备考攻略丨AP化学最全知识点，搞定这科只要9天！

好了，回归正题，下面来说说到底怎么把这门知识点繁多，号称“ 理科中的文科”高效复习好。

考虑到多数同学都会同时备考几门AP课程，这里只需要你分配给化学九天，每天两个小时，真的不能再省了。

当然还有个前题，比如你已经上过某些培训机构的强化课程，或者已经把普林斯顿类的教材自学了至少一遍，或者现在随意做套真题正确率至少能达到一半；如果连这个基础都没有，那就请把每天的学习时间延长，达到同样的目标要求即可。

综述一下，整个计划的前七天以逐章复习知识点和刷习题为主，忏悔之前的懒惰为辅；后两天以练成套真题为主，查漏补缺和记单词为辅。

知识点：

1）了解Dalton, Thomson, Millikan, Rutherford探索原子结构时的主要手段和成果；熟悉Bohr模型和L.de Broglie波粒二相性的理论和相关公式， 会用Heisenberg测不准原理解释原子结构。

2）能懂且会用四个量子数表示电子排步。

3）理解Pauli, Aufbau, Hund, Energy Overlay这四条电子排步原则，熟记各条反例，如Cr, Cu, Mo, Ag这些半满轨道排步。

4）能解释原／离子半径、电离能、电亲和势、电负性的周期性递变原因；熟记s/p-block、半金属元素的符号缩写和英文全拼。

5）牢记核衰变反应的定义，各类核反应释放出的微粒or射线实质；熟练配平反应式和计算半衰期。

Electron model

1. Black body radiation—undermine classical physics--Mac Plank E=hv -- photoelectric effect

2. Spectra: continuous spectrum(all color), emission lines spectra(color with special energy are on the spectra), absorption spectra (black lines, reverse of emission lines)

3. En=-Rn(1/n^2)     1/wavelength=Rh(1/(n1)^2-1/(n2)^2)

4. For one electron atoms or ions: Bohr Model (classic physics+ Rutherford model+ quantum theory)

(1)angular momentum(energy) is quantized, electron in orbit radiate no energy

(2)photon-excitization-excited state-move back-electromagnetic radiation

(3)e can exist in possible circular orbit with fixed radius

5. E=-2.18*10^-18/n^2

6. First ionization energy of H: 2.18*10^-18

7. wave and particle duality: De Broglie wavelength=h/p=h/mv=10^-10m

8. Heisenberg uncertainty principle: dx*dp>=k/4pi. It is impossible to determine position and momentum at the same time.

9. Wave mechanical model:

(1)calculate possible energy states and positions

(2) Quantum number and wave function (probability of locating an e in a region in space)

10. Quantum numbers:

(1) principle quantum number: n, determine size and energy of orbital

(2) angular momentum number: l (0——n-1) shape of orbital

(3) magnetic quantum numbers: ml (-l——l) orientation

(4) Spin quantum number: ms=+-1/2 spin

11.  when Z>1 : nuclear charge is greater, e and e repulsion, penetration (cause of fraction Zeff)

Period:

1. Group1: alkali metal, group2:alkali earth metal, group5:pnictogens(stifle), group6: chalcogens (elements to make ore), group7:halogen, group8: noble gas

2. Transition metal: 3-12. Inner transition element: actinides and lanthanides

3. Metallic character decreases from Fr to F

4. Semimetal: conduct electricity and very low temperature, superconductor

5. D-block: colored compound, complex ion, many oxidation states, magnetic properties, catalysis

6. Atomic radius: increase down a group because: valence n increases, valence e further from nucleus, an extra full shell repels other e to make it bigger

Decrease across a period because: e is added to the same valence shell, shielding by inner shell is constant, Zeff increases so valence e is pulled closer

7. Radius of ions: cation is smaller and anion is bigger.

8. Electronegativity: ability of a bonded atom to attract a shared pair of e.

9. Down a group and En decreases because atoms have bigger radius. Across a period En increases because atom is smaller and Zeff increases.

