[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-1-en-105":3,"doc-detail-572268-en":53,"doc-seo-572268-105":74},{"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":5,"data":54},{"doc_id":55,"user_id":56,"nickname":57,"user_avatar":58,"doc_module":9,"category_id":50,"category_name":51,"doc_title":59,"doc_description":60,"doc_content":61,"file_id":62,"file_url":63,"file_type":64,"file_size":65,"view_count":66,"is_deleted":4,"is_public":9,"is_downloadable":9,"audit_status":9,"page_count":9,"language":67,"language_code":68,"site_id":69,"html_lang":68,"table_of_contents":70,"faqs":71,"seo_title":72,"seo_description":60,"update_tm":73,"read_time":4},572268,962090896061,"AfterMidnight","https://ap-avatar.wpscdn.com/davatar_9964176cb1d06d4a9deccf72a44ae3dc","AP Chemistry Periodic Trends Cheat Sheet","AP Chemistry periodic trends cheat sheet focusing on effective nuclear charge, ionization energy, atomic size, electron configurations, ion size, and electron affinity. Summarizes key relationships such as Zeffective = Z − S, how electron shielding and repulsion affect valence behavior, and that ionization energy generally increases left to right while decreasing top to bottom. Includes concise rules for cation/anion size changes and how electron removal/addition follows highest-n and lowest-n orbitals. Provides example ions and brief notes/questions section.","AP Chemistry Periodic Trends Cheat Sheet [by](by chakraoishee via cheatography.com/40046/cs/13170/)[ chakraoishee](by chakraoishee via cheatography.com/40046/cs/13170/)[ via](by chakraoishee via cheatography.com/40046/cs/13170/)[ cheatography.com/40046/cs/13170/](by chakraoishee via cheatography.com/40046/cs/13170/)  \nEffective Nuclear Charge  \nZ effective \u003C Z actual b/c Z effective also accounts for repulsion of an electron by other electron  \nZ effective = Z-S  \nelectrons int he same shell do not screen but repel each other  \nEXAMPLE  \n2 2 6 2 Na: 1s 2s 2p 3s  \n+ - +  \n11 {number of protons} - 10 {number of electrons in Ne core} = 1 {effective nuclear charge of the 3s valence electron}  \nIonization Energy  \nionization energy = minimal energy needed to remove an electron from a neutral atom  \nfirst ionization = energy required to remove first electron  \n+ -  \nEXAMPLE Na (g) -- > Na (g) + e  \nsecond ionization = energy required to remove second election + 2+ -  \nEXAMPLE Na (g) -- > Na (g) + e  \nthe greater the ionization energy , the more difficult to remove the electron  \nmoving from left to right , ionization values increase ionization values decrease from top to bottom  \nSize of Atoms  \nelectron clouds of colliding atoms cannot penetrate each other to any significant extent  \nnonbonding atomic radius > bonding atomic radius why is bonding atomic radius 0.5d?  \nbonding atomic radius increases from top to bottom of table  \nbonding atomic raius decreases from left to right  \nElectron Configurations  \nwhen electrons are removed from an atom to form a cation , they are removed from orbitals with the largest n value  \nwhen electrons are added to an atom , they are added to the orbitals with the lowest n value  \nSize of Ions  \ncations are smaller than the parent atom  \nanions are bigger than parent atom  \nis there are a trend for ion size in the periodic table?  \nElectron Affinity  \nelectron affinity = measurement of attraction of the atom for the added electron  \nhow is affinity measured?  \n\n|  |\n| --- |\n|  |\n\nNotes/Questions  \nBy chakraoishee  \n[cheatography.com/chakraoishee/](cheatography.com/chakraoishee/)  \nNot published yet.  \nLast updated 18th October, 2017. Page 1 of 1.  \nSponsored by Readable.com Measure your website readability!  \n[https://readable.com](https://readable.com)","cbCaiavrdfvmW9b2","https://ap.wps.com/l/cbCaiavrdfvmW9b2","pdf",39602,8,"English","en",105,"# Effective Nuclear Charge\n# Ionization Energy\n# Size of Atoms\n# Electron Configurations\n# Size of Ions\n# Electron Affinity","[{\"question\":\"How is effective nuclear charge (Zeffective) calculated in periodic trends?\",\"answer\":\"Use Zeffective = Z − S, where Z is the number of protons and S accounts for the screening effect. Effective nuclear charge also reflects repulsion from other electrons.\"},{\"question\":\"What general trends occur for ionization energy across the periodic table?\",\"answer\":\"Ionization energy increases from left to right and decreases from top to bottom. Higher ionization energy means the electron is harder to remove.\"},{\"question\":\"How do cations and anions differ in size compared with their parent atoms?\",\"answer\":\"Cations are smaller than the parent atom because electrons are removed from higher-energy orbitals. Anions are larger than the parent atom because added electrons increase electron-electron repulsion and size.\"}]","AP Chemistry Periodic Trends Cheat Sheet | PDF",1791926497,{"code":4,"msg":75,"data":76},"ok",{"site_id":69,"language":68,"slug":77,"title":59,"keywords":78,"description":60,"schema_data":79,"social_meta":135,"head_meta":137,"extra_data":139,"updated_unix":140},"ap-chemistry-periodic-trends-cheat-sheet","",{"@graph":80,"@context":134},[81,97,117],{"@type":82,"itemListElement":83},"BreadcrumbList",[84,88,91,94],{"item":85,"name":86,"@type":87,"position":9},"https://docshare.wps.com","Home","ListItem",{"item":89,"name":10,"@type":87,"position":90},"https://docshare.wps.com/template/",2,{"item":92,"name":51,"@type":87,"position":93},"https://docshare.wps.com/template/general/",3,{"item":95,"name":59,"@type":87,"position":96},"https://docshare.wps.com/template/ap-chemistry-periodic-trends-cheat-sheet/572268/",4,{"url":95,"name":59,"@type":98,"image":99,"author":104,"headline":59,"publisher":106,"fileFormat":109,"inLanguage":68,"description":60,"dateModified":110,"datePublished":111,"encodingFormat":109,"isAccessibleForFree":112,"interactionStatistic":113},"DigitalDocument",{"url":100,"@type":101,"width":102,"height":103},"https://docshare.wps.com/thumbnails/ap-chemistry-periodic-trends-cheat-sheet/572268.png","ImageObject",442,249,{"name":57,"@type":105},"Person",{"url":85,"name":107,"@type":108},"DocShare","Organization","application/pdf","2026-10-19","2026-10-13",true,{"@type":114,"interactionType":115,"userInteractionCount":66},"InteractionCounter",{"@type":116},"ViewAction",{"@type":118,"mainEntity":119},"FAQPage",[120,126,130],{"name":121,"@type":122,"acceptedAnswer":123},"How is effective nuclear charge (Zeffective) calculated in periodic trends?","Question",{"text":124,"@type":125},"Use Zeffective = Z − S, where Z is the number of protons and S accounts for the screening effect. Effective nuclear charge also reflects repulsion from other electrons.","Answer",{"name":127,"@type":122,"acceptedAnswer":128},"What general trends occur for ionization energy across the periodic table?",{"text":129,"@type":125},"Ionization energy increases from left to right and decreases from top to bottom. Higher ionization energy means the electron is harder to remove.",{"name":131,"@type":122,"acceptedAnswer":132},"How do cations and anions differ in size compared with their parent atoms?",{"text":133,"@type":125},"Cations are smaller than the parent atom because electrons are removed from higher-energy orbitals. Anions are larger than the parent atom because added electrons increase electron-electron repulsion and size.","https://schema.org",{"og:url":95,"og:type":136,"og:title":59,"og:site_name":107,"og:description":60},"article",{"robots":138,"canonical":95},"index,follow",{"doc_id":55,"site_id":69},1792008958]