Reactions Flashcards
Alkane + Halogen ⟶
Alkane + halogen ⟶ Haloalkane + HX
Free radical substitution (Cl•, Br• etc)
Need UV Light
Initiation, Propagation, Termination
Alkene + H₂ ⟶
Alkene + H₂ ⟶ Alkane
Nickel Catalyst @ 150°C
Alkene + Halogen ⟶
Alkene + Halogen ⟶ Dihaloalkane
Electrophilic addition
If Bromine used: decolourisation!
Alkene + Hydrogen Halide ⟶
Alkene + Hydrogen Halide ⟶ Haloalkane
Electrophilic Addition
Unsymmetrical alkene? major and minor product
Alkene + H₂O (g) ⇌
Alkene + H₂O (g) ⇌ Alcohol
Steam hydration Phosphoric acide (H₃PO₄) Catalyst @300°C, 60-70atm
Alcohol + Halide ion ⟶
Alcohol + Halide ion ⟶ Haloalkane + OH⁻⁻⁻
Nucleophilic substitution
React with NaBr + an acid catalyst (H₂SO₄) + Heat
Alcohol ⟶
Alcohol ⟶ Alkene + water
Dehydration/elimination of H₂O
Acid catalyst: Conc. H₂SO₄ or Conc. H₃PO₄ + heat
Alcohol + Oxygen ⟶
Alcohol + Oxygen ⟶ Carbon Dioxide + water
Combustion: alcohol = oxidised
Primary Alcohol + [O] ⟶
Primary Alcohol + [O] ⟶ Aldehyde + Water
Oxidation
Gently heat in distillation apparatus with H⁺/Cr₂O₇⁻⁻⁻
Distil aldehyde off as formed to prevent COOH forming
Primary Alcohol + 2[O] ⟶
Primary Alcohol + 2[O] ⟶ Carboxylic Acid + water
Oxidation
Heat under reflux with excess H⁺/Cr₂O₇⁻⁻⁻
Excess ensures complete oxidation
Secondary Alcohol + [O] ⟶
Secondary Alcohol + [O] ⟶ Ketone + water
Oxidation
(distillation) or reflux with H⁺/Cr₂O₇⁻⁻⁻
Tertiary Alcohol + [O] ⟶
Tertiary Alcohol + [O] ⟶ CANNOT BE OXIDISED
Haloalkane + OH⁻⁻⁻ ⟶
Haloalkane + OH⁻⁻⁻ ⟶ Alcohol + X⁻⁻⁻
Nucleophilic substitution (:OH⁻⁻)
Warm aqueous alkali + heated under reflux
Water can also act as nucleophile but much slower
Benzene + NO₂ ⁺ ⟶
Benzene + NO₂ ⁺ ⟶ Nitrobenzene + H⁺
Electrophilic substitution
Conc. HNO₃ and Conc. H₂SO₄ catalyst
50°C for mono nitration
Benzene + Halogen ⟶
Benzene + Halogen ⟶ Halobenzene + HX
Electrophilic substitution (Cl ⁺ or Br ⁺ ) Halogen (e.g.Cl₂) + Halogen Carrier catalyst (e.g. AlCl₃/FeCl₃)
Benzene + Haloalkane ⟶
Benzene + Haloalkane ⟶ Alkylbenzene + HX
Electrophilic substitution ( CH₃⁺) = alkylation Halogen carrier catalyst + reflux +anhydrous conditions Friedel-Crafts reaction
Benzene + Acyl chloride ⟶
Benzene + Acyl chloride ⟶ Phenylketone + HCl
Electrophilic substitution (CH₃C⁺O) = acylation Halogen carrier catalyst + reflux + anhydrous conditions Friedel-Crafts reactions
Phenol + HNO₃ ⟶
Phenol + HNO₃ ⟶ Nitrophenol + water
Electrophilic substitution
dilute HNO₃, no catalyst (reacts much more readily than benzene)
forms 2 isomers: 2-nitrophenol and 4-nitrophenol
Phenol + Bromine ⟶
Phenol + Bromine ⟶ Bromophenol + HBr
Electrophilic substitution
no catalyst + decolourises orange bromine
product = 2,4,6-tribromophenol =antiseptic
Phenol + NaOH ⟶
Phenol + Na ⟶
Phenol + NaOH ⟶ Sodiumphenoxide + water
Phenol + Na ⟶ Sodiumphenoxide + H₂
Neutralisation reaction
Phenol = weak acid: not acidic enough to react with carbonates :(
Aldehyde + 2[H] ⟶
Aldehyde + 2[H] ⟶ Primary Alcohol
```
Nucleophilic addition (H⁻⁻⁻
Reducing agent = NaBH₄ (supplies hydride ions)
