{"id":225542,"date":"2025-06-04T09:57:51","date_gmt":"2025-06-04T09:57:51","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=225542"},"modified":"2025-06-04T09:57:53","modified_gmt":"2025-06-04T09:57:53","slug":"complete-the-table-below-for-the-composition-of-hybrid-orbitals","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/04\/complete-the-table-below-for-the-composition-of-hybrid-orbitals\/","title":{"rendered":"Complete the table below for the composition of hybrid orbitals."},"content":{"rendered":"\n

Complete the table below for the composition of hybrid orbitals. Linear Trigonal Planar Tetrahedral Trigonal Bipyramidal Octahedral Atomic orbitals mixed Hybrid orbitals formed Unhybridized orbitals remaining s s s s s p p p p p d d sp s
s
s
d s
d
p p p d d<\/p>\n\n\n\n

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

Here’s the completed table for the composition of hybrid orbitals:<\/p>\n\n\n\n

Molecular Geometry<\/strong><\/th>Atomic Orbitals Mixed<\/strong><\/th>Hybrid Orbitals Formed<\/strong><\/th>Unhybridized Orbitals Remaining<\/strong><\/th><\/tr><\/thead>
Linear<\/strong><\/td>1 s, 1 p<\/td>sp<\/td>2 p<\/td><\/tr>
Trigonal Planar<\/strong><\/td>1 s, 2 p<\/td>sp\u00b2<\/td>1 p<\/td><\/tr>
Tetrahedral<\/strong><\/td>1 s, 3 p<\/td>sp\u00b3<\/td>0<\/td><\/tr>
Trigonal Bipyramidal<\/strong><\/td>1 s, 3 p, 1 d<\/td>sp\u00b3d<\/td>4 d<\/td><\/tr>
Octahedral<\/strong><\/td>1 s, 3 p, 2 d<\/td>sp\u00b3d\u00b2<\/td>3 d<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n
\n\n\n\n

Explanation<\/h3>\n\n\n\n

Hybridization is a concept in valence bond theory where atomic orbitals mix to form new, equivalent hybrid orbitals. These hybrids explain molecular shapes more accurately, aligning with VSEPR (Valence Shell Electron Pair Repulsion) theory predictions.<\/p>\n\n\n\n

    \n
  1. Linear Geometry (sp hybridization)<\/strong>: This involves the mixing of one s and one p orbital, forming two sp hybrid orbitals that arrange linearly at 180\u00b0. The two remaining unhybridized p orbitals can be used in forming \u03c0 bonds, as seen in molecules like BeCl\u2082 or CO\u2082.<\/li>\n\n\n\n
  2. Trigonal Planar Geometry (sp\u00b2 hybridization)<\/strong>: One s and two p orbitals mix to form three sp\u00b2 hybrid orbitals arranged in a trigonal planar shape (120\u00b0 bond angles). One p orbital remains unhybridized, available for \u03c0 bonding, as in BF\u2083 or ethene (C\u2082H\u2084).<\/li>\n\n\n\n
  3. Tetrahedral Geometry (sp\u00b3 hybridization)<\/strong>: One s and three p orbitals combine to form four sp\u00b3 orbitals, oriented at 109.5\u00b0 to each other. This accounts for molecules like CH\u2084 and NH\u2083. All valence orbitals are hybridized, so no unhybridized p orbitals remain.<\/li>\n\n\n\n
  4. Trigonal Bipyramidal Geometry (sp\u00b3d hybridization)<\/strong>: One s, three p, and one d orbital mix to create five sp\u00b3d hybrid orbitals, giving rise to a trigonal bipyramidal shape (e.g., PCl\u2085). Four d orbitals remain unhybridized.<\/li>\n\n\n\n
  5. Octahedral Geometry (sp\u00b3d\u00b2 hybridization)<\/strong>: One s, three p, and two d orbitals combine to form six sp\u00b3d\u00b2 hybrid orbitals, yielding an octahedral geometry (e.g., SF\u2086). Three d orbitals remain unhybridized.<\/li>\n<\/ol>\n\n\n\n

    These hybridizations help explain the observed bond angles, molecular shapes, and bonding behaviors of covalently bonded molecules.<\/p>\n\n\n\n

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

    Complete the table below for the composition of hybrid orbitals. Linear Trigonal Planar Tetrahedral Trigonal Bipyramidal Octahedral Atomic orbitals mixed Hybrid orbitals formed Unhybridized orbitals remaining s s s s s p p p p p d d sp sssd sdp p p d d The Correct Answer and Explanation is: Here’s the completed table […]<\/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-225542","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/225542","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=225542"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/225542\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=225542"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=225542"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=225542"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}