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organic synthesis Flashcards

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1
Q

alkene to poly alkene

A

high pressure and catalyst

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2
Q

alkene to dihalogenoalkane

A

Br2, Cl2 at room tempreature

electrophilic addition

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3
Q

alkene to halogenoalkane

A

HCl, HBr at room temperature

electrophilic addition

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4
Q

dihalogenoalkane to diol

A

KOH aqueous
heat under reflux
aqueous Nucleophillic substitution

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5
Q

dihalogenoalkane to alcohol

A

KOH aqueous
heat under reflux
Nucleophillic substitution

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6
Q

alkene to alcohol

A

Acid catalysed addition mechanism for hydration of alkene

  • conc H2SO4 electrophilic addition of an hydrogen
    -H2O warm hydrolysis
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7
Q

alcohol to alkene

A

Acid catalysed elimination mechanism alcohols to alkenes dehydration reaction

add conc H2SO4 or H3PO4

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8
Q

alkane to halogenoalkane

A

Br2,Cl2

under UV light

free radical substitution

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9
Q

halogenoalkane to alkene

A

Elimination

KOH alcoholic
heat under reflux

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10
Q

primary alcohol to aldehyde

A

partial oxidisation
Na2Cr2O7(sodium dichromate or potassium dichromate ) /H+
heat and distill

(the colour change should be from green to orange the alcohol is oxidised and the dichromate ions Cr2O7 2− to the green of chromium(III) ions (Cr3+) )

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11
Q

aldehyde to carboxylic acid

A

Na2Cr2O7 (sodium dichromate or potassium dichromate) /H+

heat under reflux + excess oxidising agent

full Oxidation

(the colour change should be from green to orange the alcohol is oxidised and the dichromate ions Cr2O7 2− to the green of chromium(III) ions (Cr3+) )

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12
Q

secondary alcohol to ketone

A

partial oxidisation
Na2Cr2O7(sodium dichromate or potassium dichromate ) /H+
heat and distill

(the colour change should be from green to orange the alcohol is oxidised and the dichromate ions Cr2O7 2− to the green of chromium(III) ions (Cr3+) )

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13
Q

ketone/aldehyde back to an alcohol

A

NaBH4 (:H-)
H+ from water or weak acid
Reduction
Nucleophillic Addition

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14
Q

alcohol to ester

A

esterification
carboxylic acid
H2SO4
heat

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15
Q

ketone/aldehyde to hydroxynitrile

A

NaCN + H2SO4
Nucleophillic Addition

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16
Q

halogenoalkane to nitrile

A

KCN alcoholic
heat under reflux and aqueous

17
Q

halogenoalkane to primary amine

A

Alcoholic NH3 excess
heat under pressure

18
Q

primary amine to secondary, tertiary, quaternary amine

A

halogenoalkane
NuSub
excess ammonia (not for quaternary tho)

19
Q

nitrile to primary amine

A

LiAlH4 acts as a reducing agent with

Ni and H2 catalyst
high temperatures

20
Q

primary amine to secondary amide

A

Acyl chloride room temp Nucleophilli addition/elimination

21
Q

Acyl chloride/ acid anhydride to alcohol

A

H2O at room temp

22
Q

Acyl chloride/ acid anhydride to ester

A

Alcohol room temp

23
Q

Acyl chloride/ acid anhydride to primary amide

A

NH3 at room temperature

24
Q

Acyl chloride/ acid anhydride to secondary amide

A

primary amine at room temp

25
Q

benzene to nitro benzene

A

-conc sulphuric acid and nitric acid
-electrophillic substitution

26
Q

nitrobenzene to phenyl amine

A

Sn and HCl
reduction

27
Q

primary amine benzene to secondary phenyl amine

A

CH3Cl (halogenoalkane)
Nu sub

28
Q

phenyl amine to phenyl amide

A

add acyl chloride nucleophilic addition elimantion

29
Q

what is organic synthesis

A

using reaction mechanisms to produce target product from starting molecule

30
Q

why do chemists try to design section mechanisms that do not require a solvent

A

solvents are difficult to remove from reaction mixture and can cause loss of percentage yield and costly

31
Q

why do chemists designprocesses with as few steps as possible

A

less energy used and better yield

less wastage

32
Q

Suggest why chemists usually aim to design production methods with a high percentage atom economy

A

Less waste OR Less pollution
OR maximises the use of raw materials in the process into useful products, saves resources

33
Q

percentage atom economy

A

mr of desired products/ over total products x 100

34
Q

what does tin and HCL reduce

A

NO2 to NH2

35
Q

How does nickel catalyst work

A

Nickel catalysts, on the other hand, are often used in hydrogenation reactions where hydrogen gas (H2) is added to unsaturated bonds (e.g., C=C double bonds) to form saturated bonds (e.g., single C-C bonds).

Chemistry (10 decks)

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