Add water)
~~~
Ketone + 2[H] ⟶
Ketone + 2[H] ⟶ Secondary alcohol
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Nucleophilic addition (H⁻⁻⁻
Reducing agent = NaBH₄ (supplies hydride ions)
Then add water)
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Carbonyl + Hydrogen Cyanide ⟶
Carbonyl + Hydrogen Cyanide ⟶ Hydroxynitrile
Hydroxynitrile = molecule with OH and CN group
Nucleophilic addition (:CN⁻⁻⁻)
HCN = weak acid, partially dissociates in water ⟶ CN⁻⁻⁻
CN⁻⁻⁻ attacks δ+ carbon on carbonyl group
Extends carbon chain
H⁺ (from H₂O or HCN) bonds to oxygen = hydroxyl group
Carboxylic acid + Metal ⟶
Carboxylic acid + Metal ⟶ Salt + H₂(g)
Redox reaction/neutralisation
N.B. salts of carboxylic acids end in –oate
Carboxylic acid + Metal Carbonate ⟶
Carboxylic acid + Metal Carbonate ⟶ Salt + H₂O + CO₂
Neutralisation
Carboxylic acid + Alkali ⟶
Carboxylic acid + Alkali ⟶ Salt + water
Alkali = metal hydroxide
Neutralisation
Carboxylic acid + Metal Oxide ⟶
Carboxylic acid + Metal Oxide ⟶ Salt + water
Neutralisation
Carboxylic acid + SOCl₂ ⟶
Carboxylic acid + SOCl₂ ⟶ Acyl Chloride + HCl + SO₂
SOCl₂ = thionyl chloride
OH group replaced by Cl group
Acyl Chloride + Alcohol ⟶
Acyl Chloride + Alcohol ⟶ Ester + HCl
Much easier + faster way to make an ester than with carboxylic acid + alcohol
Acyl Chloride + phenol ⟶
Acyl Chloride + phenol ⟶ Ester + HCl
Faster than using a carboxylic acid + phenol
Acyl Chloride + Water ⟶
Acyl Chloride + Water ⟶ Carboxylic acid + HCl
Vigorous reaction with cold water
Acyl Chloride + Ammonia ⟶
Acyl Chloride + Ammonia ⟶ Primary Amide + HCl
In the lab: HCl reacts with NH₃: produce NH₄Cl
Acyl Chloride + Amine ⟶
Acyl Chloride + Amine ⟶ Secondary Amide + HCl
Use a primary amine
Alcohol + Carboxylic acid ⟶
Alcohol + Carboxylic acid ⟶ Ester + Water
Heat with acid catalysts (H₂SO₄)
Reversible reaction: separate product as it forms using fractional distillation
N.B Oxygen in ester bonds comes from alcohol
Alcohol + Acid Anhydride ⟶
Alcohol + Acid Anhydride ⟶ Ester + carboxylic Acid
Acid anhydride = 2 carboxylic acid molecules
slow: speed up by warming
Ester + water ⇌
Ester + water ⇌ Carboxylic acid + alcohol
Acid hydrolysis
Reflux ester with hot quests acid e.g. HCl, H₂SO₄ (dilute)
Ester + Alkali ⟶
Ester + Alkali ⟶ Carboxylate salt + alcohol
Base hydrolysis
reflux ester with a hot aqueous alkali e.g. NaOH (dilute)
Amine + Acid ⟶
Amine + Acid ⟶ Ammonium salt
Neutralisation: amines = bases
Ammonia + Haloalkane ⟶
Ammonia + Haloalkane ⟶ Primary Aliphatic Amine + NH₄X
Nucleophilic substitution
excess ethanol ammonia used
forms a primary aliphatic (no benzene) amine
Primary Amine + Haloalkane ⟶
Primary Amine + Haloalkane ⟶ Secondary Aliphatic Amine + NH₄X
Nucleophilic substitution
Substitution continues: get a mixture of primary, secondary + tertiary amines + quaternary ammonium salts (separate by fractional distillation)
Nitrobenzene + 6[H] ⟶
Nitrobenzene + 6[H] ⟶ Phenylamine + 2H₂O
Heating under reflux with tin catalysts + conc. HCl
if 2 substitutions: 12[H] and 4H₂O !!
