[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-seo-657109-105":3,"detail-sidebar-cat-0-en-105":80,"doc-detail-657109-en":130},{"code":4,"msg":5,"data":6},0,"ok",{"site_id":7,"language":8,"slug":9,"title":10,"keywords":11,"description":12,"schema_data":13,"social_meta":73,"head_meta":75,"extra_data":77,"updated_unix":79},105,"en","lewis-structures-shapes-polarities-vsepr-theory-and-molecular-shape","Lewis structures, shapes & polarities - VSEPR theory and molecular shape","","Revision notes explain how Lewis structures and VSEPR theory predict molecular shapes and bond angles by minimizing electron-pair repulsions between bonding pairs and lone pairs. It covers molecules with double/triple bonds as single charge regions, then shows common geometries for 2–4 electron domains, including linear, trigonal planar, tetrahedral, trigonal pyramidal, and bent forms. The notes connect shape symmetry or asymmetry with whether bond dipoles cancel to determine overall molecular polarity, and include worked sample questions.",{"@graph":14,"@context":72},[15,34,55],{"@type":16,"itemListElement":17},"BreadcrumbList",[18,23,27,31],{"item":19,"name":20,"@type":21,"position":22},"https://docshare.wps.com","Home","ListItem",1,{"item":24,"name":25,"@type":21,"position":26},"https://docshare.wps.com/document/","Document",2,{"item":28,"name":29,"@type":21,"position":30},"https://docshare.wps.com/document/exam/","Exam",3,{"item":32,"name":10,"@type":21,"position":33},"https://docshare.wps.com/document/lewis-structures-shapes-polarities-vsepr-theory-and-molecular-shape/657109/",4,{"url":32,"name":10,"@type":35,"image":36,"author":41,"headline":10,"publisher":44,"fileFormat":47,"inLanguage":8,"description":12,"dateModified":48,"datePublished":49,"encodingFormat":47,"isAccessibleForFree":50,"interactionStatistic":51},"DigitalDocument",{"url":37,"@type":38,"width":39,"height":40},"https://docshare.wps.com/thumbnails/lewis-structures-shapes-polarities-vsepr-theory-and-molecular-shape/657109.png","ImageObject",300,407,{"name":42,"@type":43},"sagouaw","Person",{"url":19,"name":45,"@type":46},"DocShare","Organization","application/pdf","2026-10-30","2026-10-26",true,{"@type":52,"interactionType":53,"userInteractionCount":30},"InteractionCounter",{"@type":54},"ViewAction",{"@type":56,"mainEntity":57},"FAQPage",[58,64,68],{"name":59,"@type":60,"acceptedAnswer":61},"How does VSEPR theory predict the shape of a molecule?","Question",{"text":62,"@type":63},"VSEPR predicts shape by considering repulsions between electron pairs around a central atom, including bonding pairs and lone pairs. The geometry that keeps repulsive forces to a minimum gives the observed shape and bond angles.","Answer",{"name":65,"@type":60,"acceptedAnswer":66},"Why do double or triple bonds count as single regions of negative charge in VSEPR?",{"text":67,"@type":63},"In a double or triple bond, the electron pairs stay together, so the bonded electrons are treated as one region of negative charge. This allows the model to use electron-domain counts to determine overall geometry.",{"name":69,"@type":60,"acceptedAnswer":70},"How do symmetry and molecular shape determine whether a molecule is polar?",{"text":71,"@type":63},"First identify polar bonds and draw bond dipoles. Then compare the overall molecular shape: if it is symmetrical, bond dipoles cancel and the molecule is non-polar; if asymmetrical, dipoles do not cancel and the molecule is polar overall.","https://schema.org",{"og:url":32,"og:type":74,"og:title":10,"og:site_name":45,"og:description":12},"article",{"robots":76,"canonical":32},"index,follow",{"doc_id":78,"site_id":7},657109,1792974281,{"code":4,"msg":81,"data":82},"success",[83,87,91,94,99,104,109,114,119,122,126],{"id":22,"doc_module":4,"doc_module_name":25,"category_name":84,"show_sort_weight":85,"slug":86},"Story & Novel",90,"story-novel",{"id":26,"doc_module":4,"doc_module_name":25,"category_name":88,"show_sort_weight":89,"slug":90},"Literature",80,"literature",{"id":33,"doc_module":4,"doc_module_name":25,"category_name":29,"show_sort_weight":92,"slug":93},70,"exam",{"id":95,"doc_module":4,"doc_module_name":25,"category_name":96,"show_sort_weight":97,"slug":98},5,"Comic",60,"comic",{"id":100,"doc_module":4,"doc_module_name":25,"category_name":101,"show_sort_weight":102,"slug":103},6,"Technology",50,"technology",{"id":105,"doc_module":4,"doc_module_name":25,"category_name":106,"show_sort_weight":107,"slug":108},7,"Healthcare",40,"healthcare",{"id":110,"doc_module":4,"doc_module_name":25,"category_name":111,"show_sort_weight":112,"slug":113},8,"Research & Report",30,"research-report",{"id":115,"doc_module":4,"doc_module_name":25,"category_name":116,"show_sort_weight":117,"slug":118},9,"Religion & Spirituality",20,"religion-spirituality",{"id":117,"doc_module":4,"doc_module_name":25,"category_name":120,"show_sort_weight":117,"slug":121},"World Cup","world-cup",{"id":123,"doc_module":4,"doc_module_name":25,"category_name":124,"show_sort_weight":123,"slug":125},10,"Lifestyle","lifestyle",{"id":127,"doc_module":4,"doc_module_name":25,"category_name":128,"show_sort_weight":95,"slug":129},19,"General","general",{"code":4,"msg":81,"data":131},{"doc_id":78,"user_id":132,"nickname":42,"user_avatar":133,"doc_module":4,"category_id":33,"category_name":29,"doc_title":10,"doc_description":12,"doc_content":134,"file_id":135,"file_url":136,"file_type":137,"file_size":138,"view_count":30,"is_deleted":4,"is_public":22,"is_downloadable":22,"audit_status":22,"page_count":30,"language":139,"language_code":8,"site_id":7,"html_lang":8,"table_of_contents":140,"faqs":141,"seo_title":142,"seo_description":12,"update_tm":79,"read_time":110},3985747862151,"https://ap-avatar.wpscdn.com/davatar_a8503ba1806abce46bf441b54a3ca4cd","Describe the nature of structure and bonding in different substances  \nLevel 2 Credits 4  \nRevision notes for “Lewis structures, shapes & polarities”  \nValence shell electron pair repulsion theory  \nThis is used to predict the shapes of simple molecules and ions by considering the repulsions between pairs of electrons (bonding pairs and non-bonding (lone) pairs) . The shape that results isone that keeps repulsive forces to a minimum (ie the arrangement that keeps the regions of negative charge as far apart as possible) .  \nShapes of Molecules with Double or Triple Bonds  \nSince in a double or triple bond, the electron pairs stay together, we treat them as single regions of negative charge. Eg, in carbon dioxide (CO2) the oxygen atoms are double bonded to the central carbon atom. The carbon atom has no  \nO ~~ ~~ C  \nO  \nlone pairs. The two double bonds are two regions of negative charge. The molecule is linear.  \n\n| Regions of\u003Cbr>negative\u003Cbr>charge | Shape around central atom & bond angles | Example | Shapes |\n| --- | --- | --- | --- |\n| 2 | Linear, 180o | | linear |\n| 3 | Trigonal planar, 120o | | 3 bond pairs / regions of negative charge – trigonal planar\u003Cbr>2 bond pairs & 1 lone pair = angular (approx 120o) |\n| 4 | Tetrahedral, 109.5o | | 4 bond pairs = tetrahedral eg NH4+ , CCl4\u003Cbr>3 bond pairs & 1 lone pair = trigonal pyramidal eg NH3 (approx 107o)*\u003Cbr>2 bond pairs & 2 lone pairs = angular or v-shaped eg H2O (approx 105o)** |\n\n*Ammonia: 3 bond pairs and 1 lone pair (total = 4 pairs) so the shape is based on a tetrahedron. As the lone pair-bond pair repulsions are greater than bond pair-bond pair repulsions the H-N-H bond angle is reduced from 109.5° to 107° .  \n**Water: 2 bond pairs and 2 lone pairs (total = 4 pairs) so the shape is based on a tetrahedron. The lone pair-lone pair repulsion pushes the H-O-H bond angle down further to about 105° .  \nSpecies with lone pairs. Lone pairs have a greater repulsive force than bonding pairs so their presence affects bond angles. The order of repulsion is:  \nlone pair – lone pair > lone pair – bonding pair > bonding pair-bonding pair  \nAlso the actual shape of the molecule does not include the lone responsible for determining the shape.  \nEg water has 4 electron pairs around the O atom but the shape is angular or V-shaped.  \npairs even though they are  \noverall  \nH  \nO ~~ ~~ H  \n\\Examples  \n􀁇􀀎 􀁇 􀀐 􀁇􀀎 􀁇 􀀐  \nThe B-F and P-F bonds would be polar.  \n\n| BF3 | F\u003Cbr>\u003Cbr>\u003Cbr>B ~~ ~~ F  F\u003Cbr>\u003Cbr>| trigonal\u003Cbr>planar | Repulsion of 3 regions of negative charge around -all are bonding\u003Cbr>B is electron deficient | BF3 is non-polar. The trigonal pyramid molecule is symmetrical about the central B atom, so bond dipoles cancel / there is a symmetrical distribution of charge about the central atom. |\n| --- | --- | --- | --- | --- |\n| PF3 | \u003Cbr> F \u003Cbr>\u003Cbr> F ~~ ~~ P \u003Cbr>\u003Cbr> F  | trigonal\u003Cbr>pyramid | Repulsion of four regions of negative charge around Pthree bonding, one non bonding | PF3 is polar. The trigonal pyramid molecule is asymmetrical about the central P atom, so the P–F bond dipoles add to give a net dipole / thereis an asymmetric distribution of charge about the central atom. |\n\nExplaining why a molecule is polar or not. Think    \n1. Are there polar bonds? (Think F O N/Cl   S   H) . If yes draw in the dipole over the bonds.􀁇􀀎 􀁇 􀀐   \nH – O or H-O  \n2. Consider the shape of the overall molecule; write one of the following statements: Choose ONE of the middle four options (!) but don’t mix and match “dipoles” and “centres” and “charge distribution” randomly. Learn a pair of statements you will be able to remember and use.  \n\n| Molecule is\u003Cbr>symmetrical | SO | bond dipoles cancel out there is no net dipole the centres of +ve and –ve charge coincide there is an even distribution of charge about central atom | AND | molecule is therefore NON POLAR OVERALL |  |\n| --- | --- | --- | --- | --- | --- |\n| Molecule is\u003Cbr>asymmetrical\u003Cbr>(not\u003Cbr>symmetrical) | SO | the bond dipoles do not cancel out ","cbCaiiZjJVSvebC9","https://ap.wps.com/l/cbCaiiZjJVSvebC9","pdf",431575,"English","# Valence shell electron pair repulsion theory\n## Predicting molecular shapes from electron-pair repulsions\n# Shapes with double or triple bonds\n# Electron-domain count and common geometries\n## 2 domains: linear\n## 3 domains: trigonal planar\n## 4 domains: tetrahedral and variants\n# Lone pairs and repulsion order\n# Determining whether a molecule is polar or non-polar\n## Polar bonds and dipole cancellation\n## Symmetrical vs asymmetrical molecules\n# Sample questions and answers","[{\"question\":\"How does VSEPR theory predict the shape of a molecule?\",\"answer\":\"VSEPR predicts shape by considering repulsions between electron pairs around a central atom, including bonding pairs and lone pairs. The geometry that keeps repulsive forces to a minimum gives the observed shape and bond angles.\"},{\"question\":\"Why do double or triple bonds count as single regions of negative charge in VSEPR?\",\"answer\":\"In a double or triple bond, the electron pairs stay together, so the bonded electrons are treated as one region of negative charge. This allows the model to use electron-domain counts to determine overall geometry.\"},{\"question\":\"How do symmetry and molecular shape determine whether a molecule is polar?\",\"answer\":\"First identify polar bonds and draw bond dipoles. Then compare the overall molecular shape: if it is symmetrical, bond dipoles cancel and the molecule is non-polar; if asymmetrical, dipoles do not cancel and the molecule is polar overall.\"}]","Lewis structures, shapes & polarities - VSEPR theory and molecular shape | PDF"]