[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-0-en-105":3,"doc-seo-657097-105":59,"doc-detail-657097-en":130},{"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":123,"head_meta":125,"extra_data":127,"updated_unix":129},105,"en","lecture-note-lewis-dot-diagrams","Lecture Note - Lewis Dot Diagrams","","Lesson notes explain how to construct Lewis dot diagrams by using valence electrons around an element symbol, and how electron sharing creates bonding. Definitions cover valence electrons, bonding spots, lone pairs, bonding pairs, octet and sub-octet, and compare structural diagrams using lines instead of dots. The notes classify bonding into covalent, ionic, and polar/non-polar covalent using electronegativity and electronegativity differences, then practice with bimolecular compounds, central-atom molecules, multiple bonds, polyatomic ions, and dipole labeling exercises.",{"@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/lecture-note-lewis-dot-diagrams/657097/",{"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/lecture-note-lewis-dot-diagrams/657097.png","ImageObject",300,407,{"name":92,"@type":93},"pop out","Person",{"url":74,"name":95,"@type":96},"DocShare","Organization","application/pdf","2026-10-30","2026-10-26",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 does a Lewis dot diagram represent and how do you determine the number of dots?","Question",{"text":112,"@type":113},"A Lewis dot diagram represents the valence electrons of an atom. The number of dots (or x’s) equals the number of valence electrons in the atom’s outer energy level.","Answer",{"name":115,"@type":110,"acceptedAnswer":116},"How are bonding spots, lone pairs, and bonding pairs defined?",{"text":117,"@type":113},"Bonding spots are the available places where bonding can occur. Lone pairs are electron pairs in the outer shell not used in bonding, and bonding pairs are pairs of shared electrons that form a bond.",{"name":119,"@type":110,"acceptedAnswer":120},"How do electronegativity values determine whether a bond is polar or ionic?",{"text":121,"@type":113},"Electronegativity measures an atom’s tendency to attract a bonding pair. When the electronegativity difference (ΔEN) is 0 the bond is non-polar covalent; if ΔEN is greater than 0 but less than 1.7 it is polar covalent, and if ΔEN is greater than 1.7 it is ionic.","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},657097,1793006520,{"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":34,"language":139,"language_code":63,"site_id":62,"html_lang":63,"table_of_contents":140,"faqs":141,"seo_title":142,"seo_description":67,"update_tm":143,"read_time":144},962090760408,"https://ap-avatar.wpscdn.com/davatar_085a072bc5b1113ac321206ff7593b45","Unit \\#1-Module \\#6 – Lecture Note – Lewis Dot Diagrams:  \nLesson and Guided Learning:  \nCovalent bonding Lewis Dot Diagrams: (electrons are shared)  \nA Lewis dot diagram is a representation of the valence electrons of an atom that uses dots (or x’s) around the symbol of the element. The number of dots (x’s) equals the number of valence electrons in the atom.  \nValence Electrons – number of electrons in the outermost energy level (these are involved in bonding)  \nTable 1: Atoms  \n\n| Atom | Group | Valence Electrons | Lewis Dot Diagram | \\# of available\u003Cbr>Bonding spots | \\# of lone pairs |\n| --- | --- | --- | --- | --- | --- |\n| N |  |  |  |  |  |\n| O |  |  |  |  |  |\n| F |  |  |  |  |  |\n| H |  |  |  |  |  |\n| B |  |  |  |  |  |\n| O2- |  |  |  |  |  |\n| Br- |  |  |  |  |  |\n\nTerminology:  \nBonding spots: Number of places available for bonding to take place.  \nLone Pairs: a pair of electrons in the outermost shell of an atom that are not used in bonding  \nBonding Pairs: a pair of electrons that is shared to create a bond  \nOctet: a grouping of eight electrons in an outer energy level of an atom (usually implies stability);  \nSub-octet: a group of less than eight electrons in an outer energy level of an atom (stability occurs if hydrogen has two electrons/ boron has six otherwise for the most part unstable)  \nSingle Bonds – two electrons are shared in a bond  \nStructural diagram – the “shared” electrons are replaced with a line (rather than dots/x’s)  \nTable 2 : Bimolecular (two non-metal atoms in a bond)  \n\n| Molecule | Total available electrons | Lewis Dot Diagram | Structural diagram |\n| --- | --- | --- | --- |\n| Cl2 | 2 x 7 e- = 14 e- |  |  |\n| H2 |  |  |  |\n| F2 |  |  |  |\n\nTable 3 : Molecules with a Central Atom  \n• The central atom is usually the atom with the most bonding sites available;  \n• The central atom can also be shown by being underlined;  \n\n| Molecule | Available\u003Cbr>Electrons | Lewis Dot Diagram | Lone Pairs on the central atom | Bonding pairson the central atom | Structural Diagram |\n| --- | --- | --- | --- | --- | --- |\n| CF4 |  |  |  |  |  |\n\n\n|  |  |  |  |  |  |\n| --- | --- | --- | --- | --- | --- |\n| H2S |  |  |  |  |  |\n| PH3 |  |  |  |  |  |\n| BCl3 |  |  |  |  |  |\n| H2O |  |  |  |  |  |\n\nTable 4 : Molecules with multiple bonds  \n•  Multiple bond is sharing 4 or 6 electrons;  \n•  Double bond – four electrons are shared in a bond; Triple bond – six electrons are shared in a bond;  \n\n| Molecule | Available\u003Cbr>Electrons | Lewis Dot Diagram | Lone Pairs on the central atom | Bonding pairson the central atom | Structural Diagram |\n| --- | --- | --- | --- | --- | --- |\n| CO2 |  |  |  |  |  |\n| HCN |  |  |  |  |  |\n| C2H4 |  |  |  |  |  |\n\nTable 5 : Polyatomic Ions  \n• Molecules with a positive or negative charge  \n\n| Molecule | Available\u003Cbr>Electrons | Lewis Dot Diagram | Lone Pairson the central atom | Bonding pairson the central atom | Structural Diagram |\n| --- | --- | --- | --- | --- | --- |\n| PH4+ |  |  |  |  |  |\n\n\n|  |  |  |  |  |  |\n| --- | --- | --- | --- | --- | --- |\n| ClO- |  |  |  |  |  |\n\nIonic Bonding Lewis Dot Diagrams: (Transfer of Electrons)  \n[Na]+ [F] -[Mg]+2[O]-2  \n[Be]+2[F]2-[K]2+ [O]-2  \nPolar Bonds:  \nElectronegativity is the measure of the tendency of an atom to attract a bonding pair of electrons; Trend in EN – increases up and to the right towards fluorine (being the highest at 4 .0)  \nElectronegativity difference (ᐃEN) is the difference in electronegativities of two bonded atoms. Non-polar covalent bond is when the (ᐃEN) is 0  \nPolar covalent bond is when the (ᐃEN) is greater than 0 but less than 1.7 (may differ slightly in biology); Ionic bond is when the (ᐃEN) is greater than 1.7.  \nDipole is difference in electronegativity between the different atoms;  \nBond dipole difference in electronegativity along a bond.  \nKeeping it simple:  \n(Document Camera examples)  \nIndividual Learning  \n1. Fill in the following chart:  \n\n| Molecule | Available\u003Cbr>Electrons | Lewis Dot Diagram | Lone","cbCaibYVCmRZfpOs","https://ap.wps.com/l/cbCaibYVCmRZfpOs","pdf",295683,"English","# Covalent bonding Lewis dot diagrams\n## Key terms and definitions\n## Lewis dot diagrams vs structural diagrams\n# Bonding categories and electronegativity\n## Polar and non-polar bonds\n## Ionic bonding\n# Guided practice and worksheets\n## Individual learning chart completion\n## Ionic bond and polar bond drawing tasks\n## Answer section for practice problems","[{\"question\":\"What does a Lewis dot diagram represent and how do you determine the number of dots?\",\"answer\":\"A Lewis dot diagram represents the valence electrons of an atom. The number of dots (or x’s) equals the number of valence electrons in the atom’s outer energy level.\"},{\"question\":\"How are bonding spots, lone pairs, and bonding pairs defined?\",\"answer\":\"Bonding spots are the available places where bonding can occur. Lone pairs are electron pairs in the outer shell not used in bonding, and bonding pairs are pairs of shared electrons that form a bond.\"},{\"question\":\"How do electronegativity values determine whether a bond is polar or ionic?\",\"answer\":\"Electronegativity measures an atom’s tendency to attract a bonding pair. When the electronegativity difference (ΔEN) is 0 the bond is non-polar covalent; if ΔEN is greater than 0 but less than 1.7 it is polar covalent, and if ΔEN is greater than 1.7 it is ionic.\"}]","Lecture Note - Lewis Dot Diagrams | PDF",1792974040,18]