{"id":165498,"date":"2024-11-12T12:37:33","date_gmt":"2024-11-12T12:37:33","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=165498"},"modified":"2024-11-12T12:37:35","modified_gmt":"2024-11-12T12:37:35","slug":"what-is-the-formula-for-copperii-phosphide","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/12\/what-is-the-formula-for-copperii-phosphide\/","title":{"rendered":"What is the formula for copper(II) phosphide"},"content":{"rendered":"\n

What is the formula for copper(II) phosphide?
Give your answer in the form A#B# where the number is the subscript.<\/p>\n\n\n\n

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

The formula for copper(II) phosphide is Cu3P2<\/strong>.<\/p>\n\n\n\n

To determine the formula of copper(II) phosphide, we start by examining the charges of copper and phosphorus ions in this compound.<\/p>\n\n\n\n

    \n
  1. Copper Ion (Cu\u00b2\u207a)<\/strong>: The “(II)” in copper(II) phosphide indicates that copper has a +2 oxidation state, meaning each copper ion has a charge of +2. This ion is represented as ( \\text{Cu}^{2+} ).<\/li>\n\n\n\n
  2. Phosphide Ion (P\u00b3\u207b)<\/strong>: Phosphorus, when it forms an ion in compounds like phosphides, typically takes on a -3 charge. This ion is represented as ( \\text{P}^{3-} ).<\/li>\n<\/ol>\n\n\n\n

    In an ionic compound, the total positive and negative charges must balance to make the compound neutral. Therefore, we need to combine copper ions and phosphide ions in a ratio that neutralizes the charges.<\/p>\n\n\n\n

    To find this ratio, we look for the least common multiple (LCM)<\/strong> of the charges on Cu\u00b2\u207a and P\u00b3\u207b:<\/p>\n\n\n\n

      \n
    • The LCM of 2 and 3 is 6.<\/li>\n<\/ul>\n\n\n\n

      To achieve a neutral compound, we need a total of +6 charge from copper ions and -6 charge from phosphide ions:<\/p>\n\n\n\n

        \n
      • Copper ions<\/strong>: To achieve +6, we need three Cu\u00b2\u207a ions, as ( 3 \\times (+2) = +6 ).<\/li>\n\n\n\n
      • Phosphide ions<\/strong>: To achieve -6, we need two P\u00b3\u207b ions, as ( 2 \\times (-3) = -6 ).<\/li>\n<\/ul>\n\n\n\n

        Thus, the formula that balances the charges is Cu\u2083P\u2082<\/strong>, where three copper ions combine with two phosphide ions.<\/p>\n\n\n\n

        Summary:<\/h3>\n\n\n\n
          \n
        • Copper(II) phosphide has a formula of Cu\u2083P\u2082<\/strong>, meaning three copper (Cu) atoms for every two phosphorus (P) atoms.<\/li>\n\n\n\n
        • The charges of the ions, ( \\text{Cu}^{2+} ) and ( \\text{P}^{3-} ), dictate this 3:2 ratio to achieve charge neutrality.<\/li>\n<\/ul>\n\n\n\n

          This approach of balancing ionic charges is fundamental to determining formulas for ionic compounds, ensuring that the resulting compound is electrically neutral.<\/p>\n","protected":false},"excerpt":{"rendered":"

          What is the formula for copper(II) phosphide?Give your answer in the form A#B# where the number is the subscript. The Correct Answer and Explanation is: The formula for copper(II) phosphide is Cu3P2. To determine the formula of copper(II) phosphide, we start by examining the charges of copper and phosphorus ions in this compound. In an […]<\/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-165498","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/165498","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=165498"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/165498\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=165498"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=165498"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=165498"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}