10. Ionization energy: first ionizing energy: E(g)-E+(g)+e- second ionizing energy: E(g)-E2+(g)+2e-

11. Down a group IE decreases as radius increases and nuclei have less attraction of valence electron, across a period IE increases as Zeff increases, attraction increases and it is harder to pull a e away. Small trend because e is spinning paired and repulsion exist between 2e in the same orbital

12. Successive ionization energy: pick 1 element and takes away its electrons one by one, the jump of energy is orbital because: when there is less e, more attracted to nucleus, repulsion is smaller with less e, when removed a shell, it is harder to move another e as it is closer to the nucleus

13. Electron affinity: first EA: E(g)+e—E-(g)

14. Trends are not clear but basic trends are: down a group less negative as radius increases-attraction decreases-less energy released, across a period more negative as Zeff increases-attraction increases-energy released increases.

15. Group1: lowest 1stIE in periodic table, slightly negative EA, keen to give up e but weakly to accept e

16. Group7: high1stIE, high negative EA, lose e with difficult but gain easily

17. Group8: very high 1stIE, slightly positive EA, tend not to lose or gain e easily.

题－Multiple Choice (MC)选自 Barron’s 2009 ed., Free Response (FR)选自历年真题：  MC: Chp.1 –Question (Q#) 10, 12, 13, 15, 22; Chp.2 -Q6, 9, 13, 14; Chp.3 –Q1-3, 5, 7, 9。

FR: 2010年 Q6 (a-c), 2007年Form B Q2、Q7 ( a-c (i) )，2006年Form B Q7 (a, c, d)。

知识点：

1) 能判别离子、金属、共价键，以及分析前两者强弱。

2）会画共价化合物的Lewis dot structure ，20秒一个。能从重叠方式不同解释sigma和pi键的区别，知道键级、键能、键长的联系。

3）能用VBT解释共价键实质，用HOT解释中心原子如何杂化，用VSEPR解释成键电子／孤对电子间如何排斥并占据空间。

4）能分析出且熟记成键电子数 + 孤对电子数小于等于六时的各种空间构型，包括中心原子的轨道杂化方式、几何体名称、键角、分子极性。

5）根据极性不同判断出三类分子间作用力，知道其强弱各自受哪些因素影响，以及它们的相对强弱。 6）掌握化合价配平法，半分钟一个式子；关于mole运算、经验/分子式、净离子方程式...这些初中就开始练的题，怎么还好意思错呢。

Bond

1. Reason of bond: electrostatics, lower their energy

2. Bond: covalent(non-metal and non-metal), ionic(non-metal and metal), metallic(metal and metal)

3. Lewis theory: octet rule. Every atom tens to have 8 e. discovered by noble gas

4. Lattice energy: a measure of strength of attraction between ions  Na(g)+ Cl(g)- NaCl(s)   unit is KJ/mol. Measured in born-haber cycle(chemical way) and born-mayer cycle(LE=k(Z+*Z-)/r)

Ionic solid:

1. giant 3-D lattice

2. Hydration energy: energy used to make ions in water completely surround by a shell of water molecule. When LE<HE, soluble. Bigger radius, more electrons, higher HE. Endothermic dissolve is caused by entropy, like NH4NO3. HE is decided by Z and r.

3. High melting point and boiling point: it is hard to make ions vibrate so harder to pull them apart.

4. Conduct electricity: when molten or dissolved in water because ions can mobile

5. Brittle: when hit, cation and cation (anion and anion) will move and repel each other.

Metallic bonding

1. low melting point and high boiling point: it is easy to pull metal atoms apart but it is hard to completely separate an atom

2. good thermo and electric conductivity: mobile e-

3. luster

4. Malleable and ductile: forces of attraction are not broken. Ion slide over each other but still held together

5. melting point increases when Z increases: more e- and less radius

Covalent bond

1. bond length and strength: long the bond, weaker it is

2. bond energy is measured in KJ/mol

3. poor conduction of electricity: no delocalized e- (except graphite)

4. melting point and boiling point: - giant lattice: high because hard to break bond         -molecular solid: low because IMF is weak

5. diamond: -hard: 3D interlocking of covalent bond  -not conduct electricity: all valence e is used in bond

6. Graphite: -conduct electricity: delocalized e  -soft weak: LDF between layers are easy to overcome by force.

Coordination compound

1. Contains complex ion and counter ion. Ex: [Co(NH3)6]3+(complex ion) + Cl-(counter ion)

2. ligand: provide both electron for covalent bond so must have lone pairs. Are around transition metal in complex ion.

