{"id":219333,"date":"2025-05-26T03:56:54","date_gmt":"2025-05-26T03:56:54","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=219333"},"modified":"2025-05-26T03:56:56","modified_gmt":"2025-05-26T03:56:56","slug":"arrange-these-ions-according-to-ionic-radius","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/26\/arrange-these-ions-according-to-ionic-radius\/","title":{"rendered":"Arrange these ions according to ionic radius."},"content":{"rendered":"\n

Arrange these ions according to ionic radius.<\/p>\n\n\n\n

Largest radius<\/p>\n\n\n\n

Smallest radius<\/p>\n\n\n\n

N\u00b3-
Mg\u00b2+
F-
Na+
O\u00b2-<\/p>\n\n\n\n

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

Correct Order of Ions by Ionic Radius (Largest to Smallest):<\/strong><\/h3>\n\n\n\n

Largest Radius \u2192 Smallest Radius:<\/strong>
N\u00b3\u207b > O\u00b2\u207b > F\u207b > Na\u207a > Mg\u00b2\u207a<\/strong><\/p>\n\n\n\n

\n\n\n\n

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

Ionic radius refers to the size of an ion. The size of an ion depends on two main factors:<\/p>\n\n\n\n

    \n
  1. The number of electrons relative to protons<\/strong>, and<\/li>\n\n\n\n
  2. The effective nuclear charge (Z_eff)<\/strong>\u2014the net positive charge experienced by an electron in a multi-electron atom.<\/li>\n<\/ol>\n\n\n\n

    Let\u2019s examine each ion:<\/p>\n\n\n\n

      \n
    • N\u00b3\u207b, O\u00b2\u207b, and F\u207b<\/strong> are all anions<\/strong> (negatively charged). They gain electrons<\/strong>, increasing electron-electron repulsion and expanding the electron cloud, making them larger than their neutral atoms.<\/li>\n\n\n\n
    • Na\u207a and Mg\u00b2\u207a<\/strong> are cations<\/strong> (positively charged). They lose electrons<\/strong>, reducing electron repulsion and allowing the nucleus to pull remaining electrons closer, thus decreasing the ionic radius.<\/li>\n<\/ul>\n\n\n\n

      All five ions are isoelectronic<\/strong>\u2014they all have the same number of electrons (10), but different nuclear charges (number of protons):<\/p>\n\n\n\n

      Ion<\/th>Nuclear Charge (Protons)<\/th>Ionic Charge<\/th>Relative Size<\/th><\/tr><\/thead>
      N\u00b3\u207b<\/td>7<\/td>-3<\/td>Largest<\/strong><\/td><\/tr>
      O\u00b2\u207b<\/td>8<\/td>-2<\/td>Larger<\/td><\/tr>
      F\u207b<\/td>9<\/td>-1<\/td>Large<\/td><\/tr>
      Na\u207a<\/td>11<\/td>+1<\/td>Small<\/td><\/tr>
      Mg\u00b2\u207a<\/td>12<\/td>+2<\/td>Smallest<\/strong><\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n

      Despite having the same number of electrons, N\u00b3\u207b<\/strong> has the fewest protons, so its nucleus exerts the weakest pull<\/strong> on its electrons, making its radius the largest<\/strong>. In contrast, Mg\u00b2\u207a<\/strong> has the most protons, pulling the same number of electrons in more tightly, resulting in the smallest radius<\/strong>.<\/p>\n\n\n\n

      Thus, as nuclear charge increases among isoelectronic species, ionic radius decreases<\/strong>.<\/p>\n\n\n\n

      This is why the order is:
      N\u00b3\u207b > O\u00b2\u207b > F\u207b > Na\u207a > Mg\u00b2\u207a<\/strong>.<\/p>\n\n\n\n

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

      Arrange these ions according to ionic radius. Largest radius Smallest radius N\u00b3-Mg\u00b2+F-Na+O\u00b2- The Correct Answer and Explanation is: Correct Order of Ions by Ionic Radius (Largest to Smallest): Largest Radius \u2192 Smallest Radius:N\u00b3\u207b > O\u00b2\u207b > F\u207b > Na\u207a > Mg\u00b2\u207a Explanation Ionic radius refers to the size of an ion. The size of an […]<\/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-219333","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/219333","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=219333"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/219333\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=219333"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=219333"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=219333"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}