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A level Chemistry OCR > 4.2 Alcohols, Haloalkanes And Analysis > Flashcards

4.2 Alcohols, Haloalkanes And Analysis Flashcards

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1
Q

Describe the polarity of alcohols

A

They are generally polar due to the electronegative hydroxyl group which pulls the electrons in the C-OH bond away from the carbon atom

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2
Q

Describe the trend in solubility of alcohols

A

In larger alcohols, most of the molecule is a non polar carbon chain, so there’s less attraction for the H2O molecules.

So increase in alcohol size, decreases in water solubility

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3
Q

Compare the volatility and boiling point of alcohols to alkanes

A

Alkanes have a much lower boiling point than an alcohol with the same number of carbons

  • In alkanes the intermolecular forces are only weak induced dipoles (London Forces)
  • In alcohols, the OH group can form hydrogen bonds, which are much stronger
  • These hydrogen bonds require much more energy to be broken
  • So boiling points are higher and they are less volatile.
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4
Q

How can you tell whether an alcohol is primary, secondary or tertiary?

A

Primary- OH attached to a C that is attached to 1 other Carbon

Secondary- OH attached to a C that is attached to 2 Carbons

Tertiary- OH attached to a C that is attached to 3 Carbons

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5
Q

Write an equation for the combustion of ethanol

A

C2H5OH + 3O2 —> 2CO2 + 3H2O

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6
Q

What oxidising agents can be used to oxidise alcohols

What colour is at first and after it reacts?

A 
Acidified dichromate(vi) mildly oxidies alcohols
Orange dichromate(vi) reduced to Green chromium(iii)

Cr2O7^(2–) /H+
eg.
K2Cr2O7 or H2SO4

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7
Q

What happens when you distill a primary alcohol?
and oxidise again under reflux?

(With oxidising agent)

A

Makes aldehyde and H2O

Makes carboxylic acid

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8
Q

What happens when you reflux a secondary alcohol?

With oxidising agent

A

Makes Ketones and H2O

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9
Q

What is an oxidising agent represented as?

A

[O]

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10
Q

What happens when you oxidise a tertiary alcohol?

A

They can’t. As No hydrogen atoms on the carbon atom that holds the alcohol group

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11
Q

What is it meant by dehydration of an alcohol? (elimination reaction)

(Reactants, products, conditions?)

A
  • H2O can be eliminated from alcohols to give ALKENES

- Heat under reflux with a strong acid catalyst eg. concentrated H2SO4/H3PO4

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12
Q

What are some things to be careful of for dehydration of alcohol questions?

A
  • Often 2 possible alkene products from one elimination reaction depending on which side of the hydroxyl group the hydrogen is eliminated from
  • watch out if alkene products can form E/Z isomers (if they can mix of both isomers form)
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13
Q

What is meant by substitution reaction of alcohol with halide ion?

(Alcohol to haloalkane)

Give conditons.

A

-OH group replaced by Cl-/Br-/I-
•ROH + HX –> RX + H2O (X halogen)

  • H2SO4 is added along with the NaX and the mixture is WARMED (20.c)
  • This doesn’t work for iodine as it’s oxidised by H2SO4 to give I2 so the yield is poor so H3PO4 instead
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14
Q

What is meant by hydrolysis of haloalkane in a substitution reaction by aqueous alkali?

(Haloalkane to alcohol)

Give conditons.

A

This is where a nucleophile (an electron pair donor)
usually OH- reacts with a halogenoalkane due to its
polar C–X bond (x = halogen).

The OH- donates its electrons to the polar C, this than
causes the C–X bond to break and X– is formed and alcohol.

NaOH or KOH used
Done under reflux conditions

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15
Q

How could you compare experimentally the rates of hydrolysis of different carbon-halogen bonds?

Why cant flouroalkanes be used?

A

Haloalkanes react with AgNO3 and water
•Halide ion leaves during the reaction
•This reacts with Ag+ to give a precipitate
an use how long the precipitate takes to appear to determine how fast reactions of different haloalkanes are
(EXPERIMENT)
•Use this to determine bond strengths of different C-X bonds
•Stronger bonds will lead to a slower reaction so precipitate will take longer to appear
•Fluoroalkanes can’t be used because FNO3 is soluble, not a precipitate

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16
Q

What are the main steps of the experiment to determine rates of hydrolysis of different carbon-halogen bonds?

