1. PCl3 (Phosphorus Trichloride)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Phosphorus (P) is in the center with three chlorine (Cl) atoms surrounding it. Each Cl atom is single-bonded to P. Phosphorus has one lone pair of electrons.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp3<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Tetrahedral<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Trigonal Pyramidal (due to one lone pair)<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The lone pair on phosphorus creates an asymmetry in the electron cloud, leading to a net dipole.<\/li>\n<\/ul>\n\n\n\n
2. PCl5 (Phosphorus Pentachloride)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Phosphorus is the central atom with five chlorine atoms attached via single bonds. No lone pairs on phosphorus.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp3d<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Bipyramidal<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Trigonal Bipyramidal<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar. The symmetry of the five chlorine atoms around phosphorus cancels out any dipoles.<\/li>\n<\/ul>\n\n\n\n
3. C2H4Cl2 (1, 1-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Each carbon is double-bonded to the other and each is single-bonded to a hydrogen and a chlorine. The chlorine atoms are on the same carbon.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar, with each carbon in a trigonal planar arrangement.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines on the same carbon create a dipole moment, resulting in an overall polar molecule.<\/li>\n<\/ul>\n\n\n\n
4. C2H4Cl2 (1, 2-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Similar to 1, 1-Dichloroethene, but the chlorines are on different carbons.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines on opposite sides create a net dipole moment, making the molecule polar.<\/li>\n<\/ul>\n\n\n\n
5. C2H2Cl2 (1, 1-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Each carbon is triple-bonded to the other and single-bonded to a hydrogen and a chlorine. Both chlorines are on the same carbon.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Linear (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The two chlorines on the same carbon result in an overall dipole moment.<\/li>\n<\/ul>\n\n\n\n
6. C2H2Cl2 (1, 2-Dichloroethene, Cis form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on the same side of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized with trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines being on the same side result in a net dipole moment.<\/li>\n<\/ul>\n\n\n\n
7. C2H2Cl2 (1, 2-Dichloroethene, Trans form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on opposite sides of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar. The opposing directions of the dipoles cancel out, making the molecule nonpolar.<\/li>\n<\/ul>\n\n\n\n
\n\n\n\nThese are the main structures, hybridizations, geometries, and polarities for each molecule based on their respective bonding.<\/p>\n\n\n\n![\"\"](\"https:\/\/learnexams.com\/blog\/wp-content\/uploads\/2025\/07\/learnexams-banner6-1185.jpeg\")
<\/figure>\n","protected":false},"excerpt":{"rendered":"Molecule AE Lewis Structure EC Hyb’d about X Electronic Geometry Molecular Geometry 3-D P or NP PC13 PC15 C2H4Cl2(1, 1) C2H4Cl2(1, 2) C2H2Cl2(1,1) C2H2Cl2 (1,2-cis) C2H2Cl2 (1,2-trans) The Correct Answer and Explanation is: 1. PCl3 (Phosphorus Trichloride) 2. PCl5 (Phosphorus Pentachloride) 3. C2H4Cl2 (1, 1-Dichloroethene) 4. C2H4Cl2 (1, 2-Dichloroethene) 5. C2H2Cl2 (1, 1-Dichloroethene) 6. C2H2Cl2 […]<\/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-261843","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843","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=261843"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=261843"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=261843"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=261843"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
2. PCl5 (Phosphorus Pentachloride)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Phosphorus is the central atom with five chlorine atoms attached via single bonds. No lone pairs on phosphorus.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp3d<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Bipyramidal<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Trigonal Bipyramidal<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar. The symmetry of the five chlorine atoms around phosphorus cancels out any dipoles.<\/li>\n<\/ul>\n\n\n\n
