{"id":183361,"date":"2025-01-16T08:24:16","date_gmt":"2025-01-16T08:24:16","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=183361"},"modified":"2025-01-16T08:24:29","modified_gmt":"2025-01-16T08:24:29","slug":"chemical-formula-name-of-chemical-formula","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/01\/16\/chemical-formula-name-of-chemical-formula\/","title":{"rendered":"Chemical formula: Name of chemical formula"},"content":{"rendered":"\n<p>L . BF4 \u2022 Chemical formula: Name of chemical formula: \u2022 Total number of valence electrons: \u2022 Lewis dot structure: \u2022 Calculate formal charges: \u2022 VSEPR Electron Pair Geometry: \u2022 Molecular Geometry: \u2022 Polar or Non-polar: \u2022 Hybridization of the central atom(s): \u2022 Resonance structures when applicable: I XeF \u2022 Chemical formula: \u2022 Name of chemical formula: \u2022 Total number of valence electrons: \u2022 Lewis dot structure: \u2022 Calculate formal charges: \u2022 VSEPR Electron Pair Geometry: \u2022 Molecular Geometry: \u2022 Polar or Non-polar: \u2022 Hybridization of the central atom(s); \u2022 Resonance structures when applicable: . HO* Chemical formula: Name of chemical formula: Total number of valence electrons: Lewis dot structure: Calculate formal charges \u2022 VSEPR Electron Pair Geometry: Molecular Geometry: Polar or Non-polar \u2022 Hybridization of the central atom(s); Resonance structures when applicable: . . .<\/p>\n\n\n\n<p><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-6-color\"><strong>The Correct Answer and Explanation is :<\/strong><\/mark><\/p>\n\n\n\n<p>Here&#8217;s the detailed breakdown of the given compounds:<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>1. BF\u2084\u207b<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Chemical Formula:<\/strong> BF\u2084\u207b<\/li>\n\n\n\n<li><strong>Name of Chemical Formula:<\/strong> Tetrafluoroborate ion<\/li>\n\n\n\n<li><strong>Total Number of Valence Electrons:<\/strong><br>Boron (B): 3, Fluorine (F): 7 \u00d7 4 = 28, Additional electron for the negative charge: +1<br><strong>Total = 32 electrons<\/strong><\/li>\n\n\n\n<li><strong>Lewis Dot Structure:<\/strong><br>Boron is the central atom bonded to four fluorine atoms. Each fluorine has three lone pairs, and all single bonds form a complete octet for fluorine and boron.<\/li>\n\n\n\n<li><strong>Formal Charges:<\/strong><br>All atoms have a formal charge of 0 since boron shares four electrons and fluorine achieves octet.<\/li>\n\n\n\n<li><strong>VSEPR Electron Pair Geometry:<\/strong> Tetrahedral<\/li>\n\n\n\n<li><strong>Molecular Geometry:<\/strong> Tetrahedral<\/li>\n\n\n\n<li><strong>Polar or Non-Polar:<\/strong> Non-polar (symmetrical charge distribution)<\/li>\n\n\n\n<li><strong>Hybridization of the Central Atom:<\/strong> sp\u00b3<\/li>\n\n\n\n<li><strong>Resonance Structures:<\/strong> Not applicable (single, stable structure)<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>2. XeF\u2082<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Chemical Formula:<\/strong> XeF\u2082<\/li>\n\n\n\n<li><strong>Name of Chemical Formula:<\/strong> Xenon difluoride<\/li>\n\n\n\n<li><strong>Total Number of Valence Electrons:<\/strong><br>Xenon (Xe): 8, Fluorine (F): 7 \u00d7 2 = 14<br><strong>Total = 22 electrons<\/strong><\/li>\n\n\n\n<li><strong>Lewis Dot Structure:<\/strong><br>Xenon is the central atom with two single bonds to fluorine. Xenon also has three lone pairs.<\/li>\n\n\n\n<li><strong>Formal Charges:<\/strong><br>All atoms have a formal charge of 0.<\/li>\n\n\n\n<li><strong>VSEPR Electron Pair Geometry:<\/strong> Trigonal bipyramidal (five regions of electron density)<\/li>\n\n\n\n<li><strong>Molecular Geometry:<\/strong> Linear (lone pairs are equatorial)<\/li>\n\n\n\n<li><strong>Polar or Non-Polar:<\/strong> Non-polar (linear geometry cancels dipole moments)<\/li>\n\n\n\n<li><strong>Hybridization of the Central Atom:<\/strong> sp\u00b3d<\/li>\n\n\n\n<li><strong>Resonance Structures:<\/strong> Not applicable<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\"><strong>3. H\u2082O<\/strong><\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Chemical Formula:<\/strong> H\u2082O<\/li>\n\n\n\n<li><strong>Name of Chemical Formula:<\/strong> Water<\/li>\n\n\n\n<li><strong>Total Number of Valence Electrons:<\/strong><br>Hydrogen (H): 1 \u00d7 2 = 2, Oxygen (O): 6<br><strong>Total = 8 electrons<\/strong><\/li>\n\n\n\n<li><strong>Lewis Dot Structure:<\/strong><br>Oxygen is the central atom with two single bonds to hydrogen and two lone pairs.<\/li>\n\n\n\n<li><strong>Formal Charges:<\/strong><br>All atoms have a formal charge of 0.<\/li>\n\n\n\n<li><strong>VSEPR Electron Pair Geometry:<\/strong> Tetrahedral<\/li>\n\n\n\n<li><strong>Molecular Geometry:<\/strong> Bent<\/li>\n\n\n\n<li><strong>Polar or Non-Polar:<\/strong> Polar (asymmetrical charge distribution)<\/li>\n\n\n\n<li><strong>Hybridization of the Central Atom:<\/strong> sp\u00b3<\/li>\n\n\n\n<li><strong>Resonance Structures:<\/strong> Not applicable<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Valence Electrons:<\/strong> Sum of valence electrons of each atom and charge contributions determine the total.<\/li>\n\n\n\n<li><strong>Lewis Dot Structure:<\/strong> Arranged to satisfy octet rules and minimize formal charges.<\/li>\n\n\n\n<li><strong>Formal Charges:<\/strong> Calculated using ( \\text{Formal Charge} = \\text{Valence Electrons} &#8211; (\\text{Lone Electrons} + \\frac{\\text{Bonding Electrons}}{2}) ).<\/li>\n\n\n\n<li><strong>VSEPR Theory:<\/strong> Electron pairs arrange to minimize repulsion, defining geometry.<\/li>\n\n\n\n<li><strong>Polarity:<\/strong> Assessed by geometry and bond dipoles.<\/li>\n\n\n\n<li><strong>Hybridization:<\/strong> Determined by the number of electron regions around the central atom.<\/li>\n<\/ul>\n","protected":false},"excerpt":{"rendered":"<p>L . BF4 \u2022 Chemical formula: Name of chemical formula: \u2022 Total number of valence electrons: \u2022 Lewis dot structure: \u2022 Calculate formal charges: \u2022 VSEPR Electron Pair Geometry: \u2022 Molecular Geometry: \u2022 Polar or Non-polar: \u2022 Hybridization of the central atom(s): \u2022 Resonance structures when applicable: I XeF \u2022 Chemical formula: \u2022 Name of [&hellip;]<\/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-183361","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183361","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=183361"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/183361\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=183361"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=183361"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=183361"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}