{"id":254466,"date":"2025-07-12T14:03:32","date_gmt":"2025-07-12T14:03:32","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=254466"},"modified":"2025-07-12T14:03:35","modified_gmt":"2025-07-12T14:03:35","slug":"draw-the-lewis-structure-for-sef5-showing-the-formal-charge-on-each-atom-mention-the-electron-and-molecular-geometry-bond-angles-and-polarity","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/12\/draw-the-lewis-structure-for-sef5-showing-the-formal-charge-on-each-atom-mention-the-electron-and-molecular-geometry-bond-angles-and-polarity\/","title":{"rendered":"Draw the lewis structure for [SeF5]-, showing the formal charge on each atom. mention the electron and molecular geometry, bond angles, and polarity"},"content":{"rendered":"\n
Draw the lewis structure for [SeF5]-, showing the formal charge on each atom. mention the electron and molecular geometry, bond angles, and polarity<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
Lewis Structure for [SeF5]\u207b:<\/h3>\n\n\n\n\n
Step 1: Count the valence electrons<\/strong>
Selenium (Se) is in group 16, so it has 6 valence electrons.<\/li>
Each fluorine (F) atom is in group 17, so it contributes 7 valence electrons.<\/li>
The negative charge (\u207b) means we add 1 extra electron.<\/li><\/ul>Total valence electrons:<\/strong>\n
\n
Se = 6<\/li>\n\n\n\n
5 F atoms = 5 * 7 = 35<\/li>\n\n\n\n
1 extra electron for the charge = 1<\/li>\n\n\n\n
Total = 6 + 35 + 1 = 42 electrons.<\/strong><\/li>\n<\/ul>\n<\/li>\n\n\n\n
Step 2: Draw the skeleton structure<\/strong>\n
\n
Place Se in the center and arrange the 5 F atoms around it. Each F atom forms a single bond with Se.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
Step 3: Distribute electrons<\/strong>\n
\n
Initially, 5 bonds use 10 electrons (2 electrons per bond).<\/li>\n\n\n\n
Distribute the remaining 32 electrons as lone pairs on the fluorine atoms. Each fluorine gets 6 electrons (3 lone pairs).<\/li>\n\n\n\n
After assigning the lone pairs to fluorines, we are left with no electrons for the selenium atom, so we put the remaining electrons on Se.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
Step 4: Check for octet rule<\/strong>\n
\n
Selenium can expand its octet because it is in period 4, so it can hold more than 8 electrons.<\/li>\n\n\n\n
The structure satisfies the octet for all fluorine atoms, and Se has 10 electrons in its valence shell.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
Formal charge = 7 – (6 + 2\/2) = 7 – 7 = 0<\/li><\/ul><\/li><\/ul>So, the formal charge on Se is +1, and each F atom has a formal charge of 0.<\/li>\n<\/ol>\n\n\n\n
Molecular Geometry:<\/h3>\n\n\n\n
\n
The molecular geometry of [SeF5]\u207b is trigonal bipyramidal<\/strong>.\n
\n
This is due to the 5 bonding pairs around the central Se atom.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
Electron Geometry:<\/h3>\n\n\n\n
\n
The electron geometry is also trigonal bipyramidal<\/strong>, as there are 5 bonding pairs and no lone pairs on Se.<\/li>\n<\/ul>\n\n\n\n
Bond Angles:<\/h3>\n\n\n\n
\n
In a trigonal bipyramidal structure, the bond angles are:\n
\n
90\u00b0 and 120\u00b0 between equatorial and axial positions.<\/li>\n\n\n\n
120\u00b0 between the equatorial positions.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
Polarity:<\/h3>\n\n\n\n
\n
Polarity<\/strong>: The molecule is polar<\/strong>. Although the individual F-Se bonds are polar, the geometry is asymmetrical (due to the presence of the negative charge), leading to an overall dipole moment.<\/li>\n<\/ul>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
Draw the lewis structure for [SeF5]-, showing the formal charge on each atom. mention the electron and molecular geometry, bond angles, and polarity The Correct Answer and Explanation is: Lewis Structure for [SeF5]\u207b: Molecular Geometry: Electron Geometry: Bond Angles: Polarity:<\/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-254466","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/254466","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=254466"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/254466\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=254466"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=254466"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=254466"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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<\/figure>\n","protected":false},"excerpt":{"rendered":"