[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-seo-572269-105":3,"detail-sidebar-cat-1-en-105":81,"doc-detail-572269-en":127},{"code":4,"msg":5,"data":6},0,"ok",{"site_id":7,"language":8,"slug":9,"title":10,"keywords":11,"description":12,"schema_data":13,"social_meta":74,"head_meta":76,"extra_data":78,"updated_unix":80},105,"en","the-ultimate-ap-chemistry-cheat-sheet-v2","The Ultimate AP Chemistry Cheat Sheet - v2","","Comprehensive AP Chemistry reference covering core exam topics from atomic structure to chemical reactions and kinetics. Summarizes electron configuration, periodic trends, ions, shielding, PES, and Lewis structures including formal charge, resonance, VSEPR geometry and hybridization, plus polarity rules. Details intermolecular forces, KMT and gas laws, solution chemistry, chromatography and distillation, spectroscopy fundamentals, and Beer–Lambert law. Includes reaction stoichiometry, limiting reagent, net ionic and redox, alongside rate laws, integrated rate equations, and Arrhenius concepts.",{"@graph":14,"@context":73},[15,34,56],{"@type":16,"itemListElement":17},"BreadcrumbList",[18,23,27,31],{"item":19,"name":20,"@type":21,"position":22},"https://docshare.wps.com","Home","ListItem",1,{"item":24,"name":25,"@type":21,"position":26},"https://docshare.wps.com/template/","Template",2,{"item":28,"name":29,"@type":21,"position":30},"https://docshare.wps.com/template/general/","General",3,{"item":32,"name":10,"@type":21,"position":33},"https://docshare.wps.com/template/the-ultimate-ap-chemistry-cheat-sheet-v2/572269/",4,{"url":32,"name":10,"@type":35,"image":36,"author":41,"headline":10,"publisher":44,"fileFormat":47,"inLanguage":8,"description":12,"dateModified":48,"datePublished":49,"encodingFormat":47,"isAccessibleForFree":50,"interactionStatistic":51},"DigitalDocument",{"url":37,"@type":38,"width":39,"height":40},"https://docshare.wps.com/thumbnails/the-ultimate-ap-chemistry-cheat-sheet-v2/572269.png","ImageObject",442,249,{"name":42,"@type":43},"BigDaveOnline","Person",{"url":19,"name":45,"@type":46},"DocShare","Organization","application/pdf","2026-10-22","2026-10-13",true,{"@type":52,"interactionType":53,"userInteractionCount":55},"InteractionCounter",{"@type":54},"ViewAction",9,{"@type":57,"mainEntity":58},"FAQPage",[59,65,69],{"name":60,"@type":61,"acceptedAnswer":62},"What do the cheat sheet’s periodic trends and ion rules help you predict?","Question",{"text":63,"@type":64},"They guide how atomic radius and related properties change across and down the periodic table, and how ions differ in size compared with their parent atoms.","Answer",{"name":66,"@type":61,"acceptedAnswer":67},"How does the document recommend constructing Lewis structures and determining formal charge?",{"text":68,"@type":64},"It specifies counting valence electrons, choosing a central atom with the lowest electronegativity (excluding H), completing octets with multiple bonds when needed, then computing formal charge and minimizing the absolute value.",{"name":70,"@type":61,"acceptedAnswer":71},"What approach does the cheat sheet give for solving reaction and kinetics problems?",{"text":72,"@type":64},"For reactions it outlines stoichiometry workflow, limiting reagent determination, and net ionic/redox steps. For kinetics it emphasizes deriving rate laws from experiments, using order rules and integrated rate equations, then applying Arrhenius relationships at a conceptual