Must add NaOH (phenyl amine +HCl ⟶ salt :( )
Reduction
Amino Acid + Acid ⟶
Amino Acid + Acid ⟶ Salt
If pH is lower than isoelectric point, amino acid behaves as a base: amino group reacts
NH₂ ⟶ NH₃⁺ = cation
Amino Acid + Base ⟶
Amino Acid + Base ⟶ Salt + Water
If pH is higher than isoelectric point, amino acid behaves as an acid: COOH group reacts
COOH ⟶ COO⁻⁻⁻ = anion
Amino acid + Alcohol ⟶
Amino acid + Alcohol ⟶ Ester + water
Strong acid catalyst (H₂SO₄)
Amino Acid + Amino Acid ⟶
Amino Acid + Amino Acid ⟶ Amide (dipeptide)
Condensation reaction: elimination of H₂O
Forms a dipeptide = secondary amide
Dicarboxylic acid + Diamine ⟶
Dicarboxylic acid + Diamine ⟶ Polyamide + water
Condensation polymer (loses H₂O)
Dicarboxylic acid + Diol ⟶
Dicarboxylic acid + Diol ⟶ Polyester + water
Condensation polymer (loses H₂O)
H⁺
Polyamide + 2H₂O ⟶
H⁺
Polyamide + 2H₂O ⟶ Dicarboxylix acid + diamine
Polyamide hydrolyses more easily with an acid than a base = acid hydrolysis
Polyester + 2NaOH ⟶
Polyester + 2NaOH ⟶ Dicarboxylix acid salt + Diol
Polyesters hydrolysis more easily with a base than an acid = base hydrolysis
Haloalkane + CN⁻⁻⁻ ⟶
Haloalkane + CN⁻⁻⁻ ⟶ Nitrile + X⁻⁻⁻
Nucleophilic substitution
Reflux haloalkane with potassium cyanide in ETHANOL SOLVENT
Nitrile + 4[H] ⟶
Nitrile + 4[H] ⟶ Primary amine
Reduction (method 1)
Use Lithium Aluminium Hydride: LiAlH₄, which is a strong reducing agent, and dilute acid
Nitrile + 2H₂ (g) ⟶
Nitrile + 2H₂ (g) ⟶ Primary amine
Reduction (method 2 - used in industry)
Hydrogen gas, metal catalyst (e.g. Platinum or Nickel)
High temp + pressure
N.B Nitriles can also be reduced with sodium metal and ethanol !!
Nitrile + 2H₂O + HCl ⟶
Nitrile + 2H₂O + HCl ⟶ Carboxylic acid + NH₄Cl
Acid hydrolysis
reflux nitrile in dilute HCl (with heat)
Haber Process
N₂ (g) + 3H₂ (g) ⇌ 2NH₃ (g)
Forward reaction = exothermic
High pressure favours forward reaction
BUT
low temp decreases yield so compromise @ 450°C
High pressure = dangerous & expensive compromise of 200 atm.
Finely divided porous iron catalyst