{"id":233089,"date":"2025-06-12T14:29:09","date_gmt":"2025-06-12T14:29:09","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=233089"},"modified":"2025-06-12T14:29:12","modified_gmt":"2025-06-12T14:29:12","slug":"how-do-the-p-ci-single-bond-lengths-in-pcl5-pcl4-and-pcl6-generally-compare","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/06\/12\/how-do-the-p-ci-single-bond-lengths-in-pcl5-pcl4-and-pcl6-generally-compare\/","title":{"rendered":"How do the P-Ci single bond lengths in PCl5, PCl4+, and PCl6- generally compare"},"content":{"rendered":"\n
How do the P-Ci single bond lengths in PCl5, PCl4+, and PCl6- generally compare? 4. Identify the type of bonding the central atom undergoes in PCl5 and PCl6-.<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n
Answer:<\/h3>\n\n\n\n
\n
P\u2013Cl single bond lengths trend<\/strong>: PCl\u2084\u207a < PCl\u2085 < PCl\u2086\u207b<\/strong><\/li>\n\n\n\n
The phosphorus-chlorine (P\u2013Cl) bond lengths in phosphorus halides such as PCl\u2084\u207a<\/strong>, PCl\u2085<\/strong>, and PCl\u2086\u207b<\/strong> vary systematically based on the molecule\u2019s structure, electron count, and bonding environment. These differences stem from changes in electron repulsion, oxidation state, and hybridization of the central phosphorus atom.<\/p>\n\n\n\n
In PCl\u2084\u207a<\/strong>, phosphorus forms four bonds and carries a positive charge, resulting in increased effective nuclear charge on the phosphorus center. This leads to stronger attraction between P and Cl atoms and thus shorter P\u2013Cl bond lengths<\/strong>. The molecule adopts a tetrahedral geometry<\/strong>, and phosphorus undergoes sp\u00b3 hybridization<\/strong>.<\/p>\n\n\n\n
In PCl\u2085<\/strong>, phosphorus forms five P\u2013Cl bonds in a trigonal bipyramidal geometry<\/strong>, requiring sp\u00b3d hybridization<\/strong>. The axial P\u2013Cl bonds are typically longer than the equatorial ones due to increased electron repulsion in the axial positions. Overall, the average bond length in PCl\u2085 is longer than in PCl\u2084\u207a, due to reduced positive charge density and increased repulsion from the extra bonded pair.<\/p>\n\n\n\n
In PCl\u2086\u207b<\/strong>, phosphorus is surrounded by six chlorine atoms and an extra electron (due to the negative charge), further increasing electron\u2013electron repulsion. The molecule adopts an octahedral geometry<\/strong> and undergoes sp\u00b3d\u00b2 hybridization<\/strong>. The additional electron density causes P\u2013Cl bond lengths to be the longest<\/strong> among the three species, as repulsion pushes the ligands farther apart.<\/p>\n\n\n\n
Hence, the general trend in P\u2013Cl bond length is: PCl\u2084\u207a < PCl\u2085 < PCl\u2086\u207b<\/strong>, reflecting increasing number of bonds and electron repulsion effects.<\/p>\n\n\n\n
The bonding in PCl\u2085<\/strong> and PCl\u2086\u207b<\/strong> requires the use of d-orbitals to accommodate more than an octet of electrons around phosphorus, enabling it to form five and six bonds, respectively. This leads to the sp\u00b3d<\/strong> and sp\u00b3d\u00b2 hybridizations<\/strong>, necessary for the trigonal bipyramidal and octahedral shapes.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
How do the P-Ci single bond lengths in PCl5, PCl4+, and PCl6- generally compare? 4. Identify the type of bonding the central atom undergoes in PCl5 and PCl6-. The Correct Answer and Explanation is: Answer: Explanation The phosphorus-chlorine (P\u2013Cl) bond lengths in phosphorus halides such as PCl\u2084\u207a, PCl\u2085, and PCl\u2086\u207b vary systematically based on 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-233089","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233089","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=233089"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/233089\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=233089"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=233089"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=233089"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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