IB Chemistry HL暗記物リスト

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• IBChemistry 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
  • 
  • 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
    • 
  • 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
    • 
    • Remember ligands, coordination No, etc
      • 

Chapter 4: Chemical bonding and structure

• 

  • 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
  • 
  • 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
• 

• 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

    • 

  • Bases to remember

    • 

  • 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.
• 
• Benzene
  • no addition, only substitution
  • with benzene = “aromatic” (not aliphiatic)
• Alkane
  • non-reactive except 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