{"id":195518,"date":"2025-02-28T10:35:11","date_gmt":"2025-02-28T10:35:11","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=195518"},"modified":"2025-02-28T10:35:13","modified_gmt":"2025-02-28T10:35:13","slug":"molecular-formula-fcn","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/28\/molecular-formula-fcn\/","title":{"rendered":"Molecular formula FCN"},"content":{"rendered":"\n
Molecular formula FCN (a) Draw the Lewis structure (b) Formal charge of C (c) Polar or nonpolar<\/p>\n\n\n\n
The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n
(a) Lewis Structure of FCN (Fluorocyanide)<\/strong><\/h3>\n\n\n\n
Carbon is the central atom (it is the least electronegative except for hydrogen).<\/li>\n\n\n\n
Carbon forms a single bond with fluorine (F)<\/strong> and a triple bond with nitrogen (N)<\/strong> to satisfy the octet rule.<\/li>\n<\/ul>\n\n\n\n\n
Carbon follows the octet rule with four bonds (one with fluorine, three with nitrogen)<\/strong>.<\/li>\n\n\n\n
Nitrogen gets a lone pair to complete its octet.<\/li>\n\n\n\n
Fluorine gets three lone pairs to complete its octet.<\/li>\n<\/ul>\n\n\n\n
The correct Lewis structure<\/strong> has F\u2014C\u2261N<\/strong>, where:<\/p>\n\n\n\n
\n
A single bond<\/strong> exists between C and F<\/strong>.<\/li>\n\n\n\n
A triple bond<\/strong> exists between C and N<\/strong>.<\/li>\n\n\n\n
Lone pairs<\/strong> are present on F<\/strong> and N<\/strong>.<\/li>\n<\/ul>\n\n\n\n\n\n\n\n
(b) Formal Charge on Carbon<\/strong><\/h3>\n\n\n\n
The formal charge is calculated as: [ \\text{Formal Charge} = \\text{Valence Electrons} – \\text{Nonbonding Electrons} – \\frac{\\text{Bonding Electrons}}{2} ]<\/p>\n\n\n\n
For Carbon (C)<\/strong> in FCN:<\/p>\n\n\n\n
\n
Valence electrons: 4<\/strong><\/li>\n\n\n\n
Nonbonding electrons: 0<\/strong><\/li>\n\n\n\n
Bonding electrons: 8<\/strong> (one single bond with F = 2, one triple bond with N = 6) [ 4 – 0 – \\frac{8}{2} = 4 – 4 = 0 ] Thus, the formal charge on Carbon is 0<\/strong>.<\/li>\n<\/ul>\n\n\n\n\n\n\n\n
(c) Polarity: Polar or Nonpolar?<\/strong><\/h3>\n\n\n\n
FCN is a polar molecule.<\/strong><\/p>\n\n\n\n
\n
Reasoning:<\/strong><\/li>\n\n\n\n
The molecule is linear (F\u2014C\u2261N<\/strong>), but the atoms have different electronegativities<\/strong>:\n
The C\u2013F<\/strong> bond is highly polar<\/strong>, pulling electrons towards fluorine.<\/li>\n\n\n\n
The C\u2261N<\/strong> bond is also polar, but less so than C\u2013F.<\/li>\n\n\n\n
Since fluorine is much more electronegative than nitrogen, the molecule has a net dipole moment<\/strong>, making it polar<\/strong>.<\/li>\n<\/ul>\n\n\n\n\n\n\n\n
Conclusion<\/strong><\/h3>\n\n\n\n
\n
Lewis Structure:<\/strong> F\u2014C\u2261N<\/strong><\/li>\n\n\n\n
Formal Charge of Carbon:<\/strong> 0<\/strong><\/li>\n\n\n\n
Polarity:<\/strong> Polar molecule<\/strong> due to electronegativity differences and molecular dipole.<\/li>\n<\/ul>\n\n\n\n
Now, I’ll generate the image of the Lewis structure<\/strong> for FCN.<\/p>\n\n\n\n<\/figure>\n\n\n\n
Here is the Lewis structure diagram for the FCN (fluorocyanide) molecule. Let me know if you need any modifications or further explanations!<\/p>\n","protected":false},"excerpt":{"rendered":"
Molecular formula FCN(a) Draw the Lewis structure(b) Formal charge of C(c) Polar or nonpolar The Correct Answer and Explanation is : (a) Lewis Structure of FCN (Fluorocyanide) To draw the Lewis structure of FCN: The correct Lewis structure has F\u2014C\u2261N, where: (b) Formal Charge on Carbon The formal charge is calculated as:[\\text{Formal Charge} = \\text{Valence […]<\/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-195518","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/195518","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=195518"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/195518\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=195518"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=195518"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=195518"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
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