{"id":222205,"date":"2025-05-31T06:38:50","date_gmt":"2025-05-31T06:38:50","guid":{"rendered":"https:\/\/learnexams.com\/blog\/?p=222205"},"modified":"2025-05-31T06:38:52","modified_gmt":"2025-05-31T06:38:52","slug":"mcb-cher-a-g-bro-pl-dyn-lonc-pcp-quiz-q-pled-2013-cop-www-awn-aleks-com-alekscgi-x-1sl-exe-10_u-ignsikr7j8p3jh-iqs_p9bn453jabyqwg5vhdj-zao-nbo8y5220402","status":"publish","type":"post","link":"https:\/\/www.learnexams.com\/blog\/2025\/05\/31\/mcb-cher-a-g-bro-pl-dyn-lonc-pcp-quiz-q-pled-2013-cop-www-awn-aleks-com-alekscgi-x-1sl-exe-10_u-ignsikr7j8p3jh-iqs_p9bn453jabyqwg5vhdj-zao-nbo8y5220402\/","title":{"rendered":"MCB Cher A.* G bro: PL Dyn LONC PCP Quiz Q Pled 2013 cop www-awn.aleks.com\/alekscgi\/x\/1sl.exe\/10_u-IgNsikr7j8P3jH-IQs_p9bn453jabYqwg5vhdj Zao-NbO8y5220402"},"content":{"rendered":"\n<p>MCB Cher A.* G bro: PL Dyn LONC PCP Quiz Q Pled 2013 cop www-awn.aleks.com\/alekscgi\/x\/1sl.exe\/10_u-IgNsikr7j8P3jH-IQs_p9bn453jabYqwg5vhdj Zao-NbO8y5220402<\/p>\n\n\n\n<p>CHEMICAL BONDING<\/p>\n\n\n\n<p>Predicting deviations from ideal bond angles<\/p>\n\n\n\n<p>Consider the carbonyl fluoride (CF<sub>2<\/sub>O) molecule. What is the central atom? Enter its chemical symbol.<\/p>\n\n\n\n<p>O<\/p>\n\n\n\n<p>How many lone pairs are around the central atom?<\/p>\n\n\n\n<p>What is the ideal angle between the carbon-fluorine bonds?<\/p>\n\n\n\n<p>Compared to the ideal angle, you would expect the actual angle between the carbon-fluorine bonds to (choose one) be (choose one) about the same, bigger, smaller.<\/p>\n\n\n\n<p>Explanation<\/p>\n\n\n\n<p>Check Type here to search<\/p>\n\n\n\n<p><strong><mark style=\"background-color:rgba(0, 0, 0, 0)\" class=\"has-inline-color has-ast-global-color-1-color\">The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n<p><strong>Correct Answers:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Central atom:<\/strong> <strong>C<\/strong><\/li>\n\n\n\n<li><strong>Number of lone pairs around the central atom:<\/strong> <strong>0<\/strong><\/li>\n\n\n\n<li><strong>Ideal angle between the carbon-fluorine bonds:<\/strong> <strong>120\u00b0<\/strong><\/li>\n\n\n\n<li><strong>Compared to the ideal angle, the actual angle between the carbon-fluorine bonds would be:<\/strong> <strong>slightly smaller<\/strong><\/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>Explanation (300 words):<\/strong><\/h3>\n\n\n\n<p>The compound <strong>carbonyl fluoride (CF\u2082O)<\/strong> consists of a central <strong>carbon (C)<\/strong> atom bonded to two fluorine (F) atoms and one oxygen (O) atom. Carbon is the central atom because it is less electronegative than oxygen and typically forms four bonds, making it the logical central element in most organic molecules.<\/p>\n\n\n\n<p>To determine the molecular geometry and predict deviations from the ideal bond angle, we apply <strong>Valence Shell Electron Pair Repulsion (VSEPR) theory<\/strong>. The carbon atom in CF\u2082O forms three sigma bonds: two with fluorine and one with oxygen. In addition, it forms a <strong>pi bond<\/strong> with the oxygen (as part of the carbonyl group), making a total of <strong>three regions of electron density<\/strong> around the central carbon atom.<\/p>\n\n\n\n<p>According to VSEPR theory, three regions of electron density around a central atom adopt a <strong>trigonal planar geometry<\/strong>, which ideally results in bond angles of <strong>120\u00b0<\/strong>. However, real molecules often deviate from ideal angles due to differences in <strong>electronegativity<\/strong> and <strong>bond character<\/strong>.<\/p>\n\n\n\n<p>In CF\u2082O, oxygen is more electronegative than fluorine and pulls electron density toward itself, strengthening the C=O double bond. The <strong>double bond occupies more space<\/strong> than a single bond due to its higher electron density. This increased repulsion pushes the two C\u2013F bonds slightly closer together, resulting in a <strong>bond angle between the two fluorine atoms that is slightly less than 120\u00b0<\/strong>.<\/p>\n\n\n\n<p>Additionally, there are <strong>no lone pairs on the central carbon<\/strong>, so the deviation is mainly due to differences in bonding types and electronegativity effects\u2014not lone pair repulsion.<\/p>\n\n\n\n<p>In summary, while the <strong>ideal angle is 120\u00b0<\/strong>, the <strong>actual F\u2013C\u2013F angle<\/strong> is <strong>slightly smaller<\/strong>, due to the <strong>electron-dense C=O double bond<\/strong> exerting greater repulsive forces than the single C\u2013F bonds.