{"id":203242,"date":"2025-03-19T04:04:41","date_gmt":"2025-03-19T04:04:41","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=203242"},"modified":"2025-03-19T04:04:43","modified_gmt":"2025-03-19T04:04:43","slug":"draw-lewis-structures-showing-all-possible-equivalent-resonance-forms-for-the-nitronium-ion-no2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/19\/draw-lewis-structures-showing-all-possible-equivalent-resonance-forms-for-the-nitronium-ion-no2\/","title":{"rendered":"Draw Lewis structure(s) showing all possible equivalent resonance forms for the nitronium ion ( NO2+ )"},"content":{"rendered":"\n<p>Draw Lewis structure(s) showing all possible equivalent resonance forms for the nitronium ion ( NO2+ ). Draw one structure per sketcher box, and separate any added sketcher boxes with the \u2194 symbol. Do NOT show any ion charges in your drawings. Do not draw double bonds to oxygen unless they are needed for the central atom to obey the octet rule. NO2+ :<\/p>\n\n\n\n<p>part b.) What is the bond order of the N &#8211; O bonds in the nitrite ion ? (enter a decimal number)<\/p>\n\n\n\n<p>In which species (NO2- or NO2+) are the N-O bond(s) longer? _________nitrite ionnitronium ion<\/p>\n\n\n\n<p>In which species (NO2- or NO2+) are the N-O bond(s) weaker? _________nitrite ionnitronium ion<\/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>Part A: Lewis Structures of NO\u2082\u207a (Nitronium Ion)<\/strong><\/h3>\n\n\n\n<p>The nitronium ion (NO\u2082\u207a) consists of a central nitrogen atom bonded to two oxygen atoms. To determine the resonance structures:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Valence Electrons Calculation<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Nitrogen (N) has 5 valence electrons.<\/li>\n\n\n\n<li>Oxygen (O) has 6 valence electrons \u00d7 2 = 12.<\/li>\n\n\n\n<li>The ion has a <strong>+1 charge<\/strong>, meaning <strong>1 electron is lost<\/strong>.<\/li>\n\n\n\n<li>Total valence electrons = <strong>5 + 12 &#8211; 1 = 16<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Drawing the Lewis Structure<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Place nitrogen in the center with two oxygens attached.<\/li>\n\n\n\n<li>To satisfy the <strong>octet rule<\/strong>, nitrogen forms <strong>two double bonds<\/strong> (N=O) with oxygen.<\/li>\n\n\n\n<li>There are <strong>no lone pairs on nitrogen<\/strong>.<\/li>\n\n\n\n<li>Each oxygen has <strong>two lone pairs<\/strong>.<\/li>\n\n\n\n<li>The formal charge on nitrogen is <strong>+1<\/strong>, and both oxygens have <strong>0 formal charge<\/strong>.<\/li>\n\n\n\n<li>The molecule is <strong>linear (180\u00b0 bond angle)<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Resonance Structures<\/strong>:<br>Since both N=O bonds are equivalent, the two resonance structures are: <strong>O=N\u207a=O \u2194 O=N\u207a=O<\/strong> The resonance structures are identical because of the symmetrical arrangement.<\/li>\n<\/ol>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>Part B: Bond Order of N-O Bonds in NO\u2082\u207b (Nitrite Ion)<\/strong><\/h3>\n\n\n\n<p>The <strong>nitrite ion (NO\u2082\u207b)<\/strong> has <strong>one double bond (N=O) and one single bond (N\u2013O) in resonance<\/strong>.<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Bond order formula<\/strong>:<br>[<br>\\text{Bond Order} = \\frac{\\text{Total Number of Bonds}}{\\text{Total Resonance Structures}}<br>]<br>Since nitrite has <strong>two resonance structures<\/strong> where the single and double bonds alternate: [<br>\\text{Bond Order} = \\frac{1 + 2}{2} = 1.5<br>] <strong>Bond Order of N\u2013O in NO\u2082\u207b = 1.5<\/strong>.<\/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>Part C: Comparing Bond Length and Strength<\/strong><\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Which species has longer N-O bonds?<\/strong><br><strong>Answer: Nitrite ion (NO\u2082\u207b)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The <strong>higher the bond order, the shorter the bond<\/strong>.