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Whats In Medicine Flashcards

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1
Q

What is the prefix of aldehydes

A

-al

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2
Q

What is the prefix for ketones

A

-one

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3
Q

What is the prefix for carboxylic acid

A

-oic acid

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4
Q

What is the prefix for acid anhydride

A

-oic anhydride

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5
Q

What is the prefix for Ester’s

A

-oate

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6
Q

What is the prefix for ethers

A

-oxy-

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7
Q

What is used in the process of oxidising ethanol to ethanal

A

Using powerful oxidising agent - acidified potassium dichromate (V)
Distillation

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8
Q

How is an aldehyde oxidised into a carboxylic acid

A

Acidified potassium dichromate (V)

Reflux

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9
Q

What happens to the colour of acidified potassium dichromate when oxidised

A

Turns from orange to purple (carboxylic acid)

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10
Q

What is a primary alcohol

A 
A carbon which an -OH group and two C-H bonds with one carbon chain -R
      H
       |
R - C - OH 
       |
      H
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11
Q

What is a secondary alcohol

A 
One C-H bond on the carbon with one -OH and two carbon chains -R 
      H
       |
R - C - OH 
       |
      R
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12
Q

What is a tertiary alcohol

A 
Has no hydrogens attached to the carbon atom with the -OH group
      R
       |
R - C - OH 
       |
      R
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13
Q

How does -OH react with water

A

R-OH + H2O <=>R-O^- + H3O^+

Makes acidic H3O^+

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14
Q

How does water react with itself to form an acidic solution

A

H-OH + H2O <=> H-O^- + H3O^+

Forms acidic solution

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15
Q

What property does H^+(aq) ions and H3O^+ give

A

Make any solution acidic

Ions formed depends on stability of negatively charged ion

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16
Q

What is the most acidic structure and why

A

RCOO^-
Is most stable as electrons are delocalised
pH3/4

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17
Q

How acidic is phenol

A

Middle pH 6

Electrons are delocalised so quite stable

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18
Q

What is the least acidic structure

A

R-O^-
No delocalisation, ions unstable
pH7

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19
Q

What can react with strong bases(and an example) to form salts and water

A

Phenols and carboxylic acids are strong enough to react with strong bases e.g. Sodium hydroxide to form salts and water

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20
Q

What is the test for carboxylic acids

A

Only one capable of reacting with carbonate to give salt, water and carbon dioxide

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21
Q

Why doe phenols not react with carbonate

A

Not as high enough H^+(aq) concentration in phenol solution

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22
Q

What is the test for phenol

A

Reaction with neutral iron (III) chloride solution (FeCl3) which is orange, shake them and turns purple

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23
Q

What happens to the phenol when reacting with neutral iron (III) chloride solution

A

C=C-OH group (enol) forms complex ion with Fe^3+ ions in iron (III) chloride

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24
Q

An example of esterification

A

Ethanoic acid react with ethanol if add few drops concentrated sulfuric acid as catalyst to make ethyl ethanoate (ester)

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25
Q

What is the word equation for esterification

A

c.H2SO4

Alcohol + carboxylic acid ———-> ester + water

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26
Q

What smell do Ester’s have

A

Strong sweet

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27
Q

What esters are used as energy storage compounds and where are they used

A

Fats and oils

In plants and animals

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28
Q

What is an acid anhydride

A

Derived from carboxylic acids

More reactive than -COOH

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29
Q

Why are acid anhydrides used instead of carboxylic acids in esterification reactions

A

React completely with alcohol on warming, give much higher yield of ester

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30
Q

How can Ester’s be formed using a carboxylic acid

What type of reaction is it (other than esterification)

A

R acting with alcohol as C.H2SO4 as a catalyst

Reversible reaction

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31
Q

In an esterification reaction that is reversible what is the forward reaction called

A

Esterification or condensation

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32
Q

In an esterification reaction that is reversible what is the backward reaction called

