[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"detail-sidebar-cat-0-en-105":3,"doc-seo-343679-105":59,"doc-detail-343679-en":131},{"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":124,"head_meta":126,"extra_data":128,"updated_unix":130},105,"en","topic-3-periodicity","Topic 3 - Periodicity","","Topic 3 explains periodicity as repeating patterns in the physical and chemical properties of elements. It outlines how the periodic table is structured into blocks (s, p, d, f), groups and periods, and links an element’s position to electron configuration and valence information. It then develops periodic trends for atomic radius, ionic radius, ionization energy, electron affinity, electronegativity, melting points, and metallic character, concluding with behavior across groups and period 3, including comparisons between alkali metals and halogens.",{"@graph":69,"@context":123},[70,84,106],{"@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/topic-3-periodicity/343679/",{"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/topic-3-periodicity/343679.png","ImageObject",300,407,{"name":92,"@type":93},"Eliana","Person",{"url":74,"name":95,"@type":96},"DocShare","Organization","application/vnd.openxmlformats-officedocument.wordprocessingml.document","2026-11-05","2026-09-22",true,{"@type":102,"interactionType":103,"userInteractionCount":105},"InteractionCounter",{"@type":104},"ViewAction",13,{"@type":107,"mainEntity":108},"FAQPage",[109,115,119],{"name":110,"@type":111,"acceptedAnswer":112},"How are the blocks, groups, and periods on the periodic table related to electron structure?","Question",{"text":113,"@type":114},"The periodic table is arranged into four blocks (s, p, d, f) associated with the last orbital. Elements are grouped into vertical columns (groups) and horizontal rows (periods), where group number relates to valence electrons and period number relates to the number of shells.","Answer",{"name":116,"@type":111,"acceptedAnswer":117},"What happens to atomic radius across a period and down a group?",{"text":118,"@type":114},"Atomic radius decreases across a period and increases down a group. Down a group, more electron shells are added, and across a period the nuclear charge increases, strengthening attraction to outer electrons.",{"name":120,"@type":111,"acceptedAnswer":121},"How do ionization energy and metallic character trend across the periodic table?",{"text":122,"@type":114},"Ionization energy increases across a period and decreases down a group. Metallic character increases down a group and decreases across a period, reflecting how easily atoms lose electrons.","https://schema.org",{"og:url":83,"og:type":125,"og:title":65,"og:site_name":95,"og:description":67},"article",{"robots":127,"canonical":83},"index,follow",{"doc_id":129,"site_id":62},343679,1790819133,{"code":4,"msg":5,"data":132},{"doc_id":129,"user_id":133,"nickname":92,"user_avatar":134,"doc_module":4,"category_id":19,"category_name":20,"doc_title":65,"doc_description":67,"doc_content":135,"file_id":136,"file_url":137,"file_type":138,"file_size":139,"view_count":105,"is_deleted":4,"is_public":8,"is_downloadable":8,"audit_status":8,"page_count":29,"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,"preview_page_count":4},4398048949847,"https://ap-avatar.wpscdn.com/avatar/400002536579ef2da7f?_k=1778318612642679267","Topic 3: Periodicity\n3.1\nPeriodic Table\n3.1.1\nThe periodic table is arranged into four blocks associated with the four sub-levels – s, p, d, and f\n3.1.2\nThe periodic table consists of groups (vertical columns) and periods (horizontal rows)\n3.1.3\nThe period number (n) is the outer energy level that is occupied by electrons\n3.1.4\nThe number of the principal energy level and the number of the valence electrons in an atom can be deduced from its position on the periodic table\n3.1.5\nThe periodic table shows the position of metals, non-metals and metalloids\n3.1.6\nDeduction of the electron configuration of an atom from the element’s position on the periodic table, and vice versa\nPeriodic Table Arrangement\nThe periodic table is arranged into 4 blocks associated with their last orbital: s, p, d and f\nElements in the periodic table are arranged by increasing atomic number\nGroup: A vertical column of elements\nGroup number is the same as the number of valence electrons\nPeriod: A horizontal row of elements\nPeriod number is the same number of shells