Name: BF3 Boron Trifluoride Lewis Structure: 3-D Sketch: F: B-F 1: F: F Hybridization: Polarity: sp non-polar Molecular Shape: Bond Angle: Trigonal Planar 120\u00b0<\/p>\n\n\n\n
Name: CIF: Lewis Structure: Chlorine Trifluoride 3-D Sketch: Hybridization: Polarity: Molecular Shape: Bond Angle:<\/p>\n\n\n\n
Name: KrCl4 Krypton Tetrachloride Lewis Structure: 3-D Sketch: Hybridization: Polarity: Molecular Shape: Bond Angle:<\/p>\n\n\n\n
Name: SeCl4 Selenium Tetrachloride Lewis Structure: 3-D Sketch: Hybridization: Polarity: Molecular Shape: Bond Angle:<\/p>\n\n\n\n
Name: CH2Cl2 Dichloromethane Lewis Structure: 3-D Sketch: Hybridization: Polarity: Molecular Shape: Bond Angle:<\/p>\n\n\n\n
The Correct Answer and Explanation is:<\/mark><\/strong><\/p>\n\n\n\n Here’s a complete chart filled in for the molecules you listed, followed by a 300-word explanation:<\/p>\n\n\n\n Understanding molecular geometry starts with drawing Lewis structures<\/strong>, which show how atoms share electrons. Once this is done, we apply the Valence Shell Electron Pair Repulsion (VSEPR)<\/strong> theory to predict molecular shapes, hybridization, bond angles, and polarity.<\/p>\n\n\n\n Let\u2019s begin with BF\u2083<\/strong>. Boron forms three bonds with fluorine and has no lone pairs, forming a trigonal planar<\/strong> structure with sp\u00b2 hybridization<\/strong>. The symmetry leads to a non-polar<\/strong> molecule with 120\u00b0 bond angles<\/strong>.<\/p>\n\n\n\n Next, ClF\u2083<\/strong> is more complex. Chlorine bonds with three fluorines and has two lone pairs. This gives a T-shaped<\/strong> structure (from a trigonal bipyramidal arrangement), and the hybridization is sp\u00b3d<\/strong>. The uneven lone pairs make it polar<\/strong>, and the bond angles are slightly less than 90\u00b0<\/strong> due to lone pair repulsion.<\/p>\n\n\n\n KrCl\u2084<\/strong>, a rare compound, has krypton surrounded by four chlorine atoms and two lone pairs. This leads to a square planar<\/strong> geometry (common in d\u2078 metal complexes, but also applies here), with sp\u00b3d\u00b2 hybridization<\/strong>. The molecule is non-polar<\/strong> due to its symmetry, and the bond angles are 90\u00b0<\/strong>.<\/p>\n\n\n\n SeCl\u2084<\/strong> features selenium with four bonded Cl atoms and one lone pair, resulting in a see-saw<\/strong> shape from a trigonal bipyramidal arrangement. The hybridization is sp\u00b3d<\/strong>, and because of the lone pair-induced asymmetry, it is polar<\/strong>. Bond angles are <120\u00b0 and <90\u00b0<\/strong>.<\/p>\n\n\n\n Finally, CH\u2082Cl\u2082<\/strong> (dichloromethane) has a tetrahedral<\/strong> shape with sp\u00b3 hybridization<\/strong>. Since chlorine is more electronegative than hydrogen, the molecule is polar<\/strong>, even though the shape is symmetric. Bond angles are close to 109.5\u00b0<\/strong>.<\/p>\n\n\n\n By combining Lewis structures with VSEPR and hybridization theory, we can reliably predict a molecule’s 3D geometry and chemical behavior.<\/p>\n","protected":false},"excerpt":{"rendered":" Name: BF3 Boron Trifluoride Lewis Structure: 3-D Sketch: F: B-F 1: F: F Hybridization: Polarity: sp non-polar Molecular Shape: Bond Angle: Trigonal Planar 120\u00b0 Name: CIF: Lewis Structure: Chlorine Trifluoride 3-D Sketch: Hybridization: Polarity: Molecular Shape: Bond Angle: Name: KrCl4 Krypton Tetrachloride Lewis Structure: 3-D Sketch: Hybridization: Polarity: Molecular Shape: Bond Angle: Name: SeCl4 Selenium […]<\/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-215504","post","type-post","status-publish","format-standard","hentry","category-exams-certification"],"_links":{"self":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/215504","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=215504"}],"version-history":[{"count":0,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/posts\/215504\/revisions"}],"wp:attachment":[{"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/media?parent=215504"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/categories?post=215504"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.learnexams.com\/blog\/wp-json\/wp\/v2\/tags?post=215504"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}
\n\n\n\n\u2705 Completed Molecular Chart:<\/h3>\n\n\n\n
Name<\/th> Lewis Structure Summary<\/th> 3-D Sketch (Shape Summary)<\/th> Hybridization<\/th> Polarity<\/th> Molecular Shape<\/th> Bond Angle<\/th><\/tr><\/thead> BF\u2083<\/strong> (Boron Trifluoride)<\/td> B central atom, 3 single bonds to F, no lone pairs<\/td> Trigonal Planar<\/td> sp\u00b2<\/td> Non-polar<\/td> Trigonal Planar<\/td> 120\u00b0<\/td><\/tr> ClF\u2083<\/strong> (Chlorine Trifluoride)<\/td> Cl central atom, 3 bonded F atoms, 2 lone pairs<\/td> T-shaped<\/td> sp\u00b3d<\/td> Polar<\/td> T-shaped<\/td> ~87.5\u00b0<\/td><\/tr> KrCl\u2084<\/strong> (Krypton Tetrachloride)<\/td> Kr central atom, 4 bonded Cl atoms, 2 lone pairs<\/td> Square Planar<\/td> sp\u00b3d\u00b2<\/td> Non-polar<\/td> Square Planar<\/td> 90\u00b0<\/td><\/tr> SeCl\u2084<\/strong> (Selenium Tetrachloride)<\/td> Se central atom, 4 bonded Cl atoms, 1 lone pair<\/td> See-Saw<\/td> sp\u00b3d<\/td> Polar<\/td> See-Saw<\/td> <120\u00b0, <90\u00b0<\/td><\/tr> CH\u2082Cl\u2082<\/strong> (Dichloromethane)<\/td> C central atom, 2 H atoms, 2 Cl atoms<\/td> Tetrahedral<\/td> sp\u00b3<\/td> Polar<\/td> Tetrahedral<\/td> 109.5\u00b0<\/td><\/tr><\/tbody><\/table><\/figure>\n\n\n\n
\n\n\n\n\ud83e\udde0 300-Word Explanation:<\/h3>\n\n\n\n