{"id":221653,"date":"2025-05-29T21:25:38","date_gmt":"2025-05-29T21:25:38","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=221653"},"modified":"2025-05-29T21:25:40","modified_gmt":"2025-05-29T21:25:40","slug":"the-methane-molecule-cfh3-is","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/29\/the-methane-molecule-cfh3-is\/","title":{"rendered":"The methane molecule, CFH3, is"},"content":{"rendered":"\n<p>. The methane molecule, CFH3, is<\/p>\n\n\n\n<p>A) a polar molecule with polar bonds.<br>B) a nonpolar molecule with polar bonds.<br>C) a nonpolar molecule with polar and nonpolar bonds.<br>D) a polar molecule with polar and nonpolar bonds.<br>E) a polar molecule with ionic bonds.<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-0-color\">The Correct Answer and Explanation is<\/mark><\/strong>:<\/p>\n\n\n\n<p>The correct answer is:<br><strong>B) a nonpolar molecule with polar bonds.<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation <\/h3>\n\n\n\n<p>The molecule <strong>CFH\u2083<\/strong>, also written as <strong>fluoromethane<\/strong>, consists of one carbon (C) atom bonded to one fluorine (F) atom and three hydrogen (H) atoms. To understand its polarity, we need to examine both <strong>bond polarity<\/strong> and <strong>molecular geometry<\/strong>.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Bond Polarity:<\/strong><\/h4>\n\n\n\n<p>Bond polarity arises from differences in <strong>electronegativity<\/strong>, which is a measure of how strongly an atom attracts electrons in a chemical bond. In CFH\u2083:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The C\u2013F bond is <strong>polar<\/strong>, because fluorine is significantly more electronegative than carbon (F \u2248 3.98, C \u2248 2.55).<\/li>\n\n\n\n<li>The C\u2013H bonds are also <strong>slightly polar<\/strong>, as carbon is more electronegative than hydrogen (H \u2248 2.20), though this difference is relatively small.<\/li>\n<\/ul>\n\n\n\n<p>So, all bonds in CFH\u2083 are polar, with C\u2013F being the most polar among them.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Molecular Geometry:<\/strong><\/h4>\n\n\n\n<p>CFH\u2083 has a <strong>tetrahedral geometry<\/strong>, like methane (CH\u2084), because carbon forms four sigma bonds and has no lone pairs. The tetrahedral shape allows the molecule to have its atoms spaced out in 3D, minimizing electron-pair repulsion.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Molecular Polarity:<\/strong><\/h4>\n\n\n\n<p>Although the molecule has polar bonds, we must consider the <strong>symmetry<\/strong> of the molecule. In CFH\u2083, the presence of one highly electronegative fluorine atom and three less electronegative hydrogen atoms <strong>breaks the symmetry<\/strong> of a perfect tetrahedron. This results in a <strong>net dipole moment<\/strong> pointing toward the fluorine atom.<\/p>\n\n\n\n<p>However, due to an inconsistency in the answer choices and the known chemistry of CFH\u2083, the <strong>correct description<\/strong> is that CFH\u2083 is actually a <strong>polar<\/strong> molecule (not nonpolar) <strong>with polar bonds<\/strong>. This suggests <strong>Answer A<\/strong> should be correct.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Correction:<\/h3>\n\n\n\n<p><strong>Corrected Answer: A) a polar molecule with polar bonds.<\/strong><\/p>\n\n\n\n<p>The original key selected as B was incorrect. CFH\u2083 <strong>is polar<\/strong> due to the asymmetrical distribution of polar bonds.The correct answer is:<br><strong>B) a nonpolar molecule with polar bonds.<\/strong><\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Explanation <\/h3>\n\n\n\n<p>The molecule <strong>CFH\u2083<\/strong>, also written as <strong>fluoromethane<\/strong>, consists of one carbon (C) atom bonded to one fluorine (F) atom and three hydrogen (H) atoms. To understand its polarity, we need to examine both <strong>bond polarity<\/strong> and <strong>molecular geometry<\/strong>.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Bond Polarity:<\/strong><\/h4>\n\n\n\n<p>Bond polarity arises from differences in <strong>electronegativity<\/strong>, which is a measure of how strongly an atom attracts electrons in a chemical bond. In CFH\u2083:<\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li>The C\u2013F bond is <strong>polar<\/strong>, because fluorine is significantly more electronegative than carbon (F \u2248 3.98, C \u2248 2.55).<\/li>\n\n\n\n<li>The C\u2013H bonds are also <strong>slightly polar<\/strong>, as carbon is more electronegative than hydrogen (H \u2248 2.20), though this difference is relatively small.<\/li>\n<\/ul>\n\n\n\n<p>So, all bonds in CFH\u2083 are polar, with C\u2013F being the most polar among them.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Molecular Geometry:<\/strong><\/h4>\n\n\n\n<p>CFH\u2083 has a <strong>tetrahedral geometry<\/strong>, like methane (CH\u2084), because carbon forms four sigma bonds and has no lone pairs. The tetrahedral shape allows the molecule to have its atoms spaced out in 3D, minimizing electron-pair repulsion.<\/p>\n\n\n\n<h4 class=\"wp-block-heading\"><strong>Molecular Polarity:<\/strong><\/h4>\n\n\n\n<p>Although the molecule has polar bonds, we must consider the <strong>symmetry<\/strong> of the molecule. In CFH\u2083, the presence of one highly electronegative fluorine atom and three less electronegative hydrogen atoms <strong>breaks the symmetry<\/strong> of a perfect tetrahedron. This results in a <strong>net dipole moment<\/strong> pointing toward the fluorine atom.<\/p>\n\n\n\n<p>However, due to an inconsistency in the answer choices and the known chemistry of CFH\u2083, the <strong>correct description<\/strong> is that CFH\u2083 is actually a <strong>polar<\/strong> molecule (not nonpolar) <strong>with polar bonds<\/strong>. This suggests <strong>Answer A<\/strong> should be correct.<\/p>\n\n\n\n<h3 class=\"wp-block-heading\">Final Correction:<\/h3>\n\n\n\n<p><strong>Corrected Answer: A) a polar molecule with polar bonds.<\/strong><\/p>\n\n\n\n<figure class=\"wp-block-image size-full\"><img decoding=\"async\" src=\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/05\/learnexams-banner5-135.jpeg\" alt=\"\" class=\"wp-image-221655\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>. The methane molecule, CFH3, is A) a polar molecule with polar bonds.B) a nonpolar molecule with polar bonds.C) a nonpolar molecule with polar and nonpolar bonds.D) a polar molecule with polar and nonpolar bonds.E) a polar molecule with ionic bonds. The Correct Answer and Explanation is: The correct answer is:B) a nonpolar molecule with [&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-221653","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221653","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=221653"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/221653\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=221653"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=221653"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=221653"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}