5 - What's in a Medicine? (WM) Flashcards
(94 cards)
1
Q
Typical reactions of the OH group
A
-Can behave as acids
-Can react to form esters
-Can be oxidised by reaction with oxidising agents
2
Q
Acidity of the OH group
A
Least: Alcohols
Phenols
Most: Carboxylic acids
3
Q
Test for phenols
A
Use neutral iron (III) chloride
4
Q
What is the colour change for a phenol test if a phenol is present?
A
Solution will turn purple
5
Q
Reaction of OH group with weak base (Na2CO3)
A
-Will react with carboxylic acid only
-Produces salt, CO2 and water
6
Q
Reaction of OH group with strong base (NaOH)
A
-Will react with carboxylic acid and phenol
-Produces salt and water
7
Q
How is the OH group acidic?
A
OH group will be more acidic if the anion formed following dissociation is more stable
8
Q
What is the oxidising agent to oxidise alcohols?
A
Sodium dichromate
9
Q
What are the products for the oxidation of primary (1°) alcohols?
A
1: Aldehyde + Water
2: Carboxylic acid
10
Q
What are the products for the oxidation of secondary (2°) alcohols?
A
Ketone + Water (only one reaction)
11
Q
Can tertiary alcohols (3º) be oxidised?
A
No
12
Q
Describe primary (1º) alcohol
A
-Carbon bonded to 2 hydrogens
-1 R group
13
Q
Describe secondary (2º) alcohol
A
- Only 1 hydrogen bonded
-2 R groups
14
Q
Describe tertiary (3º) alcohol
A
-No hydrogens bonded
-3 R groups
15
Q
pH of ethanol
A
7
16
Q
pH of phenol
A
5
17
Q
pH of salicylic acid
A
2
18
Q
pH of ethanoic acid
A
2
19
Q
Reaction of iron (III) chloride and ethanol
A
No change
20
Q
Reaction of iron (III) chloride and phenol
A
Turns purple
21
Q
Reaction of iron (III) chloride and salicylic acid
A
Turns purple
22
Q
Reaction of iron (III) chloride and ethanoic acid
A
No change
23
Q
Warming acidified dichromate with ethanol
A
Turned green
24
Q
Warming acidified dichromate with phenol
A
No change
25
Warming acidified dichromate with salicylic acid
No change
26
Warming acidified dichromate with ethanoic acid
No change
27
Reacting sodium carbonate with ethanol
No change
28
Reacting sodium carbonate with phenol
No change
29
Reacting sodium carbonate with salicylic acid
Bubbling - CO2 produced
30
Reacting sodium carbonate with ethanoic acid
Bubbling - CO2 produced
31
Define functional group
Part of the molecule responsible for the way the molecule reacts.
Also allow for differenciation of homologous series
32
General formula of alcohols
ROH
33
General formula of aldehydes
RCHO (double bond with O)
34
General formula of ketones
RCOR' (double bond with O)
35
General formula of carboxylic acids
RCOOH (double bond with 1 O)
36
General formula of acid anhydrides
(RCO)2O (double bond with 2 Os)
37
General formula of ethers
ROR'
38
General formula of esters
RCOOR' (double bond with 1 O)
39
General formula of phenols
Benzene ring and OH
40
Prefix/suffix of alcohols
-ol
41
Prefix/suffix of aldehydes
-al
42
Prefix/suffix of ketones
-one
43
Prefix/suffix of carboxylic acids
-oic acid
44
Prefix/suffix of acid anhydrides
-oic anhydride
45
Prefix/suffix of ethers
-oxy-
46
Prefix/suffix of esters
alkyl-____-anoate
47
Reaction forming ester with carboxylic acid and alcohol
Carboxylic acid + alcohol -->
ester + water
48
What condition must be met to form an ester with a carboxylic acid and alcohol?
Sulfuric acid catalyst
49
Reaction forming ester with acid anhydride and alcohol
Acid anhydride + alcohol -->
ester + carboxylic acid
50
What type of reaction is forming an ester with an alcohol (and other reactant)?
Condensation
51
Reaction to form aldehyde with 1º alcohol
Alcohol + Potassium dichromate (K2Cr2O7) ---> Aldehyde
52
Conditions for forming an aldehyde from an alcohol
-H2SO4 catalyst
-Under distillation
53
What type of reaction is forming an aldehyde with an alcohol (and other reactant)?
