Consider the molecule germanium tetrachloride, GeCl4 The electronegativity values for Ge and I are 1.8 and 3.0, respectively. Based on these values and on consideration of molecular geometry, the Ge bond is and the molecules Hint: Draw Lewis Dot Structure]<\/p>\n\n\n\n
a. Polar Covalent: Polar<\/p>\n\n\n\n
b. Polar Covalent: Non-Polar c<\/p>\n\n\n\n
c Non-Polar Covalent: Non-Polar<\/p>\n\n\n\n
d. Non-Polar Covalent, Polar<\/p>\n\n\n\n
e. None of the above<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n The correct answer is a. Polar Covalent: Polar.<\/strong><\/p>\n\n\n\n To determine the polarity of the bonds and the overall molecule, let’s break down the steps:<\/p>\n\n\n\n Thus, germanium tetrachloride has polar covalent bonds<\/strong> and is a polar molecule<\/strong>.<\/p>\n\n\n\n Consider the molecule germanium tetrachloride, GeCl4 The electronegativity values for Ge and I are 1.8 and 3.0, respectively. Based on these values and on consideration of molecular geometry, the Ge bond is and the molecules Hint: Draw Lewis Dot Structure] a. Polar Covalent: Polar b. Polar Covalent: Non-Polar c c Non-Polar Covalent: Non-Polar d. Non-Polar […]<\/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-191178","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191178","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=191178"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191178\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=191178"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=191178"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=191178"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Explanation:<\/h3>\n\n\n\n
\n
The electronegativity of germanium (Ge) is 1.8, and the electronegativity of chlorine (Cl) is 3.0. The difference in electronegativity between these two elements is: [
\\Delta \\chi = 3.0 – 1.8 = 1.2
] A difference of 1.2 is considered to indicate a polar covalent bond<\/strong>. In a polar covalent bond, electrons are shared unequally between the two atoms, with the more electronegative atom (chlorine in this case) pulling electron density towards itself, creating a dipole. Therefore, each Ge-Cl bond in GeCl4 is polar.<\/li>\n\n\n\n
The molecular geometry of germanium tetrachloride (GeCl4) is tetrahedral<\/strong>. Germanium (Ge) is the central atom surrounded by four chlorine atoms, and each bond is polar due to the electronegativity difference. However, because of the symmetrical tetrahedral arrangement<\/strong> of the molecule, the individual dipoles cancel out. This results in the overall molecule being polar<\/strong> despite the symmetry of the bonds.<\/li>\n\n\n\n
While the individual Ge-Cl bonds are polar, the molecule as a whole is polar<\/strong> due to the dipole moments of the bonds not cancelling out entirely. The electronegativity difference (1.2) and the molecular geometry lead to a net dipole in the direction of the chlorine atoms.<\/li>\n<\/ol>\n\n\n\nSummary:<\/h3>\n\n\n\n
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