[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-1-en-105":3,"doc-seo-571999-105":53,"doc-detail-571999-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","drawing-molecules-lewis-structures-cheat-sheet","Drawing Molecules – Lewis Structures - Cheat Sheet","","Drawing Molecules – Lewis Structures cheat sheet consolidates core terminology and step-by-step rules for constructing Lewis structures. It defines valence shell and valence bond ideas, distinguishes covalent and ionic bonding, and summarizes bond types from single through triple bonds. Guidance covers arranging atoms, distributing valence electrons, selecting hydrogen/halogen positions, checking octets, and handling common exceptions. Separate sections address covalent and ionic drawings, valence electron determination, and an alternative approach using total valence electrons plus lone-pair placement. Mnemonics like HONC and octet exceptions support memorization.",{"@graph":63,"@context":118},[64,80,101],{"@type":65,"itemListElement":66},"BreadcrumbList",[67,71,74,77],{"item":68,"name":69,"@type":70,"position":9},"https://docshare.wps.com","Home","ListItem",{"item":72,"name":10,"@type":70,"position":73},"https://docshare.wps.com/template/",2,{"item":75,"name":46,"@type":70,"position":76},"https://docshare.wps.com/template/paper-templates/",3,{"item":78,"name":59,"@type":70,"position":79},"https://docshare.wps.com/template/drawing-molecules-lewis-structures-cheat-sheet/571999/",4,{"url":78,"name":59,"@type":81,"image":82,"author":87,"headline":59,"publisher":90,"fileFormat":93,"inLanguage":57,"description":61,"dateModified":94,"datePublished":95,"encodingFormat":93,"isAccessibleForFree":96,"interactionStatistic":97},"DigitalDocument",{"url":83,"@type":84,"width":85,"height":86},"https://docshare.wps.com/thumbnails/drawing-molecules-lewis-structures-cheat-sheet/571999.png","ImageObject",442,249,{"name":88,"@type":89},"Emma Wilson","Person",{"url":68,"name":91,"@type":92},"DocShare","Organization","application/pdf","2026-10-15","2026-10-13",true,{"@type":98,"interactionType":99,"userInteractionCount":9},"InteractionCounter",{"@type":100},"ViewAction",{"@type":102,"mainEntity":103},"FAQPage",[104,110,114],{"name":105,"@type":106,"acceptedAnswer":107},"What are the key terms you need to know before drawing Lewis structures?","Question",{"text":108,"@type":109},"The cheat sheet explains valence shell, valence bond theory, covalent and ionic bonding, the octet rule, and the meaning of Lewis structures, lone pairs, and bonding pairs.","Answer",{"name":111,"@type":106,"acceptedAnswer":112},"How do you draw covalent Lewis structures step by step?",{"text":113,"@type":109},"Arrange atoms, determine valence electrons, place valence electrons without doubling prematurely, check full valences, then form double or triple bonds by moving electrons as needed. If non-adjacent atoms require multiple bonding, adjust by moving a hydrogen to create adjacent bonding demand.",{"name":115,"@type":106,"acceptedAnswer":116},"What exceptions to the octet rule are listed?",{"text":117,"@type":109},"Hydrogen and helium hold 2 electrons, boron and beryllium can be full with 6, and elements in period 3 or below may exceed 8 due to available d orbitals. It also notes free radicals with one unpaired electron do not follow the octet rule.","https://schema.org",{"og:url":78,"og:type":120,"og:title":59,"og:site_name":91,"og:description":61},"article",{"robots":122,"canonical":78},"index,follow",{"doc_id":124,"site_id":56},571999,1792067153,{"code":4,"msg":5,"data":127},{"doc_id":124,"user_id":128,"nickname":88,"user_avatar":129,"doc_module":9,"category_id":45,"category_name":46,"doc_title":59,"doc_description":61,"doc_content":130,"file_id":131,"file_url":132,"file_type":133,"file_size":134,"view_count":9,"is_deleted":4,"is_public":9,"is_downloadable":9,"audit_status":9,"page_count":9,"language":135,"language_code":57,"site_id":56,"html_lang":57,"table_of_contents":136,"faqs":137,"seo_title":138,"seo_description":61,"update_tm":139,"read_time":4},3848291630094,"https://eur-avatar.wpscdn.com/davatar_085a072bc5b1113ac321206ff7593b45","| 16: Drawing Molecules – Lewis Structures |  |\n| --- | --- |\n| Key Lewis Structure Terms | Arranging Atoms in Lewis Structures |\n| 􀁸 Valence Shell: Electrons in the outermost shell that are involved in bonding.\u003Cbr>􀁸 Valence Bond Theory: Overlap of atomic orbitals forming the bond.\u003Cbr>􀁸 Covalent Bond: Bond formed between two nonmetals that involves shared electrons.\u003Cbr>􀁸 Octet Rule: Atoms are most stable with a full valence shell (in most cases is “8”) .\u003Cbr>􀁸 Lewis Structure: A 2D representation of a molecule and its bonds.\u003Cbr>􀁸 Lone Pair: Pair of electrons not being shared in a bond.\u003Cbr>􀁸 Bonding Pair: A pair of electrons is to form a bond. Both atoms sharing the electrons can “count” them in their valence shell.\u003Cbr>􀁸 Single bond: One pair of shared electrons.