{"id":184570,"date":"2025-01-21T07:17:10","date_gmt":"2025-01-21T07:17:10","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=184570"},"modified":"2025-01-21T07:17:12","modified_gmt":"2025-01-21T07:17:12","slug":"given-a-molecule-of-becl2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/21\/given-a-molecule-of-becl2\/","title":{"rendered":"Given a molecule of BeCl2"},"content":{"rendered":"\n

Given a molecule of BeCl2. Follow the steps below to determine if the molecule is polar or nonpolar. Step 1: The Be-Cl bonds ar ? Select ] polar nonpolar Step 2: The molecular geometry is (Select] Step 3: So the molecule is (Select) \u00ab Previni Given a molecule of BeCl2. Follow the steps below to determine if the molecule is polar or nonpolar. Step 1: The Be-Cl bonds are [Select] Step 2: The molecular geometry (Select ] linear bent Step 3: So the molecule is (Selec trigonal planar Given a molecule of BeCl2. Follow the steps below to determine if the molecule is polar or nonpolar. Step 1: The Be-Cl bonds are [Select] Step 2: The molecular geometry is (Select] Step 3: So the molecule Select ] polar nonpolar<\/p>\n\n\n\n

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

Answer:<\/h3>\n\n\n\n
    \n
  1. Step 1<\/strong>: The Be-Cl bonds are polar<\/strong>.<\/li>\n\n\n\n
  2. Step 2<\/strong>: The molecular geometry is linear<\/strong>.<\/li>\n\n\n\n
  3. Step 3<\/strong>: So the molecule is nonpolar<\/strong>.<\/li>\n<\/ol>\n\n\n\n
    \n\n\n\n

    Explanation:<\/h3>\n\n\n\n

    To determine whether BeCl\u2082 is polar or nonpolar, let’s analyze each step in detail.<\/p>\n\n\n\n

    Step 1: Are the Be-Cl bonds polar?<\/h4>\n\n\n\n

    The bond polarity depends on the difference in electronegativity between the bonded atoms. Beryllium (Be) has an electronegativity of 1.57, and chlorine (Cl) has an electronegativity of 3.16. The difference in electronegativity (3.16 – 1.57 = 1.59) indicates that the Be-Cl bond is polar. In a polar bond, electrons are unequally shared, creating partial charges (\u03b4\u207a on Be and \u03b4\u207b on Cl). Thus, each Be-Cl bond is polar.<\/p>\n\n\n\n

    \n\n\n\n

    Step 2: What is the molecular geometry of BeCl\u2082?<\/h4>\n\n\n\n

    The molecular geometry is determined by the number of bonding pairs and lone pairs around the central atom. In BeCl\u2082:<\/p>\n\n\n\n

      \n
    • Beryllium is the central atom, bonded to two chlorine atoms.<\/li>\n\n\n\n
    • Beryllium has only two valence electrons and forms two single bonds with chlorine atoms.<\/li>\n\n\n\n
    • There are no lone pairs on the central atom.<\/li>\n<\/ul>\n\n\n\n

      This leads to a linear geometry with a bond angle of 180\u00b0.<\/p>\n\n\n\n

      \n\n\n\n

      Step 3: Is the molecule polar or nonpolar?<\/h4>\n\n\n\n

      Even though the Be-Cl bonds are polar, the linear geometry ensures that the dipoles from the two Be-Cl bonds cancel each other out. This happens because the two chlorine atoms are symmetrically positioned, pulling the electron density in opposite directions with equal magnitude. As a result, there is no net dipole moment.<\/p>\n\n\n\n

      Thus, the molecule as a whole is nonpolar<\/strong> due to its symmetrical linear geometry.<\/p>\n\n\n\n

      Summary:<\/h3>\n\n\n\n
        \n
      • Be-Cl bonds are polar<\/strong> (unequal sharing of electrons).<\/li>\n\n\n\n
      • BeCl\u2082 molecule is linear<\/strong>, leading to dipole cancellation.<\/li>\n\n\n\n
      • BeCl\u2082 is a nonpolar molecule<\/strong>.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"

        Given a molecule of BeCl2. Follow the steps below to determine if the molecule is polar or nonpolar. Step 1: The Be-Cl bonds ar ? Select ] polar nonpolar Step 2: The molecular geometry is (Select] Step 3: So the molecule is (Select) \u00ab Previni Given a molecule of BeCl2. Follow the steps below to […]<\/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-184570","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184570","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=184570"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184570\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=184570"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=184570"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=184570"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}