Draw the correct Lewis structure of CCl4 and then use it to answer the questions below. a) How many bonding pairs of electrons are in the Lewis Structure? [ Select] b) How many lone pairs of electrons are present on the central atom in the Lewis structure? [ Select] c) What is the molecular geometry of CCIA? [Select ] d) Which best describes the CI-C-Cl bond angles in CCl4? [Select] e) Use electronegativity values and determine if the C-Cl bond is classified as covalent, polar covalent, or ionic. [Select ] f) Is the CCl4 molecule polar or nonpolar? [Select ] g) What is the correct name of the CCl4 molecule? (Select]<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n To draw the Lewis structure of carbon tetrachloride (( \\mathbf{CCl_4} )):<\/p>\n\n\n\n The Lewis structure of ( \\mathbf{CCl_4} ) shows a central carbon atom bonded to four chlorine atoms, with no lone pairs on carbon. Each chlorine has three lone pairs.<\/p>\n\n\n\n a) Bonding Pairs of Electrons<\/strong>: b) Lone Pairs on Central Atom<\/strong>: c) Molecular Geometry<\/strong>: d) Bond Angles<\/strong>: e) C-Cl Bond Type<\/strong>: f) Polarity of Molecule<\/strong>: g) Correct Name<\/strong>: The Lewis structure and VSEPR theory confirm that ( \\mathbf{CCl_4} ) has a tetrahedral molecular geometry with equal bond angles of 109.5\u00b0. While the C-Cl bonds are polar covalent due to the electronegativity difference, the molecule is nonpolar because the symmetry cancels the dipoles. Understanding the Lewis structure is essential for determining molecular geometry, bond angles, and polarity. Carbon tetrachloride is a stable compound often used in industrial applications, but its toxicity and environmental impact limit its use today.<\/p>\n","protected":false},"excerpt":{"rendered":" Draw the correct Lewis structure of CCl4 and then use it to answer the questions below. a) How many bonding pairs of electrons are in the Lewis Structure? [ Select] b) How many lone pairs of electrons are present on the central atom in the Lewis structure? [ Select] c) What is the molecular geometry […]<\/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-184386","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184386","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=184386"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/184386\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=184386"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=184386"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=184386"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}Lewis Structure of ( \\mathbf{CCl_4} ):<\/h3>\n\n\n\n
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\n\n\n\nAnswers to Questions:<\/h3>\n\n\n\n
There are 4 bonding pairs<\/strong> of electrons in ( \\mathbf{CCl_4} ).<\/p>\n\n\n\n
There are 0 lone pairs<\/strong> on the central carbon atom.<\/p>\n\n\n\n
The geometry is tetrahedral<\/strong> due to four electron regions around carbon.<\/p>\n\n\n\n
The bond angles are approximately 109.5\u00b0<\/strong>, characteristic of a tetrahedral shape.<\/p>\n\n\n\n
Using electronegativity values (C: 2.55, Cl: 3.16), the difference is 0.61. The bond is polar covalent<\/strong>.<\/p>\n\n\n\n
The molecule is nonpolar<\/strong> because the dipoles of the four polar C-Cl bonds cancel due to symmetry.<\/p>\n\n\n\n
The name of ( \\mathbf{CCl_4} ) is carbon tetrachloride<\/strong>.<\/p>\n\n\n\n
\n\n\n\nExplanation:<\/h3>\n\n\n\n