{"id":244335,"date":"2025-07-05T04:29:59","date_gmt":"2025-07-05T04:29:59","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=244335"},"modified":"2025-07-05T04:30:01","modified_gmt":"2025-07-05T04:30:01","slug":"draw-all-of-the-resonance-structures-for-the-n_2o_4-molecule-and-determine-the-average-n-o-bond-order","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/05\/draw-all-of-the-resonance-structures-for-the-n_2o_4-molecule-and-determine-the-average-n-o-bond-order\/","title":{"rendered":"Draw all of the resonance structures for the N_(2)O_(4) molecule and determine the average N-O bond order."},"content":{"rendered":"\n

Draw all of the resonance structures for the N_(2)O_(4) molecule and determine the average N-O bond order. The skeletal structure of the molecule is able[[O,O],[N,N],[O,]] 8.113 Draw all of the resonance structures for the N,O4 mol ecule and determine the average N-O bond order. The skeletal structure of the molecule is 0 0 N N 0 0<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

\u2705\u202fCorrect Answer<\/strong>: The molecule N\u2082O\u2084 has four major resonance structures. In each, the N\u2013N bond remains a single bond, while the N\u2013O bonds alternate between single and double bonds across the resonance forms. The average N\u2013O bond order is\u202f1.5<\/strong>.<\/p>\n\n\n\n

\ud83e\udde0\u202fExplanation<\/strong><\/p>\n\n\n\n

Dinitrogen tetroxide (N\u2082O\u2084) is a covalent molecule composed of two nitrogen atoms and four oxygen atoms. Its skeletal structure is symmetric, with each nitrogen atom bonded to two oxygen atoms and to the other nitrogen atom. The key to understanding its bonding lies in resonance theory, which describes how electrons can be delocalized across multiple atoms, leading to multiple valid Lewis structures.<\/p>\n\n\n\n

In N\u2082O\u2084, the N\u2013N bond is always a single bond in all resonance forms. The variation occurs in the N\u2013O bonds. Each nitrogen is bonded to two oxygen atoms, and the double bonds can shift among these oxygens. This results in four major resonance structures, each with two N=O double bonds and two N\u2013O single bonds. The double bonds are not fixed in one location but are delocalized across the molecule.<\/p>\n\n\n\n

To determine the average N\u2013O bond order, we consider the total number of N\u2013O bonds and how many are double versus single across the resonance forms. In each resonance structure, there are four N\u2013O bonds: two are single (bond order 1), and two are double (bond order 2). The total bond order contribution is:<\/p>\n\n\n\n

(2 \u00d7 1) + (2 \u00d7 2) = 2 + 4 = 6<\/p>\n\n\n\n

Dividing this total by the number of N\u2013O bonds (4) gives the average bond order:<\/p>\n\n\n\n

6 \u00f7 4 = 1.5<\/p>\n\n\n\n

This means that each N\u2013O bond in N\u2082O\u2084 has partial double bond character, consistent with experimental observations such as bond lengths that are intermediate between typical N\u2013O single and double bonds. The resonance hybrid is more stable than any individual structure and reflects this delocalization.<\/p>\n\n\n\n

Thus, the average N\u2013O bond order in N\u2082O\u2084 is\u202f1.5<\/strong>.<\/p>\n\n\n\n

\"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

Draw all of the resonance structures for the N_(2)O_(4) molecule and determine the average N-O bond order. The skeletal structure of the molecule is able[[O,O],[N,N],[O,]] 8.113 Draw all of the resonance structures for the N,O4 mol ecule and determine the average N-O bond order. The skeletal structure of the molecule is 0 0 N N […]<\/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-244335","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/244335","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=244335"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/244335\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=244335"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=244335"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=244335"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}