{"id":196618,"date":"2025-03-05T16:46:24","date_gmt":"2025-03-05T16:46:24","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=196618"},"modified":"2025-03-05T16:46:27","modified_gmt":"2025-03-05T16:46:27","slug":"the-bond-angles-in-h2o2-are-approximately","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/05\/the-bond-angles-in-h2o2-are-approximately\/","title":{"rendered":"The bond angles in H2O2 are approximately"},"content":{"rendered":"\n

The bond angles in H2O2 are approximately:
A. 90\u00b0
B. 105\u00b0
C. 109.5\u00b0
D. 120\u00b0
\u0395. 180\u00b0<\/p>\n\n\n\n

The correct answer and explanation is :<\/strong><\/mark><\/p>\n\n\n\n

The correct answer is C. 109.5\u00b0<\/strong>.<\/p>\n\n\n\n

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

Hydrogen peroxide (H\u2082O\u2082<\/strong>) has a non-linear, skewed or “open book”<\/strong> structure due to its molecular geometry and the presence of lone pairs on the oxygen atoms.<\/p>\n\n\n\n

1. Molecular Structure of H\u2082O\u2082:<\/strong><\/h4>\n\n\n\n
    \n
  • Hydrogen peroxide consists of two oxygen atoms<\/strong> connected by a single bond (O\u2013O)<\/strong>, with each oxygen atom also bonded to a hydrogen atom<\/strong>.<\/li>\n\n\n\n
  • The structure exhibits hydrogen bonding<\/strong> and a non-planar arrangement.<\/li>\n\n\n\n
  • The O\u2013O bond is not linear<\/strong> due to repulsions from lone pairs on oxygen.<\/li>\n<\/ul>\n\n\n\n

    2. Hybridization and Bond Angles:<\/strong><\/h4>\n\n\n\n
      \n
    • Each oxygen atom in H\u2082O\u2082<\/strong> is sp\u00b3 hybridized<\/strong>. This is similar to water (H\u2082O<\/strong>), which has an ideal tetrahedral<\/strong> geometry.<\/li>\n\n\n\n
    • Due to the lone pairs on oxygen, the actual bond angle is slightly less than the tetrahedral angle of 109.5\u00b0<\/strong> but close to it.<\/li>\n<\/ul>\n\n\n\n

      3. Influence of Lone Pairs:<\/strong><\/h4>\n\n\n\n
        \n
      • Lone pairs exert greater repulsion<\/strong> than bonding pairs, causing a deviation from the perfect tetrahedral angle.<\/li>\n\n\n\n
      • The O\u2013H bonds are bent due to these repulsions.<\/li>\n<\/ul>\n\n\n\n

        4. Observed Bond Angle:<\/strong><\/h4>\n\n\n\n
          \n
        • The experimentally determined H\u2013O\u2013O bond angle<\/strong> in H\u2082O\u2082 is approximately 111.5\u00b0 in the gas phase<\/strong>, close to the ideal tetrahedral value of 109.5\u00b0<\/strong>.<\/li>\n\n\n\n
        • This makes option C (109.5\u00b0) the closest approximation<\/strong>.<\/li>\n<\/ul>\n\n\n\n

          Conclusion:<\/strong><\/h4>\n\n\n\n

          H\u2082O\u2082 has a bent, skewed structure<\/strong> due to lone pair repulsions and sp\u00b3 hybridization<\/strong>, leading to a bond angle near 109.5\u00b0<\/strong>.<\/p>\n\n\n\n

          Now, I’ll generate an image of the molecular structure.<\/p>\n\n\n\n

          \"\"<\/figure>\n\n\n\n

          Here is the 3D molecular structure of hydrogen peroxide (H\u2082O\u2082<\/strong>), showing its skewed or “open book” shape with a bond angle close to 109.5\u00b0<\/strong>. <\/p>\n","protected":false},"excerpt":{"rendered":"

          The bond angles in H2O2 are approximately:A. 90\u00b0B. 105\u00b0C. 109.5\u00b0D. 120\u00b0\u0395. 180\u00b0 The correct answer and explanation is : The correct answer is C. 109.5\u00b0. Explanation: Hydrogen peroxide (H\u2082O\u2082) has a non-linear, skewed or “open book” structure due to its molecular geometry and the presence of lone pairs on the oxygen atoms. 1. Molecular Structure […]<\/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-196618","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196618","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=196618"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/196618\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=196618"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=196618"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=196618"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}