{"id":199206,"date":"2025-03-10T20:18:09","date_gmt":"2025-03-10T20:18:09","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=199206"},"modified":"2025-03-10T20:18:11","modified_gmt":"2025-03-10T20:18:11","slug":"what-is-the-molecular-geometry-of-ses2","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/10\/what-is-the-molecular-geometry-of-ses2\/","title":{"rendered":"\u00a0What is the Molecular Geometry of SeS2"},"content":{"rendered":"\n

\u00a0What is the Molecular Geometry of SeS2<\/sub><\/p>\n\n\n\n

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

Molecular Geometry of SeS\u2082<\/strong> (Selenium Disulfide)<\/h3>\n\n\n\n

The molecular geometry of SeS\u2082<\/strong> is Bent (V-shaped)<\/strong>.<\/p>\n\n\n\n

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

To determine the molecular geometry of SeS\u2082<\/strong>, we follow VSEPR (Valence Shell Electron Pair Repulsion) theory<\/strong>, which helps predict the shape of molecules based on electron repulsion.<\/p>\n\n\n\n

    \n
  1. Determine the Lewis Structure:<\/strong><\/li>\n<\/ol>\n\n\n\n
      \n
    • Selenium (Se<\/strong>) is the central atom because it is less electronegative than sulfur (S<\/strong>).<\/li>\n\n\n\n
    • Selenium has 6 valence electrons<\/strong>, and each sulfur (S)<\/strong> atom contributes 6 valence electrons<\/strong> (since sulfur belongs to group 16 of the periodic table).<\/li>\n\n\n\n
    • Two sulfur atoms form single bonds<\/strong> with selenium, using 2 electron pairs<\/strong> (one for each bond).<\/li>\n\n\n\n
    • After bonding, selenium has two lone pairs<\/strong> of electrons remaining.<\/li>\n<\/ul>\n\n\n\n
        \n
      1. Find the Steric Number (Electron Domains Around the Central Atom):<\/strong><\/li>\n<\/ol>\n\n\n\n
          \n
        • Selenium has two bonding pairs<\/strong> (Se\u2013S bonds) and two lone pairs<\/strong> of electrons.<\/li>\n\n\n\n
        • The total steric number is 4<\/strong> (2 bonding pairs + 2 lone pairs).<\/li>\n<\/ul>\n\n\n\n
            \n
          1. Predict the Molecular Shape Using VSEPR Theory:<\/strong><\/li>\n<\/ol>\n\n\n\n
              \n
            • A steric number of 4<\/strong> typically leads to a tetrahedral electron geometry<\/strong> if there are no lone pairs.<\/li>\n\n\n\n
            • However, two lone pairs<\/strong> of electrons exert strong repulsion, which pushes the sulfur atoms downward, creating a bent shape<\/strong>.<\/li>\n\n\n\n
            • This is similar to H\u2082O (water), which also has a bent shape due to lone pair repulsion<\/strong>.<\/li>\n<\/ul>\n\n\n\n
                \n
              1. Bond Angles:<\/strong><\/li>\n<\/ol>\n\n\n\n
                  \n
                • The ideal bond angle for a tetrahedral arrangement is 109.5\u00b0<\/strong>, but due to lone pair repulsion<\/strong>, the angle decreases<\/strong>, typically around ~105\u00b0 to 110\u00b0<\/strong>.<\/li>\n<\/ul>\n\n\n\n

                  Final Answer:<\/h3>\n\n\n\n
                    \n
                  • Molecular Geometry:<\/strong> Bent (V-shaped)<\/strong><\/li>\n\n\n\n
                  • Electron Geometry:<\/strong> Tetrahedral<\/strong><\/li>\n\n\n\n
                  • Bond Angle:<\/strong> ~105\u00b0 – 110\u00b0<\/strong><\/li>\n\n\n\n
                  • Reason:<\/strong> Lone pair repulsions cause a deviation from linear geometry.<\/strong><\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"

                    \u00a0What is the Molecular Geometry of SeS2 The correct answer and explanation is : Molecular Geometry of SeS\u2082 (Selenium Disulfide) The molecular geometry of SeS\u2082 is Bent (V-shaped). Explanation: To determine the molecular geometry of SeS\u2082, we follow VSEPR (Valence Shell Electron Pair Repulsion) theory, which helps predict the shape of molecules based on electron […]<\/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-199206","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199206","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=199206"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/199206\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=199206"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=199206"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=199206"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}