{"id":220156,"date":"2025-05-27T15:56:25","date_gmt":"2025-05-27T15:56:25","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=220156"},"modified":"2025-05-27T15:56:26","modified_gmt":"2025-05-27T15:56:26","slug":"no3-is-an-molecule-that-does-not-satisfy-the-octet-rule","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/27\/no3-is-an-molecule-that-does-not-satisfy-the-octet-rule\/","title":{"rendered":"NO3 is an molecule that does not satisfy the octet rule"},"content":{"rendered":"\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/image-463.png\" alt=\"\" class=\"wp-image-220157\"\/><\/figure>\n\n\n\n<p>illustrate clearly, using Lewis dot structures, why it is considered an exception. Discuss whether resonance structures can account for its stability. A: NO3 is an molecule that does not satisfy the octet rule. The Lewis dot structure for nitrogen trioxide is :O.N.:O: It does satisfy the octet rule because each atom in the molecule only has access to 7 electrons, instead of the eight required, as shown by the circled atoms. O\u00c2\u00b7NO:<\/p>\n\n\n\n<p>The molecule shown in the image is incorrectly labeled and explained. The species <strong>NO\u2083<\/strong> mentioned in the text is actually <strong>NO\u2083\u207b (nitrate ion)<\/strong>, which <strong>does follow<\/strong> the octet rule through resonance. However, the <strong>structure in the image corresponds to NO\u2082 (nitrogen dioxide)<\/strong> or more likely <strong>NO (nitric oxide)<\/strong> derivatives, not NO\u2083\u207b. Based on the image and the description of each atom having only 7 electrons, the molecule that actually <strong>displays an exception to the octet rule<\/strong> is <strong>NO (nitric oxide)<\/strong>, not NO\u2083\u207b. Let&#8217;s correct and explain the concept clearly:<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Correct Answer:<\/h3>\n\n\n\n<p><strong>Nitric oxide (NO)<\/strong> is a molecule that <strong>does not satisfy the octet rule.<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Lewis Dot Structure for NO:<\/h3>\n\n\n\n<pre class=\"wp-block-code\"><code> :N\u2261O:\u2022\n<\/code><\/pre>\n\n\n\n<p>In this structure:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Nitrogen forms a triple bond with oxygen and has one lone electron (an odd number of electrons).<\/li>\n\n\n\n<li>This results in <strong>7 valence electrons around nitrogen<\/strong> and <strong>8 around oxygen<\/strong>, violating the octet rule for nitrogen.<\/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\">Explanation<\/h3>\n\n\n\n<p>The octet rule states that atoms tend to form molecules in which each atom has eight electrons in its valence shell, achieving a noble gas configuration. However, <strong>nitric oxide (NO)<\/strong> is a well-known exception. It is a <strong>free radical<\/strong>, meaning it contains an <strong>unpaired electron<\/strong>, which results in one of its atoms (nitrogen) having only <strong>seven valence electrons<\/strong>.<\/p>\n\n\n\n<p>The Lewis structure of NO shows a nitrogen atom triple-bonded to an oxygen atom, with one unpaired electron residing on nitrogen. This configuration provides oxygen with a full octet but leaves nitrogen with only seven electrons, making NO <strong>an odd-electron molecule<\/strong>. This makes NO inherently reactive, but it does exist stably due to delocalization of electrons and molecular orbital stabilization.<\/p>\n\n\n\n<p>Unlike molecules that obey the octet rule, <strong>NO cannot form a resonance structure<\/strong> that distributes the extra electron to give both atoms a full octet. However, <strong>molecular orbital theory<\/strong> explains NO\u2019s stability through delocalized bonding. The half-filled \u03c0* antibonding orbital reduces the bond order slightly, but gives some stability to the structure.<\/p>\n\n\n\n<p>In contrast, <strong>NO\u2083\u207b (nitrate ion)<\/strong> <strong>does obey the octet rule<\/strong> and has <strong>three equivalent resonance structures<\/strong>, where the double bond rotates between the three oxygen atoms, delocalizing the negative charge and enhancing stability.<\/p>\n\n\n\n<p>In conclusion, <strong>NO is a true exception to the octet rule<\/strong>, and its stability cannot be fully explained using simple Lewis structures or resonance but rather through molecular orbital theory.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/learnexams-banner8-43.jpeg\" alt=\"\" class=\"wp-image-220158\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>illustrate clearly, using Lewis dot structures, why it is considered an exception. Discuss whether resonance structures can account for its stability. A: NO3 is an molecule that does not satisfy the octet rule. The Lewis dot structure for nitrogen trioxide is :O.N.:O: It does satisfy the octet rule because each atom in the molecule only [&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-220156","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/220156","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=220156"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/220156\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=220156"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=220156"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=220156"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}