{"id":241793,"date":"2025-07-04T03:34:25","date_gmt":"2025-07-04T03:34:25","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=241793"},"modified":"2025-07-04T03:34:27","modified_gmt":"2025-07-04T03:34:27","slug":"identify-the-lewis-base-in-this-balanced-equation","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/07\/04\/identify-the-lewis-base-in-this-balanced-equation\/","title":{"rendered":"Identify the Lewis base in this balanced equation"},"content":{"rendered":"\n

Identify the Lewis base in this balanced equation: B is bonded to F above, below left, and below right. The F’s have pairs of electron dots on the 3 sides that do not have bonds. Plus. A central N has two electron dots to the left and is bonded to H above, below, and to the right. right arrow. B is bonded above, below, and to the left to F’s each with pairs of electron dots on the 3 sides without bonds; and to the right to N, which is bonded above, below, and to the right to H.<\/p>\n\n\n\n

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

In this scenario, we are tasked with identifying the Lewis base in the given chemical reaction. To approach this, let’s first break down the provided details and clarify the nature of a Lewis base.<\/p>\n\n\n\n

A Lewis base<\/strong> is a species that donates a pair of electrons to form a covalent bond with a Lewis acid (an electron pair acceptor).<\/p>\n\n\n\n

Breakdown of the Molecules<\/h3>\n\n\n\n
    \n
  1. First Molecule (Before the Arrow)<\/strong>:\n
      \n
    • B is bonded to F<\/strong>: This suggests that boron (B) is bonded to fluorine (F) atoms. Fluorine, being a halogen, has lone pairs of electrons (three lone pairs in the absence of bonding).<\/li>\n\n\n\n
    • N with electron dots to the left<\/strong>: Nitrogen (N) has two lone pairs of electrons to the left, which may be significant in the reaction.<\/li>\n\n\n\n
    • Hydrogen atoms (H) bonded to N<\/strong>: Nitrogen is bonded to three hydrogen atoms, creating a structure like ammonia (NH3).<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Second Molecule (After the Arrow)<\/strong>:\n
        \n
      • B bonded to F atoms<\/strong>: This structure is similar to the first molecule, with B bonded to F atoms and each F atom having lone pairs of electrons.<\/li>\n\n\n\n
      • N bonded to H<\/strong>: Nitrogen is bonded to H atoms, suggesting a similar bonding arrangement as before.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

        Identifying the Lewis Base<\/h3>\n\n\n\n

        In this context, the Lewis base<\/strong> will be the species donating electrons. Nitrogen (N) in the first molecule<\/strong> has two lone pairs of electrons and is likely to donate these electrons to form a bond with another molecule. Given that nitrogen is bonded to three hydrogens (NH3), it has a lone pair that can be donated, making it a Lewis base.<\/p>\n\n\n\n

        Thus, NH3 (ammonia)<\/strong> is the Lewis base<\/strong>, as it is donating an electron pair to another species (likely a Lewis acid like boron, B, or another acceptor in the reaction).<\/p>\n\n\n\n

        Conclusion<\/h3>\n\n\n\n

        The Lewis base<\/strong> in this reaction is the ammonia molecule (NH3)<\/strong>, where nitrogen donates its lone pair of electrons.<\/p>\n\n\n\n

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

        Identify the Lewis base in this balanced equation: B is bonded to F above, below left, and below right. The F’s have pairs of electron dots on the 3 sides that do not have bonds. Plus. A central N has two electron dots to the left and is bonded to H above, below, and to […]<\/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-241793","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/241793","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=241793"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/241793\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=241793"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=241793"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=241793"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}