[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-0-en-105":3,"doc-seo-657106-105":59,"doc-detail-657106-en":134},{"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":127,"head_meta":129,"extra_data":131,"updated_unix":133},105,"en","lewis-structures-notes-part-1-basic-review","LEWIS STRUCTURES NOTES - PART 1 - BASIC REVIEW","","Lewis structures notes covering basic review and step-by-step procedures for drawing Lewis dot diagrams of atoms, molecules, and polyatomic ions. Explains bonding principles between atoms, the octet/noble-gas rule for ions, and how to identify valence electrons using periodic-table group numbers. Provides rules for placing hydrogen, choosing a central atom, counting bonding electrons and bonding pairs, forming single bonds, and completing octets. Includes practice examples for common compounds and an introduction to resonance structures using nitrate as an example.",{"@graph":69,"@context":126},[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/lewis-structures-notes-part-1-basic-review/657106/",{"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/lewis-structures-notes-part-1-basic-review/657106.png","ImageObject",300,407,{"name":92,"@type":93},"dabgoudw","Person",{"url":74,"name":95,"@type":96},"DocShare","Organization","application/pdf","2026-10-30","2026-10-26",true,{"@type":102,"interactionType":103,"userInteractionCount":29},"InteractionCounter",{"@type":104},"ViewAction",{"@type":106,"mainEntity":107},"FAQPage",[108,114,118,122],{"name":109,"@type":110,"acceptedAnswer":111},"How do you determine the number of valence electrons for drawing a Lewis structure?","Question",{"text":112,"@type":113},"Use the element’s group number on the periodic table to find the valence electrons (electrons available for bonding). Then write the element and place that number of dots around the symbol.","Answer",{"name":115,"@type":110,"acceptedAnswer":116},"What are the key rules when drawing Lewis structures for molecules or atoms?",{"text":117,"@type":113},"Place hydrogen on the outside if present, choose the central atom as the element usually closest to the noble gases on the periodic table, count total bonding electrons, determine bonding pairs by dividing by 2, form single bonds from the central atom to end atoms, then add remaining electron pairs to satisfy full octets.",{"name":119,"@type":110,"acceptedAnswer":120},"How are Lewis structures for polyatomic ions with charges handled?",{"text":121,"@type":113},"The steps are the same, but you add or subtract electrons based on the charge. For a negative charge, add electrons; for a positive charge, subtract electrons.",{"name":123,"@type":110,"acceptedAnswer":124},"What is resonance, and how is it illustrated for nitrate?",{"text":125,"@type":113},"Resonance means a molecule or polyatomic ion can have more than one correct Lewis structure using the same sequence of atoms. For nitrate, different valid structures are generated by moving the placement of double bonds and valence electrons.","https://schema.org",{"og:url":83,"og:type":128,"og:title":65,"og:site_name":95,"og:description":67},"article",{"robots":130,"canonical":83},"index,follow",{"doc_id":132,"site_id":62},657106,1793006513,{"code":4,"msg":5,"data":135},{"doc_id":132,"user_id":136,"nickname":92,"user_avatar":137,"doc_module":4,"category_id":19,"category_name":20,"doc_title":65,"doc_description":67,"doc_content":138,"file_id":139,"file_url":140,"file_type":141,"file_size":142,"view_count":29,"is_deleted":4,"is_public":8,"is_downloadable":8,"audit_status":8,"page_count":39,"language":143,"language_code":63,"site_id":62,"html_lang":63,"table_of_contents":144,"faqs":145,"seo_title":146,"seo_description":67,"update_tm":147,"read_time":46},3985747860484,"https://ap-avatar.wpscdn.com/davatar_276721f389ce27ea32af1340a28f341c","LEWIS STRUCTURES NOTES:PART 1  \nName:YEY  \n   \n。  \n# *BASIC REVIEW\n\n-A chemical bond is a bond that happens between any two atoms.It is the principle bond that takes place between thenucleus and electrons.The overall charge of the nucleus isve.The charge of an electron is_Since one is positive and one is negative,there is anforce in an atom,keeping it together.+YuctivenecahivePoshve  \n   \n   \n-Therule states that ions (elements with a charge)want to look like a noble gas.This means that theywantelectrons in the valence shell.Elements in group's1and the lwill lose electrons producing a positive ion.Elements in group's14,andwill gain electrons producing a negative ion.will never gain or lose electrons because it has aoctet.