\u003Cbr>􀁸 Double bond: Two pairs of shared electrons. Shorter and stronger than a single bond.\u003Cbr>􀁸 Triple bond: Three pairs of shared electrons. Shorter and stronger than a double bond.\u003Cbr>􀁸 Polyatomic Ion: Group of atoms covalently bonded together that have a net charge.\u003Cbr>􀁸 Ionic Compound: Electrons are transferred from one atom to another. Transfer of electrons results in net charges, which bond with electrostatic attraction. | 1. For molecules with only 2 elements, arrange the atoms symmetrically.\u003Cbr>2. “COOH” is a carboxylic acid (both O’s bond to the C and the H goes on one of the O’s) .\u003Cbr>3. Hydrogen and halogens cannot go in the middle.\u003Cbr>4. Write the remaining atoms in the order they appear in the formula.\u003Cbr>5. Write the hydrogen and halogen atoms around the element they are written next to in the formula. |\n|  | Drawing Covalent Lewis Structures |\n|  | 1. Arrange the atoms as above.\u003Cbr>2. Determine the \\# of valence electrons for each atom.\u003Cbr>3. Draw the valence electrons—do not double up where a bond is going to form between two atoms.\u003Cbr>4. Count to see if all atoms have full valences (notice the exceptions) .\u003Cbr>5. If two atoms adjacent to each other do not have full valences, move in an electron from each to form a double bond. Repeat for triple bond if necessary.\u003Cbr>6. If two atoms that are not adjacent to each other need to double bond, try moving a hydrogen to one of them to cause two atoms adjacent to each other to need the double bond.\u003Cbr>Single bonds: \u003Cbr>Double bonds: \u003Cbr>Polyatomic anion:  |\n| Determining \\# of Valence Electrons |  |\n| Determining valence electrons from the periodic table:\u003Cbr>1\u003Cbr>8\u003Cbr>2 3 4 5 6 7\u003Cbr>\u003Cbr>Note: Valence electrons in transition metals are not as\u003Cbr>reliable and predictable as the ones in main group elements. |  |\n| Drawing Lewis Structures for an Element |  |\n| 1. Use the element symbol to represent the nucleus and core electrons.\u003Cbr>2. Determine \\# of valence electrons.\u003Cbr>3. Draw valence electrons—placing one on each side before doubling up.\u003Cbr>HONC Valence Rule Mnemonic: The electrons needed for full valence shell and covalent bonds formed are H(1), O(2), N(3) and C(4) = HONC. |  |\n|  | Drawing Ionic Lewis Structures |\n|  | Transfer the electrons from the metal to the nonmetals until all have full valences and the net charge = 0\u003Cbr>Ionic compound (BaF2) : Ba+2 2F-1\u003Cbr>|\n| Exceptions to the Octet Rule |  |\n| 1. Hydrogen and Helium can only hold 2 electrons (they only have a 1s orbital) .\u003Cbr>2. Boron and Beryllium can be full with 6 electrons.\u003Cbr>3. Any element in period 3 or below can have more than 8 electrons (they have empty d orbitals that can hold them) .\u003Cbr>Octet Exception Mnemonic: H&He: 2(full valence); Be: 4; B = 6; S&P > 8 = “2 Hawks and Hens (2-legs); 4 Bears (4-legs); 6 Bugs (6-legs); many SPiders (\u003C8 legs) .”\u003Cbr>Note: Elements in period 3 and below have empty “d”\u003Cbr>orbitals that can be used to hold more than 8 valence electrons (18 Electrons Rule) . Free radicals with one unpaired electron clearly do not follow the Octet rule. |  |\n|  | Another Approach to Lewis Structures |\n|  | 1. Arrange the atoms as above.\u003Cbr>2. Determine the total \\# of valence electrons for the whole molecule.\u003Cbr>3. Put one bond","cbCaib6n9fim7FLp","https://ap.wps.com/l/cbCaib6n9fim7FLp","pdf",141548,"English","# Drawing Molecules – Lewis Structures\n## Key Lewis Structure Terms\n## Arranging Atoms in Lewis Structures\n## Drawing Covalent Lewis Structures\n## Determining # of Valence Electrons\n## Drawing Lewis Structures for an Element\n## Drawing Ionic Lewis Structures\n## Exceptions to the Octet Rule\n## Another Approach to Lewis Structures\n## How to Use This Cheat Sheet","[{\"question\":\"What are the key terms you need to know before drawing Lewis structures?\",\"answer\":\"The cheat sheet explains valence shell, valence bond theory, covalent and ionic bonding, the octet rule, and the meaning of Lewis structures, lone pairs, and bonding pairs.\"},{\"question\":\"How do you draw covalent Lewis structures step by step?\",\"answer\":\"Arrange atoms, determine valence electrons, place valence electrons without doubling prematurely, check full valences, then form double or triple bonds by moving electrons as needed. If non-adjacent atoms require multiple bonding, adjust by moving a hydrogen to create adjacent bonding demand.\"},{\"question\":\"What exceptions to the octet rule are listed?\",\"answer\":\"Hydrogen and helium hold 2 electrons, boron and beryllium can be full with 6, and elements in period 3 or below may exceed 8 due to available d orbitals. It also notes free radicals with one unpaired electron do not follow the octet rule.\"}]","Drawing Molecules – Lewis Structures - Cheat Sheet | PDF",1791924917]