[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-1-en-105":3,"doc-seo-562206-105":53,"doc-detail-562206-en":126},{"code":4,"msg":5,"data":6},0,"success",[7,14,19,24,29,34,39,44,49],{"id":8,"doc_module":9,"doc_module_name":10,"category_name":11,"show_sort_weight":12,"slug":13},11,1,"Template","Presentations",90,"presentations",{"id":15,"doc_module":9,"doc_module_name":10,"category_name":16,"show_sort_weight":17,"slug":18},12,"Resumes",80,"resumes",{"id":20,"doc_module":9,"doc_module_name":10,"category_name":21,"show_sort_weight":22,"slug":23},14,"Invoices",70,"invoices",{"id":25,"doc_module":9,"doc_module_name":10,"category_name":26,"show_sort_weight":27,"slug":28},15,"Posters",60,"posters",{"id":30,"doc_module":9,"doc_module_name":10,"category_name":31,"show_sort_weight":32,"slug":33},16,"Social Media",50,"social-media",{"id":35,"doc_module":9,"doc_module_name":10,"category_name":36,"show_sort_weight":37,"slug":38},17,"Forms",40,"forms",{"id":40,"doc_module":9,"doc_module_name":10,"category_name":41,"show_sort_weight":42,"slug":43},18,"Letters",30,"letters",{"id":45,"doc_module":9,"doc_module_name":10,"category_name":46,"show_sort_weight":47,"slug":48},21,"Paper Templates",5,"papers-templates",{"id":50,"doc_module":9,"doc_module_name":10,"category_name":51,"show_sort_weight":4,"slug":52},158,"General","general-158",{"code":4,"msg":54,"data":55},"ok",{"site_id":56,"language":57,"slug":58,"title":59,"keywords":60,"description":61,"schema_data":62,"social_meta":119,"head_meta":121,"extra_data":123,"updated_unix":125},105,"en","molecular-geometry-chart","Molecular Geometry Chart","","This reference chart provides a comprehensive overview of molecular geometry based on the Valence Shell Electron Pair Repulsion (VSEPR) theory. It details the relationship between the number of electron groups, the count of lone pairs, electron pair arrangements, and resulting molecular geometries. The document covers configurations ranging from two to six electron groups, including specific examples like linear, trigonal planar, tetrahedral, trigonal bipyramidal, and octahedral shapes. It also includes associated approximate bond angles for each geometric configuration, offering a clear guide for students and professionals to predict molecular structures effectively.",{"@graph":63,"@context":118},[64,80,101],{"@type":65,"itemListElement":66},"BreadcrumbList",[67,71,74,77],{"item":68,"name":69,"@type":70,"position":9},"https://docshare.wps.com","Home","ListItem",{"item":72,"name":10,"@type":70,"position":73},"https://docshare.wps.com/template/",2,{"item":75,"name":51,"@type":70,"position":76},"https://docshare.wps.com/template/general/",3,{"item":78,"name":59,"@type":70,"position":79},"https://docshare.wps.com/template/molecular-geometry-chart/562206/",4,{"url":78,"name":59,"@type":81,"image":82,"author":87,"headline":59,"publisher":90,"fileFormat":93,"inLanguage":57,"description":61,"dateModified":94,"datePublished":95,"encodingFormat":93,"isAccessibleForFree":96,"interactionStatistic":97},"DigitalDocument",{"url":83,"@type":84,"width":85,"height":86},"https://docshare.wps.com/thumbnails/molecular-geometry-chart/562206.png","ImageObject",442,249,{"name":88,"@type":89},"pixelkiddo","Person",{"url":68,"name":91,"@type":92},"DocShare","Organization","application/pdf","2026-10-27","2026-10-12",true,{"@type":98,"interactionType":99,"userInteractionCount":20},"InteractionCounter",{"@type":100},"ViewAction",{"@type":102,"mainEntity":103},"FAQPage",[104,110,114],{"name":105,"@type":106,"acceptedAnswer":107},"What is the molecular geometry for a molecule with 4 electron groups and 2 lone pairs?","Question",{"text":108,"@type":109},"The molecular geometry for 4 electron groups with 2 lone pairs is classified as bent, with bond angles of