{"id":221250,"date":"2025-05-29T10:17:24","date_gmt":"2025-05-29T10:17:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=221250"},"modified":"2025-05-29T10:17:27","modified_gmt":"2025-05-29T10:17:27","slug":"what-would-be-the-structure-predicted-by-using-lewis-dot-structures-for-calcium-phosphide","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/29\/what-would-be-the-structure-predicted-by-using-lewis-dot-structures-for-calcium-phosphide\/","title":{"rendered":"What Would Be The Structure Predicted By Using Lewis Dot Structures For Calcium Phosphide"},"content":{"rendered":"\n

What Would Be The Structure Predicted By Using Lewis Dot Structures For Calcium Phosphide? CaP CaP_2 Ca_2P Ca_2P_2 Ca_3P_2<\/p>\n\n\n\n

What would be the structure predicted by using Lewis dot structures for calcium phosphide CaP CaP2 Ca2P Ca2P2 Ca3P2<\/p>\n\n\n\n

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

The correct formula for calcium phosphide based on Lewis dot structure predictions and known ionic bonding behavior is Ca\u2083P\u2082<\/strong>.<\/p>\n\n\n\n

\n\n\n\n

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

To predict the structure of calcium phosphide using Lewis dot structures<\/strong>, we must analyze the typical electron behavior of calcium (Ca)<\/strong> and phosphorus (P)<\/strong> atoms:<\/p>\n\n\n\n

    \n
  • Calcium (Ca)<\/strong> is a Group 2 alkaline earth metal<\/strong>, which means it has 2 valence electrons<\/strong>. Calcium readily loses 2 electrons<\/strong> to achieve a stable noble gas configuration (like Argon), forming a Ca\u00b2\u207a<\/strong> ion.<\/li>\n\n\n\n
  • Phosphorus (P)<\/strong> is a Group 15 nonmetal<\/strong>, with 5 valence electrons<\/strong>. It gains 3 electrons<\/strong> to complete its octet, forming a P\u00b3\u207b<\/strong> ion.<\/li>\n<\/ul>\n\n\n\n

    Since Ca wants to lose 2 electrons (Ca\u00b2\u207a) and P wants to gain 3 electrons (P\u00b3\u207b), we need to balance the total charges of the ions to form a neutral compound<\/strong>.<\/p>\n\n\n\n

    To balance charges:<\/p>\n\n\n\n

      \n
    • 3 Ca\u00b2\u207a ions contribute a total of +6<\/strong> charge.<\/li>\n\n\n\n
    • 2 P\u00b3\u207b ions contribute a total of \u20136<\/strong> charge.<\/li>\n<\/ul>\n\n\n\n

      Thus, the simplest ratio that results in a neutral compound is: 3 Ca2++2 P3\u2212\u2192Ca3P2\\text{3 Ca}^{2+} + \\text{2 P}^{3-} \\rightarrow \\text{Ca}_3\\text{P}_2<\/p>\n\n\n\n

      This gives the empirical formula Ca\u2083P\u2082<\/strong>, which is the correct ionic compound<\/strong> formed between calcium and phosphorus. The Lewis dot structure would show:<\/p>\n\n\n\n

        \n
      • Each calcium atom losing two electrons (becoming Ca\u00b2\u207a).<\/li>\n\n\n\n
      • Each phosphorus atom gaining three electrons (becoming P\u00b3\u207b).<\/li>\n<\/ul>\n\n\n\n

        This results in an ionic lattice<\/strong> structure, where the Ca\u00b2\u207a and P\u00b3\u207b ions are held together by strong electrostatic forces, not by shared electrons (as in covalent bonds), consistent with ionic bonding in salts.<\/p>\n\n\n\n

        Therefore, among the options (CaP, CaP\u2082, Ca\u2082P, Ca\u2082P\u2082, Ca\u2083P\u2082), Ca\u2083P\u2082<\/strong> is the only formula that correctly represents the charge balance based on Lewis structure predictions.<\/p>\n\n\n\n

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

        What Would Be The Structure Predicted By Using Lewis Dot Structures For Calcium Phosphide? CaP CaP_2 Ca_2P Ca_2P_2 Ca_3P_2 What would be the structure predicted by using Lewis dot structures for calcium phosphide CaP CaP2 Ca2P Ca2P2 Ca3P2 The Correct Answer and Explanation is: The correct formula for calcium phosphide based on Lewis dot structure […]<\/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-221250","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221250","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=221250"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221250\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=221250"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=221250"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=221250"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}