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The material explains valence electrons, Lewis structures, ionic charge patterns by group, and electromagnetic radiation categories and wave-particle duality. It further covers electron distribution in energy levels using orbitals, quantum numbers, sublevels, orbital shapes, capacities, and spin concepts. Finally, it summarizes electron configuration rules such as Aufbau, Pauli, and Hund, plus example configurations for nitrogen and cadmium.",{"@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/ch-7-notes-completing-the-model-of-the-atom/657084/",{"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/ch-7-notes-completing-the-model-of-the-atom/657084.png","ImageObject",300,407,{"name":92,"@type":93},"BigDaveOnline","Person",{"url":74,"name":95,"@type":96},"DocShare","Organization","application/pdf","2026-10-30","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 does valence determine bonding and ionic charge in these notes?","Question",{"text":112,"@type":113},"Valence electrons are the outermost shell level and are exposed for bonding. Atoms try to become like noble gases by losing, gaining, or sharing electrons, which corresponds to typical ionic charges by group.","Answer",{"name":115,"@type":110,"acceptedAnswer":116},"What does the wave-particle duality statement mean here?",{"text":117,"@type":113},"It states that waves can behave like particles and particles can behave like waves. This appears alongside the review of electromagnetic radiation categories and wave dimensions.",{"name":119,"@type":110,"acceptedAnswer":120},"What are the three key rules for writing electron configurations?",{"text":121,"@type":113},"The notes list the Aufbau Principle (fill low-energy orbitals first), the Pauli Exclusion Principle (no more than two electrons per orbital with compatible spins), and Hund’s Rule (fill degenerate orbitals singly before pairing).","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},657084,1793080861,{"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":34,"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},962090896214,"https://ap-avatar.wpscdn.com/davatar_155a257f0dc6eb9ab79c44ca47cae57d","Ch. 7 NOTES ~ Completing the Model of the Atom  \nNOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.  \n7.1 Notes  \nI. Developing a Model of Atomic Structure  \nA. Review of atomic theory development  \n1) ancient Greece: Democritus of Abdera  \n􀁸 proposed the existence of atoms (atoma)  \n􀁸 went against Aristotle’s idea of continuous matter (hyle)  \n2) 1803: Dalton’s atomic theory  \n\n| DALTON’S ATOMIC THEORY |\n| --- |\n| 1) All elements are composed of submicroscopic, indivisible particles called atoms.(He didn’t know about subatomic particles and how to split an atom.)\u003Cbr>2) Atoms of the same element are identical. (He didn’t know about isotopes.) Atoms of different elements are different.\u003Cbr>3) Atoms of elements can physically mix or form compounds by chemically combining in whole-number ratios. (Law of Multiple Proportions)\u003Cbr>4) Chemical reactions involve the separation, joining, or rearranging of atoms. Atoms of an element are never changed into atoms of another element in a chemical reaction. (He didn’t know about nuclear reactions.) |\n\n3) 1897: Thomson’s plum pudding model  \n􀁸 electrons embedded in a positive ball  \n4) 1909-1911: Rutherford: gold foil experiment  \n􀁸 the atom is mostly space  \n5) 1913: Bohr’splanetary model of the atom  \n􀁸 nucleus in the center, electrons in orbit around it  \n6) 1935+ : modern 3-D electron-cloud model; probability model  \nB. review of valence electrons and Lewis structures (electron dot diagrams)  \n1) valence = outermost electron shell or level  \n2) valence electrons are exposed and available for bonding  \n3) atoms will try to become like Noble Gases  \n(they don’t change what’s in the nucleus, but they change the valence shell)  \na) gain electrons to become anions (ionic bonding) ORb) lose electrons to become cations (ionic bonding) ORc) share electrons with other atoms (covalent bonding)  \nUPDATED ELECTRON INFORMATION TABLE:  \n\n| GROUP \\# | \\# VAL. e- | \\# DOTS | STATUS | ACTION IONIC CHARGE |  |\n| --- | --- | --- | --- | --- | --- |\n| IA (1) | 1 | 1 | 1 / 8 | lose 1 | + 1 |\n| IIA (2) | 2 | 2 | 2 / 8 | lose 2 | + 2 |\n| IIIA (13) | 3 | 3 | 3 / 8 | lose 3 | + 3 |\n| IVA (14) | 4 | 4 | 4 / 8 , half full | lose, gain, or neither | varies (“mixed”) |\n| VA (15) | 5 | 5 | 5 / 8 | gain 3 | -3 |\n| VIA (16) | 6 | 6 | 6 / 8 | gain 2 | -2 |\n| VIIA (17) | 7 | 7 | 7 / 8 | gain 1 | -1 |\n| VIIIA (18) | 8 | 8 | 8 / 8, full | nothing 0: | does not form ions |\n\n“Charge Chant”: +1 +2 +3 mixed -3 -2 -1 0  \n+2 in the middle, unless they tell you otherwise  \nC. review of em (electromagnetic) radiation  \n1) em radiation includes  \nRADIO WAVES, MICROWAVES, INFRARED (IR) RADIATION, VISIBLE LIGHT (―ROYGBIV‖: red, orange,yellow, green, blue, indigo, violet), ULTRAVIOLET (uv), X-RAYS, GAMMA RAYS  \n2) review of wave dimensions  \nSlow wave with low energy, low frequency, Fast wave with high energy, high frequency,  \nsmall amplitude, and large wavelength large amplitude, and small wavelength  \n3) review WAVE-PARTICLE DUALITY OF NATURE:  \nwaves can act as particles AND particles can act as waves  \nII. Distribution of Electrons in Energy Levels  \nA. atomic orbitals  \n1) orbitals are areas of high probability (~95%) of finding electrons  \n2) Heisenberg Uncertainty Principle—it is not possible to know both the exact position and velocity of an object simultaneously  \na) if you measure the position, you have to stop it (technically), so you cannot find the velocity or momentum  \nb) if you measure the velocity, it is moving, so you cannot pinpoint one position to measure  \nB. principal quantum number = n  \n1) electron energy level or ―shell‖ number  \n2) n = 1, 2, 3, 4, 5, 6, 7  \nC. energy sublevels—divisions within a level  \n1) many similar energy states grouped together in a level  \n2) different shapes: spherical, dumbbell, cloverleaf  \n3) sublevels: s, p, d, f  \n(s p d f stand for sharp, principal, diffuse, fundamental)  \n4) maximum number of e- in a principal energy level = 2n2  \n n   SUBL","cbCaiiKj57qZd1Y9","https://ap.wps.com/l/cbCaiiKj57qZd1Y9","pdf",575762,"English","# 7.1 Notes\n## I. Developing a Model of Atomic Structure\n## II. Distribution of Electrons in Energy Levels\n## III. Electron Configurations","[{\"question\":\"How does valence determine bonding and ionic charge in these notes?\",\"answer\":\"Valence electrons are the outermost shell level and are exposed for bonding. Atoms try to become like noble gases by losing, gaining, or sharing electrons, which corresponds to typical ionic charges by group.\"},{\"question\":\"What does the wave-particle duality statement mean here?\",\"answer\":\"It states that waves can behave like particles and particles can behave like waves. This appears alongside the review of electromagnetic radiation categories and wave dimensions.\"},{\"question\":\"What are the three key rules for writing electron configurations?\",\"answer\":\"The notes list the Aufbau Principle (fill low-energy orbitals first), the Pauli Exclusion Principle (no more than two electrons per orbital with compatible spins), and Hund’s Rule (fill degenerate orbitals singly before pairing).\"}]","Ch. 7 NOTES - Completing the Model of the Atom | PDF",1792973608,18]