{"id":164015,"date":"2024-11-09T09:50:26","date_gmt":"2024-11-09T09:50:26","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=164015"},"modified":"2024-11-09T09:50:29","modified_gmt":"2024-11-09T09:50:29","slug":"what-is-the-formal-charge-on-phosporus-in-h3po4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/09\/what-is-the-formal-charge-on-phosporus-in-h3po4\/","title":{"rendered":"What is the formal charge on phosporus in H3PO4"},"content":{"rendered":"\n

What is the formal charge on phosporus in H3PO4<\/p>\n\n\n\n

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

The formal charge on phosphorus in H\u2083PO\u2084 (phosphoric acid) is 0<\/strong>.<\/p>\n\n\n\n

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

To determine the formal charge on phosphorus in H\u2083PO\u2084, we follow a systematic approach using the formula for formal charge:<\/p>\n\n\n\n

[
\\text{Formal Charge} = \\text{Valence electrons} – (\\text{Lone electrons} + \\frac{\\text{Bonding electrons}}{2})
]<\/p>\n\n\n\n

Step 1: Determine the Valence Electrons of Phosphorus<\/h4>\n\n\n\n

Phosphorus (P) is in group 15 of the periodic table, so it has 5 valence electrons<\/strong>.<\/p>\n\n\n\n

Step 2: Electron Distribution in H\u2083PO\u2084<\/h4>\n\n\n\n

In H\u2083PO\u2084, phosphorus is at the center of the molecule, surrounded by four oxygen atoms (one of which is double-bonded to phosphorus, and three single-bonded). The structure of H\u2083PO\u2084 consists of:<\/p>\n\n\n\n

    \n
  • One double bond between phosphorus and one oxygen atom.<\/li>\n\n\n\n
  • Three single bonds between phosphorus and three other oxygen atoms.<\/li>\n\n\n\n
  • Each of the three single-bonded oxygen atoms carries a hydrogen atom (OH group).<\/li>\n<\/ul>\n\n\n\n

    Step 3: Count Lone Pair and Bonding Electrons<\/h4>\n\n\n\n
      \n
    • In the molecule, phosphorus forms a double bond<\/strong> with one oxygen atom and single bonds<\/strong> with the other three oxygens.<\/li>\n\n\n\n
    • Since phosphorus is bonded to four oxygens, it will share electrons with them in bonding (8 electrons total), which are equally divided between the bonds.<\/li>\n\n\n\n
    • The oxygen atoms<\/strong> involved in single bonds each have lone pairs of electrons. The oxygen atom involved in the double bond also has lone pairs.<\/li>\n<\/ul>\n\n\n\n

      Step 4: Calculate Formal Charge<\/h4>\n\n\n\n
        \n
      • The formal charge on phosphorus is calculated by considering the number of electrons phosphorus “owns” in H\u2083PO\u2084:<\/li>\n\n\n\n
      • Phosphorus contributes 5 valence electrons, and it is involved in 4 bonds, sharing 8 electrons.<\/li>\n\n\n\n
      • Since phosphorus is equally sharing bonding electrons, it “owns” 4 electrons (2 electrons per bond for the 2 single bonds and 2 electrons for the double bond).<\/li>\n\n\n\n
      • The number of lone electrons on phosphorus is 0, as it does not have any lone pairs.<\/li>\n<\/ul>\n\n\n\n

        Thus, the formal charge on phosphorus is:<\/p>\n\n\n\n

        [
        \\text{Formal Charge} = 5 – (0 + \\frac{8}{2}) = 5 – 4 = 0
        ]<\/p>\n\n\n\n

        Therefore, the formal charge on phosphorus in H\u2083PO\u2084 is 0<\/strong>. This indicates that phosphorus in H\u2083PO\u2084 is neutral.<\/p>\n","protected":false},"excerpt":{"rendered":"

        What is the formal charge on phosporus in H3PO4 The Correct Answer and Explanation is : The formal charge on phosphorus in H\u2083PO\u2084 (phosphoric acid) is 0. Explanation: To determine the formal charge on phosphorus in H\u2083PO\u2084, we follow a systematic approach using the formula for formal charge: [\\text{Formal Charge} = \\text{Valence electrons} – (\\text{Lone […]<\/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-164015","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/164015","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=164015"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/164015\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=164015"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=164015"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=164015"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}