3. name: name cation first, include oxidation state of cation, then name anion  ex: hexaamminecobalt(iii) chloride

4. Formation reason: d orbital of metal is empty and overlap with electron orbital of ligand.

5. dative bond: a covalent bond In which the pair of e- is supplied by one of the 2 balanced atoms (Lewis base provides e- while Lewis acid do not)

Lewis structure

1. Decide Lewis structure: -formula  –central atom(one with lowest EN except H)  –count e- -draw skeletal structure  –add e-

2. electron deficient compound may violent octet rule    ex: BF3

3. Formal charge: the electric charge an atom would have if all bonding electrons were shared equally with its bonded neighbor. Normally between -1 and +1

4. resonance is actually delocalized pi-bonds

5. Bond order: the bonds between two atoms, resonance are calculated by taking average

Molecular shape and inter molecular force

1. VSEPR theory: valence e- pairs repelling to minimize energy of molecule or polyatomic ion. Valence e- maximizes distance apart and determine the shape of molecules.

2. geometry shape:

3. all lone pairs are not include in the geometry shape

4. hybridization: (1)sp linear BeH2 (2) sp2 trigonal planar BF3 (3) sp3 tetrahedral (4)sp3d trigonal bipyramid PCl5, XeF2  (5)sp3d2 octahedral SF6, XeF4O, XeF4

5. molecular orbital theory: explains resonance like benzene

6. polarity:

• non polar: no permanent polarity, no dipole
• Polar: delta EN not zeros

7. Intermolecular forces:

(1)LDF electron fast moving causes temporary dipole. Down a group stronger because of more electrons (more polarizable) and bigger(less attraction of electron), more surface area contact stronger

(2) Hydrogen bond: because of (a)highly EN FONCl(b) no inner shells in H(c) small size of FONCl

(3) Ion dipole: ion + polar mole

(4) dipole-dipole

8. Like dissolves like: polar-polar force to overcome lattice energy, non polar- non polar because of entropy and enthalpy.

题：

MC: Chp.5 – Q10, 11, 13, 14; Chp.6 – Q5, 14, 17, 18, 20

FR: 2014年Form B Q5，2012年 Q4, 2006年Q7 (a-b)。

知识点：

1) 灵活应用气体分子的总／平均动能计算公式，以及可爱的Graham’s Law, 知道由PV=nRT推出来的系列公式所对应的不同恒定量假设。

2）牢记理想气体的三个假设及其宏观影响、Van der Waal’s Eq.里a、b的对应含义，会应用气体分压概念进行各种定量运算。

3）能找出三相图、加热／冷却曲线图里的各种特殊点或线，尤其特殊的水。

4）了解溶液和电解质的定义，牢记浓度的两种表达方式、四个colligative properties的含义和定量计算。

5）牢记可溶物和难溶物各自的溶解规律及溶解度表示，理解Ksp和同离子效应的定量运算。

Gases

1. Pressure:1.01*10^5Pa=1atm=760mmHg

2. Temperature: K=C+273.15

3. Boyle’s law: PV=k(n,T is kept constant) Charle’s law: V=kT(P,n is kept constant) Avogadro’s law: V=kn(P,T is kept constant)

4. Kinetic molecular theory: assume(1)volume is neglectable (2) no IMF (3)elastic collision (4) average KE=T

5. Peak of number of molecule vs speed graph is approximately average KE

6. m1/m2=average v2^2/average v1^2   v1/v2=√m2/m1

7.Graham’s law of diffusion :average KE=1.5RT=0.5MV^2(for 1 mol)   average v=√3RT/Mr (root-mean-square speed)

8. Real gas: tend to act like ideal gas when: T is high and P is low

9. (P+an^2/v(volume)^2)(V-bn)=nRT  题：

MC: Chp.7 – Q8, 19, 20; Chp.8 – Q3, 13-16; Chp.9 – Q14, 17, 18, 20, 21。

FR: 2014年Q1、Q4 (a-b), 2013年Q1, 2012年 Q2 (a-e), 2011年 Form B Q2 (a-c),  2010年Q1。

知识点：

1）熟练运用实验法找出任一反应的Rate Law, 任一反应物的rxn order，k的数值和单位，熟记0，1，2级反应的对应的公式和各种表达图像，理解线性图像的特殊意义。

