Let’s evaluate each molecule for its net dipole moment based on its molecular geometry and electronegativity differences:<\/p>\n\n\n\n
- \n
- BF3 (Boron Trifluoride)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- \n
- Geometry: Trigonal planar.<\/li>\n\n\n\n
- The boron atom in BF3 is surrounded symmetrically by three fluorine atoms. While the B-F bonds themselves are polar due to the significant electronegativity difference between B and F, the symmetry of the molecule (due to its trigonal planar shape) cancels out the individual dipoles. As a result, BF3 has no net dipole moment<\/strong>.<\/li>\n<\/ul>\n\n\n\n
- \n
- CCl4 (Carbon Tetrachloride)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- \n
- Geometry: Tetrahedral.<\/li>\n\n\n\n
- CCl4 has four C-Cl bonds, and while these bonds are polar, the molecule’s symmetrical tetrahedral shape means the dipoles cancel each other out. This results in no net dipole moment<\/strong>.<\/li>\n<\/ul>\n\n\n\n
- \n
- (CH3)2O (Dimethyl Ether)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- \n
- Geometry: Bent (due to lone pairs on oxygen).<\/li>\n\n\n\n
- The molecule has two C-H bonds and one C-O bond, which is polar. Oxygen is more electronegative than carbon, so the C-O bond contributes to the dipole. The bent geometry causes the dipoles to not cancel out, and thus, (CH3)2O has a net dipole moment<\/strong>.<\/li>\n<\/ul>\n\n\n\n
- \n
- CH2Cl2 (Dichloromethane)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- \n
- Geometry: Tetrahedral.<\/li>\n\n\n\n
- CH2Cl2 has two C-H bonds and two C-Cl bonds. The C-Cl bonds are polar, and the molecule\u2019s geometry prevents the dipoles from canceling out. Therefore, CH2Cl2 has a net dipole moment<\/strong>.<\/li>\n<\/ul>\n\n\n\n
- \n
- CO2 (Carbon Dioxide)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- \n
- Geometry: Linear.<\/li>\n\n\n\n
- The C=O bonds are polar, but because the molecule is linear and the dipoles are equal and opposite, they cancel out. Thus, CO2 has no net dipole moment<\/strong>.<\/li>\n<\/ul>\n\n\n\n
Molecules with a net dipole moment:<\/h3>\n\n\n\n
- \n
- (CH3)2O<\/li>\n\n\n\n
- CH2Cl2<\/li>\n<\/ul>\n\n\n\n
I’ll also generate an image to visualize the molecular shapes of these molecules.<\/p>\n\n\n\n
Here is the illustration showing the molecular structures of (CH3)2O, CH2Cl2, BF3, CCl4, and CO2 with their respective geometries and polar bonds. As we discussed:<\/p>\n\n\n\n
- \n
- (CH3)2O<\/strong> and CH2Cl2<\/strong> have a net dipole moment due to their bent or asymmetrical geometries that prevent the cancellation of dipoles.<\/li>\n\n\n\n
- BF3<\/strong>, CCl4<\/strong>, and CO2<\/strong> have no net dipole moment due to their symmetric molecular shapes.<\/li>\n<\/ul>\n\n\n\n
Let me know if you’d like more details!<\/p>\n\n\n\n
![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/02\/image-1012.png\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"Identify the molecules that have a net dipole moment. Select all that apply: BF3 CCl4 (CH3)2O CH2Cl2 CO2 The Correct Answer and Explanation is : Let’s evaluate each molecule for its net dipole moment based on its molecular geometry and electronegativity differences: Molecules with a net dipole moment: I’ll also generate an image to visualize […]<\/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-193364","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/193364","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=193364"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/193364\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=193364"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=193364"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=193364"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
- BF3<\/strong>, CCl4<\/strong>, and CO2<\/strong> have no net dipole moment due to their symmetric molecular shapes.<\/li>\n<\/ul>\n\n\n\n
- (CH3)2O<\/strong> and CH2Cl2<\/strong> have a net dipole moment due to their bent or asymmetrical geometries that prevent the cancellation of dipoles.<\/li>\n\n\n\n
- CO2 (Carbon Dioxide)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- CH2Cl2 (Dichloromethane)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- (CH3)2O (Dimethyl Ether)<\/strong>:<\/li>\n<\/ol>\n\n\n\n
- CCl4 (Carbon Tetrachloride)<\/strong>:<\/li>\n<\/ol>\n\n\n\n