{"id":224903,"date":"2025-06-03T15:24:51","date_gmt":"2025-06-03T15:24:51","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=224903"},"modified":"2025-06-03T15:24:53","modified_gmt":"2025-06-03T15:24:53","slug":"draw-the-lewis-structure-of-aso43-showing-all-lone-pairs-2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/03\/draw-the-lewis-structure-of-aso43-showing-all-lone-pairs-2\/","title":{"rendered":"Draw the Lewis structure of AsO4^3- showing all lone pairs"},"content":{"rendered":"\n
Draw the Lewis structure of AsO4^3- showing all lone pairs. Identify the molecular geometry of AsO4^3-. What is the hybridization of the central As atom? What are the approximate bond angles in AsO4^3-? Is AsO4^3- polar or nonpolar? Please answer all parts.<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
Answer:<\/strong><\/h3>\n\n\n\n
\n
Lewis Structure of AsO\u2084\u00b3\u207b<\/strong>: The central atom is As (arsenic)<\/strong>, surrounded by four O (oxygen)<\/strong> atoms. Each O forms a single bond with As. Each oxygen has 3 lone pairs<\/strong> of electrons. The overall ion has a \u20133 charge<\/strong>, typically distributed as one oxygen atom bearing the full \u20131 charge (with an extra lone pair), and the other three being neutral due to resonance.<\/li>\n\n\n\n
The Lewis structure of AsO\u2084\u00b3\u207b<\/strong> begins with arsenic (As) as the central atom, surrounded by four oxygen atoms. Arsenic has 5 valence electrons, and each oxygen has 6, totaling 29 valence electrons. Adding 3 electrons for the \u20133 charge gives 32 valence electrons.<\/p>\n\n\n\n
Each As\u2013O bond is a single bond, which uses 8 electrons (4 bonds \u00d7 2 electrons). The remaining 24 electrons are distributed as lone pairs around the oxygens. Each oxygen gets 6 electrons (3 lone pairs), satisfying their octets. This structure also accommodates the \u20133 charge, usually delocalized across the four oxygens due to resonance. In reality, this ion exhibits resonance<\/strong>, meaning the negative charge is shared among the oxygen atoms, making all As\u2013O bonds equivalent.<\/p>\n\n\n\n
The molecular geometry<\/strong> is tetrahedral<\/strong>, as there are four regions of electron density (four bonded oxygens) around the central arsenic atom and no lone pairs on As. According to VSEPR theory, this leads to a tetrahedral shape to minimize electron repulsion.<\/p>\n\n\n\n
The hybridization<\/strong> of arsenic in this tetrahedral structure is sp\u00b3<\/strong>, indicating that one s and three p orbitals mix to form four equivalent sp\u00b3 orbitals used to bond with the oxygens.<\/p>\n\n\n\n
The bond angles<\/strong> in a perfect tetrahedron are approximately 109.5\u00b0<\/strong>.<\/p>\n\n\n\n
Finally, although AsO\u2084\u00b3\u207b carries an overall charge, its molecular shape is symmetrical<\/strong>. The equal distribution of charge and geometry causes the dipole moments to cancel out, making the ion nonpolar overall<\/strong>, even though individual As\u2013O bonds are polar due to electronegativity differences.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
Draw the Lewis structure of AsO4^3- showing all lone pairs. Identify the molecular geometry of AsO4^3-. What is the hybridization of the central As atom? What are the approximate bond angles in AsO4^3-? Is AsO4^3- polar or nonpolar? Please answer all parts. The Correct Answer and Explanation is: Answer: Explanation The Lewis structure of AsO\u2084\u00b3\u207b […]<\/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-224903","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/224903","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=224903"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/224903\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=224903"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=224903"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=224903"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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