<strong>Correct Answers:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Central atom:<\/strong> <strong>C<\/strong><\/li>\n\n\n\n<li><strong>Number of lone pairs around the central atom:<\/strong> <strong>0<\/strong><\/li>\n\n\n\n<li><strong>Ideal angle between the carbon-fluorine bonds:<\/strong> <strong>120\u00b0<\/strong><\/li>\n\n\n\n<li><strong>Compared to the ideal angle, the actual angle between the carbon-fluorine bonds would be:<\/strong> <strong>slightly smaller<\/strong><\/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>Explanation (300 words):<\/strong><\/h3>\n\n\n\n<p>The compound <strong>carbonyl fluoride (CF\u2082O)<\/strong> consists of a central <strong>carbon (C)<\/strong> atom bonded to two fluorine (F) atoms and one oxygen (O) atom. Carbon is the central atom because it is less electronegative than oxygen and typically forms four bonds, making it the logical central element in most organic molecules.<\/p>\n\n\n\n<p>To determine the molecular geometry and predict deviations from the ideal bond angle, we apply <strong>Valence Shell Electron Pair Repulsion (VSEPR) theory<\/strong>. The carbon atom in CF\u2082O forms three sigma bonds: two with fluorine and one with oxygen. In addition, it forms a <strong>pi bond<\/strong> with the oxygen (as part of the carbonyl group), making a total of <strong>three regions of electron density<\/strong> around the central carbon atom.<\/p>\n\n\n\n<p>According to VSEPR theory, three regions of electron density around a central atom adopt a <strong>trigonal planar geometry<\/strong>, which ideally results in bond angles of <strong>120\u00b0<\/strong>. However, real molecules often deviate from ideal angles due to differences in <strong>electronegativity<\/strong> and <strong>bond character<\/strong>.<\/p>\n\n\n\n<p>In CF\u2082O, oxygen is more electronegative than fluorine and pulls electron density toward itself, strengthening the C=O double bond. The <strong>double bond occupies more space<\/strong> than a single bond due to its higher electron density. This increased repulsion pushes the two C\u2013F bonds slightly closer together, resulting in a <strong>bond angle between the two fluorine atoms that is slightly less than 120\u00b0<\/strong>.<\/p>\n\n\n\n<p>Additionally, there are <strong>no lone pairs on the central carbon<\/strong>, so the deviation is mainly due to differences in bonding types and electronegativity effects\u2014not lone pair repulsion.<\/p>\n\n\n\n<p>In summary, while the <strong>ideal angle is 120\u00b0<\/strong>, the <strong>actual F\u2013C\u2013F angle<\/strong> is <strong>slightly smaller<\/strong>, due to the <strong>electron-dense C=O double bond<\/strong> exerting greater repulsive forces than the single C\u2013F bonds.<\/p>\n\n\n\n<p><strong>Correct Answers:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Central atom:<\/strong> <strong>C<\/strong><\/li>\n\n\n\n<li><strong>Number of lone pairs around the central atom:<\/strong> <strong>0<\/strong><\/li>\n\n\n\n<li><strong>Ideal angle between the carbon-fluorine bonds:<\/strong> <strong>120\u00b0<\/strong><\/li>\n\n\n\n<li><strong>Compared to the ideal angle, the actual angle between the carbon-fluorine bonds would be:<\/strong> <strong>slightly smaller<\/strong><\/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>Explanation<\/strong><\/h3>\n\n\n\n<p>The compound <strong>carbonyl fluoride (CF\u2082O)<\/strong> consists of a central <strong>carbon (C)<\/strong> atom bonded to two fluorine (F) atoms and one oxygen (O) atom. Carbon is the central atom because it is less electronegative than oxygen and typically forms four bonds, making it the logical central element in most organic molecules.<\/p>\n\n\n\n<p>To determine the molecular geometry and predict deviations from the ideal bond angle, we apply <strong>Valence Shell Electron Pair Repulsion (VSEPR) theory<\/strong>. The carbon atom in CF\u2082O forms three sigma bonds: two with fluorine and one with oxygen. In addition, it forms a <strong>pi bond<\/strong> with the oxygen (as part of the carbonyl group), making a total of <strong>three regions of electron density<\/strong> around the central carbon atom.<\/p>\n\n\n\n<p>According to VSEPR theory, three regions of electron density around a central atom adopt a <strong>trigonal planar geometry<\/strong>, which ideally results in bond angles of <strong>120\u00b0<\/strong>. However, real molecules often deviate from ideal angles due to differences in <strong>electronegativity<\/strong> and <strong>bond character<\/strong>.