(CUp 14GYCp18neines 1411业i5hnansihim MeralSSomehales 143280ctet  \n   \n   \n   \n   \n   \n   \n   \n   \n   \n   \n   \n第30  \n   \nJanisns  \n6  \n*LEWIS DOT DIAGRAMS OF ELEMENTS:  \n-To determine how many electrons we can use to bond elements together,we have to look at theirCanonty beValene (ve  \n   \nelectrons.We can determine this by the group number they are in.Label the following periodic table with their valenceelectrons(electrons available for bonding)  \n-8  \nve→ow  \nalence elechcnS  \nma  \nby gícup/clvmn  \nJ8  \nOivein He  \n0VteVMCS+  \nenerys ell  \nIn order to draw the lewis structure,we must first write the element and then place the number of valence electronsaround the element symbol.  \nExamples:  \n。  \nH  \n\\#dc3:2Ve?=2·He。  \nVe⁻?=1  \n√e=5  \n\\#dots?=1  \n\\#dB:5  \n   \niniale fthe  srocf  \nSTRUCTURAL FORMULAS(LEWIS DOT DIAGRAMS)  \n-When drawing the lewis structures for an atom remember the following rules:  \n1.Hydrogen willalways go at the_because it only has one electron that can bond.end  \n   \n   \n2.The central element is usually the one closest to the oble aaseS on the periodic table because it has thleast attraction for shared electrons in the molecule.→vnless ycv nave Cacbo-then ib  \n   \n   \nne encmhero ae  \n3.Find the total number of electrons available for bonding.This is the total number of_electrons.  \n   \nolivdiA04.Determine the number of bonding pairs by_the number of electrons available by2☆This is because there are always Zeina single bend  \n   \n5.Place one bond(single bond)between the central atom and each of the end atoms.  \n6.Subtract the number of pairs used in the bonds from the total number of pairs of electrons available.If thereis any electron pairs available,place them around the atom or atoms that need to form full octets.  \n文aas  ntaneven叶lcdg  \nLets do an example:  \nCarbe:)十teabfemide  \nIBrl  \ncentea九M.the Goc theexTae jeftoveY→ fyo have anyfst“hap3fuitatoareDMake sure end  \nCb  \n\\#ve=4+i|4):2  \n+IT-  \n=32dots  \ntne single elewev  \nBrl  \ncf l lines  \n SSyt   \niathe cente( I  \nTry to draw the lewis structure for each of the following:  \nNO Me H!  \neH04de  \na.NF₃  \nN  \n5+7(3)=2e  \n一一  \nbut:2.dot  \nCalled lone  \n正--F  \nai(So  \neftover!  \n   \nPJt themDn  \nthe centYal atom  \nIFi  \nb.CS₂  \n2  \nonly  \nle  \n+8ifwe  \nVe Ce  \n0W a  \nhu  \nsHARE  \n   \nsedA  \nd  \nAe  \n色  \nCH,C  \nc.H₂O  \normale  \nLewis Diagrams Practice  \nDraw the lewis dot diagrams for each of the following:  \n\n|  | CH  \u003Cbr>CH²   | NF₃   |\n| --- | --- | --- |\n| CO₃²   | H₂S   | SO₄²-   |\n| PH₃   | O₃   | BF₃   |\n| NH₄   | SCl₄   | BrF₃   |\n| CS₂   | BrO₃   |  |\n\nLewis Diagrams Practice  \n   \nDraw the lewis dot diagrams for each of the following  \n\n| SiCL   IM TetaMCY  \u003Cbr>4+7(4)=32e~> 1o ine   | CH₂O   | NF₃   |\n| --- | --- | --- |\n| CO₃²-  \u003Cbr>4+3)+2=  \u003Cbr>水  \u003Cbr>3+2=24e→12hnes  \u003Cbr>CaYpenu+e 1GY   | 2()+:8e“上→ Line5  \u003Cbr>5  \u003Cbr>H₂S iHydrogen Swihde   | SO₄²-  \u003Cbr>Suifz+e ion  \u003Cbr>2=32e→\\b lines   |\n| PH  \u003Cbr>月  \u003Cbr>5+13)=8e→4lieS  \u003Cbr>3Pesprstd   | O₃  \u003Cbr>02one  \u003Cbr>O=0-C  \u003Cbr>☆  \u003Cbr>318e→91ines   | BF₃  \u003Cbr>0C+e+.  \u003Cbr>exce ho  \u003Cbr>3+73)24e→12 lines  \u003Cbr>CY0n txiflucride   |\n| NH₄  \u003Cbr>润   | 1  \u003Cbr>octet  \u003Cbr>(  \u003Cbr>exqa:ded  \u003Cbr>k  \u003Cbr>exceph.  \u003Cbr>(  \u003Cbr>a  \u003Cbr>+7434e  \u003Cbr>SCl₄ Suifuv lehucnloride   | BrF₃  \u003Cbr>给  \u003Cbr>cc+e+  \u003Cbr>expan","cbCaiaFGGAaDYCfT","https://ap.wps.com/l/cbCaiaFGGAaDYCfT","pdf",4592312,"English","# BASIC REVIEW\n## Basic bonding and octet/noble-gas rule\n## Lewis dot diagrams of elements\n## Structural formulas (Lewis dot diagrams)\n## Lewis diagrams practice\n## Polyatomic ions and charged species\n## Resonance structures","[{\"question\":\"How do you determine the number of valence electrons for drawing a Lewis structure?\",\"answer\":\"Use the element’s group number on the periodic table to find the valence electrons (electrons available for bonding). Then write the element and place that number of dots around the symbol.\"},{\"question\":\"What are the key rules when drawing Lewis structures for molecules or atoms?\",\"answer\":\"Place hydrogen on the outside if present, choose the central atom as the element usually closest to the noble gases on the periodic table, count total bonding electrons, determine bonding pairs by dividing by 2, form single bonds from the central atom to end atoms, then add remaining electron pairs to satisfy full octets.\"},{\"question\":\"How are Lewis structures for polyatomic ions with charges handled?\",\"answer\":\"The steps are the same, but you add or subtract electrons based on the charge. For a negative charge, add electrons; for a positive charge, subtract electrons.\"},{\"question\":\"What is resonance, and how is it illustrated for nitrate?\",\"answer\":\"Resonance means a molecule or polyatomic ion can have more than one correct Lewis structure using the same sequence of atoms. For nitrate, different valid structures are generated by moving the placement of double bonds and valence electrons.\"}]","LEWIS STRUCTURES NOTES - PART 1 - BASIC REVIEW | PDF",1792974246]