approximately 105 degrees.","Answer",{"name":111,"@type":106,"acceptedAnswer":112},"How do lone pairs affect bond angles in molecular geometry?",{"text":113,"@type":109},"Lone pairs exert greater repulsive forces than bonding pairs, which typically leads to a reduction in the bond angles compared to the ideal geometry of a molecule without lone pairs.",{"name":115,"@type":106,"acceptedAnswer":116},"What is the approximate bond angle for a linear molecule with 2 electron groups and 0 lone pairs?",{"text":117,"@type":109},"A linear molecule with 2 electron groups and 0 lone pairs has an approximate bond angle of 180 degrees.","https://schema.org",{"og:url":78,"og:type":120,"og:title":59,"og:site_name":91,"og:description":61},"article",{"robots":122,"canonical":78},"index,follow",{"doc_id":124,"site_id":56},562206,1792008169,{"code":4,"msg":5,"data":127},{"doc_id":124,"user_id":128,"nickname":88,"user_avatar":129,"doc_module":9,"category_id":50,"category_name":51,"doc_title":59,"doc_description":61,"doc_content":130,"file_id":131,"file_url":132,"file_type":133,"file_size":134,"view_count":20,"is_deleted":4,"is_public":9,"is_downloadable":9,"audit_status":9,"page_count":9,"language":135,"language_code":57,"site_id":56,"html_lang":57,"table_of_contents":136,"faqs":137,"seo_title":138,"seo_description":61,"update_tm":139,"read_time":4},962090883892,"https://ap-avatar.wpscdn.com/avatar/e00115db34f3e0f11b?x-image-process=image/resize,m_fixed,w_180,h_180&k=1790152879550218658","Molecular Geometry Chart  \n\n| \\# of Electron\u003Cbr>Groups | Number of\u003Cbr>Lone Pairs | Electron Pair\u003Cbr>Arrangement | Molecular Geometry |  |  |  |  | Approximate\u003Cbr>Bond Angles |\n| --- | --- | --- | --- | --- | --- | --- | --- | --- |\n| 2 | 0 | linear | 180o |  |  |  |  | 180° |\n| 3 | 0 | trigonal planar | \u003Cbr>120o |  |  |  |  | 120° |\n|  | 1 | bent | \u003Cbr>\u003C120o |  |  |  |  | \u003C120° |\n| 4 | 0 | tetrahedral | \u003Cbr>109.5o |  |  |  |  | 109.5° |\n|  | 1 | trigonal pyramid | \u003Cbr>\u003Cbr>\u003C109 .5o |  |  |  |  | \u003C109 .5° ( ~ 107°) |\n|  | 2 | bent | \u003Cbr> \u003C109 .5o |  |  |  |  | \u003C109 .5°(~ 105°) |\n| 5 | 0 | trigonal\u003Cbr>bipyramidal | 120o\u003Cbr>\u003Cbr>|  |  |  |  | 90°, 120° |\n|  | 1 | see-saw | \u003C90o \u003Cbr>\u003Cbr>\u003Cbr>\u003C120o\u003Cbr>\u003Cbr>\u003Cbr>\u003Cbr>\u003Cbr>\u003Cbr>\u003Cbr>|  |  |  |  | \u003C90°, \u003C120° |\n|  | 2 | T-structure | \u003Cbr>\u003C90o\u003Cbr>|  |  |  |  | \u003C90° |\n|  | 3 | linear | |  |  | 180o |  | 180° |\n| 6 | 0 | octahehral | |  | 90o\u003Cbr>\u003Cbr> 90o\u003Cbr>|  |  | 90°, 90° |\n|  | 1 | square pyramidal | \u003C90o | \u003Cbr>|  |  | 90o | 90°, \u003C90° |\n|  | 2 | square planar | \u003Cbr>\u003Cbr>\u003Cbr>\u003Cbr>90o |  |  |  |  | 90° |","cbCaip2vqB1UJAsd","https://ap.wps.com/l/cbCaip2vqB1UJAsd","pdf",541119,"English","# Molecular Geometry Analysis\n## Electron Group Configurations\n## Bond Angle Reference","[{\"question\":\"What is the molecular geometry for a molecule with 4 electron groups and 2 lone pairs?\",\"answer\":\"The molecular geometry for 4 electron groups with 2 lone pairs is classified as bent, with bond angles of approximately 105 degrees.\"},{\"question\":\"How do lone pairs affect bond angles in molecular geometry?\",\"answer\":\"Lone pairs exert greater repulsive forces than bonding pairs, which typically leads to a reduction in the bond angles compared to the ideal geometry of a molecule without lone pairs.\"},{\"question\":\"What is the approximate bond angle for a linear molecule with 2 electron groups and 0 lone pairs?\",\"answer\":\"A linear molecule with 2 electron groups and 0 lone pairs has an approximate bond angle of 180 degrees.\"}]","Molecular Geometry Chart | PDF",1791808022]