{"id":239519,"date":"2025-07-03T03:11:13","date_gmt":"2025-07-03T03:11:13","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=239519"},"modified":"2025-07-03T03:11:16","modified_gmt":"2025-07-03T03:11:16","slug":"construct-the-molecular-orbital-diagram-for-n2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/03\/construct-the-molecular-orbital-diagram-for-n2\/","title":{"rendered":"Construct the molecular orbital diagram for N2"},"content":{"rendered":"\n
Construct the molecular orbital diagram for N2.<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
To construct the molecular orbital diagram for nitrogen (N\u2082), we first need to understand the basic principles of molecular orbitals (MOs). The diagram represents the combination of atomic orbitals (AOs) from two nitrogen atoms, and it shows the energy levels of the molecular orbitals formed.<\/p>\n\n\n\n
Steps for constructing the molecular orbital diagram of N\u2082:<\/h3>\n\n\n\n\n
Atomic Orbitals:<\/strong> Each nitrogen atom has the following electron configuration: 1s\u00b2 2s\u00b2 2p\u00b3. The valence electrons (in the 2s and 2p orbitals) will be involved in bonding and antibonding interactions.<\/li>\n\n\n\n
Molecular Orbitals (MOs):<\/strong> The atomic orbitals combine to form molecular orbitals. The s orbitals combine to form a bonding \u03c3(2s) and an antibonding \u03c3*(2s). Similarly, the p orbitals combine in different ways:
Bonding MOs:<\/strong> \u03c3(2p) and \u03c0(2p)<\/li>
Antibonding MOs:<\/strong> \u03c3*(2p) and \u03c0*(2p)<\/li><\/ul>The energy order of MOs for molecules with fewer than 8 electrons in the p orbitals (like N\u2082) follows this pattern:\n
Electron Configuration:<\/strong> Nitrogen has 10 valence electrons, which we place in the molecular orbitals as follows:\n
\n
The first two electrons go into the bonding \u03c3(2s) orbital.<\/li>\n\n\n\n
The next two electrons go into the antibonding \u03c3*(2s) orbital.<\/li>\n\n\n\n
The next two electrons go into the bonding \u03c3(2p) orbital.<\/li>\n\n\n\n
The remaining four electrons will be placed in the degenerate \u03c0(2p) orbitals, two electrons in each.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
Bond Order Calculation:<\/strong> The bond order is calculated by the formula: Bond\u00a0Order=Number\u00a0of\u00a0electrons\u00a0in\u00a0bonding\u00a0orbitals\u2212Number\u00a0of\u00a0electrons\u00a0in\u00a0antibonding\u00a0orbitals2\\text{Bond Order} = \\frac{\\text{Number of electrons in bonding orbitals} – \\text{Number of electrons in antibonding orbitals}}{2}Bond\u00a0Order=2Number\u00a0of\u00a0electrons\u00a0in\u00a0bonding\u00a0orbitals\u2212Number\u00a0of\u00a0electrons\u00a0in\u00a0antibonding\u00a0orbitals\u200b For N\u2082:\n
Antibonding electrons: 2 (\u03c3*(2s)) Bond order = (8 – 2) \/ 2 = 3<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n
Thus, N\u2082 has a bond order of 3, indicating a triple bond between the two nitrogen atoms.<\/p>\n\n\n\n
Conclusion:<\/h3>\n\n\n\n
The molecular orbital diagram for N\u2082 consists of six molecular orbitals: \u03c3(2s), \u03c3*(2s), \u03c3(2p), \u03c0(2p), \u03c0*(2p), and \u03c3*(2p). The electron configuration places electrons in these orbitals in a way that gives N\u2082 a triple bond, which is consistent with the observed properties of the molecule.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
Construct the molecular orbital diagram for N2. The Correct Answer and Explanation is: To construct the molecular orbital diagram for nitrogen (N\u2082), we first need to understand the basic principles of molecular orbitals (MOs). The diagram represents the combination of atomic orbitals (AOs) from two nitrogen atoms, and it shows the energy levels of the […]<\/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-239519","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/239519","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=239519"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/239519\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=239519"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=239519"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=239519"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner5-41.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"