[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-0-en-105":3,"doc-seo-664704-105":59,"doc-detail-664704-en":122},{"code":4,"msg":5,"data":6},0,"success",[7,13,18,23,28,33,38,43,48,51,55],{"id":8,"doc_module":4,"doc_module_name":9,"category_name":10,"show_sort_weight":11,"slug":12},1,"Document","Story & Novel",90,"story-novel",{"id":14,"doc_module":4,"doc_module_name":9,"category_name":15,"show_sort_weight":16,"slug":17},2,"Literature",80,"literature",{"id":19,"doc_module":4,"doc_module_name":9,"category_name":20,"show_sort_weight":21,"slug":22},4,"Exam",70,"exam",{"id":24,"doc_module":4,"doc_module_name":9,"category_name":25,"show_sort_weight":26,"slug":27},5,"Comic",60,"comic",{"id":29,"doc_module":4,"doc_module_name":9,"category_name":30,"show_sort_weight":31,"slug":32},6,"Technology",50,"technology",{"id":34,"doc_module":4,"doc_module_name":9,"category_name":35,"show_sort_weight":36,"slug":37},7,"Healthcare",40,"healthcare",{"id":39,"doc_module":4,"doc_module_name":9,"category_name":40,"show_sort_weight":41,"slug":42},8,"Research & Report",30,"research-report",{"id":44,"doc_module":4,"doc_module_name":9,"category_name":45,"show_sort_weight":46,"slug":47},9,"Religion & Spirituality",20,"religion-spirituality",{"id":46,"doc_module":4,"doc_module_name":9,"category_name":49,"show_sort_weight":46,"slug":50},"World Cup","world-cup",{"id":52,"doc_module":4,"doc_module_name":9,"category_name":53,"show_sort_weight":52,"slug":54},10,"Lifestyle","lifestyle",{"id":56,"doc_module":4,"doc_module_name":9,"category_name":57,"show_sort_weight":24,"slug":58},19,"General","general",{"code":4,"msg":60,"data":61},"ok",{"site_id":62,"language":63,"slug":64,"title":65,"keywords":66,"description":67,"schema_data":68,"social_meta":115,"head_meta":117,"extra_data":119,"updated_unix":121},105,"en","molecular-shapes-laboratory-introduction-to-vsepr-theory","Molecular Shapes Laboratory - Introduction to VSEPR Theory","","Molecular Shapes Laboratory introduces Valence Shell Electron Pair Repulsion (VSEPR) theory as a method for predicting molecular geometry and bonding. Students learn how to sketch Lewis structures, determine steric numbers and electron group geometry, and relate these to molecular shape using ligand number. The material explains sigma and pi bonds and shows how orbital overlap sketches visualize lone pairs and electron density. Computer models are used to verify predictions against experimental validation.",{"@graph":69,"@context":114},[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":40,"@type":76,"position":81},"https://docshare.wps.com/document/research-report/",3,{"item":83,"name":65,"@type":76,"position":19},"https://docshare.wps.com/document/molecular-shapes-laboratory-introduction-to-vsepr-theory/664704/",{"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/molecular-shapes-laboratory-introduction-to-vsepr-theory/664704.png","ImageObject",300,407,{"name":92,"@type":93},"Syukur Setiap Hari","Person",{"url":74,"name":95,"@type":96},"DocShare","Organization","application/pdf","2026-10-30","2026-10-29",true,{"@type":102,"interactionType":103,"userInteractionCount":81},"InteractionCounter",{"@type":104},"ViewAction",{"@type":106,"mainEntity":107},"FAQPage",[108],{"name":109,"@type":110,"acceptedAnswer":111},"What is an orbital overlap sketch and why is it used?","Question",{"text":112,"@type":113},"An orbital overlap sketch is a geometric representation that shows atoms along with lone pairs and bonding pairs. It visualizes sigma (σ) and pi (π) bonds so the electron-pair geometry and resulting molecular shape can be understood clearly.","Answer","https://schema.org",{"og:url":83,"og:type":116,"og:title":65,"og:site_name":95,"og:description":67},"article",{"robots":118,"canonical":83},"index,follow",{"doc_id":120,"site_id":62},664704,1793267802,{"code":4,"msg":5,"data":123},{"doc_id":120,"user_id":124,"nickname":92,"user_avatar":125,"doc_module":4,"category_id":39,"category_name":40,"doc_title":65,"doc_description":67,"doc_content":126,"file_id":127,"file_url":128,"file_type":129,"file_size":130,"view_count":81,"is_deleted":4,"is_public":8,"is_downloadable":8,"audit_status":8,"page_count":131,"language":132,"language_code":63,"site_id":62,"html_lang":63,"table_of_contents":133,"faqs":134,"seo_title":135,"seo_description":67,"update_tm":121,"read_time":136},962093541965,"https://ap-avatar.wpscdn.com/davatar_276721f389ce27ea32af1340a28f341c","Molecular Shapes Laboratory  \nIntroduction to VSEPR Theory  \nThis laboratory introduces the concept of Valence Shell Electron Pair Repulsion (VSEPR) theory and the molecular geometry and bonding that it describes. In this exercise, we use VSEPR theory to predict the shapes of various molecules. This process is critical to a proper understanding of general chemistry. The VSEPR theory’s description of bonding is also essential to a detailed comprehension of chemical properties and reactions.  \nVSEPR theory deals with covalent bonding in molecules (bonding that shares pairs of electrons between two or more atoms) . By assigning electrons to bonding and non-bonding pairs and distributing these pairs of electrons around an atom, it is possible to predict the preferred spatial arrangement of bonds by simply spacing the electrons as far apart from each other as possible. To determine this arrangement, you must first sketch a Lewis structure of the molecule. Next, use the Lewis structure to find the steric number of the central atom or atoms. The steric number determines the electron group geometry and hybridization. The ligand number is the number of atoms which are bonded to the central atom. The molecular shape is determined by the electron group geometry and the ligand number.  \nFigure 1: Steric number = 4, tetrahedral  \nelectron group geometry of H2O  \nFigure 2: Ligand number = 2, bent molecular  \nshape of H2O  \nFigures 1 and 2 illustrate the difference between electron group geometry and molecular shape. On the next page, Table 1 lists the possible molecular shapes and how they are derived from steric numbers, electron group geometries, and ligand numbers.  \n\n| Steric \\# | Electron Group Geometry | Ligand \\# | Molecular Shape | Bond Angles |\n| --- | --- | --- | --- | --- |\n| 2 | Linear | 2 | Linear | 180 |\n| 3 | Trigonal plane | 3 | Trigonal plane | 120 |\n|  |  | 2 | Bent | \u003C120 |\n| 4 | Tetrahedron | 4 | Tetrahedron | 109.5 |\n|  |  | 3 | Trigonal pyramid | \u003C109 .5 |\n|  |  | 2 | Bent | \u003C109 .5 |\n| 5 | Trigonal bipyramid | 5 | Trigonal bipyramid | 120, 90 |\n|  |  | 4 | See-saw | \u003C120, \u003C90 |\n|  |  | 3 | Tee | \u003C90 |\n|  |  | 2 | Linear | 180 |\n| 6 | Octahedron | 6 | Octahedron | 90 |\n|  |  | 5 | Square pyramid | \u003C90 |\n|  |  | 4 | Square planar | 90 |\n\nTable 1: Molecular Shapes  \nWe will be using computer models to verify the VSEPR predictions we make. These models have been validated by experiment, so we will not need to experimentally measure any molecules. In later chemistry courses, you will have the opportunity to learn some of the methods that are used to test computational models.  \nOrbital Overlap Sketches  \nThe best way to visualize the electron pair repulsion described by the VSEPR theory is to draw a geometric representation of each model that we will call an orbital overlap sketch. The sketch will display each atom, represented by a letter or two of text, surrounded with lone pair and bonding pair electrons. Covalent bonding pairs of electrons can come in two varieties: sigma (σ) and pi (π) bonds. Each of these will be represented by a different geometry that is clearly visible in the orbital overlap sketch. An orbital overlap sketch for ethene (also known as ethylene, C2H4) is shown in Figure 3.  \nFigure 3. Orbital overlap sketch of ethene.  \nIn this sketch, each carbon atom is represented by a C and each hydrogen atom by an H, and they are spaced apart to make the best possible two-dimensional representation of a three-dimensional molecule. On each H atom is a spherical 1s shell of electron density that is used in bonding, and on each C atom are three oval sp2 orbitals that construct a σ bond between each C and H and between the two carbons. There is a shared pair of electrons in each of these σ bonds. There is also a π bond in ethene, shown as the“goalposts” above and below the plane of the rest of the C2H4 molecule. A dashed line above and below the central σ bond represents the single π bond in this molecule.  \nIt is ","cbCais3zsr3iwbEz","https://ap.wps.com/l/cbCais3zsr3iwbEz","pdf",686309,11,"English","# Molecular Shapes Laboratory\n## Introduction to VSEPR Theory\n## Predicting Molecular Shapes with VSEPR\n## Steric Number, Electron Group Geometry, and Ligand Number\n## Molecular Shapes Table\n## Verifying Predictions with Computer Models\n## Orbital Overlap Sketches\n## Sigma and Pi Bonds\n## Examples: Ethene and E thyne\n## Example: Acetic Acid and Lewis Dot Diagrams","[{\"question\":\"What is an orbital overlap sketch and why is it used?\",\"answer\":\"An orbital overlap sketch is a geometric representation that shows atoms along with lone pairs and bonding pairs. It visualizes sigma (σ) and pi (π) bonds so the electron-pair geometry and resulting molecular shape can be understood clearly.\"}]","Molecular Shapes Laboratory - Introduction to VSEPR Theory | PDF",28]