IB Chemistry HL暗記物リスト
理想的には暗記以上のレベルまで持っていきたいけど、時間的にきついのでとりあえず短期的に覚える物のリスト
あくまでも僕がまた覚えてないなーと思ったもののリストなので、ここに書かれてないことでも暗記必要なものあると思う
暗記必要な物でも自分の中で自明になったことは省いている
202106 昔は自明だと感じていたことも忘れかけているよう
ex: electronegativityのtrendの理由とか
表面は毎回暗記していたけど、その裏の部分を放置してきた（大体わかるだろと思っていた）ので忘れかけている
なので、それをreviewしないといけない
Chapter 1
Relative Atomic Mass
Def: Average mass of its atoms, compared to 1/12th the mass of a carbon-12 atom.
Unit: g mol-1
1atm = 1.01x10^5 Pa
Chapter 2
Visible Spectrum: Transition between * and n=2, n=3
Terms
“Shell”: 1,2,3とか
“Subshell”: 1s, 2p, 3dとか
“Orbital”: 2px, 2py, 2pzとか
Irregular (anti-Aufbau)
Cr config. [Ar] 3d5 4s1 (not 3d4 4s2)
Cu config. [Ar] 3d10 4s1 (not 3d9 4s2)
1st ionization E
Def: Energy for 1 mol of gaseous atom when losing 1 mol of electron (in standard thermodynamic conditions)
= Convergence limit of spectrum from n=1 (use E=hf)
Chapter 3
Trend
Electron shielding = repulsion between E level
“Nuclear charge” vs repulsion between same shell electrons
左下に増える: atomic radius, metallic character
右上に増える: electronegativity, magnitude of electron affinity, ionization energy
Ionization E, subshell変わるかorbitalでpair組み始めた時はrepulsion増えてE減る
複雑: melting point(bondingによって大きく変わる)
左の方はmetallic bondでまあまあ高い、真ん中はgiant covalentで一番高い、右はcovalent/noble gasで低い
Group 1
“Alkali metal”
Reaction with Oxygen/Water
More reactive down the group
Group 17
“Halogens”
Reaction with Alkali Metal 2A(s) + H2 -> 2AH(s) (colorless, neutral)
Displacement Reaction
Lesser period Halogen with Larger period Halide
Ex: Cl2 + 2KBr -> 2KCl + Br2
Less reactive down the group
Period 3 Oxide
https://gyazo.com/f4fab068dc7c6e70f54331d3d0d803e9
Structure of oxide
Na, Mg, Al: Giant Ionic (strong = solid)
Si: Giant covalent (solid)
P, S, Cl: Molecular compound (weak intermolecular force = gas/liquid)
Reaction of oxide with water
Basic: XO + H2O -> 2X(OH)n (acidic)
Acidic: XO + H2O -> HnXOm (alkaline)
(logic: solid dissolved neutral water = basic product, then solid is basic)
Transition Elements
Zn not Transition element
Multiple oxidation states
All has +2
https://gyazo.com/313bcf1e23985b446c42f5015cc96a55
Magnetism
Paramagnetic: Unpaired electron -> attracted by field
Diamagnetic: Paired electron -> repelled by field
Ferromagnetic: Many unpaired electrons aligned -> Strong magnetism Ni, Co, Fe
unpaired electrons causes magnetism
Ligands: coordinate covalent bonds
Neutral: H2O, NH3, CO
1- Ligands: Cl-, CN-, Br-
Catalyst
N2 + 3H2 ⇆ 2NH3 /w Iron
Colored complex
Repulsion with e- of ligands
Splitting of 3d orbital, 2 upper 3 lower: when ligands are attached
Absorption of light (low to high E level)
Spectrochemical series of ligands
stronger field -> more split -> absorb shorter wave length
https://gyazo.com/ed35b88f89002c6c210a47bd251887e7
Remember ligands, coordination No, etc
https://gyazo.com/3275b43bb77be70b45938ded52e20df1
Chapter 4: Chemical bonding and structure
https://gyazo.com/126d327223b580f2720eb534834c30bc
carbonate, chromate, phospate, sulfateはchargeが-1ではない
chromate, phospate, sulfateは例外、Oの数が3ではなく4
Metallic Bonding Factors
# of delocalized electrons
Charge of cation
Ionic radius of cation
Covalent Bonding
VSEPR
Lonepair-lonepair > lonepair-bondedpair > bondedpair-bondedpair
Expanded octet for period 3+ possible
https://gyazo.com/5ce8797bae856bfba8921cc596bdf775
Hybridization
結局何かというと、lone pairで+1, σ bondで+1すれば良い
言い換えると、図を書いた時にelectron pairを表す線が何辺から伸びているか
Sigma bond: round + round
Single bond
Pi bond: dumbbell + dumbbell
double, triple bond between 2 p-orbital
Cloud above and below σ bond
Formal Charge
(Valence electron in uncombined form) - (number of non-bonding electrons) - ½(number of bonding electrons)
Closer to 0 = more preferrable
Intermolecular forces (only on simple covalent) (Lower = Stronger)
London Force: Instantaneous dipole-inducded dipole
Dipole-Induced-dipole
Dipole-dipole
Hydrogen Bond: strong Dipole-dipole (H to N,O,F)
More electron = more intermolecular F
Similar intermolecular force = soluble
