[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-1-en-105":3,"doc-seo-562231-105":53,"doc-detail-562231-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","dp-ib-chemistry-hl-141-more-structures-shapes-covalent-bonds-and-lewis-structures","DP IB Chemistry - HL - 14.1 More Structures & Shapes - Covalent Bonds and Lewis Structures","","Revision notes for DP IB Chemistry HL covering 14.1 More Structures & Shapes, with a focus on how covalent bonds form through molecular orbital overlap. Explains sigma (σ) bonds from head-on overlap and electron density symmetry between nuclei, then describes pi (π) bonds from sideways p-orbital overlap and their representation in double and triple bonds. Includes worked guidance on bond types in N2 and HCN using orbital overlap and electronic configurations, followed by an introduction to Lewis structures and octet rule exceptions such as incomplete 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 \n 14.1.3 Further VSEPR Theory  \n 14.1.4 Formal Charge  \nPage 1 of 22  \n© 2015 − 2025 Save My Exams, Ltd. · Revision Notes, Topic Questions, Past Papers  \nYour notes  \nHead to www.savemyexams. com for more awesome resources  \n14.1.1 Covalent Bonds  \nSigma Bonds  \nBond overlap in covalent bonds  \n A single covalent bond is formed when two nonmetals combine  \n Each atom that combines has an atomic orbital containing a single unpaired electron  \n When a covalent bond is formed, the atomic orbitals overlap to form a combined orbital containing two electrons  \n This new orbital is called the molecular orbital  \n The greater the atomic orbital overlap, the stronger the bond  \n Sigma (σ) bonds are formed from the head-on/ end-to-end overlap of atomic orbitals  \n The electron density is concentrated between the two nuclei  \n S orbitals overlap this way as well as p to p, and swith p orbitals  \nSigma orbitals can be formed from the end-on overlap ofs orbitals  \nHydrogen }uoride has sigma bonds between sand p orbitals  \nPage 2 of 22  \n© 2015 − 2025 Save My Exams, Ltd. · Revision Notes, Topic Questions, Past Papers  \nYour notes  \nHead to www.savemyexams. com for more awesome resources  \nFluorine has sigma bonds between p orbitals  \n The electron density in a σ bond is symmetrical about a line joining the nuclei of the atoms forming the bond  \n The pair of electrons is found between the nuclei of the two atoms  \n The electrostatic attraction between the electrons and nuclei bonds the atoms to each other  \nPage 3 of 22  \n© 2015 − 2025 Save My Exams, Ltd. · Revision Notes, Topic Questions, Past Papers  \nYour notes  \nHead to www.savemyexams. com for more awesome resources  \nPi Bonds  \nπ bonds  \n Pi (π) bonds are formed from the sideways overlap of adjacent p orbitals  \n The two lobes that make up the π bond lie above and below the plane of the σ bond  \n This maximises overlap of the p orbitals  \n A single π bond is drawn as two electron clouds one arising from each lobe of the p orbitals  \n The two clouds of electrons in a π bond represent one bond containing two electrons  \nπ orbitals are formed by the end-on overlap of p orbitals  \nExamples of sigma & pi bonds Hydrogen  \n The hydrogen atom has only ones orbital  \n Thes orbitals ofthe two hydrogen atoms will overlap to form a σ bond  \nDirect overlap of the 1s orbitalsofthe hydrogen atoms results in the formation of a σ bond  \nEthene  \nPage 4 of 22  \n© 2015 − 2025 Save My Exams, Ltd. · Revision Notes, Topic Questions, Past Papers  \nYour notes  \nHead to www.savemyexams. com for more awesome resources  \n Each carbon atom uses three of its four electrons to form σ bonds  \n Two σ bonds are formed with the hydrogen atoms  \n One σ bond is formed with the other carbon atom  \n The fourth electron from each carbon atom occupies a p orbital which overlaps sideways with another p orbital on the other carbon atom to form a π bond  \n This means that the C-C is a double bond: one σ and one π bond  \nOverlap of thep orbitals results in the forming of a π bond in ethene  \nPage 5 of 22  \n© 2015 − 2025 Save My Exams, Ltd. · Revision Notes, Topic Questions, Past Papers  \nYour notes  \nHead to www.savemyexams. com for more awesome resources  \nEach carbon atom in ethene forms two sigma bonds with hydrogen atoms and one σ bond with another carbon atom. The fourth electron is used to forma π bond between the two carbon atoms  \nEthyne  \n This molecule contains a triple bond formed from two π bonds (at right angles to each other) and one σ bond  \n Each carbon atom uses two of its four electrons to form σ bonds  \n One σ bond is formed with the hydrogen atom  \n One σ bond is formed with the other carbon atom  \n Two electrons are used to form two π bonds with the other carbon atom  \nEthynehasa triple bond formed from two π bonds and one σ bond ","cbCaitLXHmffMgWf","https://ap.wps.com/l/cbCaitLXHmffMgWf","pdf",3080856,22,"English","# 14.1 More Structures & Shapes\n## 14.1.1 Covalent Bonds\n## 14.1.2 More Lewis Structures","[{\"question\":\"How are sigma (σ) bonds formed in covalent bonding?\",\"answer\":\"Sigma bonds form from head-on (end-to-end) overlap of atomic orbitals, concentrating electron density between the two nuclei.\"},{\"question\":\"What is the difference between pi (π) bonds and sigma (σ) bonds?\",\"answer\":\"Pi bonds form from sideways overlap of adjacent p orbitals, creating electron density above and below the plane of the sigma bond.\"},{\"question\":\"How does the octet rule relate to Lewis structures, and what are common exceptions?\",\"answer\":\"The octet rule states that atoms aim for 8 electrons in their valence shell, but exceptions include elements that can form incomplete octets (as listed for elements such as H, Li, Be, B, and Al).\"}]","DP IB Chemistry - HL - 14.1 More Structures & Shapes - Covalent Bonds and Lewis Structures | PDF",1791808067,8]