{"id":155361,"date":"2024-10-16T05:19:31","date_gmt":"2024-10-16T05:19:31","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=155361"},"modified":"2024-10-16T05:19:34","modified_gmt":"2024-10-16T05:19:34","slug":"what-is-the-formula-for-cobaltiii-sulfide","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/10\/16\/what-is-the-formula-for-cobaltiii-sulfide\/","title":{"rendered":"What is the formula for cobalt(III) sulfide"},"content":{"rendered":"\n<p>What is the formula for cobalt(III) sulfide?<br>a. Co3S<br>b. CoS3<br>c. Co2S3<br>d. Cu2S3<\/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(III) sulfide is <strong>c. Co\u2082S\u2083<\/strong>.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<p>Cobalt(III) sulfide is a compound formed from cobalt ions in the +3 oxidation state and sulfide ions. To derive the correct formula, we need to consider the charges of the ions involved.<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Understanding Ion Charges<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Cobalt (Co) can exist in several oxidation states, including +2 and +3. In cobalt(III) sulfide, cobalt is in the +3 oxidation state (Co\u00b3\u207a).<\/li>\n\n\n\n<li>Sulfide (S) has a charge of -2 (S\u00b2\u207b).<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Balancing the Charges<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>To form a neutral compound, the total positive charge must equal the total negative charge. Since cobalt is +3, we need to determine how many cobalt ions are required to balance the charge of sulfide ions.<\/li>\n\n\n\n<li>Each sulfide ion has a charge of -2. If we have three sulfide ions (3 \u00d7 -2 = -6), we will need enough cobalt ions to balance this charge.<\/li>\n\n\n\n<li>To balance the -6 charge from the three sulfide ions, we need two cobalt ions (2 \u00d7 +3 = +6).<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Constructing the Formula<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>With two cobalt ions (Co\u00b2\u207a) and three sulfide ions (S\u00b2\u207b), we can write the empirical formula for cobalt(III) sulfide as Co\u2082S\u2083.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Why the Other Options Are Incorrect<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>a. Co\u2083S<\/strong>: This suggests three cobalt ions and one sulfide ion, which would lead to an overall charge of +9, not balanced.<\/li>\n\n\n\n<li><strong>b. CoS\u2083<\/strong>: This indicates one cobalt ion and three sulfide ions, leading to an unbalanced +3 to -6 charge.<\/li>\n\n\n\n<li><strong>d. Cu\u2082S\u2083<\/strong>: This is incorrect as it suggests copper (Cu) rather than cobalt (Co).<\/li>\n<\/ul>\n\n\n\n<p>In summary, cobalt(III) sulfide is correctly represented by the formula Co\u2082S\u2083, which accurately reflects the charges and composition of the compound.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>What is the formula for cobalt(III) sulfide?a. Co3Sb. CoS3c. Co2S3d. Cu2S3 The Correct Answer and Explanation is : The correct formula for cobalt(III) sulfide is c. Co\u2082S\u2083. Explanation: Cobalt(III) sulfide is a compound formed from cobalt ions in the +3 oxidation state and sulfide ions. To derive the correct formula, we need to consider the [&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-155361","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/155361","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=155361"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/155361\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=155361"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=155361"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=155361"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}