<\/p>\n\n\n\n<p>In CF\u2082O, oxygen is more electronegative than fluorine and pulls electron density toward itself, strengthening the C=O double bond. The <strong>double bond occupies more space<\/strong> than a single bond due to its higher electron density. This increased repulsion pushes the two C\u2013F bonds slightly closer together, resulting in a <strong>bond angle between the two fluorine atoms that is slightly less than 120\u00b0<\/strong>.<\/p>\n\n\n\n<p>Additionally, there are <strong>no lone pairs on the central carbon<\/strong>, so the deviation is mainly due to differences in bonding types and electronegativity effects\u2014not lone pair repulsion.<\/p>\n\n\n\n<p>In summary, while the <strong>ideal angle is 120\u00b0<\/strong>, the <strong>actual F\u2013C\u2013F angle<\/strong> is <strong>slightly smaller<\/strong>, due to the <strong>electron-dense C=O double bond<\/strong> exerting greater repulsive forces than the single C\u2013F bonds.<strong>Correct Answers:<\/strong><\/p>\n\n\n\n<ul class=\"wp-block-list\">\n<li><strong>Central atom:<\/strong> <strong>C<\/strong><\/li>\n\n\n\n<li><strong>Number of lone pairs around the central atom:<\/strong> <strong>0<\/strong><\/li>\n\n\n\n<li><strong>Ideal angle between the carbon-fluorine bonds:<\/strong> <strong>120\u00b0<\/strong><\/li>\n\n\n\n<li><strong>Compared to the ideal angle, the actual angle between the carbon-fluorine bonds would be:<\/strong> <strong>slightly smaller<\/strong><\/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>Explanation (300 words):<\/strong><\/h3>\n\n\n\n<p>The compound <strong>carbonyl fluoride (CF\u2082O)<\/strong> consists of a central <strong>carbon (C)<\/strong> atom bonded to two fluorine (F) atoms and one oxygen (O) atom. Carbon is the central atom because it is less electronegative than oxygen and typically forms four bonds, making it the logical central element in most organic molecules.<\/p>\n\n\n\n<p>To determine the molecular geometry and predict deviations from the ideal bond angle, we apply <strong>Valence Shell Electron Pair Repulsion (VSEPR) theory<\/strong>. The carbon atom in CF\u2082O forms three sigma bonds: two with fluorine and one with oxygen. In addition, it forms a <strong>pi bond<\/strong> with the oxygen (as part of the carbonyl group), making a total of <strong>three regions of electron density<\/strong> around the central carbon atom.<\/p>\n\n\n\n<p>According to VSEPR theory, three regions of electron density around a central atom adopt a <strong>trigonal planar geometry<\/strong>, which ideally results in bond angles of <strong>120\u00b0<\/strong>. However, real molecules often deviate from ideal angles due to differences in <strong>electronegativity<\/strong> and <strong>bond character<\/strong>.<\/p>\n\n\n\n<p>In CF\u2082O, oxygen is more electronegative than fluorine and pulls electron density toward itself, strengthening the C=O double bond. The <strong>double bond occupies more space<\/strong> than a single bond due to its higher electron density. This increased repulsion pushes the two C\u2013F bonds slightly closer together, resulting in a <strong>bond angle between the two fluorine atoms that is slightly less than 120\u00b0<\/strong>.<\/p>\n\n\n\n<p>Additionally, there are <strong>no lone pairs on the central carbon<\/strong>, so the deviation is mainly due to differences in bonding types and electronegativity effects\u2014not lone pair repulsion.<\/p>\n\n\n\n<p>In summary, while the <strong>ideal angle is 120\u00b0<\/strong>, the <strong>actual F\u2013C\u2013F angle<\/strong> is <strong>slightly smaller<\/strong>, due to the <strong>electron-dense C=O double bond<\/strong> exerting greater repulsive forces than the single C\u2013F bonds.<\/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-banner7-148.jpeg\" alt=\"\" class=\"wp-image-222206\"\/><\/figure>\n","protected":false},"excerpt":{"rendered":"<p>MCB Cher A.* G bro: PL Dyn LONC PCP Quiz Q Pled 2013 cop www-awn.aleks.com\/alekscgi\/x\/1sl.exe\/10_u-IgNsikr7j8P3jH-IQs_p9bn453jabYqwg5vhdj Zao-NbO8y5220402 CHEMICAL BONDING Predicting deviations from ideal bond angles Consider the carbonyl fluoride (CF2O) molecule. What is the central atom? Enter its chemical symbol. O How many lone pairs are around the central atom? What is the ideal angle between [&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-222205","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222205","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=222205"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/222205\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=222205"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=222205"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=222205"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}