{"id":260957,"date":"2025-07-19T17:44:08","date_gmt":"2025-07-19T17:44:08","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=260957"},"modified":"2025-07-19T17:44:10","modified_gmt":"2025-07-19T17:44:10","slug":"which-molecules-are-described-by-molecular-orbital-theory-as-having-a-bond-order-of-2-0","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/19\/which-molecules-are-described-by-molecular-orbital-theory-as-having-a-bond-order-of-2-0\/","title":{"rendered":"Which molecules are described by molecular orbital theory as having a bond order of 2.0"},"content":{"rendered":"\n<p>Which molecules are described by molecular orbital theory as having a bond order of 2.0?<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The correct answer is <strong>O\u2082 (Oxygen molecule)<\/strong>.<\/p>\n\n\n\n<p><strong>Explanation:<\/strong><\/p>\n\n\n\n<p>Molecular orbital (MO) theory provides a way to describe the bonding in molecules by combining atomic orbitals to form molecular orbitals. These molecular orbitals can be classified into bonding, anti-bonding, and non-bonding orbitals. The bond order in MO theory is determined by the difference between the number of electrons in bonding and anti-bonding molecular orbitals, divided by two.<\/p>\n\n\n\n<p>The bond order (BO) is calculated using the formula: Bond&nbsp;order=12(Number&nbsp;of&nbsp;electrons&nbsp;in&nbsp;bonding&nbsp;orbitals\u2212Number&nbsp;of&nbsp;electrons&nbsp;in&nbsp;anti-bonding&nbsp;orbitals)\\text{Bond order} = \\frac{1}{2} \\left( \\text{Number of electrons in bonding orbitals} &#8211; \\text{Number of electrons in anti-bonding orbitals} \\right)<\/p>\n\n\n\n<p>For the O\u2082 molecule, the molecular orbitals are filled with electrons as follows:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The O\u2082 molecule has a total of 16 electrons (8 from each oxygen atom).<\/li>\n\n\n\n<li>These electrons fill the molecular orbitals in order of increasing energy: \u03c3(1s), \u03c3*(1s), \u03c3(2s), \u03c3*(2s), \u03c0(2p), \u03c0*(2p).<\/li>\n\n\n\n<li>Oxygen&#8217;s molecular orbitals are filled as: \u03c3(1s)\u00b2, \u03c3*(1s)\u00b2, \u03c3(2s)\u00b2, \u03c3*(2s)\u00b2, \u03c0(2p)\u2074, \u03c0*(2p)\u00b2.<\/li>\n\n\n\n<li>There are 10 electrons in bonding molecular orbitals (2 from \u03c3(2s)\u00b2, 2 from \u03c3*(2s)\u00b2, 4 from \u03c0(2p)\u2074) and 6 electrons in anti-bonding molecular orbitals (2 from \u03c0*(2p)\u00b2).<\/li>\n<\/ul>\n\n\n\n<p>Now, the bond order calculation: Bond&nbsp;order=12(10\u22126)=12\u00d74=2\\text{Bond order} = \\frac{1}{2} \\left( 10 &#8211; 6 \\right) = \\frac{1}{2} \\times 4 = 2<\/p>\n\n\n\n<p>Thus, O\u2082 has a bond order of 2. This means that the oxygen molecule has a double bond between the two oxygen atoms.<\/p>\n\n\n\n<p>The bond order of 2 is common in molecules that have a similar electron configuration, such as O\u2082, and it indicates that there are two bonding electron pairs in the molecule, leading to a relatively strong and stable bond.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Which molecules are described by molecular orbital theory as having a bond order of 2.0? The correct answer and explanation is: The correct answer is O\u2082 (Oxygen molecule). Explanation: Molecular orbital (MO) theory provides a way to describe the bonding in molecules by combining atomic orbitals to form molecular orbitals. These molecular orbitals can be [&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-260957","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/260957","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=260957"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/260957\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=260957"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=260957"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=260957"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}