ch 14 alcohols Flashcards

1
Q

what are the three ways to make alcohols

A
  • hydration (electrophilic addition)
  • fermentation
  • hydrolysis (nucleophilic subsitution)
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2
Q

alkene->alcohol

A
  • hydration of alkene
  • electrophilic addition
  • H3PO4
  • 300 degrees
  • steam
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3
Q

glucose->alcohol

A
  • 37 degrees
  • anerobic respiration
  • yeast catalyst
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4
Q

haloalkane->alcohol

A
  • hydrolysis
  • reflux
  • nucleophilic subsitution
  • NaOH aq
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5
Q

evaluate hydration vs fermentation to produce alcohols

A

Hydration of ethene:
ADVANTAGES
100% atom economy
95% yield
Continuous operation
DISADVANTAGES
Ethene is obtained from crude oil which is a finite
energy resource

Fermentation:
ADVANTAGES
Glucose is a renewabl resource
DISADVANTAGES
The concentration of ethanol produced is about
15% ethanol. Distillation increases the
concentration of the alcohol
Food prices may increase with the new market
for glucose.

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6
Q

Uses of methanol:

A
  • clean burning fuel.
  • feedstock for the chemical industry.
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7
Q

Uses of ethanol:

A
  • Ethanol in alcoholic drinks:
  • perfumes.
  • Ethanol as a fuel:
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8
Q

The physical properties of alcohols are influenced by

A

their ability to form hydrogen bonds:

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9
Q

Definition: Volatility

A

is the
ease that a liquid turns
into a gas. Volatility
increases as boiling point
decreases.

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10
Q

Volatility and boiling points of alcohols

A

Alcohols have hydrogen bonds whereas their corresponding alkane (by Mr) has
London forces of attraction. As hydrogen bonds are stronger than London
forces they have higher boiling points. This means that their volatility is
much lower.

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11
Q

The physical properties of alcohols are influenced by their ability to form
hydrogen bonds.

A
  • Alcohols are soluble in water (or other polar solvents) as they will form hydrogen bonds with water (whereas alkanes will not).
  • The solubility of alcohols decreases as the carbon chain increases.
  • Only the first 3 alcohols are soluble in water.
  • The hydrocarbon chain does not form
    hydrogen bonds and as it gets longer
    it interferes with the ability for the OH
    group to hydrogen bond with water.
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12
Q

Polyols

A

Polyols are molecules that contain more than one –OH
group. When alcohols contain more than 1 hydroxyl group
they are known as diols (2), triols (3) etc.

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13
Q

Classification of alcohols:

A

This is a Primary (1o) alcohol.
When the OH carbon (*) is
attached to only 1 other
carbon atom.

This is a Secondary (2o)
alcohol. When the OH
carbon (*) is attached to 2
other carbon atoms.

This is a Tertiary (3o) alcohol.
When the OH carbon (*) is
attached to 3 other carbon

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14
Q

state the Reactions of Alcohols

A
  • Combustion of alcohols
  • Oxidation of alcohols:
  • Esterification (condensation reaction.)
  • Dehydration
  • SUBSTITUTION
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15
Q

Combustion of alcohols

A
  • In a plentiful supply of oxygen, alcohols will burn to form carbon dioxide and water.
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16
Q

Oxidation of alcohols:

A

To oxidise alcohols we use acidified potassium or sodium dichromate solution.
This is orange in colour and is a mixture of sulfuric acid, H2SO4/K2Cr2O7 or
H2SO4/Na2Cr2O7.

The orange colour is due to the Cr6+ ions in Cr2O72-
The potassium dichromate is an oxidising agent. This means that it can cause a
species to become oxidised which in turn means that the dichromate becomes
reduced. When this occurs the dichromate becomes green. The green solution
is due to Cr3+ ions.

17
Q

dichromate will remain
orange.

A

If the alcohol is resistant to oxidation

18
Q

If a large excess of dichromate is used
why might it be difficult to see if an
oxidation of the alcohol has occurred?

A

Excess of orange colour may mask the
formation of the green solution.

19
Q

Primary alcohol oxidise to form

A

Aldehyde or carboxylic acid

20
Q

Primary alcohol to an Aldehyde

A

Gentle heating of primary alcohols with acidified potassium dichromate make
an aldehyde. The aldehyde must be distilled immediately as it forms.

21
Q

Primary alcohol to a carboxylic acid

A

On stronger heating with excess acidified potassium dichromate the alcohol
will be completely oxidised passing through the aldehyde stage to form a
carboxylic acid.

22
Q

Secondary alcohol to a ketone

A
  • Kr2Cr2O7 / h2so4
  • heat
  • reflux
23
Q

Tertiary alcohols oxidation?

A

Tertiary alcohols cannot be oxidised by acidified potassium dichromate. The
dichromate remains orange and no reaction occurs.

24
Q

drawing

Apparatus for the oxidation of primary alcohols:

A

Common errors include:
The water being connected the wrong way to the condenser.

A sealed system - never cut off the condensers as this makes a closed system (increases
the pressure - explosion).

The bulb of the thermometer at the incorrect height - should be parallel to condenser.

25
Q

Distinguishing between the products of oxidation:

A

Carboxylic acid:

If refluxed, a primary alcohol forms a carboxylic acid. The acid formed can be identified
by reaction with a base e.g. sodium carbonate. The reaction will produce bubbles as an
immediate observation.

Acid + metal carbonate → salt + water + carbon dioxide

26
Q

Preparation of esters

A

Warming a carboxylic acid and alcohol in a
boiling tube with a few drops of concentrated
sulphuric acid catalyst will produce an ester.

27
Q

Definition: Condensation is
the reaction

A

whereby two
molecules are joined with
the loss of a small molecule
e.g. water

28
Q

naming esters

A

alky alcaonate
alkyl alchohol
alcanote from carboxylic acid

29
Q

Esterification

A

An ester is formed when an alcohol is warmed with a
carboxylic acid in the presence of an acid catalyst.

Esterification is an example of a condensation reaction.

30
Q

Uses of esters

A

Are used as good solvents and in adhesives.

They have a sweet smell so are more known for their uses in perfumes and
food flavour additives:

31
Q

Definition: Dehydration

A

Definition: Dehydration is
an elimination reaction in
which water is removed
from a saturated molecule
to make an unsaturated
molecule.

32
Q

alcohol->alkene

A
  • dehydration
  • conc h2so4
  • heat under reflux
  • The H and OH
    atoms are lost from
    adjacent carbon
    atoms. The double
    bond then forms
    between these
    carbon atoms.
33
Q
A