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Chemistry IAL EDEXCEL A-Level > Unit 4 > Flashcards

Unit 4 Flashcards

(62 cards)

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1
Q

Acyl chlorides + water form?

A

Carboxylic acid + HCl gas (misty fumes)

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2
Q

Acyl chlorides + alcohol ->

A

Ester + HCl gas

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3
Q

Acyl chlorides + concentrated ammonia

A

Amide (-CONH2) + HCl

Further reaction to NH4Cl

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4
Q

Acyl chlorides + primary amine

A

N-substituted (RCONHR’) + HCl

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5
Q

Acyl chlorides + secondary amines ->

A

N,N-disubstituted amide (RCONH(R’)(R”) + HCl

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6
Q

Carboxylic acid + alcohol ->

A

In presence of acid catalyst (H2SO4) ester + H2O

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7
Q

Physical properties of esters

A

Low boiling point
Insoluble in water
Pleasant smells

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8
Q

Carboxylate salt (-COO-) COO with negative charge and a positive ion + H2SO4 ->

A

Carboxylic acid + metal salt

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9
Q

Types of reverse esterification

A

Acidic hydrolysis
Alkaline hydrolysis

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10
Q

How to do acidic hydrolysis in esters

A

Ester + warm water -> (acid catalyst H2SO4) carboxylic acid + alcohol
It is an equilibrium for and backward arrow needed

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11
Q

Alkaline hydrolysis in esters

A

Ester + NaOH -> carboxylate salt + alcohol
Complete reaction

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12
Q

What happens in condensation polymerisation

A

Diol (two OH groups at each end + dicarboxylic acid -> polyester + H2O

OH from COOH and H from OH (Acyl chlorides can be used to form HCL)

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13
Q

Stationary phase in chromatography

A

Liquid/ solid that does not move

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14
Q

Mobile phase in chromatography

A

Liquid moves through stationary phase transporting the substance tested

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15
Q

How do mobile and stationary allow chromatography to separate solvents

A

Chemicals more attracted to stationary phase and only slightly attracted to mobile phase will move less up the paper

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16
Q

Mobile phase in Paper chromatography

A

Solvent

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17
Q

Mobile phase in TLC chromatography

A

Solvent

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18
Q

Stationary phase in paper chromatography

A

Water trapped in the fibres of chromatography paper

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19
Q

Stationary phase in TLC chromatography

A

Sheet of glass coated with silica or alumina

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20
Q

Stationary phase of column chromatography

A

Alumina or silica soaked in solvent

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21
Q

Mobile face in solemn chromatography

A

The solvent added when pouring the mixture of top of the stationary phase

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22
Q

How is HPLC chromatography different to column chromatography

A

Solvent is forced through HPLC tube by high pressure

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23
Q

Stationary phase in HPLC chromatography

A

silica

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24
Q

What does a polar substance attract

A

Polar molecules

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25
Mobile phase in HPLC chromatography
Hexane (non-polar)
26
How are the different components measured in HPLC chromatography
By the absorption of UV light measured
27
What state are the substances being measured in HPLC chromatography
Liquids
28
What does Gas and HPLC measure
The retention time- time taken to detect the separation of components
29
What is the mobile phase in gas chromatography
Inert gas
30
What is the stationary phase in gas chromatography
The solid/liquid coated in the inside of tube
31
How those the stationary phase affect the retention time
The weaker the attraction to stationary phase the shorter the retention time
32
What does C13 NMR measure
Number of different chemical environments (Peaks show different groups the carbon are connected to)
33
Physical properties of Carboxylic acids
High boiling point which increase with Mr Soluble but this decreases as chain length increases
34
Oxidation reaction to make -COOH
Primary alcohol or aldehyde + acidified potassium dichromate with acid catalyst under reflux -> -COOH
35
What does the hydrolysis of Nitriles produce
-COOH + another compound
36
Types of hydrolysis of nitriles
Acidic hydrolysis Alkaline hydrolysis
37
Describe acidic hydrolysis of nitriles
1 step Nitrile + dilute acid (H+) + H2O under reflux -> -COOH + NH4+
38
Describe alkaline hydrolysis of nitriles
2 steps Nitrile + NaOH + H2O under reflux -> -COO-Na+ + NH3 Further -COO-Na + H+ -> -COOH
39
Reducing COOH
COOH + LiAlH4 in dry ether -> primary alcohol
40
Halogenation of -COOH
-COOH + PCL5 in anhydrous conditions -> -RCOCl +POCl3 + HCl which results in misty fumes
41
Esterification of -COOH
-COOH + -OH (acid catalyst) -> ester + water
42
Neutralisation of -COOH
-COOH + OH- (strong alkali) -> carboxylate salt + water
43
Reduction of aldehydes
Aldehydes + LiAlH4 in dry ether -> primary alcohol
44
Oxidation of aldehydes
Aldehyde + acidified potassium dichromate + conc. acid under reflux -> -COOH This will produce a colour change from orange to green
45
Reduction of ketones
Ketone + LiAlH4 in dry ether -> secondary alcohol
46
Oxidation of ketones
Ketones are not easily oxidised
47
Test to distinguish from ketones and aldehydes
Fehlings solution: Deep blue to red ppt Tollens reagent: Colourless solution to silver mirror
48
What does the triodomethane (iodoform) test for
CH3CO group Present in ethanal and methyl ketones
49
Iodoform test equation
Methyl ketone + iodoform in alkaline sol. -> CHI3 (pale yellow ppt)
50
Conditions and product of nucleophilic addition of Carbonyls + HCN
Happens in alkaline solution containing KCN Makes hydroxynitriles
51
What is 2,4-DNPH used for
It is a test which through nucleophilic addition forms an orange ppt with carbonyl compounds It’s derivatives ( chemicals produced) can be filtered, purified, dried and melting point determined
52
What is Sn1
Nucleophilic substitution Seen in tertiary halogenoalkanes Has 2 steps Has one species in RDS
53
What is Sn2
Nucleophilic substitution Seen in primary halogenoalkanes With 1 step (has transition stage) Has 2 species in its RDS
54
What is the end-point of a titration
The colour change from the indicator which is past the equivalence point at an imbalance of acid or base
55
What is the equivalence point in a titration
The exact proportions of acid and base in the titration
56
Ph of equivalence point titration of strong acid + strong base
Ph=7
57
Ph of equivalence point titration of strong acid + weak base
Ph= <7
58
Ph of equivalence point titration of weak acid + strong base
> 7
59
where can’t the equivalence point be determined
In the titration of weak acid with weak base because there is an absence of sharp decrease in the graph, only a point of inflection
60
How do indicators work
Through dissociation HI -><- I + H+ therefore when [H]=[In] [H] = KIn
61
What are buffer solutions made out of
Weak acid/ base and their conjugate base/ acid
62
Assumptions made when calculating pH of buffer solutions
Remember to add up volume! -dissociation is negligible -conc of acid and salt is half when volume is doubled

Chemistry IAL EDEXCEL A-Level (7 decks)

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