{"id":201067,"date":"2025-03-14T18:56:00","date_gmt":"2025-03-14T18:56:00","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=201067"},"modified":"2025-03-14T18:56:02","modified_gmt":"2025-03-14T18:56:02","slug":"formula-for-cobalt-ii-chlorite","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/14\/formula-for-cobalt-ii-chlorite\/","title":{"rendered":"formula for cobalt (II) chlorite"},"content":{"rendered":"\n<p>formula for cobalt (II) chlorite?<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>The correct formula for cobalt(II) chlorite is <strong>Co(ClO\u2082)\u2082<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Understanding Cobalt(II):<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The Roman numeral (II) in <strong>cobalt(II)<\/strong> indicates that cobalt has a <strong>+2 oxidation state<\/strong>, meaning its ionic charge is <strong>+2<\/strong>.<\/li>\n\n\n\n<li>The symbol for cobalt is <strong>Co<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Understanding the Chlorite Ion:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Chlorite<\/strong> is a polyatomic ion with the formula <strong>ClO\u2082\u207b<\/strong>.<\/li>\n\n\n\n<li>It has a <strong>-1 charge<\/strong>.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Balancing Charges:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Since <strong>Co\u00b2\u207a<\/strong> has a <strong>+2 charge<\/strong> and <strong>ClO\u2082\u207b<\/strong> has a <strong>-1 charge<\/strong>, two <strong>chlorite (ClO\u2082\u207b) ions<\/strong> are needed to balance the charge.<\/li>\n\n\n\n<li>This results in the formula <strong>Co(ClO\u2082)\u2082<\/strong>.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Why Parentheses?<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The parentheses around <strong>ClO\u2082<\/strong> indicate that <strong>two chlorite ions<\/strong> are present in the compound.<\/li>\n\n\n\n<li>Without parentheses, it might be misinterpreted as <strong>CoClO\u2082\u2082<\/strong>, which is incorrect.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Verification of Charge Balance:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Cobalt(II) ion charge:<\/strong> +2<\/li>\n\n\n\n<li><strong>Two chlorite ions charge:<\/strong> 2 \u00d7 (-1) = -2<\/li>\n\n\n\n<li><strong>Total charge = 0<\/strong>, meaning the compound is electrically neutral.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Common Mistakes to Avoid:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Confusing Chlorite with Other Chlorine Oxyanions:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Chlorate (ClO\u2083\u207b)<\/strong> and <strong>Perchlorate (ClO\u2084\u207b)<\/strong> are different from <strong>Chlorite (ClO\u2082\u207b)<\/strong>.<\/li>\n\n\n\n<li>Be careful not to mix up chlorite with <strong>hypochlorite (ClO\u207b)<\/strong> either.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Incorrectly Writing the Formula as CoClO\u2082:<\/strong><\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>This would imply only one chlorite ion is present, which does not balance the cobalt(II) charge.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Applications of Cobalt(II) Chlorite:<\/h3>\n\n\n\n<p>While cobalt(II) chlorite is <strong>not very common<\/strong>, cobalt compounds are used in batteries, pigments, and catalysts. Chlorite compounds, in general, are used in bleaching and disinfecting applications.<\/p>\n\n\n\n<p>Thus, the correct formula for cobalt(II) chlorite is <strong>Co(ClO\u2082)\u2082<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>formula for cobalt (II) chlorite? The correct answer and explanation is : The correct formula for cobalt(II) chlorite is Co(ClO\u2082)\u2082. Explanation: Why Parentheses? Verification of Charge Balance: Common Mistakes to Avoid: Applications of Cobalt(II) Chlorite: While cobalt(II) chlorite is not very common, cobalt compounds are used in batteries, pigments, and catalysts. Chlorite compounds, in general, [&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-201067","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201067","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=201067"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201067\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=201067"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=201067"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=201067"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}