{"id":167021,"date":"2024-11-14T17:56:40","date_gmt":"2024-11-14T17:56:40","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=167021"},"modified":"2024-11-14T17:56:43","modified_gmt":"2024-11-14T17:56:43","slug":"which-of-the-following-species-is-the-best-oxidizing-agent-and-which-of-the-best-reducing-agent-fe-fe2-cu-zn","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2024\/11\/14\/which-of-the-following-species-is-the-best-oxidizing-agent-and-which-of-the-best-reducing-agent-fe-fe2-cu-zn\/","title":{"rendered":"Which of the following species is the best oxidizing agent and which of the best reducing agent fe, fe2 , cu , zn"},"content":{"rendered":"\n<p>Which of the following species is the best oxidizing agent and which of the best reducing agent fe, fe2 , cu , zn<\/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>To determine the best oxidizing and reducing agents from the list (Fe, Fe\u00b2\u207a, Cu, Zn), we need to understand the concepts of oxidizing and reducing agents in terms of electron transfer.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Oxidizing Agent:<\/h3>\n\n\n\n<p>An <strong>oxidizing agent<\/strong> is a substance that gains electrons in a chemical reaction, causing another substance to be oxidized (lose electrons). The strength of an oxidizing agent is determined by its ability to accept electrons.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Reducing Agent:<\/h3>\n\n\n\n<p>A <strong>reducing agent<\/strong> is a substance that loses electrons, thereby causing another substance to be reduced (gain electrons). The strength of a reducing agent is determined by its ability to donate electrons.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Fe (Iron, Fe)<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Iron can exist in two common oxidation states: Fe\u00b2\u207a and Fe\u00b3\u207a. In its elemental form (Fe), it is in the lowest oxidation state and would be more likely to lose electrons (oxidize) to form Fe\u00b2\u207a or Fe\u00b3\u207a.<\/li>\n\n\n\n<li><strong>Fe is a better reducing agent<\/strong> because it readily loses electrons to form Fe\u00b2\u207a (and possibly Fe\u00b3\u207a), meaning it has a strong tendency to be oxidized.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Fe\u00b2\u207a (Iron(II) ion)<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Fe\u00b2\u207a can be oxidized to Fe\u00b3\u207a, meaning it can lose electrons. Fe\u00b2\u207a is thus a <strong>reducing agent<\/strong>.<\/li>\n\n\n\n<li>In the context of oxidation states, Fe\u00b2\u207a is a <strong>moderate reducing agent<\/strong> because it is more readily oxidized to Fe\u00b3\u207a than Fe is to Fe\u00b2\u207a.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Cu (Copper)<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Copper exists mainly in the +2 oxidation state (Cu\u00b2\u207a), but it can also exist in the +1 state (Cu\u207a). Cu is known to be a relatively <strong>poor reducing agent<\/strong>, as it does not easily lose electrons compared to Fe.<\/li>\n\n\n\n<li><strong>Cu\u00b2\u207a is a better oxidizing agent<\/strong> because it can easily accept electrons and reduce to Cu.<\/li>\n<\/ul>\n\n\n\n<ol class=\"wp-block-list\">\n<li><strong>Zn (Zinc)<\/strong>:<\/li>\n<\/ol>\n\n\n\n<ul class=\"wp-block-list\">\n<li>Zinc in its elemental form is a <strong>good reducing agent<\/strong> because it readily loses electrons to form Zn\u00b2\u207a.<\/li>\n\n\n\n<li><strong>Zn is a better reducing agent<\/strong> than Fe, as it has a stronger tendency to lose electrons to form Zn\u00b2\u207a.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Best Oxidizing Agent:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Cu\u00b2\u207a<\/strong> is the best oxidizing agent in this case, as it readily accepts electrons to be reduced to Cu.<\/li>\n<\/ul>\n\n\n\n<h3 class=\"wp-block-heading\">Best Reducing Agent:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Zn<\/strong> is the best reducing agent because it has the strongest tendency to lose electrons and form Zn\u00b2\u207a.<\/li>\n<\/ul>\n\n\n\n<p>Thus, the best <strong>oxidizing agent<\/strong> is <strong>Cu\u00b2\u207a<\/strong>, and the best <strong>reducing agent<\/strong> is <strong>Zn<\/strong>.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Which of the following species is the best oxidizing agent and which of the best reducing agent fe, fe2 , cu , zn The Correct Answer and Explanation is: To determine the best oxidizing and reducing agents from the list (Fe, Fe\u00b2\u207a, Cu, Zn), we need to understand the concepts of oxidizing and reducing agents [&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-167021","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/167021","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=167021"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/167021\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=167021"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=167021"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=167021"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}