{"id":207751,"date":"2025-04-25T07:13:31","date_gmt":"2025-04-25T07:13:31","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=207751"},"modified":"2025-04-25T07:13:34","modified_gmt":"2025-04-25T07:13:34","slug":"which-statement-is-false-regarding-the-lewis-structure-for-xef4","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/04\/25\/which-statement-is-false-regarding-the-lewis-structure-for-xef4\/","title":{"rendered":"Which statement is FALSE regarding the Lewis structure for XeF4"},"content":{"rendered":"\n

Which statement is FALSE regarding the Lewis structure for XeF4?
A The formal charge on the central atom is not zero.
B A total of 36 valence electrons are represented.
C The central atom has lone-pair electrons.
D It includes only single bonds.<\/p>\n\n\n\n

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

The FALSE<\/strong> statement regarding the Lewis structure for XeF4 is:<\/p>\n\n\n\n

D. It includes only single bonds.<\/strong><\/p>\n\n\n\n

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

To understand why option D<\/strong> is false, let’s break down the Lewis structure for xenon tetrafluoride (XeF4):<\/p>\n\n\n\n

    \n
  1. XeF4 and its Electron Configuration:<\/strong>
    Xenon (Xe) is a noble gas in group 18, so it has 8 valence electrons. Fluorine (F) is a halogen, and each fluorine atom has 7 valence electrons. XeF4 consists of one xenon atom and four fluorine atoms, so the total number of valence electrons is:<\/li>\n<\/ol>\n\n\n\n
      \n
    • Xe: 8 electrons<\/li>\n\n\n\n
    • 4 \u00d7 F: 4 \u00d7 7 = 28 electrons<\/li>\n\n\n\n
    • Total = 8 + 28 = 36 valence electrons.<\/strong><\/li>\n<\/ul>\n\n\n\n
        \n
      1. Bonds in the Lewis Structure:<\/strong>
        The four fluorine atoms form single bonds with the xenon atom, as fluorine typically forms a single bond with other atoms (due to its 7 valence electrons, which leaves it needing only one more electron to complete its octet). This satisfies the bonding requirements for each fluorine atom.<\/li>\n\n\n\n
      2. Lone Pairs and Formal Charges:<\/strong>
        After forming the single bonds, 32 electrons are used (4 bonds \u00d7 2 electrons per bond), leaving 4 electrons, which are placed as lone pairs on the xenon atom. Xenon, being in period 5, can accommodate more than 8 electrons in its valence shell, and it does so in this case. This gives xenon 2 lone pairs.<\/li>\n\n\n\n
      3. Formal Charges:<\/strong>
        The formal charge on the xenon atom in XeF4 is not zero<\/strong>. Calculating formal charge on xenon involves comparing the number of valence electrons (8) with the number of electrons it “owns” in the Lewis structure. In XeF4, xenon is surrounded by 4 bonding pairs and 2 lone pairs. The resulting formal charge on xenon is typically +2<\/strong>, which is nonzero.<\/li>\n<\/ol>\n\n\n\n

        Why is D False?<\/h3>\n\n\n\n

        Option D<\/strong> suggests that XeF4 contains only single bonds, but this is misleading because while each fluorine forms a single bond with xenon, XeF4 includes lone pairs on xenon<\/strong>, not only single bonds. This is a more nuanced feature of the structure and is essential for its correct representation.<\/p>\n\n\n\n

        In summary, D<\/strong> is false because the statement oversimplifies the structure, ignoring the presence of lone pairs on xenon.<\/p>\n","protected":false},"excerpt":{"rendered":"

        Which statement is FALSE regarding the Lewis structure for XeF4?A The formal charge on the central atom is not zero.B A total of 36 valence electrons are represented.C The central atom has lone-pair electrons.D It includes only single bonds. The correct answer and explanation is : The FALSE statement regarding the Lewis structure for XeF4 […]<\/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-207751","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/207751","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=207751"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/207751\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=207751"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=207751"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=207751"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}