{"id":263714,"date":"2025-07-21T08:34:26","date_gmt":"2025-07-21T08:34:26","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=263714"},"modified":"2025-07-21T08:34:28","modified_gmt":"2025-07-21T08:34:28","slug":"a-so2-b-h2s-c-so4-d-s8-e-scl2-f-sf6-g-fe2so33-h-hso4-i-nh42so4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/21\/a-so2-b-h2s-c-so4-d-s8-e-scl2-f-sf6-g-fe2so33-h-hso4-i-nh42so4\/","title":{"rendered":"(a) SO2 (b) H2S (c) SO4 (d) S8 (e) SCl2 (f) SF6 (g) Fe2(SO3)3 (h) HSO4 (i) (NH4)2SO4"},"content":{"rendered":"\n<p>(a) SO2 (b) H2S (c) SO4 (d) S8 (e) SCl2 (f) SF6 (g) Fe2(SO3)3 (h) HSO4 (i) (NH4)2SO4<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p>To determine the oxidation state of sulfur in each of these compounds, we need to follow the rules for oxidation states:<\/p>\n\n\n\n<ol class=\"wp-block-list\">\n<li>The oxidation state of an atom in a free element is 0.<\/li>\n\n\n\n<li>In compounds, the oxidation state of hydrogen is usually +1, and the oxidation state of oxygen is usually -2.<\/li>\n\n\n\n<li>The sum of oxidation states in a neutral compound is zero, and the sum in a polyatomic ion is equal to the charge of the ion.<\/li>\n<\/ol>\n\n\n\n<p>Let&#8217;s apply these rules to each compound:<\/p>\n\n\n\n<p><strong>(a) SO2 (Sulfur Dioxide):<\/strong><br>In SO2, oxygen is assigned an oxidation state of -2. Since there are two oxygens, the total contribution from oxygen is -4. The compound is neutral, so the oxidation state of sulfur must balance this, giving sulfur an oxidation state of +4.<\/p>\n\n\n\n<p><strong>(b) H2S (Hydrogen Sulfide):<\/strong><br>In H2S, hydrogen has an oxidation state of +1. Since there are two hydrogens, the total contribution from hydrogen is +2. The compound is neutral, so the oxidation state of sulfur must balance this, giving sulfur an oxidation state of -2.<\/p>\n\n\n\n<p><strong>(c) SO4^2- (Sulfate Ion):<\/strong><br>In the sulfate ion (SO4^2-), oxygen is assigned an oxidation state of -2. Since there are four oxygens, the total contribution from oxygen is -8. The ion has a -2 charge, so the oxidation state of sulfur must be +6 to balance this charge.<\/p>\n\n\n\n<p><strong>(d) S8 (Sulfur Molecule):<\/strong><br>In S8, sulfur is in its elemental form, so the oxidation state of sulfur is 0.<\/p>\n\n\n\n<p><strong>(e) SCl2 (Sulfur Dichloride):<\/strong><br>In SCl2, chlorine has an oxidation state of -1. Since there are two chlorines, the total contribution from chlorine is -2. The compound is neutral, so the oxidation state of sulfur must be +2 to balance this.<\/p>\n\n\n\n<p><strong>(f) SF6 (Sulfur Hexafluoride):<\/strong><br>In SF6, fluorine has an oxidation state of -1. Since there are six fluorines, the total contribution from fluorine is -6. The compound is neutral, so the oxidation state of sulfur must be +6 to balance this.<\/p>\n\n\n\n<p><strong>(g) Fe2(SO3)3 (Iron(III) Sulfite):<\/strong><br>In Fe2(SO3)3, each sulfite ion (SO3^2-) has a charge of -2. The total charge of the sulfite ions is -6. The two iron ions must balance this charge, so each iron has an oxidation state of +3. In each sulfite ion, sulfur must have an oxidation state of +4 (since oxygen contributes -6, and the total charge is -2).<\/p>\n\n\n\n<p><strong>(h) HSO4^- (Hydrogen Sulfate Ion):<\/strong><br>In HSO4^-, hydrogen has an oxidation state of +1, and oxygen has an oxidation state of -2. Since there are four oxygens, the total contribution from oxygen is -8. The ion has a -1 charge, so the oxidation state of sulfur must be +6 to balance the charge.<\/p>\n\n\n\n<p><strong>(i) (NH4)2SO4 (Ammonium Sulfate):<\/strong><br>In (NH4)2SO4, the ammonium ion (NH4+) has a charge of +1, so two ammonium ions contribute a total of +2. The sulfate ion (SO4^2-) has a charge of -2. Therefore, the oxidation state of sulfur in the sulfate ion is +6.<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Summary of Oxidation States:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>SO2:<\/strong> +4<\/li>\n\n\n\n<li><strong>H2S:<\/strong> -2<\/li>\n\n\n\n<li><strong>SO4^2-:<\/strong> +6<\/li>\n\n\n\n<li><strong>S8:<\/strong> 0<\/li>\n\n\n\n<li><strong>SCl2:<\/strong> +2<\/li>\n\n\n\n<li><strong>SF6:<\/strong> +6<\/li>\n\n\n\n<li><strong>Fe2(SO3)3:<\/strong> +4<\/li>\n\n\n\n<li><strong>HSO4-:<\/strong> +6<\/li>\n\n\n\n<li><strong>(NH4)2SO4:<\/strong> +6<\/li>\n<\/ul>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-1321.jpeg\" alt=\"\" class=\"wp-image-263718\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>(a) SO2 (b) H2S (c) SO4 (d) S8 (e) SCl2 (f) SF6 (g) Fe2(SO3)3 (h) HSO4 (i) (NH4)2SO4 The Correct Answer and Explanation is: To determine the oxidation state of sulfur in each of these compounds, we need to follow the rules for oxidation states: Let&#8217;s apply these rules to each compound: (a) SO2 (Sulfur [&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 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