2）应运碰撞理论和Arrhenius Eq.分析反应速率；牢记激活能、反应物浓度、温度、压强与反应速率的正负相关性。

3）理解基元反应的molecularity概念，会用多步反应中slow-determining step的反应机制替代总反应机制 。

4）牢记平衡常数的定义式，熟练掌握8种特殊情况下的Keq计算法。

5）熟练应用Le Chatelier’s Law, 分分钟解释Haber process。

Reaction Rate

1.collision theory: reaction is caused by collision with right orientation and enough Ea

2.-surface are increases: more probable of successful collision   -temperature increases: more molecules with energy more than Ea

3.Archenius  k=Ae^(-Ea/RT)   A is pre-exponential constant R=8.314J/mol*K

4.rate= k[A]

5.Ea= Rln(k2/k1)/[(1/t1)-(1/t2)]

6.Reaction profile: for a chemical reaction Ea is fixed. Transition state is the state with highest PE, catalyst will decrease Ea without affecting delta H

7.r= k[A]^x*[B]^y*[C]^z    x,y,z are the orders with respect to A,B,C

8.Initial rate method: (a)vary [a] and keep others constant and then (b) vary [B] and keep others constant.   Log r= log k +x*log[A]i

9.mechanism: many simples steps together to form a reaction

10.intermediate: produced in one step and consumed in another

11.one can check if his mechanism is correct by finding intermediates.

Nuclear chemistry

Different power of abilities of different rays

Biological effect:

(1) alpha: harmless, cannot penetrate skin

(2) Beta: high, can harm bones, organs

(3) Gamma: high, will ionize molecules can cause them to repeal each other

6. Fission and fusion:

(1) fission: one nuclear becomes more than one particle, like U235

(2) Fusion: two or more nuclei combine to become one nuclear

题：

MC: Chp.11-Q6, 8, 13,17, 20, 22; Chp.10 –Q7, 9,13,17, 19

FR: 2012年 Q3 (d-f), 2011年Q6 (c-d), 2010年Form B Q3 (c-f)。

知识点：

1）ΔS, ΔH, ΔG的含义和在标准非标准状态的正负值／定量运算，尤其是ΔH，那么多算法，你懂的。

2）关于热容、比热容、ΔG =ΔH - TΔS这些公式的运算和正负值含义。

3）熟练掌握酸碱的三种分类法，包括秒找共轭对，强／弱酸碱的判定，盐的弱酸／碱性判定，缓冲溶液的构成和作用原理。

4）能结合应用氧化数的增减和LEO & GER口诀，随手拆出两个半反应方程式，知道金属活动性和氧化电动势正相关。

5）理解酸碱滴定曲线的图像变化，从而适当选择指示剂；了解两种电池的运作原理；能够熟练判断电池两极，及其装置用途和实验现象。  题 (这天以知识点为主，题不多，明天集中刷定量计算)：

MC: Chp. 12-Q9-11, 12, 13, 14

FR: 2014年 Q6 (c), 2013年Q3, 2012年Q3

计算出题点：

1）强／弱酸、强／弱碱、非中性盐、缓冲溶液、滴定过程中某一时刻的pH, pOH, Ka, Kb，某离子浓度的运算，全都要会，没商量。

2）会算转移电子数，两种电池的标准/非标准电池电势；用法拉第公式计算转移电量和电流；用Nernst Eq.把ΔG，Keq, Q,和Ecell联立解决，包括Q=K或者T=298K这些特殊情况下的简化公式。

MC: Chp.14-Q4, 5, 9, 22, 24; Chp.13-Q12, 13, 16, 18, 22

FR:  酸碱> 2014年Q2, 2012年Q1, 2011年Form B Q1, 2011年Q1, 2010年Form B Q5。氧化还原> 2014年Q3, 2013年Q2, 2012年Q6, 2010年Form B Q2。

半套来源：官网考纲

链接：http://media.collegeboard.com/digitalServices/pdf/ap/IN120085263_ChemistryCED_Effective_Fall_2013_lkd.pdf

从第119页开始，26道最新版选择样题，限时40分钟，认真做吧。