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A Level Chemistry OCR B > What's in a Medicine > Flashcards

What's in a Medicine Flashcards

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1
Q

Give the general formula of alcohols.

A

ROH

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2
Q

Give the general formula of aldehydes.

A

RCOH

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3
Q

Give the general formula of ketones.

A

RCOR’

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4
Q

Give the general formula of carboxylic acids.

A

RCOOH

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5
Q

Give the general fromula of acid anhydrides.

A

(RCO)2O

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6
Q

Give the general formula of esters.

A

RCOOR’

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7
Q

Give the general formula of ethers.

A

ROR’

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8
Q

Give the structural formula of alcohols.

A

R-OH

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9
Q

Give the structural formula of aldehydes.

A

R-C=O
|
H

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10
Q

Give the structural formula of ketones.

A

R-C-R
||
O

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11
Q

Give the structural formula of carboxylic acids.

A

O
||
R-C-O-H

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12
Q

Give the structural formula of acid anhydrides.

A

O O
|| ||
R-C-O-C-R’

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13
Q

Give the structural formula of esters.

A

R
|
C=O
|
O
|
R

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14
Q

Give the structural formula of ethers.

A

R-O-R

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15
Q

Prefix/suffix of alcohols

A

-ol

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16
Q

Prefix/suffix of aldehydes

A

-al

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17
Q

Prefix/suffix of ketones

A

-one

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18
Q

Prefix/suffix of carboxylic acids

A

-oic acid

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19
Q

Prefix/suffix of acid anhydrides

A

-oic anhydride

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20
Q

Prefix/suffix of esters

A

-oate

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21
Q

Prefix/suffix of ethers

A

-oxy-

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22
Q

Describe primary alcohols.

A

When in -OH is attached to a carbon bonded to only one carbon.

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23
Q

Describe secondary alcohols.

A

When the -OH is attached to a carbon bonded to 2 carbons.

24
Q

Describe tertiary alcohols.

A

When the -OH is attached to a carbon bonded to three carbons.

25
Q

What is the structure of a phenol?

A

OH group attached to a benzene ring.

26
Q

What is the test for phenols?

A

Addition of iron(III) chloride. Solution turns purple.

27
Q

Describe the acidic nature of phenols.

A

Weak acids so partially dissociate in water to form a phenoxide ion and a H+ ion.

28
Q

Describe the reaction of phenols with alkalis.

A

React to form salt + water

29
Q

Describe the reaction of phenols with carbonates.

A

don’t react

eg. sodium carbonate is not a stong enough base to remove the hydrogen ion from phenol

30
Q

phenols - how to tell them apart from carboxylic acids

A

carboxylic acids react with carbonates (and alkalis) and give off CO2 gas

phenol doesn’t react with carbonates
phenol doesn’t give off CO2 when react with alkali

31
Q

Describe the reaction of phenols with acid anhydrides.

A

React to form an ester and a carboxylic acid.

32
Q

phenols - how to tell them apart from alcohols

A
  • alcohols react with carboxylic acids to make an ester and water
  • phenols do not react with carboxylic acids to form an ester
  • (both form an ester and carboxylic acid when reacting with acid anhydride)
33
Q

Describe the reaction of alcohols with carboxylic acids.

A

React to form esters - esterification reaction
* heat carboxylic acid and alcohol with an acid catalyst (conc. sulfuric/hydrochloric acid)
* form an ester and water

34
Q

Describe the reaction of alcohols with acid anhydrides.

A

alcohol + acid anhydride –> ester + carboxylic acid

35
Q

State the possible products from the oxidation of alcohols.

A
  • carbonyl compounds (ketone and aldehyde)
  • carboxylic acid
    need to use the oxidising agent acidified potassium dichromate(VI)
36
Q

Describe the oxidation of primary alcohols.

A

primary alcohol –> aldehyde –> carboxylic acid

37
Q

Describe the oxidation of secondary alcohols.

A

secondary alcohol –> ketone

38
Q

Describe the oxidation of tertiary alcohols.

A

Cannot be oxidised by dichromate - only by burning

39
Q

Describe the oxidation process of primary alcohols.