in the atom\nAll shells except the outer shell will be full\nThere is a division between metals and non-metals. Metals are on the left and non-metals are on the right\nThe farther sub-level occupied is found by the location of the element (which block it is in):\nThe location of the following families of the periodic table must be known: alkali metals, alkali earth metals, halogens, noble gases, transition metals, lanthanides and actinoids\n3.2\nPeriodic trends\n3.2.1\nVertical and horizontal trends in the periodic table exist for atomic radius, ionic radius\n3.2.2\nTrends in metallic and non-metallic behavior are due to the trends above\n3.2.3\nOxides change from basic through amphoteric to acidic across a period\n3.2.4\nPrediction and explanation of the metallic and non-metallic behavior of an element based on its position in the periodic table\n3.2.5\nDiscussion of the similarities and differences in the properties of elements in the same group, with reference to alkali metals and halogens\nDefinitions\nAtomic Radius – The distance from the nucleus to the outermost electron\nIonic Radius – The distance from the nucleus to the outermost electrons in an ion\nFirst ionization energy – The energy required to remove one mole of electrons from one mole of gaseous atoms. This is shown by: \u001a𝑋\u001b(𝑔)\u001b→\u001a𝑋\u001b(𝑔)\u001b+\u001b+\u001a𝑒\u001b−\u001b\nElectron affinity – The energy released when one mole of an electron is added to one mole gaseous atoms. This is shown by:    \u001a𝑋\u001b(𝑔)\u001b+\u001a𝑒\u001b−\u001b→\u001a𝑋\u001b(𝑔)\u001b−\u001b\nElectronegativity – A measure of the attraction an atom has for a shared pair of electrons in a covalent bond\nTrends in the Periodic Table\nPeriodicity refers to repeating trends or patterns of physical and chemical properties in elements\nAtomic Radius\nAtomic radius increases down a group as the number of electron shells increases\nAtomic radius decreases across a period\nThis is because electrons are added to the same main energy level (n=3) the nuclear charge also increases\nThe attraction between the nucleus and the outer electrons increases resulting in a smaller radius\nIonic Radius\nIonic radius of positive ions decrease across a period as the number of protons in the nucleus increases but the number of electrons remain the same\nIonic radius of negative ions decrease across a period as the number of protons in the nucleus increases but the number of electrons remains the same\nIonization energy\nIonization energy increases across a period\nThe increase in nuclear charge across a period causes an increase in the attraction between the outer electrons and the nucleus makes the electrons more difficult to remove\nIonization energy decreases down a group\nThe electron being removed is from the energy level furthest from the nucleus so it gets easier to remove valence electrons as atomic radius increases down a group\nValence Electrons: The outermost electrons of an atom\nElectron affinity\nGenerally, metals have a low EA and non-metals have a higher EA\nThe greater the distanc","cbCainNsh85JBVCJ","https://ap.wps.com/l/cbCainNsh85JBVCJ","docx",801531,"English","# Periodic Table\n## Periodic trends\n## Definitions\n## Trends in the Periodic Table\n## Trends Across: Group 1 – The Alkali Metals\n## Trends Across: Group 7 – Halogens\n## Trends Across: period 3","[{\"question\":\"How are the blocks, groups, and periods on the periodic table related to electron structure?\",\"answer\":\"The periodic table is arranged into four blocks (s, p, d, f) associated with the last orbital. Elements are grouped into vertical columns (groups) and horizontal rows (periods), where group number relates to valence electrons and period number relates to the number of shells.\"},{\"question\":\"What happens to atomic radius across a period and down a group?\",\"answer\":\"Atomic radius decreases across a period and increases down a group. Down a group, more electron shells are added, and across a period the nuclear charge increases, strengthening attraction to outer electrons.\"},{\"question\":\"How do ionization energy and metallic character trend across the periodic table?\",\"answer\":\"Ionization energy increases across a period and decreases down a group. Metallic character increases down a group and decreases across a period, reflecting how easily atoms lose electrons.\"}]","Topic 3 - Periodicity | DOCX",1790051785,15]