level.","https://schema.org",{"og:url":32,"og:type":75,"og:title":10,"og:site_name":45,"og:description":12},"article",{"robots":77,"canonical":32},"index,follow",{"doc_id":79,"site_id":7},572269,1792002418,{"code":4,"msg":82,"data":83},"success",[84,89,94,99,104,109,114,119,124],{"id":85,"doc_module":22,"doc_module_name":25,"category_name":86,"show_sort_weight":87,"slug":88},11,"Presentations",90,"presentations",{"id":90,"doc_module":22,"doc_module_name":25,"category_name":91,"show_sort_weight":92,"slug":93},12,"Resumes",80,"resumes",{"id":95,"doc_module":22,"doc_module_name":25,"category_name":96,"show_sort_weight":97,"slug":98},14,"Invoices",70,"invoices",{"id":100,"doc_module":22,"doc_module_name":25,"category_name":101,"show_sort_weight":102,"slug":103},15,"Posters",60,"posters",{"id":105,"doc_module":22,"doc_module_name":25,"category_name":106,"show_sort_weight":107,"slug":108},16,"Social Media",50,"social-media",{"id":110,"doc_module":22,"doc_module_name":25,"category_name":111,"show_sort_weight":112,"slug":113},17,"Forms",40,"forms",{"id":115,"doc_module":22,"doc_module_name":25,"category_name":116,"show_sort_weight":117,"slug":118},18,"Letters",30,"letters",{"id":120,"doc_module":22,"doc_module_name":25,"category_name":121,"show_sort_weight":122,"slug":123},21,"Paper Templates",5,"papers-templates",{"id":125,"doc_module":22,"doc_module_name":25,"category_name":29,"show_sort_weight":4,"slug":126},158,"general-158",{"code":4,"msg":82,"data":128},{"doc_id":79,"user_id":129,"nickname":42,"user_avatar":130,"doc_module":22,"category_id":125,"category_name":29,"doc_title":10,"doc_description":12,"doc_content":131,"file_id":132,"file_url":133,"file_type":134,"file_size":135,"view_count":55,"is_deleted":4,"is_public":22,"is_downloadable":22,"audit_status":22,"page_count":22,"language":136,"language_code":8,"site_id":7,"html_lang":8,"table_of_contents":137,"faqs":138,"seo_title":139,"seo_description":12,"update_tm":140,"read_time":4},962090896214,"https://ap-avatar.wpscdn.com/davatar_155a257f0dc6eb9ab79c44ca47cae57d","The Ultimate AP Chemistry Cheat Sheet (v2) [www.albert.io](www.albert.io)  \n\n| 1-2: Atomic & Molecular Structure (14–18%) |\n| --- |\n| Electron Config & Periodic Trends |\n| Aufbau: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p... Hund: single-fill each orbital before pairing. Pauli: max 2 e⁻/orbital (opposite spins) . Periodic trends (L→R, top→bot): radius ↓R, ↑down. IE ↑R, ↑ up. EA ↑R (dips at N, O) . EN ↑R, ↑up.\u003Cbr>Ions: +e − anion (> parent) , -e − cation (\u003C parent) . Shielding: inner e − repel outer →↓ Zeff → binding E ↓ , radius ↑ .\u003Cbr>Isoelectronic: same e⁻ count; smaller radius w/ ↑ nuclear charge.\u003Cbr>PES: peak position = binding E; peak height ∝ \\# e⁻ .\u003Cbr>Coulomb: F ∝ q1q2 /r2 , E ∝ q1q2 /r. (q = charge, r = distanc.)\u003Cbr>Lewis Structures, Formal Charge, Polarity |\n| Steps: sum valence e⁻; skeleton w/ least-EN atom central (never H); fill octets; multiple bonds if short.\u003Cbr>Formal Charge (FC) = V − N − B/2 (V=val, N=lone, B=bond e⁻); best structure has |FC| minimized; − FC on more-EN atom. Octet exceptions: H = 2; Be = 4; B/Al = 6; expanded octets for period 3+ (P, S, Cl); odd-e⁻ (NO, NO2) .\u003Cbr>Resonance: same atoms, different e⁻ position; real = weighted avg. All resonant bonds are identical (intermediate length/energy)\u003Cbr>VSEPR Geometry & Hybridization |\n| e⁻ grps Bonds LP Shape Angle Hybrid |\n| 2 2 0 linear 180° sp |\n| 3 3 0 trig planar 120° sp2 |\n| 3 2 1 bent \u003C 120° sp2 |\n| 4 4 0 tetrahedral 109.5 ° sp3 |\n| 4 3 1 trig pyr \u003C 109.5 ° sp3 |\n| 4 2 2 bent ≪ 109.5 ° sp3 |\n| ✓ Polar molecule = polar bonds + asymmetric shape. EN diff:> 1.7 ionic; 0.4–1.7 polar cov; \u003C 0.4 nonpolar. |\n\n\n| 3: Intermolecular Forces & Properties (18–22%) |\n| --- |\n|  |\n| ✓ IMF tree: H–F/O/N? → H-bond. Charged? → ion-dipole. Polar? → dipole-dipole. Else → LDF. List strongest first. |\n| IMF Types & Physical Properties |\n| Ranking: ion-dipole > H-bond > dipole-dipole > LDF. H-bonds: H–F/O/N (DNA, ice, water —abnormally high bp) . LDF: in ALL molecules; ↑ w/ surface area, e − count, polarizability (enhanced by π bonding) . Trends: ↑ IMF → ↑ bp/mp/viscosity/surface tension, ↓ Pvap. Ice \u003C water density (H-bonds) . \"Like dissolves like. \" Polar + ionic in H2 O; nonpolar in hexane/oil.