{"id":233419,"date":"2025-06-13T06:12:11","date_gmt":"2025-06-13T06:12:11","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=233419"},"modified":"2025-06-13T06:12:13","modified_gmt":"2025-06-13T06:12:13","slug":"use-the-gizmo-to-create-stable-compounds-from-the-combinations-given-below-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/13\/use-the-gizmo-to-create-stable-compounds-from-the-combinations-given-below-2\/","title":{"rendered":"Use the Gizmo to create stable compounds from the combinations given below."},"content":{"rendered":"\n

Use the Gizmo to create stable compounds from the combinations given below. After transferring electrons, arrange the atoms to demonstrate the attraction between positively charged ions and negatively charged ions. Click “Check” to check each compound: Ionic charges Chemical formula Lithium and fluorine Beryllium and oxygen: BeO Magnesium and fluorine: MgF2 Aluminum and chlorine: AlCl3 Beryllium and nitrogen: Be3N2<\/p>\n\n\n\n

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

To complete this activity using the Ionic Bonds Gizmo<\/strong>, you are expected to form stable ionic compounds<\/strong> by transferring electrons from metals<\/strong> (which lose electrons and become positively charged cations) to nonmetals<\/strong> (which gain electrons and become negatively charged anions). Here’s how each combination works, followed by a full explanation:<\/p>\n\n\n\n

\n\n\n\n

Correct Ionic Charges and Chemical Formulas:<\/strong><\/h3>\n\n\n\n
    \n
  1. Lithium and Fluorine<\/strong>\n
      \n
    • Ionic charges:<\/strong> Li\u207a and F\u207b<\/li>\n\n\n\n
    • Chemical formula:<\/strong> LiF<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Beryllium and Oxygen<\/strong>\n
        \n
      • Ionic charges:<\/strong> Be\u00b2\u207a and O\u00b2\u207b<\/li>\n\n\n\n
      • Chemical formula:<\/strong> BeO<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n
      • Magnesium and Fluorine<\/strong>\n
          \n
        • Ionic charges:<\/strong> Mg\u00b2\u207a and F\u207b<\/li>\n\n\n\n
        • Chemical formula:<\/strong> MgF\u2082<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • Aluminum and Chlorine<\/strong>\n
            \n
          • Ionic charges:<\/strong> Al\u00b3\u207a and Cl\u207b<\/li>\n\n\n\n
          • Chemical formula:<\/strong> AlCl\u2083<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n
          • Beryllium and Nitrogen<\/strong>\n
              \n
            • Ionic charges:<\/strong> Be\u00b2\u207a and N\u00b3\u207b<\/li>\n\n\n\n
            • Chemical formula:<\/strong> Be\u2083N\u2082<\/strong><\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n
              \n\n\n\n

              Textbook-Style Explanation<\/strong><\/h3>\n\n\n\n

              In ionic bonding, atoms transfer electrons to achieve full outer electron shells, similar to noble gases. Metals like lithium (Li), beryllium (Be), magnesium (Mg), and aluminum (Al) are located on the left side of the periodic table and readily lose electrons<\/strong>, forming positively charged cations<\/strong>. Nonmetals such as fluorine (F), oxygen (O), chlorine (Cl), and nitrogen (N) are found on the right side and gain electrons<\/strong>, forming negatively charged anions<\/strong>.<\/p>\n\n\n\n

              Each ionic bond forms when the total positive and negative charges balance<\/strong>, creating a neutral compound<\/strong>.<\/p>\n\n\n\n

                \n
              1. LiF:<\/strong> Lithium loses 1 electron (Li\u207a), fluorine gains 1 (F\u207b), so only one of each ion is needed.<\/li>\n\n\n\n
              2. BeO:<\/strong> Beryllium gives up 2 electrons (Be\u00b2\u207a) and oxygen takes in 2 (O\u00b2\u207b), forming a 1:1 ratio.<\/li>\n\n\n\n
              3. MgF\u2082:<\/strong> Magnesium loses 2 electrons (Mg\u00b2\u207a), and each fluorine can only accept 1 (F\u207b), so two fluorine atoms<\/strong> are required.<\/li>\n\n\n\n
              4. AlCl\u2083:<\/strong> Aluminum forms a 3+ ion (Al\u00b3\u207a), and each chlorine is 1\u2212 (Cl\u207b). To balance the charges, three chlorines<\/strong> are needed.<\/li>\n\n\n\n
              5. Be\u2083N\u2082:<\/strong> Each beryllium is 2+ (Be\u00b2\u207a), and nitrogen is 3\u2212 (N\u00b3\u207b). The lowest common multiple of 2 and 3 is 6, so three Be\u00b2\u207a (total +6) and two N\u00b3\u207b (total -6) balance to form Be\u2083N\u2082<\/strong>.<\/li>\n<\/ol>\n\n\n\n

                After forming ions, the electrostatic attraction<\/strong> between opposite charges holds the ions tightly in place, forming a crystal lattice<\/strong>. This structure is what gives ionic compounds their high melting points, brittleness, and ability to dissolve in water to conduct electricity.<\/p>\n\n\n\n

                By using the Gizmo, you visually model this process\u2014transferring electrons and then arranging ions based on their charges.<\/p>\n\n\n\n

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

                Use the Gizmo to create stable compounds from the combinations given below. After transferring electrons, arrange the atoms to demonstrate the attraction between positively charged ions and negatively charged ions. Click “Check” to check each compound: Ionic charges Chemical formula Lithium and fluorine Beryllium and oxygen: BeO Magnesium and fluorine: MgF2 Aluminum and chlorine: AlCl3 […]<\/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-233419","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233419","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=233419"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233419\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=233419"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=233419"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=233419"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}