Oxidation
54
Conditions for forming carboxylic acid from 1º alcohol/aldehyde
-Potassium dichromate other reactant
-H2SO4 catalyst
-Under reflux
55
What type of reaction is forming a carboxylic acid with an alcohol/aldehyde?
Oxidation
56
Conditions for forming a ketone with 2º alcohol
-Potassium dichromate other reactant
-H2SO4 catalyst
-Under reflux
57
What type of reaction is forming a ketone with an alcohol (and other reactant)?
Oxidation
58
How to name esters
-1st component comes from alcohol
-2nd component comes from carboxylic acid
59
What ester is formed when reacting methanol and ethanoic acid?
Methylethanoate
60
How does infrared spectroscopy work?
-Radiation absorbed by bonds in molecules, only if it causes a change to their dipole moment
-Results in different stretching and vibration
-Amount of energy absorbed depends on mass of atoms and type of movement
61
How does mass spectrometry work?
-Molecules ionised to produce molecular ion (M+)
-M+ accelerated and detected
-Molecule can fragment and form a wide variety of fragments
62
How to read infrared spectra
-Give bond and wavenumber
(data sheet)
-More information given for further differenciation
63
How to read mass spectra
The peak with the greatest m/z value corresponds to m/z equal to the molecular mass
64
What is the M+1 peak in a mass sprectrum?
The small peak with an m/z of one more than the molecular peak
65
What is the M+1 peak caused by?
Some molecules containing C-13 isotopes
66
What is chromatography?
-Separates different compounds from mixtures
-Checks purity
-Reaction progress can be measured
-Rf values can be compared
-Compound's affinity for each phase influences the distance travelled
67
What does the Rf value represent?
Measure of how far compounds have travelled
68
Define stationary phase (chromatography)
What the compounds 'stick' to
69
Define mobile phase (chromatography)
What the compounds move through
70
What does affinity mean in the context of chromatography?
Like dissolves like
71
How can the aldehyde product be separated in oxidation of alcohols?
Distillation
72
How can the carboxylic acid product be separated in the oxidation of alcohols?
Reflux
73
What is used to test for oxidation of alcohols?
Sodium dichromate
74
Positive test for oxidation with an alcohol and dichromate ions?
Colour change orange to green
75
Why is sulfuric acid used as a catalyst in many reactions?
Drying agent (removes water)
76
Define substitution reaction
Swapping functional group
77
Equation for elimination reaction of alcohols
Alcohol --> Alkene + H2O + H+
78
Conditions for elimination reactions of alcohols
- Al2O3 catalyst
-Refluxed with concentrated H2SO4
79
1st step of elimination for alcohols
Curly arrow from O to H+
(outer electrons shown on O)
80
2nd step of elimination for alcohols
Curly arrow from bond C-O to O+ ion
2 Hs attached to O+
81
3rd step of elimination for alcohols
Curly arrow from C-H bond to C-C+ bond
+H2O
82
4th step of elimination for alcohols
Alkene
+H2O
+H+ ion
83
Define nucleophile
Electron pair donor - can be ion or molecule
84
Define nucleophilic substitution
Type of substitution reaction in which a nucleophile is attracted to an electron deficient atom (Cδ+) where it donates a pair of electrons to form a new covalent bond
85
Reactants for nucleophilic substitution of alcohols
Alcohol & halogen
86
Equation for nuceleophilic substitution of alcohols
Alcohol + Halogen --> Haloalkane + H2O
87
1st step of nucleophilic substitution for alcohols
-Dipoles between C-O bond
-Curly arrow from Cl- to C (C-O)
-Curly arrow from C-O bond to H (OH)
88
2nd step of nucleophilic substitution for alcohols
Haloalkane
+H2O
89
What is the principle of waste prevention?
Better to prevent the production of waste than to deal with it after it has been created
90
Why is high atom economy better for the environment?
-Less waste produced
-Minimises damage from waste chemicals to the environment
-Less raw materials can be used
-More sustainable
91
What is the principle of less toxic syntheses?
Syntheses should be designed to have the least amount of toxic substances produced or used
92
What is the principle of safer solvents?
Syntheses should be designed to minimise the use of solvents and separating agents that are dangerous
93
How can energy use be made more efficient?
-Syntheses should be conducted at room temperature and pressure
-Use of electricity should be minimised
-Source of electricity should be assessed
94
Why are catalysts environmentally friendly?
Catalysts reduce the need for heating a reaction which reduced the amount of energy used for the reaction