\u003Cbr>Gases & KMT |\n| KMT: point particles, random motion, elastic collisions, no IMFs, KE ∝ T. Same T = same avg KE for all gases. Heavier = slower. Max-Boltz: ↑ T or ↓ mass = wider, right-shifted curve.\u003Cbr>Ideal gas: PV = nRT (R = 0.0821 L·atm/mol·K) . Combined: P1 V1 /T1 = P2 V2 /T2. STP: 0°C, 1 atm → 22.4 L/mol.\u003Cbr>Dalton: Ptot = ΣPi ; Pi = χi ⋅ Ptot (χi = ni /ntot) .\u003Cbr>KMT eq: KE = ~~12~~mv2. B/c avg KE depends only on T , lighter gases (smaller m) → higher avg velocities (effuse/diffuse faster) . Deviations: real P \u003C ideal (IMFs, worst low T); real V > ideal (particle vol, worst high P) . Ideal at high T + low P.\u003Cbr>Solutions & Separations |\n| Concentration: M = mol/L. Dilution: M1 V1 = M2 V2. Solubility of solids ↑ w/ T; gases ↓ w/ T, ↑ w/ P. Chromatog:\u003Cbr>separates by IMF differences; furthest spot = highest mobilephase affinity. Distillation: weakest IMFs (bp) boils first.\u003Cbr>Photons, Spectroscopy & Beer-Lambert |\n| Photon E = molecule's ΔE: E = hν = hc/λ . Micro = rot; IR = vib; UV/Vis = elec transitions. Beer: A = ϵbc (A ∝ c if b, λfixed) . Set λ at max A for highest sensitivity. |\n\n\n| Chemical Reactions (Unit 4, 7–9%) |\n| --- |\n|  |\n| Spectator ions cancel in net ionic. Cross same ions both sides. |\n| Mole Conversions, Empirical & Molarity |\n| Mole: n = g/MW; g = n ⋅ MW; particles\u003Cbr>= n ⋅ 6.022 × 1023. % comp: (mass element / total MW) ×100 Empirical: divide mol of each element by smallest mol → simplest whole-num ratio (multiply to clear frac, e.g. , x2 for 0.5) . Molecular formula = empirical ×(MWactual/MWempir) . Molarity: M = n/VL . Dilution: M1 V1 = M2 V2.\u003Cbr>Stoichiometry & Limiting Reagent |\n| Workflow: balance → g → n → mole ratio → n → g. Limiting: compute moles product from EACH reactant; smallest wins. Excess = total − used. % yield = (actual/theor) ×100% .\u003Cbr>Reaction Typ","cbCaiozQC5x3LF2W","https://ap.wps.com/l/cbCaiozQC5x3LF2W","pdf",291967,"English","# Atomic & Molecular Structure\n# Intermolecular Forces & Properties\n# Chemical Reactions\n# Kinetics","[{\"question\":\"What do the cheat sheet’s periodic trends and ion rules help you predict?\",\"answer\":\"They guide how atomic radius and related properties change across and down the periodic table, and how ions differ in size compared with their parent atoms.\"},{\"question\":\"How does the document recommend constructing Lewis structures and determining formal charge?\",\"answer\":\"It specifies counting valence electrons, choosing a central atom with the lowest electronegativity (excluding H), completing octets with multiple bonds when needed, then computing formal charge and minimizing the absolute value.\"},{\"question\":\"What approach does the cheat sheet give for solving reaction and kinetics problems?\",\"answer\":\"For reactions it outlines stoichiometry workflow, limiting reagent determination, and net ionic/redox steps. For kinetics it emphasizes deriving rate laws from experiments, using order rules and integrated rate equations, then applying Arrhenius relationships at a conceptual level.\"}]","The Ultimate AP Chemistry Cheat Sheet - v2 | PDF",1791926500]