3. C2H4Cl2 (1, 1-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Each carbon is double-bonded to the other and each is single-bonded to a hydrogen and a chlorine. The chlorine atoms are on the same carbon.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar, with each carbon in a trigonal planar arrangement.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines on the same carbon create a dipole moment, resulting in an overall polar molecule.<\/li>\n<\/ul>\n\n\n\n
4. C2H4Cl2 (1, 2-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Similar to 1, 1-Dichloroethene, but the chlorines are on different carbons.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines on opposite sides create a net dipole moment, making the molecule polar.<\/li>\n<\/ul>\n\n\n\n
5. C2H2Cl2 (1, 1-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Each carbon is triple-bonded to the other and single-bonded to a hydrogen and a chlorine. Both chlorines are on the same carbon.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Linear (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The two chlorines on the same carbon result in an overall dipole moment.<\/li>\n<\/ul>\n\n\n\n
6. C2H2Cl2 (1, 2-Dichloroethene, Cis form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on the same side of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized with trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines being on the same side result in a net dipole moment.<\/li>\n<\/ul>\n\n\n\n
7. C2H2Cl2 (1, 2-Dichloroethene, Trans form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on opposite sides of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar. The opposing directions of the dipoles cancel out, making the molecule nonpolar.<\/li>\n<\/ul>\n\n\n\n
\n\n\n\nThese are the main structures, hybridizations, geometries, and polarities for each molecule based on their respective bonding.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Molecule AE Lewis Structure EC Hyb’d about X Electronic Geometry Molecular Geometry 3-D P or NP PC13 PC15 C2H4Cl2(1, 1) C2H4Cl2(1, 2) C2H2Cl2(1,1) C2H2Cl2 (1,2-cis) C2H2Cl2 (1,2-trans) The Correct Answer and Explanation is: 1. PCl3 (Phosphorus Trichloride) 2. PCl5 (Phosphorus Pentachloride) 3. C2H4Cl2 (1, 1-Dichloroethene) 4. C2H4Cl2 (1, 2-Dichloroethene) 5. C2H2Cl2 (1, 1-Dichloroethene) 6. C2H2Cl2 […]<\/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-261843","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843","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=261843"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=261843"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=261843"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=261843"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
3. C2H4Cl2 (1, 1-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Each carbon is double-bonded to the other and each is single-bonded to a hydrogen and a chlorine. The chlorine atoms are on the same carbon.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar, with each carbon in a trigonal planar arrangement.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines on the same carbon create a dipole moment, resulting in an overall polar molecule.<\/li>\n<\/ul>\n\n\n\n
4. C2H4Cl2 (1, 2-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Similar to 1, 1-Dichloroethene, but the chlorines are on different carbons.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines on opposite sides create a net dipole moment, making the molecule polar.<\/li>\n<\/ul>\n\n\n\n
5. C2H2Cl2 (1, 1-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Each carbon is triple-bonded to the other and single-bonded to a hydrogen and a chlorine. Both chlorines are on the same carbon.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Linear (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The two chlorines on the same carbon result in an overall dipole moment.<\/li>\n<\/ul>\n\n\n\n
6. C2H2Cl2 (1, 2-Dichloroethene, Cis form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on the same side of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized with trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines being on the same side result in a net dipole moment.<\/li>\n<\/ul>\n\n\n\n
7. C2H2Cl2 (1, 2-Dichloroethene, Trans form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on opposite sides of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar. The opposing directions of the dipoles cancel out, making the molecule nonpolar.<\/li>\n<\/ul>\n\n\n\n