Chapter 5: Energetics
Open system: all exchange ok
Closed: only energy ok
Isolated: nothing ok
Chapter 6: Kinetics
Condition of Reaction:
Correct orientation
KE > AE
Definitions of specific enthalpy
Default:
Direction: as name states
Ex:
atomize = to single gas atom
ionization = to positive ion
Amount: 1mol of measurable (sometimes reactant, sometimes product)
Lattice enthalpy (Irregular)
Direction: From broken ions to lattice
Amount: 1mol of lattice
Enthalpyのtrendを知っておくべき（大体は直感でわかる筈）
Chapter 7: Equilibrium
Conditions:
Closed system
Rate of forward and backward reactions are same
Concentration of reactant/product is constant
Habor Process (Ammonia)
N2+3H2 ⇄ 2NH3
Exothermic, Mol decreasing
Condition for forward reaction
Low temperature
However, some temperature needed for high reaction speed
Optimum temperature: 450°C (not K)
(High reaction speed = faster to reach equilibrium)
High Pressure
Optimum pressure: 200-250 atm
Too high: plant breaks
Catalyst
Needed, otherwise have to use lower temp / higher pressure
Use “fresh” Iron
Usage: Fertilizer, explosives, etc
Contact Process (Sulfuric Acid)
S + O2 ⇄ SO2
SO2 + O2 ⇄ 2SO3 (Important step)
Exothermic, Mol decreasing
SO3 + H2O ⇄ H2SO4 / SO3 + H2SO4 ⇄ H2S2O7
Condition for the forward reaction
Low temperature
400°C or more
Catalyst only works on 400+
Catalyst
Vanadium (V) Oxide
NO High Pressure
Already enough rate
High pressure is uneconomic and dangerous
Usage: Fertilizer, Paints, etc
https://gyazo.com/8b53f5dc8cbe0a466c63b77940fb064f
At equilibrium, the Gibbs free energy is at a minimum and entropy is at a maximum.
Chapter 8 Acid and bases
Def
Bronsted-Lowry
Acid: H+ donor
base: H+ acceptor
has lone pair, H+ coordinate bond
Acid + Base → Conjugate base and acid (only for BL)
"amphiprotic" vs "amphoteric"
"amphiprotic" only for BR acid/base (狭い条件)
"amphoteric" any acid/base (広い条件)
both OK (not none, but both)
Lewis Acid
Acids to remember
https://gyazo.com/c5c5baa308e62ea25b398658b9d4bfdf
Bases to remember
https://gyazo.com/af664ee2565f451dcf5971d7defd5a2f
Classification
mono/di/triprotic acid: # of donatable proton
Note: CH3COOH is monoprotic
strong/weak
strong: all dissosiate / weak: not all dissosiate
organic acid = weak
how to distinguish
pH
conductivity (strong = more conductivity)
relative rate with metal (only for acid)
strong acid → weak conjugate base, weak acid → strong conjugate base
Reaction
Salt
def: ionic compound formed between a metal and non-metal
Acid + Metal → Salt + Water
Acid + Base → Salt + ごたごた
Acid + Metal Oxide (O) → Salt + Water
Acid + Metal Hydroixde (OH) → Salt + Water
Acid + Metal carbonate (CO) → Salt + Water + CO2
Acid + Metal Hydrogencarbonate (HCO) → Salt + Water + CO2
Neutralization (acid + base → salt + water)
Exothermic
always around -57kJ/mol
Application: antacids
Titration
"titrant" = alkali in burette (known concentration)
"analyte" = acid in beaker (unknown concentration)
indicator: phenolphthalein, etc
ionic product of water Kw = 1*10^-14
Kw increases (H2O dissosiates more in water) when temperature increase
larger Ka/Kb = smaller pKa/pKb = stronger acid/base
Ka + Kb = Kw = 14 at 297K
Buffer Solution
Def: When (1) SMALL amount of acid/base is added to
weak acid : salt
1 weak acid : 0.5 strong base
Acid Depositon Causes (i.e. acid rain)
nitric/ous acid: 2NO• from lighting and engines + O2 → NO2• / NO2• + water → nitric/ous acid
sulfuric/ous acid: S from fire power station / volcanos + O2 → SO2 / SO2 + H2O → sulfuric/ous acid
(他にも色々ゴタゴタ書いてるけど、一旦後回し）
Environmental Inpactsとか、反応のしょうさいとか
たくさん暗記が必要
Equivalence Point
Strong acid, weak base: <7
Strong base, weak acid: >7
その他
H2CO3とか出てきたら、多分H2O+CO2
Chapter 10 Organic Chem
Homologous def: CH2 dif, same Functional Group, same general formula
physical properties gradually change, chemical properties similar
Isomers: branch, functional, positional
functional ex: aldehyde/ketone, alcohol/ether
Trend: More branch = harder to approach = less IMF = lower b.p.
