{"id":191216,"date":"2025-02-14T09:54:22","date_gmt":"2025-02-14T09:54:22","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=191216"},"modified":"2025-02-14T09:54:24","modified_gmt":"2025-02-14T09:54:24","slug":"forms-ionic-compound","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/14\/forms-ionic-compound\/","title":{"rendered":"Forms Ionic Compound"},"content":{"rendered":"\n

Forms Ionic Compound? Empirical Formula Of Ionic Compound Name Of Ionic Compound Fluorine Strontium Yes No Chlorine Rubidium Yes No Bromine Oxygen Yes No Potassium Fluorine Yes No<\/p>\n\n\n\n

\"\"<\/figure>\n\n\n\n

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

To determine whether these combinations form ionic compounds and their empirical formulas and names, let’s go over each case in detail:<\/p>\n\n\n\n

1. Fluorine + Strontium (SrF\u2082)<\/strong><\/h3>\n\n\n\n
    \n
  • Forms Ionic Compound:<\/strong> Yes<\/li>\n\n\n\n
  • Empirical Formula:<\/strong> SrF\u2082<\/li>\n\n\n\n
  • Name of Ionic Compound:<\/strong> Strontium fluoride<\/li>\n<\/ul>\n\n\n\n

    Explanation:<\/strong>
    Fluorine (F) is a halogen and readily accepts an electron to form the fluoride ion (F\u207b). Strontium (Sr) is an alkaline earth metal and typically forms a 2+ ion (Sr\u00b2\u207a). The compound forms when two fluoride ions bond with one strontium ion, resulting in SrF\u2082. This is a typical ionic compound with strong electrostatic attraction between the ions, and it is called strontium fluoride<\/strong>.<\/p>\n\n\n\n

    2. Chlorine + Rubidium (RbCl)<\/strong><\/h3>\n\n\n\n
      \n
    • Forms Ionic Compound:<\/strong> Yes<\/li>\n\n\n\n
    • Empirical Formula:<\/strong> RbCl<\/li>\n\n\n\n
    • Name of Ionic Compound:<\/strong> Rubidium chloride<\/li>\n<\/ul>\n\n\n\n

      Explanation:<\/strong>
      Rubidium (Rb) is an alkali metal that readily loses one electron to form Rb\u207a. Chlorine (Cl) is a halogen and accepts one electron to form Cl\u207b. The combination of these two ions forms the ionic compound rubidium chloride<\/strong>, with the formula RbCl. The compound is stable due to the electrostatic attraction between the positive rubidium ion and the negative chloride ion.<\/p>\n\n\n\n

      3. Bromine + Oxygen (O\u2082Br)<\/strong><\/h3>\n\n\n\n
        \n
      • Forms Ionic Compound:<\/strong> No<\/li>\n\n\n\n
      • Empirical Formula:<\/strong> Not valid<\/li>\n\n\n\n
      • Name of Ionic Compound:<\/strong> Not applicable<\/li>\n<\/ul>\n\n\n\n

        Explanation:<\/strong>
        Bromine (Br) and oxygen (O) do not typically form a stable ionic compound. While bromine can form bromide ions (Br\u207b), and oxygen forms oxide ions (O\u00b2\u207b), the combination of O\u2082Br (an odd stoichiometric ratio) doesn’t align with typical ionic bonding principles. Bromine and oxygen are more likely to form covalent compounds due to their electronegativity values.<\/p>\n\n\n\n

        4. Potassium + Fluorine (KF)<\/strong><\/h3>\n\n\n\n
          \n
        • Forms Ionic Compound:<\/strong> Yes<\/li>\n\n\n\n
        • Empirical Formula:<\/strong> KF<\/li>\n\n\n\n
        • Name of Ionic Compound:<\/strong> Potassium fluoride<\/li>\n<\/ul>\n\n\n\n

          Explanation:<\/strong>
          Potassium (K) is an alkali metal that loses one electron to form K\u207a. Fluorine (F), a halogen, accepts one electron to form F\u207b. When potassium and fluorine combine, they form potassium fluoride<\/strong> with the empirical formula KF. The electrostatic attraction between the K\u207a and F\u207b ions creates a stable ionic compound.<\/p>\n\n\n\n

          Summary:<\/h3>\n\n\n\n
            \n
          • SrF\u2082<\/strong> (Strontium fluoride), RbCl<\/strong> (Rubidium chloride), and KF<\/strong> (Potassium fluoride) all form ionic compounds.<\/li>\n\n\n\n
          • O\u2082Br<\/strong> does not form a typical ionic compound and is not stable under standard conditions.<\/li>\n<\/ul>\n\n\n\n

            These ionic compounds form due to the transfer of electrons between metals (like strontium, rubidium, and potassium) and nonmetals (like fluorine and chlorine), resulting in the formation of positive and negative ions that bond through strong electrostatic forces.<\/p>\n","protected":false},"excerpt":{"rendered":"

            Forms Ionic Compound? Empirical Formula Of Ionic Compound Name Of Ionic Compound Fluorine Strontium Yes No Chlorine Rubidium Yes No Bromine Oxygen Yes No Potassium Fluorine Yes No The Correct Answer and Explanation is : To determine whether these combinations form ionic compounds and their empirical formulas and names, let’s go over each case in […]<\/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-191216","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191216","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=191216"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191216\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=191216"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=191216"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=191216"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}