{"id":162716,"date":"2024-11-07T08:15:57","date_gmt":"2024-11-07T08:15:57","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=162716"},"modified":"2024-11-07T08:15:59","modified_gmt":"2024-11-07T08:15:59","slug":"what-is-the-simplest-formula-for-copper-ii-nitride","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/07\/what-is-the-simplest-formula-for-copper-ii-nitride\/","title":{"rendered":"What is the simplest formula for copper (II) nitride"},"content":{"rendered":"\n<p>What is the simplest formula for copper (II) nitride<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>The simplest formula for copper (II) nitride is <strong>Cu\u2083N\u2082<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>To understand how we arrive at the formula <strong>Cu\u2083N\u2082<\/strong> for copper (II) nitride, we need to consider the oxidation states of copper and nitrogen, and how they combine to form a neutral compound.<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Oxidation State of Copper<\/strong>:<br>Copper (II) nitride contains copper in the <strong>+2 oxidation state<\/strong>. This means each copper (Cu) atom has lost two electrons, resulting in a charge of +2. This is denoted as <strong>Cu\u00b2\u207a<\/strong>.<\/li>\n\n\n\n<li><strong>Oxidation State of Nitrogen<\/strong>:<br>Nitrogen typically forms nitride (N\u00b3\u207b) in ionic compounds. In nitride, nitrogen has an oxidation state of <strong>-3<\/strong>.<\/li>\n\n\n\n<li><strong>Balancing Charges<\/strong>:<br>In an ionic compound, the total positive charge must balance the total negative charge to make the compound neutral. Therefore, we need to determine the ratio of copper (Cu\u00b2\u207a) ions to nitride (N\u00b3\u207b) ions.<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Each Cu\u00b2\u207a ion has a charge of +2.<\/li>\n\n\n\n<li>Each N\u00b3\u207b ion has a charge of -3. To balance these charges, we need multiples of copper and nitrogen such that their total charges equal zero.<\/li>\n\n\n\n<li>Let\u2019s say we have 3 copper ions (each with a +2 charge) and 2 nitrogen ions (each with a -3 charge):<ul><li>3 copper ions \u00d7 (+2 charge) = +6<\/li><li>2 nitrogen ions \u00d7 (-3 charge) = -6<\/li><\/ul>The total positive charge is +6, and the total negative charge is -6. Since +6 and -6 balance each other out, the compound is electrically neutral.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Final Formula<\/strong>:<br>The simplest formula, reflecting this charge balance, is <strong>Cu\u2083N\u2082<\/strong>, meaning 3 copper ions for every 2 nitrogen ions.<\/li>\n<\/ol>\n\n\n\n<p>Thus, the simplest formula for copper (II) nitride is <strong>Cu\u2083N\u2082<\/strong>, which adheres to the charge balance rule for ionic compounds.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What is the simplest formula for copper (II) nitride The Correct Answer and Explanation is: The simplest formula for copper (II) nitride is Cu\u2083N\u2082. Explanation: To understand how we arrive at the formula Cu\u2083N\u2082 for copper (II) nitride, we need to consider the oxidation states of copper and nitrogen, and how they combine to form [&hellip;]<\/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-162716","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/162716","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=162716"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/162716\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=162716"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=162716"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=162716"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}