A

Ester hydrolysis (reaction with water)

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33
Q

What an replace alcohol in an esterification reaction

A

Phenol

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34
Q

What can replace carboxylic acid in an esterification and why are they better to use

A

Acyl chloride or acid anhydride

They’re more reactive and reaction occurs faster

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35
Q

Why can two different ester be made from salicylate acid (2-hydroxybenzoic acid)

A

Depending if the -COOH or -OH group is esterified

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36
Q

What happens if the -COOH group in salicylic acid is esterified reacting with ethanoyl chloride

A

Forms aspirin

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37
Q

What happens if the -OH group in salicylic acid is esterified reacting with methanol

A

Forms oil of wintergreen

Deep heat

38
Q

What is the difference between aspirin and oil of wintergreen

A

Aspirin water soluble, absorbed in digestive system

Oil of wintergreen is fat soluble, absorbed through skin

39
Q

How can an alcohol be oxidised into a carboxylic acid

A

Alcohol distilled with acidified potassium dichromate (V) forming aldehyde
Then reflux with acidified potassium dichromate (V) to form carboxylic acid

40
Q

What alcohol can form carboxylic acids

A

Primary

41
Q

What alcohol can form ketones

A

Secondary

42
Q

How is a ketone made from a secondary alcohol

A

Reflux with acidified potassium dichromate (V)

43
Q

Why are tertiary alcohols resistant to oxidation

A

No hydrogen atom attached to carbon atom that has -OH group attached

44
Q

What conditions are used in labs for dehydration of alcohol

A

Concentrated sulfuric acid with 180 degrees

45
Q

What conditions are used in dehydration of alcohols in industry

A

Aluminium oxide with 300 degrees

46
Q

What type of reaction is dehydration of alcohol

A

Elimination reaction

47
Q

What is the word equation of dehydration of alcohol

A

c.H2SO4/180degrees
Alcohol ———————-> alkene
Al2O3/300degrees

48
Q

What does distillation form

A

Aldehyde

49
Q

What does reflux form

A

Carboxylic acid

50
Q

How can haloalkanes be prepared

A

Reacting alcohol with a hydrogen halide in a nucleophilic reaction

51
Q

When is an organic product in crude form

A

When organic solid product is synthesised as contains impurities

52
Q

What is the process of separation

A

Removes any water soluble impurities
Reaction finished pour mis in separating funnel, add water
Shake and let layers settle. Organic layer less dense
Water soluble impurities dissolved in aqueous layer, open stopped to run off this

53
Q

What is used to remove trace of water in product

A

Anhydrous salt e.g. Magnesium sulfate

54
Q

How does filtration remove solid organic products

A

Pour mix into Buchner filter with filter paper, into sealed side arm flask attached to a vacuum line
Reduced pressure in flash causes vacuum kim removing air force liquid through funnel, leaning solid on filter paper

55
Q

How does recrystallisation purify organic solvents

A

Desired compound dissolved j. Chosen hot solvent, leaving insoluble impurities to filter off
Cool product will crystallise out, leaving soluble impurities pure crystals to be filtered, washed and dried

56
Q

What is thin layer chromatography used for

A

Separates small quantities of organic compounds, purify to check purity, follow progress of reaction over time
Suitable solvent used
Different organic compounds have different affinities for particular solvent, so carried through chromatography medium (plate) at different rates
Use silica plate is thin layer

57
Q

Why is measuring melting point determination important

A

Indenture compound and its purity
Value obtained compared to published value
Pure compound should melt within 0.5 degrees of true melting point

58
Q

What is green chemistry

A

Developing chemical products especially sustainable, environmentally friendly processes

59
Q

What examples are there of green chemistry

A 
Better atom economy 
Prevention of waste product 
Less hazardous chemicals 
Design safer chemical products 
Safer solvents
Lower energy use
Renewable feedstocks 
Less reagents used / number steps
Catalyst 
Degradation 
Employ real time process monitoring 
Safer chemical processes
60
Q

