好了，回歸正題，下面來說說到底怎么把這門知識點繁多，號稱“ 理科中的文科”高效復習好。

考慮到多數(shù)同學都會同時備考幾門AP課程，這里只需要你分配給化學九天，每天兩個小時，真的不能再省了。

當然還有個前題，比如你已經(jīng)上過某些培訓機構(gòu)的強化課程，或者已經(jīng)把普林斯頓類的教材自學了至少一遍，或者現(xiàn)在隨意做套真題正確率至少能達到一半；如果連這個基礎都沒有，那就請把每天的學習時間延長，達到同樣的目標要求即可。

綜述一下，整個計劃的前七天以逐章復習知識點和刷習題為主，懺悔之前的懶惰為輔；后兩天以練成套真題為主，查漏補缺和記單詞為輔。

知識點：

1）了解Dalton, Thomson, Millikan, Rutherford探索原子結(jié)構(gòu)時的主要手段和成果；熟悉Bohr模型和L.de Broglie波粒二相性的理論和相關公式， 會用Heisenberg測不準原理解釋原子結(jié)構(gòu)。

2）能懂且會用四個量子數(shù)表示電子排步。

3）理解Pauli, Aufbau, Hund, Energy Overlay這四條電子排步原則，熟記各條反例，如Cr, Cu, Mo, Ag這些半滿軌道排步。

4）能解釋原／離子半徑、電離能、電親和勢、電負性的周期性遞變原因；熟記s/p-block、半金屬元素的符號縮寫和英文全拼。

5）牢記核衰變反應的定義，各類核反應釋放出的微粒or射線實質(zhì)；熟練配平反應式和計算半衰期。

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.

題－Multiple Choice (MC)選自 Barron’s 2009 ed., Free Response (FR)選自歷年真題： ?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)。

知識點：

1) 能判別離子、金屬、共價鍵，以及分析前兩者強弱。

2）會畫共價化合物的Lewis dot structure ，20秒一個。能從重疊方式不同解釋sigma和pi鍵的區(qū)別，知道鍵級、鍵能、鍵長的聯(lián)系。

3）能用VBT解釋共價鍵實質(zhì)，用HOT解釋中心原子如何雜化，用VSEPR解釋成鍵電子／孤對電子間如何排斥并占據(jù)空間。

4）能分析出且熟記成鍵電子數(shù) + 孤對電子數(shù)小于等于六時的各種空間構(gòu)型，包括中心原子的軌道雜化方式、幾何體名稱、鍵角、分子極性。

5）根據(jù)極性不同判斷出三類分子間作用力，知道其強弱各自受哪些因素影響，以及它們的相對強弱。 6）掌握化合價配平法，半分鐘一個式子；關于mole運算、經(jīng)驗/分子式、凈離子方程式...這些初中就開始練的題，怎么還好意思錯呢。

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.

題：

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)。

知識點：

1) 靈活應用氣體分子的總／平均動能計算公式，以及可愛的Graham’s Law, 知道由PV=nRT推出來的系列公式所對應的不同恒定量假設。

2）牢記理想氣體的三個假設及其宏觀影響、Van der Waal’s Eq.里a、b的對應含義，會應用氣體分壓概念進行各種定量運算。

3）能找出三相圖、加熱／冷卻曲線圖里的各種特殊點或線，尤其特殊的水。

4）了解溶液和電解質(zhì)的定義，牢記濃度的兩種表達方式、四個colligative properties的含義和定量計算。

5）牢記可溶物和難溶物各自的溶解規(guī)律及溶解度表示，理解Ksp和同離子效應的定量運算。

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 ?題：

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。

知識點：

1）熟練運用實驗法找出任一反應的Rate Law, 任一反應物的rxn order，k的數(shù)值和單位，熟記0，1，2級反應的對應的公式和各種表達圖像，理解線性圖像的特殊意義。

2）應運碰撞理論和Arrhenius Eq.分析反應速率；牢記激活能、反應物濃度、溫度、壓強與反應速率的正負相關性。

3）理解基元反應的molecularity概念，會用多步反應中slow-determining step的反應機制替代總反應機制 。

4）牢記平衡常數(shù)的定義式，熟練掌握8種特殊情況下的Keq計算法。

5）熟練應用Le Chatelier’s Law, 分分鐘解釋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

題：

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)。

知識點：

1）ΔS, ΔH, ΔG的含義和在標準非標準狀態(tài)的正負值／定量運算，尤其是ΔH，那么多算法，你懂的。

2）關于熱容、比熱容、ΔG =ΔH - TΔS這些公式的運算和正負值含義。

3）熟練掌握酸堿的三種分類法，包括秒找共軛對，強／弱酸堿的判定，鹽的弱酸／堿性判定，緩沖溶液的構(gòu)成和作用原理。

4）能結(jié)合應用氧化數(shù)的增減和LEO & GER口訣，隨手拆出兩個半反應方程式，知道金屬活動性和氧化電動勢正相關。

5）理解酸堿滴定曲線的圖像變化，從而適當選擇指示劑；了解兩種電池的運作原理；能夠熟練判斷電池兩極，及其裝置用途和實驗現(xiàn)象。 ?題 (這天以知識點為主，題不多，明天集中刷定量計算)：

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

FR: 2014年 Q6 (c), 2013年Q3, 2012年Q3

計算出題點：

1）強／弱酸、強／弱堿、非中性鹽、緩沖溶液、滴定過程中某一時刻的pH, pOH, Ka, Kb，某離子濃度的運算，全都要會，沒商量。

2）會算轉(zhuǎn)移電子數(shù)，兩種電池的標準/非標準電池電勢；用法拉第公式計算轉(zhuǎn)移電量和電流；用Nernst Eq.把ΔG，Keq, Q,和Ecell聯(lián)立解決，包括Q=K或者T=298K這些特殊情況下的簡化公式。

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

FR: ?酸堿> 2014年Q2, 2012年Q1, 2011年Form B Q1, 2011年Q1, 2010年Form B Q5。氧化還原> 2014年Q3, 2013年Q2, 2012年Q6, 2010年Form B Q2。

半套來源：官網(wǎng)考綱

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

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