\n\n\n\nThese are the main structures, hybridizations, geometries, and polarities for each molecule based on their respective bonding.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Molecule AE Lewis Structure EC Hyb’d about X Electronic Geometry Molecular Geometry 3-D P or NP PC13 PC15 C2H4Cl2(1, 1) C2H4Cl2(1, 2) C2H2Cl2(1,1) C2H2Cl2 (1,2-cis) C2H2Cl2 (1,2-trans) The Correct Answer and Explanation is: 1. PCl3 (Phosphorus Trichloride) 2. PCl5 (Phosphorus Pentachloride) 3. C2H4Cl2 (1, 1-Dichloroethene) 4. C2H4Cl2 (1, 2-Dichloroethene) 5. C2H2Cl2 (1, 1-Dichloroethene) 6. C2H2Cl2 […]<\/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-261843","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843","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=261843"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=261843"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=261843"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=261843"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
4. C2H4Cl2 (1, 2-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Similar to 1, 1-Dichloroethene, but the chlorines are on different carbons.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines on opposite sides create a net dipole moment, making the molecule polar.<\/li>\n<\/ul>\n\n\n\n
5. C2H2Cl2 (1, 1-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Each carbon is triple-bonded to the other and single-bonded to a hydrogen and a chlorine. Both chlorines are on the same carbon.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Linear (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The two chlorines on the same carbon result in an overall dipole moment.<\/li>\n<\/ul>\n\n\n\n
6. C2H2Cl2 (1, 2-Dichloroethene, Cis form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on the same side of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized with trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines being on the same side result in a net dipole moment.<\/li>\n<\/ul>\n\n\n\n
7. C2H2Cl2 (1, 2-Dichloroethene, Trans form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on opposite sides of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar. The opposing directions of the dipoles cancel out, making the molecule nonpolar.<\/li>\n<\/ul>\n\n\n\n
\n\n\n\nThese are the main structures, hybridizations, geometries, and polarities for each molecule based on their respective bonding.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Molecule AE Lewis Structure EC Hyb’d about X Electronic Geometry Molecular Geometry 3-D P or NP PC13 PC15 C2H4Cl2(1, 1) C2H4Cl2(1, 2) C2H2Cl2(1,1) C2H2Cl2 (1,2-cis) C2H2Cl2 (1,2-trans) The Correct Answer and Explanation is: 1. PCl3 (Phosphorus Trichloride) 2. PCl5 (Phosphorus Pentachloride) 3. C2H4Cl2 (1, 1-Dichloroethene) 4. C2H4Cl2 (1, 2-Dichloroethene) 5. C2H2Cl2 (1, 1-Dichloroethene) 6. C2H2Cl2 […]<\/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-261843","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843","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=261843"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=261843"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=261843"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=261843"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
5. C2H2Cl2 (1, 1-Dichloroethene)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Each carbon is triple-bonded to the other and single-bonded to a hydrogen and a chlorine. Both chlorines are on the same carbon.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Linear (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Linear<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The two chlorines on the same carbon result in an overall dipole moment.<\/li>\n<\/ul>\n\n\n\n
6. C2H2Cl2 (1, 2-Dichloroethene, Cis form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on the same side of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized with trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines being on the same side result in a net dipole moment.<\/li>\n<\/ul>\n\n\n\n
7. C2H2Cl2 (1, 2-Dichloroethene, Trans form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on opposite sides of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar. The opposing directions of the dipoles cancel out, making the molecule nonpolar.<\/li>\n<\/ul>\n\n\n\n
\n\n\n\nThese are the main structures, hybridizations, geometries, and polarities for each molecule based on their respective bonding.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Molecule AE Lewis Structure EC Hyb’d about X Electronic Geometry Molecular Geometry 3-D P or NP PC13 PC15 C2H4Cl2(1, 1) C2H4Cl2(1, 2) C2H2Cl2(1,1) C2H2Cl2 (1,2-cis) C2H2Cl2 (1,2-trans) The Correct Answer and Explanation is: 1. PCl3 (Phosphorus Trichloride) 2. PCl5 (Phosphorus Pentachloride) 3. C2H4Cl2 (1, 1-Dichloroethene) 4. C2H4Cl2 (1, 2-Dichloroethene) 5. C2H2Cl2 (1, 1-Dichloroethene) 6. C2H2Cl2 […]<\/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-261843","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843","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=261843"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=261843"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=261843"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=261843"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
