[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-0-en-105":3,"doc-seo-657096-105":59,"doc-detail-657096-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","molecular-structure-and-bonding-lecture-2-lewis-theory-lewis-structures-octet-rule","Molecular Structure and Bonding - Lecture 2 - Lewis Theory - Lewis Structures - Octet Rule","","Lecture 2 explains molecular bonding using Lewis theory, focusing on Lewis dot symbols and the octet rule. It describes how most elements achieve eight valence electrons in ions and covalent compounds, including the exception that hydrogen has a duet. The lecture provides basic steps for drawing Lewis structures, defining dot symbols and converting shared electron pairs into covalent bonds represented by lines. It outlines systematic rules for deciding covalent vs ionic treatment, counting total valence electrons, arranging central and ligand atoms, and distributing electron pairs to reach provisional structures.",{"@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":30,"@type":76,"position":81},"https://docshare.wps.com/document/technology/",3,{"item":83,"name":65,"@type":76,"position":19},"https://docshare.wps.com/document/molecular-structure-and-bonding-lecture-2-lewis-theory-lewis-structures-octet-rule/657096/",{"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-structure-and-bonding-lecture-2-lewis-theory-lewis-structures-octet-rule/657096.png","ImageObject",300,407,{"name":92,"@type":93},"Indoniesian Boy","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],{"name":109,"@type":110,"acceptedAnswer":111},"What does the octet rule state, and how does hydrogen differ?","Question",{"text":112,"@type":113},"The octet rule states that elements (except hydrogen) tend to have eight valence electrons in ions and covalent compounds. Hydrogen differs by following a duet of electrons.","Answer",{"name":115,"@type":110,"acceptedAnswer":116},"How is a covalent bond represented in Lewis structures?",{"text":117,"@type":113},"A covalent bond is shown as a shared pair of electrons. In Lewis structures, two dots indicating the bonding pair are replaced by a line between the two bonded atoms.",{"name":119,"@type":110,"acceptedAnswer":120},"What steps are used to draw a Lewis structure?",{"text":121,"@type":113},"First determine whether the compound is covalent or ionic. Then count total valence electrons (including charge corrections), choose a central atom (usually the least electronegative, and hydrogen is never central), and distribute electron pairs: one between central and each ligand, additional lone pairs on outer atoms (except hydrogen), and remaining pairs on the central atom.","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},657096,1793146920,{"code":4,"msg":5,"data":131},{"doc_id":128,"user_id":132,"nickname":92,"user_avatar":133,"doc_module":4,"category_id":29,"category_name":30,"doc_title":65,"doc_description":67,"doc_content":134,"file_id":135,"file_url":136,"file_type":137,"file_size":138,"view_count":29,"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":144,"read_time":145},962090760608,"https://ap-avatar.wpscdn.com/davatar_276721f389ce27ea32af1340a28f341c","Molecular Structure and  \nBonding  \nLecture 2  \n:  \nLewis Theory  \nLewis structures  \nThe octet rule  \nAll elements except hydrogen ( hydrogen have a duet of electrons) have octet of electrons once they from ions and covalent compounds.  \nThe Lewis dot symbols for atoms and ions shows how many electrons are need for a atom to fill the octet. Normally there are octet of electrons on most monoatomic ions  \nBasic rules drawing Lewis dot symbols:  \n1 . Draw the atomic symbol.  \n2 . Treat each side as a box that can hold up to two electrons.  \n3 . Count the electrons in the valence shell.  \nStart filling box-don’t make pairs unless you need to.  \nA Lewis symbol is a symbol in which the electrons in the valence shell of an atom or simple ion are represented by dots placed around the letter symbol of the element. Each dot represents one electron.  \nA covalent bond is a chemical bond formed by the sharing of a pair of electrons between two atoms. The Lewis structure of a covalent compound or polyatomic ion shows how the valence electrons are arranged among the atoms in the molecule to show the connectivity of the  \natoms   \nInstead of using two dots to indicate the two electrons that comprise the covalent bond, a line is substituted for the two dots that represent the two electrons.  \nThe Lewis structure for water  \nTwo hydrogens (H) are separately covalently bonded to the central oxygen (O) atom. The bonding electrons are indicated by the dashes between the oxygen (O) and each hydrogen (H) and the other two pairs of electrons that constitute oxygens octet, are called non-bonding electrons as they are not involved in a  \ncovalent bond .  \nRules for getting Lewis Structures  \n1.Determine whether the compound is covalent or ionic. If covalent, treat the entire molecule. If ionic, treat each ion separately. For amonoatomic ion, the electronic configuration of the ion represents the correct Lewis structure. For compounds containing complex ions, you must learn to recognize the formulas of cations and anions .  \n2. Determine the total number of valence electrons available to the molecule or ion by:  \n(a) summing the valence electrons of all the atoms in the unit  \n(b) adding one electron for each net negative charge or subtracting one electron for each net positive charge. Then divide the total number of available electrons by 2 to obtain the number of electron pairs (E.P.) available.  \n3 . Organize the atoms so there is a central atom (usually the least electronegative) surrounded by ligand (outer) atoms. Hydrogen is never the central atom.  \n4 . Determine a provisional electron distribution by arranging the electron pairs (E.P.) in the following manner until all available pairs have been distributed:  \na) One pair between the central atom and each ligand atom.  \nb) Three more pairs on each outer atom (except hydrogen, which has no additional pairs), yielding 4 E.P. (i.e. , an octet) around each ligand atom when the bonding pair is included in the count.  \nc) Remaining electron pairs (if any) on the central atom.","cbCaisgd7wzbsqpj","https://ap.wps.com/l/cbCaisgd7wzbsqpj","pdf",1086369,21,"English","# Molecular Structure and Bonding\n## Lewis Theory\n## Lewis Structures\n## Octet Rule\n## Rules for Drawing Lewis Dot Symbols\n## Lewis Structure of Water\n## Rules for Getting Lewis Structures","[{\"question\":\"What does the octet rule state, and how does hydrogen differ?\",\"answer\":\"The octet rule states that elements (except hydrogen) tend to have eight valence electrons in ions and covalent compounds. Hydrogen differs by following a duet of electrons.\"},{\"question\":\"How is a covalent bond represented in Lewis structures?\",\"answer\":\"A covalent bond is shown as a shared pair of electrons. In Lewis structures, two dots indicating the bonding pair are replaced by a line between the two bonded atoms.\"},{\"question\":\"What steps are used to draw a Lewis structure?\",\"answer\":\"First determine whether the compound is covalent or ionic. Then count total valence electrons (including charge corrections), choose a central atom (usually the least electronegative, and hydrogen is never central), and distribute electron pairs: one between central and each ligand, additional lone pairs on outer atoms (except hydrogen), and remaining pairs on the central atom.\"}]","Molecular Structure and Bonding - Lecture 2 - Lewis Theory - Lewis Structures - Octet Rule | PDF",1792974040,53]