[{"data":1,"prerenderedAt":-1},["ShallowReactive",2],{"doc-seo-572899-105":3,"detail-sidebar-cat-1-en-105":74,"doc-detail-572899-en":120},{"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":67,"head_meta":69,"extra_data":71,"updated_unix":73},105,"en","mcat-chemistry-equation-sheet-orbitals-and-electrons-quantum-numbers","MCAT Chemistry Equation Sheet - Orbitals and Electrons - Quantum Numbers","","MCAT Chemistry Equation Sheet汇总关键概念与公式，覆盖量子数与电子排布、海森堡不确定原理与泡利不相容、洪特规则与阿夫鲍原则，以及理想气体与混合气体的推导关系。内容进一步整理气体“理想性”条件、范德华力及三类分子间作用力，归纳分子/金属/网络/离子固体的成键差异。随后给出溶液浓度表示、拉乌尔定律与依数性质、渗透压计算，并系统梳理酸碱平衡（Arrhenius、Brønsted-Lowry、Lewis）与pH/pKa相关表达。",{"@graph":14,"@context":66},[15,34,49],{"@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/paper-templates/","Paper 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−log[OH−]，并列出pKa与相关关系式。","https://schema.org",{"og:url":32,"og:type":68,"og:title":10,"og:site_name":40,"og:description":12},"article",{"robots":70,"canonical":32},"index,follow",{"doc_id":72,"site_id":7},572899,1791929935,{"code":4,"msg":75,"data":76},"success",[77,82,87,92,97,102,107,112,116],{"id":78,"doc_module":22,"doc_module_name":25,"category_name":79,"show_sort_weight":80,"slug":81},11,"Presentations",90,"presentations",{"id":83,"doc_module":22,"doc_module_name":25,"category_name":84,"show_sort_weight":85,"slug":86},12,"Resumes",80,"resumes",{"id":88,"doc_module":22,"doc_module_name":25,"category_name":89,"show_sort_weight":90,"slug":91},14,"Invoices",70,"invoices",{"id":93,"doc_module":22,"doc_module_name":25,"category_name":94,"show_sort_weight":95,"slug":96},15,"Posters",60,"posters",{"id":98,"doc_module":22,"doc_module_name":25,"category_name":99,"show_sort_weight":100,"slug":101},16,"Social 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Chemistry Equation Sheet  \nORBITALS AND ELECTRONS  \nQuantum numbers descriptions  \n\n| Quantum number | Description | Possible values |\n| --- | --- | --- |\n| Principal quantum number (n) | energy level | n=1, 2, 3   |\n| Angular momentum quantum number (l) | orbital shape (s, p, d, f) | l = 0, to …n- 1 |\n| Magnetic quantum number (m) | orbital orientation (px, py, pz) | m = -l to +l |\n| Spin quantum\u003Cbr>number (ms) | describes spin of electron | ms = + ½ or-½ |\n\nEach electron has a unique set of quantum numbers.  \nELECTRONIC CONFIGURATION  \nElectron configuration: describes the location of all of the electrons in an element. e.g. Carbon = 1s22s22p2  \nHeisenberg Uncertainty Principle: the position and momentum of a particle cannot both be exactly known at the same time. Pauli exclusion principle: no two electrons in an atom can have the same set of four quantum numbers (n, l, m, ms) which means that each orbital with quantum numbers (n, l, m) can hold at most two electrons with opposite spins.  \nHund’s rule: when electrons added to orbitals of equal energy, a single electron enters each orbital before a second electron with opposite spin enters any orbital. The spins remain parallel if possible. e.g.  \nNitrogen  \nN = ↑↓ ↑↓ ↑ ↑  \n↑  \n1s 2s 2px 2py  \n2pz  \nAufbau Principle: dictates the order in which orbitals fill. Some exceptions occur in the transition elements.  \n1s  \n2s 2p  \n3s 3p 3d  \n4s 4p 4d 4f  \n5s 5p 5d 5f  \n6s 6p 6d 6f  \nTHE GAS PHASE  \nUNITS OF PRESSURE:  \n1atm = 760 mmHg = 760 torr = 101.325 kPa = 1.01325 barr  \nIDEAL GAS POSTULATES  \n1. molecules are very small compared to the distance b/w them  \n2. molecules are continuously moving  \n3. pressure of the gas – collisions ofthe  \nmolecules with container walls  \n4. molecules do not experience intermolecular forces  \n5. KEave ∝ T  \nIdeal-gas law: PV = nRT  \nCombined gas law: P1 V1   P2 V2 =  \nT T  \n1 2 Charles’ law: V1   V2  \n=  \nT1 T2  \nBoyle’s law: P1V1 = P2 V2  \nNo ones’Law: P1   P2 =  \nT1 T2  \nP = const  \nT = const V = const  \nSTP – standard temperature (0°C or 273.15 K) and pressure (1 atm)  \n1 mol of ideal gas occupies V = 22.4 L standard conditions-25°C and 1 atm  \nDalton’s law of partial pressure (mixture of the gases) P = pA + pB + K+ pN  \npA = χA ⋅ P  \nn N  \nχA =  A  =  A ntotal Ntotal  \nGRAHAM’S LAW OF EFFUSION  \nvA  =   mB  KEA =  1  mAv2A  \nvB  mA 2  \nKEA = KEB at TA = TB b/c KE ∝ T , but vA ≠ vB at TA = TB  \nWhat leads to the gas “ideality”: highT & lowP & lower molecular weight or small size of gas molecules  \nReal gases:  \n• have intermolecular attractions (non-elastic collisions) called Van der Waals forces  \n• contain molecules that have volume (or measurable size)  \n⎝⎜⎛Preal + a ~~ ~~nV22~~ ~~⎟⋅ (Vreal − nb) = nRT  \nINTERMOLECULAR FORCES  \nDISPERSION FORCES:  \nDescribe the attraction between the negatively charged electron cloud of one molecule and the positively charged nuclei of neighbouring molecules  \nDIPOLAR FORCES:  \nDescribe the attraction between the negatively charged end of a polar molecule and the positively charged ends of neighbouring polar molecules  \nHYDROGEN BONDING:  \nInvolves lone pairs of electrons on an electronegative atom of one molecule and a polar bond to hydrogen in another molecule, they are confined to molecules that contain O, N, and F atoms.  \nPOLARIZABILITY:  \nThe ease with which the electron clouds are distorted  \nMOLECULAR SOLID:  \nMolecules in molecular solids are held in place by the types of forces: dispersion forces, dipolar interactions, and/or hydrogen bonds  \nMETALLIC SOLID:  \nAtoms in metallic solids are held in place by delocalised bonding  \nNETWORK SOLID:  \nContains an array of covalent bonds linking every atom to its neighbours  \nIONIC SOLID:  \nContains cations and anions, attracted to one another by coulombic interactions  \nSOLUTIONS  \n\n| molarity (M) | moles of solute/volume of solution. M=n/V |\n| --- | --- |\n| molality (m) | moles of solute/kg of solvent |\n| mole fraction (χ) | moles of solute/total mol","cbCailpXsRruzInA","https://ap.wps.com/l/cbCailpXsRruzInA","pdf",281848,"English","# Orbitals and Electrons\n## Quantum Numbers Descriptions\n# Electronic Configuration\n# The Gas Phase\n## Units of Pressure and Ideal Gas Postulates\n## Gas Laws (Combined/Charles/Boyle)\n## Dalton’s Law and Graham’s Law\n## Real Gases and Intermolecular Forces\n# Solutions\n## Molarity, Molality, Mole Fraction, and Mass Percent\n## Raoult’s Law and Colligative Properties\n## Osmotic Pressure\n# Acid-Base Equilibria\n## Arrhenius, Brønsted-Lowry, Lewis\n## Water Equilibrium Constant and pH Scales","[{\"question\":\"每个电子的量子数包含哪些内容？\",\"answer\":\"量子数包括主量子数n（能级）、角动量量子数l（轨道形状）、磁量子数m（轨道取向）以及自旋量子数ms（自旋，+1/2或-1/2）。每个电子都对应一组独特的四个量子数。\"},{\"question\":\"理想气体的基本条件与理想气体状态方程是什么？\",\"answer\":\"理想气体基于：分子体积相对可忽略、持续随机运动、只与容器壁发生碰撞且无分子间作用力，并且平均动能与温度成正比。理想气体定律为PV = nRT。\"},{\"question\":\"文档中如何区分不同类型的酸碱理论与pH计算？\",\"answer\":\"Arrhenius酸在水溶液中产生H+，Arrhenius碱产生OH−；Brønsted-Lowry酸可给出质子、碱可接受质子，并包括两性物种；Lewis酸接受电子对、Lewis碱给出电子对。pH = −log[H3O+]，pOH = −log[OH−]，并列出pKa与相关关系式。\"}]","MCAT Chemistry Equation Sheet - Orbitals and Electrons - Quantum Numbers | PDF"]