{"id":187815,"date":"2025-02-06T07:07:39","date_gmt":"2025-02-06T07:07:39","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=187815"},"modified":"2025-02-06T07:07:41","modified_gmt":"2025-02-06T07:07:41","slug":"the-lewis-diagram-for-geh4-is","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/06\/the-lewis-diagram-for-geh4-is\/","title":{"rendered":"The Lewis diagram for GeH4 is"},"content":{"rendered":"\n

a. The Lewis diagram for GeH4<\/sub>\u00a0is:<\/p>\n\n\n\n

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

The electron-pair geometry around the greaterthanorequalto atom in GeH4 is
There are lone pair(s) around the central atom, so the geometry of GeH4 is b. The Lewis diagram for SCl2 is: <\/p>\n\n\n\n

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


The elect long-pair geometry around the S atom in SCI2 is
There are lone pair(s) around the central atom, so die geometry of SCl2 is<\/p>\n\n\n\n

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

Answers:<\/strong><\/h3>\n\n\n\n

a. GeH\u2084 (Germanium Tetrahydride)<\/strong><\/h4>\n\n\n\n
    \n
  • Electron-pair geometry around the central atom (Ge):<\/strong> Tetrahedral<\/strong><\/li>\n\n\n\n
  • Number of lone pairs on the central atom (Ge):<\/strong> 0<\/strong><\/li>\n\n\n\n
  • Molecular geometry of GeH\u2084:<\/strong> Tetrahedral<\/strong><\/li>\n<\/ul>\n\n\n\n

    b. SCl\u2082 (Sulfur Dichloride)<\/strong><\/h4>\n\n\n\n
      \n
    • Electron-pair geometry around the central atom (S):<\/strong> Tetrahedral<\/strong><\/li>\n\n\n\n
    • Number of lone pairs on the central atom (S):<\/strong> 2<\/strong><\/li>\n\n\n\n
    • Molecular geometry of SCl\u2082:<\/strong> Bent (V-shaped)<\/strong><\/li>\n<\/ul>\n\n\n\n
      \n\n\n\n

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

      The Lewis structures of molecules help determine their electron-pair geometry and molecular shape by considering valence electrons, bonding pairs, and lone pairs.<\/p>\n\n\n\n

      (a) GeH\u2084 – Germanium Tetrahydride<\/strong><\/h4>\n\n\n\n
        \n
      • Germanium (Ge) belongs to Group 14 of the periodic table and has four valence electrons<\/strong>.<\/li>\n\n\n\n
      • Hydrogen (H) atoms each contribute one valence electron<\/strong>.<\/li>\n\n\n\n
      • The total valence electron count<\/strong> is 4 + (4\u00d71) = 8<\/strong>.<\/li>\n\n\n\n
      • Ge forms four single bonds<\/strong> with four hydrogen atoms, using all its valence electrons.<\/li>\n\n\n\n
      • Since there are no lone pairs<\/strong> on the central atom, the electron-pair geometry<\/strong> follows VSEPR theory<\/strong>, which dictates a tetrahedral geometry<\/strong> with bond angles of approximately 109.5\u00b0<\/strong>.<\/li>\n\n\n\n
      • The molecular geometry<\/strong> is also tetrahedral<\/strong> since all electron regions are bonding.<\/li>\n<\/ul>\n\n\n\n

        (b) SCl\u2082 – Sulfur Dichloride<\/strong><\/h4>\n\n\n\n
          \n
        • Sulfur (S) belongs to Group 16 and has six valence electrons<\/strong>.<\/li>\n\n\n\n
        • Each chlorine (Cl) atom has seven valence electrons<\/strong>.<\/li>\n\n\n\n
        • The total valence electron count<\/strong> is 6 + (2\u00d77) = 20<\/strong>.<\/li>\n\n\n\n
        • Sulfur forms two single bonds<\/strong> with chlorine atoms, using four electrons<\/strong>.<\/li>\n\n\n\n
        • The remaining four electrons<\/strong> remain as two lone pairs<\/strong> on sulfur.<\/li>\n\n\n\n
        • According to VSEPR theory<\/strong>, four electron regions (two bonds + two lone pairs) around sulfur adopt a tetrahedral electron-pair geometry<\/strong>.<\/li>\n\n\n\n
        • However, because two of these regions are lone pairs<\/strong>, the molecular geometry is bent (V-shaped)<\/strong>, similar to H\u2082O.<\/li>\n\n\n\n
        • Lone pairs repel more strongly<\/strong> than bonding pairs, reducing the bond angle to around 103\u00b0-105\u00b0<\/strong>.<\/li>\n<\/ul>\n\n\n\n

          Thus, GeH\u2084 has a tetrahedral shape<\/strong>, while SCl\u2082 has a bent shape<\/strong> due to lone pairs on sulfur.<\/p>\n","protected":false},"excerpt":{"rendered":"

          a. The Lewis diagram for GeH4\u00a0is: The electron-pair geometry around the greaterthanorequalto atom in GeH4 isThere are lone pair(s) around the central atom, so the geometry of GeH4 is b. The Lewis diagram for SCl2 is: The elect long-pair geometry around the S atom in SCI2 isThere are lone pair(s) around the central atom, so […]<\/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-187815","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187815","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=187815"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/187815\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=187815"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=187815"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=187815"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}