A

can control how far the reaction goes
1. gently heat with potassium dichromate(VI) and sulfuric acid in a flask produces an ALDEHYDE
- to get just the ALDEHYDE need to get it out of the oxidising agent - DISTILLATION APPARATUS
(the aldehyde boils at a lower temp. than the alcohol so evaporates and is distilled off immediately)

  1. to produce CARBOXYLIC ACID needs to be vigorously oxidised
    - alcohol mixed with excess oxidising agent and heated UNDER REFLUX
40
Q

Describe the oxidation process of secondary alcohols.

A

under reflux using acidified potassium dichromate(VI)

41
Q

Describe the possible methods for dehydration of alcohols.

A
  1. Ethanol vapour is passed over a hot solid catalyst of pumice stone or aluminium oxide, Al2O3 - the catalyst provides a large surface area for the reaction.
  2. reflux with excess concentrated sulfuric acid catalyst or phosphoric acid at 170 degrees C.
42
Q

Decribe process of dehydrating alcohols using hot catalyst method.

A

mineral/ ceramic wool is soaked in ethanol, pumice stone or Al2O3 is heated, the alkene gas collects in an inverted cylinder in a water bath.

43
Q

Decribe the process of dehydrating alcohols using reflux method.

A
  • heat solution in a flask fitted with a vertical Liebig condenser - this causes the solution to continuously boil/evaporate and then condense back into the flask, giving it time to react
  • heat solution electronically; hot plates, heating mantles.
44
Q

Decribe the formation of haloalkanes.

A

Formed via substitution reaction of alcohols and halide compounds e.g. HCl. The -OH group is replaced by the halide (other product is made of the OH lost and what’s left of the halogen)

45
Q

Define elimination reaction.

A

The removal of a molecule from a saturated molecule to make an unsaturated molecule.

46
Q

How do you make an alkene from alcohol?

A

Make an alkene by eliminating water from an alcohol in a dehydration reaction.

47
Q

Mass spectra - what does it tell us?

A

helps identify compounds
relative atomic mass
relative molecular mass
relative isotopic abundance
molecular structure

48
Q

Mass spectra - how does it work?

A
  1. vapourisation - the sample is turned into a gas by an electrical heater
  2. ionisation - the gas particles are bombarded with high energy electrons to ionise them. Electrons are knocked off the particles leaving +ve ions
  3. acceleration - the +ve ions are accelerated by an electric field
  4. detection - the time taken for the +ve ions to reach the detector is measured. This depends on an ion’s mass and charge. Lighter, highly charged ions first.
49
Q

mass spectra - what is the M+ peak?

A

gives the relative molecular mass of a compound
the mass/charge value is the molecular mass
its the far right peak

50
Q

mass spectra - what is the M+1 peak?

A

a smaller peak to the right of the molecular ion peak

51
Q

mass spectra - what causes the M+1 peak?

A

caused by the presence of the carbon isotope 13C

52
Q

mass spectra - describe fragmentation

A

the bombarding electrons make some of the molecular ions break up into fragments
- the fragments the are ions show up on the mass spectrum making a fragmentation pattern

53
Q

mass spectra - what is fragmentation used for?

A

used to identify molecules and their structure

54
Q

mass spectra - how do you work out structural formula?

A
  1. work out what ion could have made each peak from its m/z value
  2. identify the fragments
  3. piece them together to form a molecule with the correct Mr
55
Q

infrared spectra - how does it work?

A
  1. a beam of infrared radiation is passes through a sample of a chemical
  2. the IR radiation is absorbed by the covalent bonds in the molecules
    - this increases their vibrational energy (they vibrate more)
  3. bonds between different atoms absorb different frequencies of IR radiation and bonds in different places in a molecule also absorb different frequencies
    eg. O-H bond in alcohol and O-H bond in carboxylic acids absorb different frequencies
56
Q

infrared spectra - what does it tell us?

A

An infrared spectrometer produces a spectrum that shows you what frequencies of radiation the molecules are absorbing

can use this to identify the functional groups in a molecule

also means that you can tell if a functional group has changed during a reaction.

A Level Chemistry OCR B (11 decks)

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