How does a better atom economy effect green chemistry

A

More feedstock incorporated in product so less waste product

61
Q

How does the prevention of waste product effect green chemistry

A

Better than treating and disposing waste

62
Q

How does using less hazardous chemicals effect green chemistry

A

Less harmful

63
Q

How does safer chemical products effect green chemistry

A

Less toxic products

64
Q

How do safer solvents effect green chemistry

A

Minimise organic solvent use

65
Q

How does a lower energy use effect green chemistry

A

Use lower temperature and pressure processes better

66
Q

How do renewable feedstocks effect green chemistry

A

Instead of depleting natural resources

67
Q

How does having less steps / reagents effect green chemistry

A

Doesn’t generate waste

68
Q

How does a catalyst effect green chemistry

A

Reduce energy usage

69
Q

How does degradation effect green chemistry

A

When release the chemical products for degradation should breakdown into innocuous products

70
Q

How would employing real time process monitoring effect green chemistry

A

Better monitor of chemical processes reduces waste products

71
Q

How does a safer chemical process effect green chemistry

A

Minimise potential of releasing gases, fires and explosions

72
Q

What examples are there of green chemistry in use

A

Ibuprofen used to synthesis in 12 steps with 40% atom economy now 4 steps with 77%
Atorvastatin now synthesised using enzyme that catalyses chemical reactions in water, less potential of polluting organic solvents

73
Q

What aspects are here to take into account when using green chemistry

A

Does the change of reagents make the reaction more expensive
Has the replacement of one reagent with another raised new health and safety issued

74
Q

What happens in an elimination reaction

A

Hydroxyl group will bond to H^+ ion from strong acid
Alcohol is protonates, oxygen atom gains positive charge
Positive oxygen attracts electrons, water ‘falls off’ creating unstable carbonation intermediate
Carbonation loses H^+ to form an alkene

75
Q

Why must molecules be ions to be used in mass spectra

A

So detected

76
Q

Why may an ion undergo fragmentation

A

Ion splits up due to further electron bombardment in ionisation chamber, into fragments
Create many smaller positively charged fragments

77
Q

Which is the most st ale peak

A

Tallest - base peak

78
Q

What is the molecular ion peak

A

The last peak

79
Q

Where would the isomer be on the graph

A

The left of the molecular ion peak would be very small

80
Q

How can covalent bonds vibrate, twist or bend

What happens to the molecule

A

If right energy absorbed from infrared spectroscopy passed through molecule
Molecule moves higher vibrational energy level

81
Q

How can you find which bonds are in a molecule

A

Quantised specific frequency of infrared radiation absorbed, characteristic of particular bond

82
Q

What does the vibration frequency depend on

A

Nature of the atoms in a bond and the bond itself

Greater mass of atoms in a bond the slower the vibration will be

83
Q

How can other atoms in the molecule influence vibration of bond

A

Multiple binds vibrate at higher frequency than single bond. Other atoms in the molecule can influence vibration

84
Q

How is the wavelength calculated

A

Wavelength = 1/wavelength (cm)

85
Q

What is the frequency of vibrations measured in

A

Hz

86
Q

What is the usual values infrared spectroscopy give

A

Reciprocal wavelength cm / cm^-1 = wavenumber

87
Q

What is the spectrum produced made of

A

Transmission, is percentage of infrared radiation that passes through same,e, against frequency of infrared radiation

88
Q

How is speed of light calculated

A

C = wavelength x frequency

89
Q

What is the fingerprint region

A

Below 1500cm^-1 spectrum can be complex, more difficult to assign absorptions to particular bonds

90
Q

What compounds show up in fingerprint region

A

Aromatic compounds often exhibit complex absorption patterns in fingerprint region

91
Q

What is the prefix of alcohol

A

-ol

Chemistry (5 decks)

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