https://gyazo.com/b521f597d0b06ce16549887b6b6db9fb
Benzene
no addition, only substitution
with benzene = "aromatic" (not aliphiatic)
Alkane
non-reactive except
table: function groups
name combustion addition substitution polymerisation oxidation reduction
benzene ✔︎ electrophilic
alkane ✔︎ ✔︎ free radical
alkene ✔︎ electrophilic ✔︎
ester ✔︎ nucleophilic
alcohol ✔︎ ✔︎ nucleophilic ✔︎
aldehyde ✔︎ nucleophilic ✔︎ ✔︎
ketone ✔︎ nucleophilic ✔︎ ✔︎
carboxylic acid ✔︎ nucleophilic ✔︎
halgenoalkanes ✔︎ nucleophilic
見通すために表にしてみた
一応先生チェック済み、シラバス外は排除済み
とりあえず全体像は把握できたので、後は細部を理解したい
その結果、この表を暗記せずともロジックで導出できるようになりたい
Reactions
Combustion
complete: produce CO2 and Water
incomplete: produce CO / C and Water (lacks Oxygen)
Produces water anyway!
Substitution
free radical
initiation (incrase free radical)
homolytic fission
propagation (no change in # of free radical)
termination (decrease free radical)
condition: UV Light
nucleophilic
attacked by nucleophile (favors positive charge)
nucleophile attacks polar C-X bond (X: δ-)
halgenoalkane
SN2(ふたまた)
rate = [halgenoalkane][nucleophile]
lower order halgenoalkanes prefers SN2
hard to attack due to bulkyness of alkyl groups, in primary
secondary: Depends
neither too bulky or too open
tertiary: SN1
rate = [halgenoalkane]
higher order halgenoalkanes prefers SN1
carbocation more stable in tertiary
Trend of rate
C-X of Halogenoalkane
X has more radius -> less bond enthalpy -> more rate
(countering trend of electronegativity difference is neglectable!)
nucleophile (ONLY for SN2 reaction, because SN1 is independent)
anion better than polar molecule
Solvent
Polar protic, prefers SN1
protic solvent helps H-X bond to break by pulling both sides
protic solvent solvates intermediate carbocation, and makes them stable
Polar aprotic, prefers SN2
aprotic doesn't dissosiate nucleophile, so nucleophiles aren't surrounded by atoms and they are reactable
nucleophile's reactability is important in SN2, while not important in SN1
special: esterification
nucleophile: alcohol
condition: heat, conc. H2SO4
write as ⇄ reaction
also an condensation
special: hydrolysis
sn1/sn2
<あとで>
electrophilic
nitration of benzene
condition: heat under reflux, 60℃
OHとかが飛んで行かないようにreflux
<あとで>
Addition
ありうるreactionの種類とそのcondition、一旦飛ばす
必要そうであれば暗記
electrophilic
alkene (C=C bond) does
electrophile: cation OR positive side of dipole
仮に二つのatomがくっつくてもしても、初手がelectrophileのattackならelectrophilic addition
Major product: One that carbon with less H becomes carbocation
less H = more atom with positive inductive effect = more stable carbocation
Example
H-Br, Br-Cl (dipole)
Br-Br (induced dipole by High density election)
H-H (hydrogenation)
nucleophilic
Application: Test by bromine water
alkane: reacts with Br2 + H2O, decolorizes
alkane/benzene: no reaction, no decolorization
Polymerization
Oxidation
agent: acidified K2Cr2O7 or acidified KMnO4
acidified = H+ exists (and used for oxidization)
primary alcohol -> aldehyde -> carboxylic acid
under reflux: complete oxidization
under distiliation: partial oxidization
(aldehyde has lower b.p.)
secondary alcohol -> ketone
Reduction
aldehyde / ketone -> alcohol
reducing agent: LiAlH4 (stronger), NaBH4
carboxylic acid -> alcohol
reducing agent: LiAlH4 ONLY
NaBH4 is weaker
Esterification
catalyst
General Laws
Polar bond is weaker
Things that causes charges
Electron Density
C=C bond is high
Dipole
Ions
Chapter 11
NMR
1,2,3ではなくsinglet, doublet, triplet
Why TMS:
high bp (easy to remove)
one signal and strong
non-reactive