{"id":201111,"date":"2025-03-15T02:47:36","date_gmt":"2025-03-15T02:47:36","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=201111"},"modified":"2025-03-15T02:47:38","modified_gmt":"2025-03-15T02:47:38","slug":"consider-the-azide-ion-n3-1","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/03\/15\/consider-the-azide-ion-n3-1\/","title":{"rendered":"Consider the\u00a0azide\u00a0ion N3-1"},"content":{"rendered":"\n

Consider the azide<\/strong><\/em> ion N3-1. Its general shape is X-X-X. A number of Lewis structures are possible. Do a Lewis calculation and select the correct statement<\/p>\n\n\n\n

A. All the possible Lewis structures involve an \u201csp2\u201d hybridization for the central atom<\/p>\n\n\n\n

B. Because the central atom lacks a lone pair in the most favorable Lewis structure, the shape of the molecule is linear<\/p>\n\n\n\n

C. There are two Lewis structures with a triple bond that form a resonance pair. They are the best choice for the electronic structure because their formal charges are minimal<\/p>\n\n\n\n

D. All of the above statements are true<\/p>\n\n\n\n

E. None of the above statements are true<\/p>\n\n\n\n

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

The correct answer is:
B. Because the central atom lacks a lone pair in the most favorable Lewis structure, the shape of the molecule is linear.<\/strong><\/p>\n\n\n\n

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

The azide ion (N3\u2212N_3^-) consists of three nitrogen atoms in a linear arrangement. To determine the best Lewis structures, we follow these steps:<\/p>\n\n\n\n

    \n
  1. Calculate the total valence electrons<\/strong>\n
      \n
    • Each nitrogen atom has 5 valence electrons<\/strong>.<\/li>\n\n\n\n
    • The negative charge (\u22121-1) adds one extra electron<\/strong>.<\/li>\n\n\n\n
    • Total electrons:<\/strong> 3\u00d75+1=163 \\times 5 + 1 = 16 valence electrons.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
    • Draw possible structures<\/strong>
      Possible Lewis structures include different arrangements of single, double, and triple bonds while maintaining the octet rule. The most favorable resonance structures involve the following:
      • Structure 1:<\/strong> \\ce[N\u2261N\u2212N]\u2212\\ce{[N\u2261N-N]^-}<\/li>
      • Structure 2:<\/strong> \\ce[N=N\u2261N]\u2212\\ce{[N=N\u2261N]^-}<\/li><\/ul>These structures involve one triple bond and one single bond or one double bond on either side<\/strong>, allowing resonance.<\/li>\n\n\n\n
      • Determine formal charges<\/strong>
        The best Lewis structures minimize formal charges, calculated as: Formal\u00a0charge=valence\u00a0electrons\u2212lone\u00a0pairs\u2212bonding\u00a0electrons2\\text{Formal charge} = \\text{valence electrons} – \\text{lone pairs} – \\frac{\\text{bonding electrons}}{2} The most stable resonance structure has formal charges of 0,+1,\u221210, +1, -1, rather than extreme charges like \u22122-2 or +2+2.<\/li>\n\n\n\n
      • Molecular shape and hybridization<\/strong>\n
          \n
        • The central nitrogen atom (N)<\/strong> forms two double bonds in resonance and lacks lone pairs.<\/li>\n\n\n\n
        • Since it is surrounded by two atoms and no lone pairs, it adopts a linear geometry (180\u00b0 bond angle)<\/strong>.<\/li>\n\n\n\n
        • The central atom is sp-hybridized<\/strong>, not sp\u00b2<\/strong>, making option A incorrect<\/strong>.<\/li>\n<\/ul>\n<\/li>\n\n\n\n
        • Why option C is incorrect<\/strong>\n
            \n
          • The best resonance forms do not<\/strong> both have a triple bond.<\/li>\n\n\n\n
          • There is one triple bond in each resonance structure, but not in both simultaneously.<\/li>\n<\/ul>\n<\/li>\n<\/ol>\n\n\n\n

            Since only option B is correct<\/strong>, the correct choice is B<\/strong>.<\/p>\n\n\n\n

            Now, generating the Lewis structure image.<\/p>\n\n\n\n

            Here is the detailed diagram of the Lewis structure for the azide ion (N3\u2212N_3^-), including resonance structures, lone pairs, formal charges, and bond types. Let me know if you need any modifications or further explanations!<\/p>\n\n\n\n

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

            Consider the azide ion N3-1. Its general shape is X-X-X. A number of Lewis structures are possible. Do a Lewis calculation and select the correct statement A. All the possible Lewis structures involve an \u201csp2\u201d hybridization for the central atom B. Because the central atom lacks a lone pair in the most favorable Lewis structure, the shape […]<\/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-201111","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201111","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=201111"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/201111\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=201111"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=201111"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=201111"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}