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Explains covalent and co-ordinate (dative covalent) bonding, including orbital overlap concepts such as sigma and pi bonds and hybridisation (sp, sp2, sp3). Uses VSEPR theory with Lewis structures to predict molecular shapes and bond angles, giving worked qualitative examples (e.g., BF3, CO2, CH4, NH3, H2O, SF6, PF5) and describing common geometries like linear, trigonal planar, tetrahedral, and distorted arrangements due to lone pairs.",{"@graph":69,"@context":122},[70,84,105],{"@type":71,"itemListElement":72},"BreadcrumbList",[73,77,79,82],{"item":74,"name":75,"@type":76,"position":8},"https://docshare.wps.com","Home","ListItem",{"item":78,"name":9,"@type":76,"position":14},"https://docshare.wps.com/document/",{"item":80,"name":20,"@type":76,"position":81},"https://docshare.wps.com/document/exam/",3,{"item":83,"name":65,"@type":76,"position":19},"https://docshare.wps.com/document/shapes-of-molecules-learning-outcomes-vsepr-and-molecular-shapes/664707/",{"url":83,"name":65,"@type":85,"image":86,"author":91,"headline":65,"publisher":94,"fileFormat":97,"inLanguage":63,"description":67,"dateModified":98,"datePublished":99,"encodingFormat":97,"isAccessibleForFree":100,"interactionStatistic":101},"DigitalDocument",{"url":87,"@type":88,"width":89,"height":90},"https://docshare.wps.com/thumbnails/shapes-of-molecules-learning-outcomes-vsepr-and-molecular-shapes/664707.png","ImageObject",300,407,{"name":92,"@type":93},"RizkyPratama_92","Person",{"url":74,"name":95,"@type":96},"DocShare","Organization","application/pdf","2026-10-30","2026-10-29",true,{"@type":102,"interactionType":103,"userInteractionCount":19},"InteractionCounter",{"@type":104},"ViewAction",{"@type":106,"mainEntity":107},"FAQPage",[108,114,118],{"name":109,"@type":110,"acceptedAnswer":111},"What is VSEPR theory and how does it predict molecular shape?","Question",{"text":112,"@type":113},"VSEPR theory states that electron pairs around the central atom arrange to minimise repulsion. By examining the Lewis structure and how bond and lone pairs position themselves, the molecular geometry and bond angles can be predicted.","Answer",{"name":115,"@type":110,"acceptedAnswer":116},"How do sigma and pi bonds relate to covalent bonding?",{"text":117,"@type":113},"Covalent bonding can be described through orbital overlap, producing sigma (σ) and pi (π) bonds. Hybridisation (sp, sp2, sp3) explains how orbitals form to create these bonding arrangements.",{"name":119,"@type":110,"acceptedAnswer":120},"Why are molecular shapes distorted in molecules with lone pairs, such as NH3?",{"text":121,"@type":113},"Lone pairs exert greater repulsion than bonding pairs. As a result, electron pairs are arranged so that lone pairs push bonding pairs closer together, distorting the shape away from the regular geometry.","https://schema.org",{"og:url":83,"og:type":124,"og:title":65,"og:site_name":95,"og:description":67},"article",{"robots":126,"canonical":83},"index,follow",{"doc_id":128,"site_id":62},664707,1793267810,{"code":4,"msg":5,"data":131},{"doc_id":128,"user_id":132,"nickname":92,"user_avatar":133,"doc_module":4,"category_id":19,"category_name":20,"doc_title":65,"doc_description":67,"doc_content":134,"file_id":135,"file_url":136,"file_type":137,"file_size":138,"view_count":19,"is_deleted":4,"is_public":8,"is_downloadable":8,"audit_status":8,"page_count":139,"language":140,"language_code":63,"site_id":62,"html_lang":63,"table_of_contents":141,"faqs":142,"seo_title":143,"seo_description":67,"update_tm":129,"read_time":144},962094243231,"https://ap-avatar.wpscdn.com/davatar_155a257f0dc6eb9ab79c44ca47cae57d","Online Classes:Megalecture@gmail.com  \n# 3 Chemical bonding\n\nThis topic introduces the different ways by which chemical bonding occurs and theeffect this can have on physical properties.  \n3.2 shapes of simple molecules  \n# SHAPES OF MOLECULES\n\nwww.megalecture.comMEGA LECTUREFor Live Online Classesmegalecture@gmail.com  \nSHAPES OF MOLECULESwww.youtube.com/megalecture  \nScan:free demo class  \n# 3 Chemical bonding\n\n3.2 Covalent bondingand co-ordinate(dative covalent)bonding includingshapes of simplemolecules  \nwww.megalecture.comMEGA LECTUREFor Live Online Classesmegalecture@gmail.com  \nMEGA LECTURE ·Stuck on this topic?  \nOnline Classes:Megalecture@gmail.com  \nThis topic introduces the different ways by which chemical bonding occurs and the effect this can haveon physical properties.  \n# Learning outcomes\n\nCandidates should be able to:  \n(i)covalent bonding,in molecules such as hydrogen,oxygen,chlorine,hydrogen chloride,carbon dioxide,methane,ethene  \n(ii)co-ordinate (dative covalent)bonding,such as in the formation of theammonium ion and in the Al₂Cl₆molecule  \nb)describe covalent bonding in terms of orbital overlap,giving σ andπbonds,including the concept of hybridisation to form sp,sp²and sp³orbitals (see also Section 14.3)  \nc)explain the shapes of,and bond angles in,molecules by using thequalitative model of electron-pair repulsion(including lone pairs),usingas simple examples:BF₃(trigonal),CO₂(linear),CH₄(tetrahedral),NH₃(pyramidal),H₂O(non-linear),SF₆(octahedral),PF₅(trigonal bipyramidal)  \nd)predict the shapes of,and bond angles in,molecules and ions analogousto those specified in 3.2(b)(see also Section 14.3)  \nSHAPES OF MOLECULESwww.youtube.com/megalecture  \nFree 1-on-1 demo class  \nWhatsApp a tutor +923367801123  \n\n| SHAPES OF MOLECULES  \u003Cbr>The shape of a molecule plays a large part in determining its properties and  \u003Cbr>reactivity.  \u003Cbr>The specific orientation of electron pairs in covalent molecules imparts a  \u003Cbr>characteristic shape to the molecules.  \u003Cbr>The shape of a molecule made of only two atoms,such as H₂or CO,is easy to  \u003Cbr>determine.Only a linear shape is possible when there are two atoms.Determining  \u003Cbr>the shapes of molecules made of more than two atoms is more complicated.  \u003Cbr>Using Valence Shell Electron Pair Repulsion (VSEPR)theory one can predict the  \u003Cbr>shape of a molecule by examining the Lewis structure of the molecule.   |\n| --- |\n\n\n| VSEPR THEORY  \u003Cbr>The electron pairs around the central atom  \u003Cbr>of the molecule arrange themselves to  \u003Cbr>Bonds are closer  \u003Cbr>minimise electronic repulsion and so that  \u003Cbr>together so repulsive  \u003Cbr>forces are greater  \u003Cbr>they can be as far away as possible from  \u003Cbr>Al  \u003Cbr>Bonds are further  \u003Cbr>each other.  \u003Cbr>apart so repulsive  \u003Cbr>forces are less  \u003Cbr>This fact is used to predict molecular shape.  \u003Cbr>All bonds are equally  \u003Cbr>Molecules contain covalent bonds.  \u003Cbr>A、  \u003Cbr>spaced out as far apart  \u003Cbr>as possible  \u003Cbr>As covalent bonds consist of a pair of  \u003Cbr>electrons,each bond will repel other bonds.   |\n| --- |\n\nwww.megalecture.comMEGA LECTUREFor Live Online Classesmegalecture@gmail.com  \nFree 1-on-1 demo class  \nMEGA LECTURE ·Stuck on this topic?  \nSHAPES OF MOLECULESwwW.youtube.com/megalecture  \nVSEPR THEORY  \nBonds willtherefore push each other as far apart as possible to reducethe repulsive forces.  \nBecause the repulsions are equal,the bonds will also be equally spaced.  \n| LINEAR  \u003Cbr>Beryllium chloride has two shared electron pairs around the beryllium  \u003Cbr>atom.  \u003Cbr>These electron pairs have minimum repulsion if they are located as far  \u003Cbr>apart as possible while still bonding the chlorine to the central atom.  \u003Cbr>This condition is met if the electron pairs are located on opposite sides of  \u003Cbr>the molecule,resulting in a linear structure,180°apart:   |\n| --- |\n\nwww.megalecture.comMEGA LECTUREFor Live Online Classesmegalecture@gmail.com  \nSHAPES OF MOLECULESwwW.youtube.com/megalecture  \nFree 1-on-1 demo class  \nMEGA LECTURE ·Stu","cbCaiqAMclSeTxq9","https://ap.wps.com/l/cbCaiqAMclSeTxq9","pdf",3608030,18,"English","# 3 Chemical bonding\n## Shapes of simple molecules\n## Learning outcomes\n## VSEPR theory\n## Linear molecules\n## Trigonal planar\n## Tetrahedral\n## Irregular shapes","[{\"question\":\"What is VSEPR theory and how does it predict molecular shape?\",\"answer\":\"VSEPR theory states that electron pairs around the central atom arrange to minimise repulsion. By examining the Lewis structure and how bond and lone pairs position themselves, the molecular geometry and bond angles can be predicted.\"},{\"question\":\"How do sigma and pi bonds relate to covalent bonding?\",\"answer\":\"Covalent bonding can be described through orbital overlap, producing sigma (σ) and pi (π) bonds. Hybridisation (sp, sp2, sp3) explains how orbitals form to create these bonding arrangements.\"},{\"question\":\"Why are molecular shapes distorted in molecules with lone pairs, such as NH3?\",\"answer\":\"Lone pairs exert greater repulsion than bonding pairs. As a result, electron pairs are arranged so that lone pairs push bonding pairs closer together, distorting the shape away from the regular geometry.\"}]","SHAPES OF MOLECULES - Learning outcomes - VSEPR and molecular shapes | PDF",45]