{"id":185063,"date":"2025-01-22T05:13:47","date_gmt":"2025-01-22T05:13:47","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=185063"},"modified":"2025-01-22T05:13:49","modified_gmt":"2025-01-22T05:13:49","slug":"how-many-lone-pairs-of-electrons-are-on-the-s-atom-in-sf4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/22\/how-many-lone-pairs-of-electrons-are-on-the-s-atom-in-sf4\/","title":{"rendered":"How many lone pairs of electrons are on the S atom in SF4"},"content":{"rendered":"\n<p>11) How many lone pairs of electrons are on the S atom in SF4 ?<\/p>\n\n\n\n<p>A) 0<\/p>\n\n\n\n<p>B) 1<\/p>\n\n\n\n<p>C) 2<\/p>\n\n\n\n<p>D) 3<\/p>\n\n\n\n<p>12) How many lone pairs are on the Br atom in BrCl2-?<\/p>\n\n\n\n<p>A) 0<\/p>\n\n\n\n<p>B) 1<\/p>\n\n\n\n<p>C) 2<\/p>\n\n\n\n<p>D) 3<\/p>\n\n\n\n<p>13) In the best Lewis structure for NO +, what is the formal charge on the N atom?<\/p>\n\n\n\n<p>A) -1<\/p>\n\n\n\n<p>B) 0<\/p>\n\n\n\n<p>C) +1<\/p>\n\n\n\n<p>D) +2<\/p>\n\n\n\n<p>4.3&nbsp;&nbsp; Short Answer Questions<\/p>\n\n\n\n<p>1) Among the compounds H3C\u2013CH3, H2C=CH2, and HC<img loading=\"lazy\" decoding=\"async\" src=\"blob:https:\/\/learnexams.com\/39fc1f40-0712-4d00-95d5-33596d24c956\" width=\"10\" height=\"17\" alt=\"\">CH, the compound with the strongest carbon-carbon bond is ________, and the compound with the longest carbon-carbon bond is ________.<\/p>\n\n\n\n<p>2) Ionic compounds consist of a single three-dimensional network of ions that are attracted to one another by strong ________ and usually exist in the solid state at room temperature, whereas covalent compounds consist of molecules that are attracted to one another by weak ________ and can exist in gaseous, liquid, or solid state at room temperature.<\/p>\n\n\n\n<p>3) Of the bonds C\u2013C, C\u2013N, C\u2013O, and C\u2013F, the bond that is most polar is ________.<\/p>\n\n\n\n<p>4) The Lewis electron-dot structure of N2 has ________ nonbonding electrons pairs, ________ bonding electron pairs, and a bond order of ________.<\/p>\n\n\n\n<p>5) The Lewis electron-dot structure of H2CO has ________ nonbonding electron pairs, ________ bonding electron pairs, and a carbon-oxygen bond order of ________.<\/p>\n\n\n\n<p>6) The number of Lewis electron dot resonance structures required to describe NO2\u2013 is ________.<\/p>\n\n\n\n<p>7) Based on formal charges, the best Lewis electron-dot structure of BF3 has a B\u2013F bond order = ________.<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Answers and Explanations:<\/strong><\/h3>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>11) How many lone pairs of electrons are on the S atom in SF\u2084?<\/strong><\/h3>\n\n\n\n<p><strong>Answer: B) 1<\/strong><\/p>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Sulfur (S) in SF\u2084 has 6 valence electrons.<\/li>\n\n\n\n<li>Each fluorine atom forms a single bond with sulfur, using 4 electrons.<\/li>\n\n\n\n<li>The remaining 2 electrons form a lone pair on sulfur.<\/li>\n\n\n\n<li>SF\u2084 adopts a seesaw geometry due to this lone pair.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>12) How many lone pairs are on the Br atom in BrCl\u2082\u207b?<\/strong><\/h3>\n\n\n\n<p><strong>Answer: D) 3<\/strong><\/p>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Bromine (Br) has 7 valence electrons. In BrCl\u2082\u207b:<\/li>\n\n\n\n<li>Each chlorine atom forms a single bond with Br, using 2 electrons total.<\/li>\n\n\n\n<li>The extra negative charge adds 1 electron.<\/li>\n\n\n\n<li>This leaves 6 electrons, or 3 lone pairs, on the Br atom.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>13) In the best Lewis structure for NO\u207a, what is the formal charge on the N atom?<\/strong><\/h3>\n\n\n\n<p><strong>Answer: C) +1<\/strong><\/p>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The nitrogen-oxygen (NO\u207a) molecule has 10 total valence electrons (N: 5, O: 6, and -1 due to the positive charge).<\/li>\n\n\n\n<li>A triple bond forms between N and O, with one lone pair on O.<\/li>\n\n\n\n<li>Formal charge on N = (5 valence electrons) &#8211; (2 nonbonding + 3 bonding pairs) = +1.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>4.3 Short Answer Questions<\/strong><\/h3>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>1) The compound with the strongest carbon-carbon bond is HC\u2261CH, and the compound with the longest carbon-carbon bond is H\u2083C\u2013CH\u2083.<\/strong><\/h4>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Triple bonds (HC\u2261CH) are stronger than double (H\u2082C=CH\u2082) and single bonds (H\u2083C\u2013CH\u2083).<\/li>\n\n\n\n<li>Single bonds are longer than double or triple bonds.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\">**2) Ionic compounds consist of a single three-dimensional network of ions that are attracted to one another by strong *<em>electrostatic forces<\/em>*, and covalent compounds consist of molecules that are attracted to one another by weak **intermolecular forces<strong>.<\/strong><\/h4>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>3) The bond that is most polar is C\u2013F.<\/strong><\/h4>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Electronegativity difference between C (2.5) and F (4.0) is greater than for the other bonds.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>4) The Lewis electron-dot structure of N\u2082 has:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Nonbonding electron pairs = 2<\/strong><\/li>\n\n\n\n<li><strong>Bonding electron pairs = 3<\/strong><\/li>\n\n\n\n<li><strong>Bond order = 3<\/strong><\/li>\n<\/ul>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>N\u2082 has a triple bond and one lone pair on each nitrogen atom.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>5) The Lewis electron-dot structure of H\u2082CO has:<\/strong><\/h4>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Nonbonding electron pairs = 2<\/strong><\/li>\n\n\n\n<li><strong>Bonding electron pairs = 4<\/strong><\/li>\n\n\n\n<li><strong>Carbon-oxygen bond order = 2<\/strong><\/li>\n<\/ul>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>H\u2082CO has a double bond between C and O, with 2 lone pairs on O.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>6) The number of Lewis electron dot resonance structures required to describe NO\u2082\u207b is 2.<\/strong><\/h4>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Resonance occurs due to delocalized electrons in the N=O bonds.<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>7) Based on formal charges, the best Lewis electron-dot structure of BF\u2083 has a B\u2013F bond order = 1.<\/strong><\/h4>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>BF\u2083 has no resonance and all B\u2013F bonds are single, as boron lacks an octet in this configuration. Formal charges are minimized this way.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>11) How many lone pairs of electrons are on the S atom in SF4 ? A) 0 B) 1 C) 2 D) 3 12) How many lone pairs are on the Br atom in BrCl2-? A) 0 B) 1 C) 2 D) 3 13) In the best Lewis structure for NO +, what is the [&hellip;]<\/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-185063","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185063","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=185063"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/185063\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=185063"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=185063"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=185063"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}