{"id":246160,"date":"2025-07-07T02:47:45","date_gmt":"2025-07-07T02:47:45","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=246160"},"modified":"2025-07-07T02:47:49","modified_gmt":"2025-07-07T02:47:49","slug":"what-is-the-oxidation-state-for-n-in-no2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/07\/what-is-the-oxidation-state-for-n-in-no2\/","title":{"rendered":"What is the oxidation state for N in NO2"},"content":{"rendered":"\n

What is the oxidation state for N in NO2<\/p>\n\n\n\n

The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n

To find the oxidation state of nitrogen (N) in the compound nitrogen dioxide (NO\u2082), we need to follow the general rules for assigning oxidation states:<\/p>\n\n\n\n

    \n
  1. Oxidation state of oxygen<\/strong>: Oxygen in most compounds has an oxidation state of -2.<\/li>\n\n\n\n
  2. Oxidation state of nitrogen (N)<\/strong>: This is what we need to determine.<\/li>\n<\/ol>\n\n\n\n

    Let\u2019s break it down:<\/p>\n\n\n\n

    In NO\u2082, there are two oxygen atoms, each with an oxidation state of -2. The total oxidation state for the two oxygen atoms will be:2\u00d7(\u22122)=\u221242 \\times (-2) = -42\u00d7(\u22122)=\u22124<\/p>\n\n\n\n

    Now, the sum of the oxidation states of all atoms in a neutral compound must equal zero. Therefore, the oxidation state of nitrogen (x) must balance the total oxidation state of the oxygen atoms to make the overall charge of the molecule zero. This gives us the following equation:x+(\u22124)=0x + (-4) = 0x+(\u22124)=0<\/p>\n\n\n\n

    Solving for xxx:x=+4x = +4x=+4<\/p>\n\n\n\n

    So, the oxidation state of nitrogen in NO\u2082 is +4.<\/p>\n\n\n\n

    Explanation:<\/h3>\n\n\n\n

    The oxidation state of an atom represents the hypothetical charge the atom would have if all the bonding electrons were assigned to the more electronegative atom. In this case, oxygen is more electronegative than nitrogen, so each oxygen atom is assigned an oxidation state of -2. The nitrogen atom\u2019s oxidation state balances the oxygen atoms to ensure the compound is neutral. Therefore, nitrogen in NO\u2082 has an oxidation state of +4.<\/p>\n\n\n\n

    This conclusion is consistent with the known behavior of nitrogen in many compounds, where it can exhibit oxidation states ranging from -3 to +5, depending on the bonding environment. In NO\u2082, the nitrogen is in a +4 state, which is typical for nitrogen in compounds with fewer bonds to oxygen, like nitrous oxide (N\u2082O) and nitrogen dioxide (NO\u2082).<\/p>\n\n\n\n

    \"\"<\/figure>\n","protected":false},"excerpt":{"rendered":"

    What is the oxidation state for N in NO2 The Correct Answer and Explanation is: To find the oxidation state of nitrogen (N) in the compound nitrogen dioxide (NO\u2082), we need to follow the general rules for assigning oxidation states: Let\u2019s break it down: In NO\u2082, there are two oxygen atoms, each with an oxidation […]<\/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-246160","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246160","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=246160"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/246160\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=246160"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=246160"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=246160"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}