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The worksheet outlines steps to draw Lewis structures: select the central atom using electronegativity rules, calculate total valence electrons from the periodic table, connect atoms with appropriate single/double/triple bonds, and apply the octet rule while placing remaining electrons as lone pairs. Worked examples (NCl3, CCl3CHO, NH4+) and practice problems reinforce electron counting, lone-pair placement, and handling charged ions with bracketed notation.",{"@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/lewis-dot-structures-a-guide-to-drawing-lewis-dot-structures-octet-rule-and-lone-pairs/657100/",{"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-dot-structures-a-guide-to-drawing-lewis-dot-structures-octet-rule-and-lone-pairs/657100.png","ImageObject",300,407,{"name":92,"@type":93},"A glass of water","Person",{"url":74,"name":95,"@type":96},"DocShare","Organization","application/pdf","2026-10-29","2026-10-26",true,{"@type":102,"interactionType":103,"userInteractionCount":24},"InteractionCounter",{"@type":104},"ViewAction",{"@type":106,"mainEntity":107},"FAQPage",[108,114,118],{"name":109,"@type":110,"acceptedAnswer":111},"How do you choose the central atom in a Lewis dot structure?","Question",{"text":112,"@type":113},"Place the least electronegative atom in the center, and keep hydrogen on the outside because it forms only one bond.","Answer",{"name":115,"@type":110,"acceptedAnswer":116},"What is the process for counting total valence electrons?",{"text":117,"@type":113},"Use the periodic table to find each atom’s valence electrons, multiply by the number of atoms, and add them for the whole molecule; then adjust for ionic charge by adding electrons for negative charge or subtracting for positive charge.",{"name":119,"@type":110,"acceptedAnswer":120},"How do you complete a Lewis dot structure using the octet rule?",{"text":121,"@type":113},"Use single, double, or triple bonds to connect atoms so that most atoms (except hydrogen) have 8 electrons around them, then place remaining electrons as lone pairs on outer atoms first and the central atom if needed. For ions, put the final Lewis structure in brackets and indicate the charge.","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},657100,1793006515,{"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":24,"is_deleted":4,"is_public":8,"is_downloadable":8,"audit_status":8,"page_count":24,"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},962090760832,"https://ap-avatar.wpscdn.com/davatar_155a257f0dc6eb9ab79c44ca47cae57d","Lewis Dot Structures  \n- A Lewis dot structure is a visual representation of the bonding between atoms in a molecule. It also shows any lone pairs of electrons that may exist on atoms.  \n- How to Draw a Lewis Dot Structure:  \no 1. Determine the Central Atom  \n§ Place the least electronegative atom in the center (never hydrogen, it always goes on the outside because it forms only one bond) .  \no 2. Count Total Valence Electrons:  \n§ Use the periodic table to determine how many valence electrons each atom contributes. Add the up for the whole molecule  \n• Group 1 has 1 valence electron  \n• Group 4 has 4 valence electrons  \n• Group 5 has 5 valence electrons  \n• Group 6 has 6 valence electrons  \n• Group 7 has 7 valence electrons  \n§ Group-based bonding patterns (for typical main group elements) are as follows:  \n• Group 1 (e.g., H) : 1 bond, no lone pairs ~~ ~~ H  \n• Group 4 (e.g., C): 4 bonds, no lone pairs  \n~~ ~~ C ~~ ~~  \n• Group 5 (e.g., N) : 3 bonds, 1 lone pair  \n~~ ~~ N ~~ ~~  \n• Group 6 (e.g., O): 2 bonds, 2 lone pairs  \n~~ ~~ O ~~ ~~  \n• Group 7 (e.g., F): 1 bonds, 3 lone pairs  \n~~ ~~ F   \no 3. Draw Bonds and Fulfill the Octet Rule  \n§ Use single, double, or triple bonds as needed to connect atoms and ensure most atoms (except hydrogen) are surrounded by 8 electrons  \n§ Place any remaining electrons as lone pairs on outer atoms first, then on the central atom if needed  \nCHEM 150 Worksheet  \n- Example 1: NCl3  \n1. Determine the Central Atom  \no Nitrogen is the central atom because it is less electronegative than chlorine  \n2. Count Total Valence Electrons  \no Nitrogen = 5 valence electrons  \no Chlorine = 7 valence electron x 3 = 21  \no Total = 5 + 21 = 26 valence electrons  \n3. Draw the Initial Bonds  \no Connect each chlorine atom to nitrogen with a single bond (3 bonds x 2 electrons = 6 electrons used)  \nCl  \nCl ~~ ~~ N ~~ ~~ Cl  \n4. Complete the Octet  \no Nitrogen has 6 electrons from the three bonds, so it needs 1 lone pair (2 electrons) to reach an octet à now nitrogen has 8 electrons.  \no Each chlorine has 2 electrons from the bond, and needs 6 more à add 3 lone pairs (6 electrons) to each Cl atom  \nCl  \nCl ~~ ~~ N ~~ ~~ Cl  \n5. Check Total Electrons  \no Bonds = 3 x 2 = 6 electrons  \no Nitrogen lone pair = 2 electrons  \no Chlorine lone pairs = 3 Cl x 3 lone pairs x 2 electrons = 18 electrons  \no Total = 6 + 2 + 18 = 26 electrons, which matches the valence electrons  \nCl   \nCl ~~ ~~ N ~~ ~~ Cl   \nCHEM 150 Worksheet  \nExample 2: CCl3CHO  \n1. Determine the Central Atom  \no Carbon atoms go in the middle because they are the least electronegative and they will form the backbone  \no One carbon is bonded to three Cl atoms, and the other is bonded to an O and an H  \n2. Count the Total Valence Electrons  \no Carbon = 4 valence electrons x 2 = 8  \no Chlorine = 7 valence electrons x = 21  \no Hydrogen = 1 valence electron = 1  \no Oxygen = 6 valence electron = 6  \no Total = 8 + 21 + 1 + 6 = 36 valence electrons  \n3. Draw the Initial Bond  \no Connect the two carbon atoms with a single bond  \nC ~~ ~~ C  \no Connect 3 Cl atoms to the first carbon  \nCl  \nCl ~~ ~~ C ~~ ~~ C  \nCl  \no Attach H and O to the second carbon  \nCl H  \nCl ~~ ~~ C ~~ ~~ C ~~ ~~ O  \nCl  \n4. Complete the Octet  \no Let’s give every atom the electrons they need:  \no Each Cl gets 3 lone pairs (6 electrons): 3 x 6 = 18 electrons  \nCl   \n    H  \n Cl ~~ ~~ C ~~ ~~ C  \nCl  O  \no Oxygen needs 6 more electrons. Because group 6 elements generally like 2 bonds and 2 lone pairs, we will add a double bond between the oxygen and carbon and 2 lone pairs  \nCl   \n  H  \n Cl ~~ ~~ C ~~ ~~ C  \nCl  O   \n5. Check the Total Electrons  \no C-Cl bonds x 3 = 6 electrons, C-C bond = 2 electrons, C=O bond = 4 electrons, CH bond = 2 electrons  \no Cl lone pairs = 6 x 3 = 18 electrons, O lone pairs = 4 electrons  \no Total: 6 + 2 + 4 + 2 + 18 + 4 = 36 electrons   \nCHEM 150 Worksheet  \nExample 3: Charged Molecule, NH4+  \n- If molecule or ion is negatively charged:  \no Add electrons to your total ","cbCaifuXjnctlRky","https://ap.wps.com/l/cbCaifuXjnctlRky","pdf",240934,"English","# How to Draw a Lewis Dot Structure\n## Determine the Central Atom\n## Count Total Valence Electrons\n## Draw Bonds and Fulfill the Octet Rule\n# Worked Examples\n## Example 1: NCl3\n## Example 2: CCl3CHO\n## Example 3: Charged Molecule, NH4+\n# Practice","[{\"question\":\"How do you choose the central atom in a Lewis dot structure?\",\"answer\":\"Place the least electronegative atom in the center, and keep hydrogen on the outside because it forms only one bond.\"},{\"question\":\"What is the process for counting total valence electrons?\",\"answer\":\"Use the periodic table to find each atom’s valence electrons, multiply by the number of atoms, and add them for the whole molecule; then adjust for ionic charge by adding electrons for negative charge or subtracting for positive charge.\"},{\"question\":\"How do you complete a Lewis dot structure using the octet rule?\",\"answer\":\"Use single, double, or triple bonds to connect atoms so that most atoms (except hydrogen) have 8 electrons around them, then place remaining electrons as lone pairs on outer atoms first and the central atom if needed. For ions, put the final Lewis structure in brackets and indicate the charge.\"}]","Lewis Dot Structures - A Guide to Drawing Lewis Dot Structures - Octet Rule and Lone Pairs | PDF",1792974047,13]