{"id":223357,"date":"2025-06-01T13:36:03","date_gmt":"2025-06-01T13:36:03","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=223357"},"modified":"2025-06-01T13:36:05","modified_gmt":"2025-06-01T13:36:05","slug":"for-the-ion-if4-draw-its-lewis-structure-and-then-answer-the-following-questions-base-on-that-structure","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/01\/for-the-ion-if4-draw-its-lewis-structure-and-then-answer-the-following-questions-base-on-that-structure\/","title":{"rendered":"For the ion IF4+, draw its Lewis Structure and then answer the following questions base on that structure"},"content":{"rendered":"\n
For the ion IF4+, draw its Lewis Structure and then answer the following questions base on that structure. (The central atom in each case is the atom with the lowest electronegativity). How many valence electrons are in the ion? (Remember to add an electron for each negative charge or to subtract one for each positive charge). How many lone pairs of electrons are in the central atom of the ion? What is the electron pair geometry of the ion? What is (are) the bond angle(s) at the central atom of the ion IF4+? Would the ion’s structure be polar, nonpolar, or ionic? For the ion IF4+, draw its Lewis Structure and then answer the following questions base on that structure. (The central atom in each case is the atom with the lowest electronegativity). How many valence electrons are in the ion? (Remember to add an electron for each negative charge or to subtract one for each positive charge). How many lone pairs of electrons are in the central atom of the ion? What is the electron pair geometry of the ion? What is (are) the bond angle(s) at the central atom of the ion IF4+? Would the ion’s structure be polar, nonpolar, or ionic?<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
Ion: IF\u2084\u207a \u2013 Analysis and Lewis Structure<\/strong><\/h3>\n\n\n\n
1. Total Valence Electrons<\/strong><\/h4>\n\n\n\n
\n
Iodine (I) has 7 valence electrons.<\/li>\n\n\n\n
Each fluorine (F) has 7 valence electrons \u00d7 4 = 28 electrons.<\/li>\n\n\n\n
The ion has a +1 charge<\/strong>, so we subtract 1 electron<\/strong>.<\/li>\n\n\n\n
Due to lone pair repulsion, angles are slightly less than 90\u00b0 and 120\u00b0<\/strong><\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n
7. Polarity<\/strong><\/h4>\n\n\n\n
\n
The ion is polar<\/strong> because the lone pair causes asymmetry<\/strong> in electron distribution, making the dipoles not cancel.<\/li>\n<\/ul>\n\n\n\n
8. Ionic or Covalent?<\/strong><\/h4>\n\n\n\n
\n
While IF\u2084\u207a is an ion, the bonds are covalent<\/strong>, not ionic, because electrons are shared between iodine and fluorine.<\/li>\n<\/ul>\n\n\n\n\n\n\n\n
Summary<\/strong><\/h3>\n\n\n\n
\n
Valence electrons<\/strong>: 34<\/li>\n\n\n\n
Lone pairs on central atom<\/strong>: 1<\/li>\n\n\n\n
Electron pair geometry<\/strong>: Trigonal bipyramidal<\/li>\n\n\n\n
Bond angles<\/strong>: <90\u00b0 and <120\u00b0<\/li>\n\n\n\n
This detailed analysis reflects how electron configuration governs molecular shape, bond angles, and polarity.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
For the ion IF4+, draw its Lewis Structure and then answer the following questions base on that structure. (The central atom in each case is the atom with the lowest electronegativity). How many valence electrons are in the ion? (Remember to add an electron for each negative charge or to subtract one for each positive […]<\/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-223357","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/223357","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=223357"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/223357\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=223357"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=223357"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=223357"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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<\/figure>\n","protected":false},"excerpt":{"rendered":"