<\/li>\n\n\n\n<li>In <strong>NO\u2082\u207a<\/strong>, the bond order is <strong>2.0<\/strong> (pure double bonds).<\/li>\n\n\n\n<li>In <strong>NO\u2082\u207b<\/strong>, the bond order is <strong>1.5<\/strong> (between single and double bonds).<\/li>\n\n\n\n<li>Since <strong>NO\u2082\u207b has a lower bond order, it has longer bonds<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Which species has weaker N-O bonds?<\/strong><br><strong>Answer: Nitrite ion (NO\u2082\u207b)<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Stronger bonds<\/strong> have <strong>higher bond order<\/strong>.<\/li>\n\n\n\n<li>Since <strong>NO\u2082\u207a has bond order 2.0<\/strong>, its bonds are stronger.<\/li>\n\n\n\n<li><strong>NO\u2082\u207b has bond order 1.5<\/strong>, meaning its bonds are <strong>weaker<\/strong>.<\/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>Explanation (300 Words)<\/strong><\/h3>\n\n\n\n<p>The <strong>nitronium ion (NO\u2082\u207a)<\/strong> is a <strong>linear molecule<\/strong> with two <strong>equivalent N=O double bonds<\/strong>, making it highly <strong>symmetrical<\/strong>. Because nitrogen has no lone pairs, it achieves a formal charge of <strong>+1<\/strong>, while both oxygens have a <strong>formal charge of 0<\/strong>. This results in a <strong>bond order of 2.0<\/strong>, meaning the N\u2013O bonds are purely double bonds.<\/p>\n\n\n\n<p>In contrast, the <strong>nitrite ion (NO\u2082\u207b)<\/strong> is <strong>bent<\/strong> due to the presence of <strong>one lone pair on nitrogen<\/strong>. It has <strong>one single bond and one double bond<\/strong>, but because of resonance, both bonds are <strong>delocalized<\/strong> and effectively have an intermediate bond order of <strong>1.5<\/strong>.<\/p>\n\n\n\n<p>Bond length and bond strength are directly related to bond order:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Higher bond order \u2192 Shorter, Stronger Bonds<\/strong>.<\/li>\n\n\n\n<li><strong>Lower bond order \u2192 Longer, Weaker Bonds<\/strong>.<\/li>\n<\/ul>\n\n\n\n<p>Since the nitronium ion (NO\u2082\u207a) has a bond order of <strong>2.0<\/strong>, its <strong>bonds are shorter and stronger<\/strong> than those in nitrite (NO\u2082\u207b), which has a bond order of <strong>1.5<\/strong>. This means that the <strong>N-O bonds in NO\u2082\u207b are longer and weaker compared to NO\u2082\u207a<\/strong>.<\/p>\n\n\n\n<p>These differences in bonding affect chemical reactivity:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>NO\u2082\u207a is an electrophile<\/strong>, often found in nitration reactions (e.g., electrophilic aromatic substitution).<\/li>\n\n\n\n<li><strong>NO\u2082\u207b is a stable anion<\/strong> and acts as a <strong>Lewis base<\/strong> in coordination chemistry.<\/li>\n<\/ul>\n\n\n\n<p>In summary:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>NO\u2082\u207a (Nitronium ion) has shorter, stronger bonds (bond order = 2.0).<\/strong><\/li>\n\n\n\n<li><strong>NO\u2082\u207b (Nitrite ion) has longer, weaker bonds (bond order = 1.5).<\/strong><\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>Draw Lewis structure(s) showing all possible equivalent resonance forms for the nitronium ion ( NO2+ ). Draw one structure per sketcher box, and separate any added sketcher boxes with the \u2194 symbol. Do NOT show any ion charges in your drawings. Do not draw double bonds to oxygen unless they are needed for the central [&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-203242","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203242","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=203242"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/203242\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=203242"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=203242"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=203242"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}