne] 3s\u00b2 3p\u00b3.\n
        \n
      • In P\u2075\u207a<\/strong>, it loses all 5 valence electrons (3s\u00b2 3p\u00b3), leaving just the [Ne] core.<\/li>\n\n\n\n
      • In P\u00b3\u207a<\/strong>, it loses three electrons (3p\u00b3), leaving the configuration [Ne] 3s\u00b2.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Tin (Sn)<\/strong> has an atomic number of 50: [Kr] 5s\u00b2 4d\u00b9\u2070 5p\u00b2.\n
          \n
        • In Sn\u2074\u207a<\/strong>, it loses all four valence electrons (5s\u00b2 5p\u00b2), resulting in [Kr] 4d\u00b9\u2070.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • Selenium (Se)<\/strong> has atomic number 34: [Ar] 4s\u00b2 3d\u00b9\u2070 4p\u2074.\n
            \n
          • In Se\u00b2\u207a<\/strong>, it loses two 4p electrons, giving [Ar] 3d\u00b9\u2070 4s\u00b2 4p\u00b2.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
          • Iodine (I)<\/strong> has atomic number 53: [Kr] 5s\u00b2 4d\u00b9\u2070 5p\u2075.\n
              \n
            • In I\u207a<\/strong>, one electron is removed from the 5p orbital, yielding [Kr] 4d\u00b9\u2070 5s\u00b2 5p\u2074.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
            • Nickel (Ni)<\/strong> has atomic number 28: [Ar] 4s\u00b2 3d\u2078.\n
                \n
              • In Ni\u00b2\u207a<\/strong>, two electrons are lost\u2014typically from the 4s orbital first, resulting in [Ar] 3d\u2078.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

                Note: Transition metals (like Ni and Sn) often lose s-electrons before d-electrons. Electron configuration helps in predicting chemical reactivity, bonding behavior, and magnetic properties of ions.<\/p>\n\n\n\n

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

                Give the electron configurations for the following ions: P5+, P3+, Sn4+, Se2+, I+, and Ni2+. The Correct Answer and Explanation is: Electron Configurations of Ions Explanation Electron configuration refers to the arrangement of electrons in an atom or ion. When atoms become ions, they either lose or gain electrons to achieve greater stability, typically aiming […]<\/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-229280","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/229280","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=229280"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/229280\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=229280"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=229280"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=229280"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}