{"id":191339,"date":"2025-02-14T19:26:57","date_gmt":"2025-02-14T19:26:57","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=191339"},"modified":"2025-02-14T19:27:00","modified_gmt":"2025-02-14T19:27:00","slug":"the-phosphonium-ion-ph4-is-formed-by-reaction-of-phosphine","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/14\/the-phosphonium-ion-ph4-is-formed-by-reaction-of-phosphine\/","title":{"rendered":"The phosphonium ion, PH4+, is formed by reaction of phosphine"},"content":{"rendered":"\n
The phosphonium ion, PH4+, is formed by reaction of phosphine, PH3, with an acid. (a) Draw the Lewis structure of the phosphonium ion. (b) Predict its molecular geometry. (c) Describe how a fourth hydrogen can be added to PH3. (d) Explain why the ion has a +1 charge<\/p>\n\n\n\n
The correct answer and explanation is:<\/mark><\/strong><\/p>\n\n\n\n
(a) Lewis Structure of PH\u2084\u207a<\/strong><\/h3>\n\n\n\n
To draw the Lewis structure of PH\u2084\u207a, follow these steps:<\/p>\n\n\n\n
\n
Determine the total valence electrons<\/strong>:\n
\n
Phosphorus (P) has 5 valence electrons.<\/li>\n\n\n\n
Hydrogen (H) has 1 valence electron each, contributing a total of 4 electrons.<\/li>\n\n\n\n
Since the ion has a +1 charge<\/strong>, one electron is removed.<\/li>\n\n\n\n
Four hydrogen atoms are bonded to phosphorus with single bonds.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
Assign electron pairs<\/strong>:\n
\n
All 8 electrons are used in bonding, forming four P\u2013H bonds.<\/li>\n\n\n\n
There are no lone pairs on phosphorus.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n
The Lewis structure consists of a central phosphorus atom with four hydrogen atoms bonded to it through single bonds.<\/p>\n\n\n\n
(b) Molecular Geometry<\/strong><\/h3>\n\n\n\n
Using VSEPR theory:<\/p>\n\n\n\n
\n
Phosphorus in PH\u2084\u207a forms four single bonds with hydrogen.<\/li>\n\n\n\n
No lone pairs remain on phosphorus.<\/li>\n\n\n\n
The molecular shape follows the tetrahedral<\/strong> geometry.<\/li>\n\n\n\n
Bond angles are approximately 109.5\u00b0<\/strong>.<\/li>\n<\/ul>\n\n\n\n
(c) Addition of a Fourth Hydrogen to PH\u2083<\/strong><\/h3>\n\n\n\n
\n
Phosphine (PH\u2083) has a lone pair on phosphorus, making it a Lewis base.<\/li>\n\n\n\n
When PH\u2083 reacts with a proton (H\u207a) from an acid, it donates its lone pair to H\u207a, forming a new P\u2013H bond<\/strong>.<\/li>\n\n\n\n
This results in the formation of PH\u2084\u207a.<\/li>\n<\/ul>\n\n\n\n
(d) Charge Explanation<\/strong><\/h3>\n\n\n\n
\n
Neutral PH\u2083 has 5 valence electrons on phosphorus.<\/li>\n\n\n\n
Upon adding a proton (H\u207a), phosphorus shares its lone pair<\/strong>, forming an extra bond.<\/li>\n\n\n\n
Since H\u207a has no electrons, the overall charge increases by +1<\/strong>, leading to PH\u2084\u207a.<\/li>\n<\/ul>\n\n\n\n
Now, I’ll generate the image of the PH\u2084\u207a Lewis structure.<\/p>\n\n\n\n
Here is the Lewis structure diagram of the phosphonium ion (PH\u2084\u207a). Let me know if you need any modifications or further explanations!<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"
The phosphonium ion, PH4+, is formed by reaction of phosphine, PH3, with an acid. (a) Draw the Lewis structure of the phosphonium ion. (b) Predict its molecular geometry. (c) Describe how a fourth hydrogen can be added to PH3. (d) Explain why the ion has a +1 charge The correct answer and explanation is: (a) […]<\/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-191339","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191339","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=191339"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/191339\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=191339"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=191339"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=191339"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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<\/figure>\n","protected":false},"excerpt":{"rendered":"