{"id":188647,"date":"2025-02-07T07:36:16","date_gmt":"2025-02-07T07:36:16","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=188647"},"modified":"2025-02-07T07:36:18","modified_gmt":"2025-02-07T07:36:18","slug":"given-a-list-of-compounds","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/02\/07\/given-a-list-of-compounds\/","title":{"rendered":"Given a list of compounds"},"content":{"rendered":"\n<p>Given a list of compounds, show the following:<br>a) General Formula, i.e., AX3E;<br>b) Lewis structure;<br>c) Name of molecular shape;<br>d) Polarity of molecule (For example, is it polar or nonpolar?)<br>NF3, XeCl4, SF6, PBr5, F2O, BCI3, SiO2, XeF2, PH3, N2<\/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 a breakdown of the compounds listed, including their general formulas, Lewis structures, molecular shapes, and polarity:<\/p>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>1. NF3 (Nitrogen trifluoride)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>General Formula<\/strong>: AX3E<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Nitrogen (N) is bonded to three fluorine (F) atoms, with one lone pair on nitrogen.<\/li>\n\n\n\n<li><strong>Molecular Shape<\/strong>: Trigonal pyramidal<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Polar\n<ul class=\"wp-block-list\">\n<li><strong>Explanation<\/strong>: The presence of a lone pair on nitrogen creates an asymmetrical shape, and because fluorine is more electronegative than nitrogen, there is a dipole moment.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>2. XeCl4 (Xenon tetrachloride)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>General Formula<\/strong>: AX4E2<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Xenon (Xe) is bonded to four chlorine (Cl) atoms, with two lone pairs on xenon.<\/li>\n\n\n\n<li><strong>Molecular Shape<\/strong>: Square planar<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar\n<ul class=\"wp-block-list\">\n<li><strong>Explanation<\/strong>: The symmetrical arrangement of chlorine atoms around xenon results in a nonpolar molecule.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>3. SF6 (Sulfur hexafluoride)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>General Formula<\/strong>: AX6<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Sulfur (S) is bonded to six fluorine (F) atoms, with no lone pairs on sulfur.<\/li>\n\n\n\n<li><strong>Molecular Shape<\/strong>: Octahedral<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar\n<ul class=\"wp-block-list\">\n<li><strong>Explanation<\/strong>: The symmetrical geometry results in no dipole moment, making it nonpolar.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>4. PBr5 (Phosphorus pentabromide)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>General Formula<\/strong>: AX5<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Phosphorus (P) is bonded to five bromine (Br) atoms, with no lone pairs on phosphorus.<\/li>\n\n\n\n<li><strong>Molecular Shape<\/strong>: Trigonal bipyramidal<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar\n<ul class=\"wp-block-list\">\n<li><strong>Explanation<\/strong>: The symmetrical geometry of the molecule results in no dipole moment.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>5. F2O (Difluorine monoxide)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>General Formula<\/strong>: AX2E2<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Oxygen (O) is bonded to two fluorine (F) atoms, with two lone pairs on oxygen.<\/li>\n\n\n\n<li><strong>Molecular Shape<\/strong>: Bent<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Polar\n<ul class=\"wp-block-list\">\n<li><strong>Explanation<\/strong>: The bent shape causes a net dipole moment due to the electronegativity difference between fluorine and oxygen.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>6. BCl3 (Boron trichloride)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>General Formula<\/strong>: AX3<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Boron (B) is bonded to three chlorine (Cl) atoms, with no lone pairs on boron.<\/li>\n\n\n\n<li><strong>Molecular Shape<\/strong>: Trigonal planar<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar\n<ul class=\"wp-block-list\">\n<li><strong>Explanation<\/strong>: The molecule is symmetrical, so there is no dipole moment, making it nonpolar.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>7. SiO2 (Silicon dioxide)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>General Formula<\/strong>: AX2 (for each SiO2 unit)<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Silicon (Si) is bonded to two oxygen (O) atoms, forming a network structure.<\/li>\n\n\n\n<li><strong>Molecular Shape<\/strong>: Linear (for individual SiO2 units), but it forms a giant covalent structure.<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar\n<ul class=\"wp-block-list\">\n<li><strong>Explanation<\/strong>: In the solid structure, the molecule\u2019s symmetry and the network of covalent bonds result in a nonpolar nature.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>8. XeF2 (Xenon difluoride)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>General Formula<\/strong>: AX2E3<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Xenon (Xe) is bonded to two fluorine (F) atoms, with three lone pairs on xenon.<\/li>\n\n\n\n<li><strong>Molecular Shape<\/strong>: Linear<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar\n<ul class=\"wp-block-list\">\n<li><strong>Explanation<\/strong>: The symmetrical arrangement of fluorine atoms around xenon makes the molecule nonpolar.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>9. PH3 (Phosphine)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>General Formula<\/strong>: AX3E<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Phosphorus (P) is bonded to three hydrogen (H) atoms, with one lone pair on phosphorus.<\/li>\n\n\n\n<li><strong>Molecular Shape<\/strong>: Trigonal pyramidal<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Polar\n<ul class=\"wp-block-list\">\n<li><strong>Explanation<\/strong>: The lone pair on phosphorus causes an asymmetrical shape, leading to a net dipole moment.<\/li>\n<\/ul>\n<\/li>\n<\/ul>\n\n\n\n<hr class=\"wp-block-separator has-alpha-channel-opacity\"\/>\n\n\n\n<p><strong>10. N2 (Nitrogen)<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>General Formula<\/strong>: AX<\/li>\n\n\n\n<li><strong>Lewis Structure<\/strong>: Two nitrogen (N) atoms are triple-bonded, with each nitrogen having one lone pair.<\/li>\n\n\n\n<li><strong>Molecular Shape<\/strong>: Linear<\/li>\n\n\n\n<li><strong>Polarity<\/strong>: Nonpolar\n<ul class=\"wp-block-list\">\n<li><strong>Explanation<\/strong>: Since both nitrogen atoms have the same electronegativity, there is no dipole moment, making the molecule nonpolar.<\/li>\n<\/ul>\n<\/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\">Summary of Molecular Shapes:<\/h3>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Trigonal pyramidal<\/strong>: NF3, PH3<\/li>\n\n\n\n<li><strong>Square planar<\/strong>: XeCl4<\/li>\n\n\n\n<li><strong>Octahedral<\/strong>: SF6<\/li>\n\n\n\n<li><strong>Trigonal bipyramidal<\/strong>: PBr5<\/li>\n\n\n\n<li><strong>Bent<\/strong>: F2O<\/li>\n\n\n\n<li><strong>Trigonal planar<\/strong>: BCl3<\/li>\n\n\n\n<li><strong>Linear<\/strong>: XeF2, N2<\/li>\n<\/ul>\n\n\n\n<p>The polarity of each molecule depends on its molecular geometry and the difference in electronegativity between the atoms involved.<\/p>\n","protected":false},"excerpt":{"rendered":"<p>Given a list of compounds, show the following:a) General Formula, i.e., AX3E;b) Lewis structure;c) Name of molecular shape;d) Polarity of molecule (For example, is it polar or nonpolar?)NF3, XeCl4, SF6, PBr5, F2O, BCI3, SiO2, XeF2, PH3, N2 The Correct Answer and Explanation is : Here&#8217;s a breakdown of the compounds listed, including their general formulas, [&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 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