{"id":214772,"date":"2025-05-15T11:23:34","date_gmt":"2025-05-15T11:23:34","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=214772"},"modified":"2025-05-15T11:23:36","modified_gmt":"2025-05-15T11:23:36","slug":"bond-polarity-in-a-covalent-bond-between-two-atoms-the-more-electronegative-atom-will-attract-more-electron-density-toward-itself-causing-a-polar-bond","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/15\/bond-polarity-in-a-covalent-bond-between-two-atoms-the-more-electronegative-atom-will-attract-more-electron-density-toward-itself-causing-a-polar-bond\/","title":{"rendered":"Bond Polarity In a covalent bond between two atoms, the more electronegative atom will attract more electron density toward itself, causing a polar bond."},"content":{"rendered":"\n<p class=\"wp-block-paragraph\">Bond Polarity In a covalent bond between two atoms, the more electronegative atom will attract more electron density toward itself, causing a polar bond. The more electronegative element is the negative pole, whereas the less electronegative element is the positive pole. The direction of the dipole is always toward the more electronegative element. This is often indicated by an arrow, as shown in the figure. (Figure 1) The magnitude of the bond polarity is the difference in electronegativity values of the atoms. For example, in the molecule Cl2, the Cl Cl bond is nonpolar because there is no difference in electronegativity between two atoms of the same element. In the ClBr molecule, however, the Cl-Br bond is polar because Cl and Br have different electronegativity values. A Cl-I bond would be more polar than a Cl-Br bond because there is a greater electronegativity difference between Cl and I than between Cl and Br Figure 1 of 1 Part A In the molecule BrI, which atom is the negative pole? O Br Sutbma Request Answer Part B Of the molecules SiCly and Sil4, which has bonds that are more polar? ? SiCl4 Sil Submit Request Answer<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Correct Answers:<\/strong><\/h3>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Part A:<\/strong><br>The <strong>Br<\/strong> atom is the <strong>negative pole<\/strong> in the Br\u2013I molecule.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Part B:<\/strong><br><strong>SiCl\u2084<\/strong> has bonds that are <strong>more polar<\/strong> than those in <strong>SiI\u2084<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Detailed Explanation (300+ words):<\/strong><\/h3>\n\n\n\n<p class=\"wp-block-paragraph\"><strong>Bond polarity<\/strong> refers to the unequal sharing of electrons between two atoms in a covalent bond due to a difference in <strong>electronegativity<\/strong>\u2014the tendency of an atom to attract electrons toward itself. The atom with the <strong>higher electronegativity<\/strong> attracts the shared electrons more strongly and becomes the <strong>negative pole<\/strong> (\u03b4\u207b), while the atom with lower electronegativity becomes the <strong>positive pole<\/strong> (\u03b4\u207a).<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Part A: Br\u2013I molecule<\/strong><\/h4>\n\n\n\n<p class=\"wp-block-paragraph\">In the diatomic molecule <strong>BrI<\/strong>, the bond is between <strong>bromine (Br)<\/strong> and <strong>iodine (I)<\/strong>.<br>The electronegativity values on the Pauling scale are approximately:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Br (bromine): 2.96<\/strong><\/li>\n\n\n\n<li><strong>I (iodine): 2.66<\/strong><\/li>\n<\/ul>\n\n\n\n<p class=\"wp-block-paragraph\">Since <strong>Br has a higher electronegativity<\/strong> than I, it pulls the shared electron pair closer to itself. As a result, Br becomes the <strong>negative pole (\u03b4\u207b)<\/strong>, and I becomes the <strong>positive pole (\u03b4\u207a)<\/strong>. Therefore, the <strong>direction of the dipole<\/strong> points <strong>toward Br<\/strong>.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Part B: Comparing SiCl\u2084 and SiI\u2084<\/strong><\/h4>\n\n\n\n<p class=\"wp-block-paragraph\">Both <strong>SiCl\u2084<\/strong> (silicon tetrachloride) and <strong>SiI\u2084<\/strong> (silicon tetraiodide) are tetrahedral molecules composed of silicon covalently bonded to four halogen atoms.<\/p>\n\n\n\n<p class=\"wp-block-paragraph\">Let\u2019s compare the <strong>electronegativity differences<\/strong> between silicon (Si) and the halogen atoms:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Si (silicon): 1.90<\/strong><\/li>\n\n\n\n<li><strong>Cl (chlorine): 3.16<\/strong><\/li>\n\n\n\n<li><strong>I (iodine): 2.66<\/strong><\/li>\n<\/ul>\n\n\n\n<p class=\"wp-block-paragraph\">Electronegativity difference:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Si\u2013Cl:<\/strong> 3.16 \u2212 1.90 = <strong>1.26<\/strong><\/li>\n\n\n\n<li><strong>Si\u2013I:<\/strong> 2.66 \u2212 1.90 = <strong>0.76<\/strong><\/li>\n<\/ul>\n\n\n\n<p class=\"wp-block-paragraph\">Since the <strong>Si\u2013Cl bond has a greater electronegativity difference<\/strong> than the Si\u2013I bond, the <strong>Si\u2013Cl bond is more polar<\/strong>. Therefore, the molecule <strong>SiCl\u2084 has more polar bonds<\/strong> than SiI\u2084.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Summary:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Br<\/strong> is the negative pole in <strong>BrI<\/strong> due to its higher electronegativity.<\/li>\n\n\n\n<li><strong>SiCl\u2084<\/strong> has more polar bonds than <strong>SiI\u2084<\/strong> because chlorine is more electronegative than iodine, resulting in a larger electronegativity difference.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Bond Polarity In a covalent bond between two atoms, the more electronegative atom will attract more electron density toward itself, causing a polar bond. The more electronegative element is the negative pole, whereas the less electronegative element is the positive pole. The direction of the dipole is always toward the more electronegative element. This is [&hellip;]<\/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-214772","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/214772","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=214772"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/214772\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=214772"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=214772"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=214772"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}