6. C2H2Cl2 (1, 2-Dichloroethene, Cis form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on the same side of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized with trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Polar. The chlorines being on the same side result in a net dipole moment.<\/li>\n<\/ul>\n\n\n\n
7. C2H2Cl2 (1, 2-Dichloroethene, Trans form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on opposite sides of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar. The opposing directions of the dipoles cancel out, making the molecule nonpolar.<\/li>\n<\/ul>\n\n\n\n
\n\n\n\nThese are the main structures, hybridizations, geometries, and polarities for each molecule based on their respective bonding.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Molecule AE Lewis Structure EC Hyb’d about X Electronic Geometry Molecular Geometry 3-D P or NP PC13 PC15 C2H4Cl2(1, 1) C2H4Cl2(1, 2) C2H2Cl2(1,1) C2H2Cl2 (1,2-cis) C2H2Cl2 (1,2-trans) The Correct Answer and Explanation is: 1. PCl3 (Phosphorus Trichloride) 2. PCl5 (Phosphorus Pentachloride) 3. C2H4Cl2 (1, 1-Dichloroethene) 4. C2H4Cl2 (1, 2-Dichloroethene) 5. C2H2Cl2 (1, 1-Dichloroethene) 6. C2H2Cl2 […]<\/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-261843","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843","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=261843"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=261843"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=261843"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=261843"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
7. C2H2Cl2 (1, 2-Dichloroethene, Trans form)<\/strong><\/h3>\n\n\n\n\n- Lewis Structure<\/strong>: Same as 1, 2-Dichloroethene, but the chlorines are on opposite sides of the double bond.<\/li>\n\n\n\n
- Hybridization<\/strong>: sp2<\/li>\n\n\n\n
- Electronic Geometry<\/strong>: Trigonal Planar (around each carbon)<\/li>\n\n\n\n
- Molecular Geometry<\/strong>: Planar. Each carbon is sp2 hybridized, with a trigonal planar geometry.<\/li>\n\n\n\n
- Polarity<\/strong>: Nonpolar. The opposing directions of the dipoles cancel out, making the molecule nonpolar.<\/li>\n<\/ul>\n\n\n\n
\n\n\n\nThese are the main structures, hybridizations, geometries, and polarities for each molecule based on their respective bonding.<\/p>\n\n\n\n<\/figure>\n","protected":false},"excerpt":{"rendered":"Molecule AE Lewis Structure EC Hyb’d about X Electronic Geometry Molecular Geometry 3-D P or NP PC13 PC15 C2H4Cl2(1, 1) C2H4Cl2(1, 2) C2H2Cl2(1,1) C2H2Cl2 (1,2-cis) C2H2Cl2 (1,2-trans) The Correct Answer and Explanation is: 1. PCl3 (Phosphorus Trichloride) 2. PCl5 (Phosphorus Pentachloride) 3. C2H4Cl2 (1, 1-Dichloroethene) 4. C2H4Cl2 (1, 2-Dichloroethene) 5. C2H2Cl2 (1, 1-Dichloroethene) 6. C2H2Cl2 […]<\/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-261843","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843","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=261843"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=261843"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=261843"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=261843"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\n
These are the main structures, hybridizations, geometries, and polarities for each molecule based on their respective bonding.<\/p>\n\n\n\n Molecule AE Lewis Structure EC Hyb’d about X Electronic Geometry Molecular Geometry 3-D P or NP PC13 PC15 C2H4Cl2(1, 1) C2H4Cl2(1, 2) C2H2Cl2(1,1) C2H2Cl2 (1,2-cis) C2H2Cl2 (1,2-trans) The Correct Answer and Explanation is: 1. PCl3 (Phosphorus Trichloride) 2. PCl5 (Phosphorus Pentachloride) 3. C2H4Cl2 (1, 1-Dichloroethene) 4. C2H4Cl2 (1, 2-Dichloroethene) 5. C2H2Cl2 (1, 1-Dichloroethene) 6. C2H2Cl2 […]<\/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-261843","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843","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=261843"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/261843\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=261843"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=261843"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=261843"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}<\/figure>\n","protected":false},"excerpt":{"rendered":"