A

○Add 1cm3 of each haloalkane to different test tubes in a water bath at 50oc
○Put test tubes with ethanol, water and aqueous silver nitrate in the water bath
○Allow them to come to the same temperature
○Add 1cm3 of ethanol, water and aqueous silver nitrate to each haloalkane
○See how long it takes for precipitate to appear

17
Q

What is a nucleophile?

A

Electron pair donor

18
Q

Describe the mechanism for nucleophilic substitution in the hydrolysis of primary haloalkanes with aqueous alkali

A

Nucleophile (mark on lone pair and negative charge,
:-OH )
Curly arrow to C δ+ attached to halogen in the hydrocarbon
Curly arrow from C-X bond to X (mark x with δ-)

ARROW–>

Haloalkane + :X-

19
Q

What does branching do to volatility and bp?

A

Branching generally decreases boiling point, and so increases volatility

20
Q

Explain the trend in the rates of hydrolysis of primary haloalkanes in terms of the bond enthalpies of carbon–halogen bonds (C–F, C–Cl, C–Br and C–I)

A
  • Going down halogens atoms increase in size
  • Bonding electrons are further from nucleus so more shielded
  • This gives lower C-X bond enthalpies
  • Easier to break the bond so reaction happen faster
21
Q

What are CFCs?

A

Chlorofluorocarbons, haloalkanes.

22
Q

What are properties of CFC’s?

A

Stable, volatile, nonflammable, non toxic

23
Q

What were the uses of CFC’s?

A

Fridges, aerosol cans, dry cleaning and air-con

24
Q

What could you say ozone in the upper atmosphere acts like?

A

Chemical sunscreen, it absorbs lots of UV radiation which can cause sunburn and skin cancer

25
Q

How is ozone formed?

Give equation

A

Oxygen molecule is broken down into 2 free radicals by UV radiation. The free radicals attack other Oxygen molecules forming ozone.

O2—UV–> O. + O.
O2 + O. –> O3

26
Q

Why are holes in Ozone layer bad?

A

Allows more harmful UV radiation to reach earth

27
Q

How are holes in the Ozone layer formed?

A
  • CFC’s in the upper atmosphere absorb UV radiation and split to form chlorine free radicals.
  • The radicals catalyse the destruction of the ozone layer, they destroy ozone molecules and regenerate to destroy more.
28
Q

Give equation for production of halogen radicals
And the breakdown of ozone
what is the Cl•

A

CF2Cl2(g) —UV—> •CF2Cl(g) +Cl•

Propagation: Cl•(g) + O3(g) —> O2(g) + ClO•(g)
Propagation: ClO•(g) + O(g) —>O2(g) + Cl•(g)

Overall: 03(g) + O(g) —> 2O2 (g)

The Cl• is the catalyst

29
Q

Give the equations for when nitrogen oxides break ozone down too

A

Propagation: ·•NO + O3 —> •NO2 + O2
Propagation: •NO2 + O —> •NO + O2
Overall: O3 + O 2O2

30
Q

Where are nitrogen oxides produced?

A

Car, aircraft engines, thunderstorms

31
Q

What are the alternatives to CFC’s and whats the problem with them?

A

HCFC’s-still damage ozone layer, greenhouse gas

HFC’s-greenhouse gas

32
Q

What do they use nowadays for aerosol cans and frdges?

A

Aerosol cans- Pump spray system or nitrogen propellant

Frdge- ammonia as coolant gas

CO2 to make foamed polymers

33
Q

The techniques and procedures for:

Use of Quickfit apparatus including for distillation and heating under reflux

A

For reflux – vertical condenser attached to flask, the water goes into the bottom of the condenser, often use water bath (flask in beaker of water) or heating element (electric heater) to heat flask rather than direct
heating with Bunsen burner as chemicals may be flammable.

For distillation – set up condenser at an angle with the higher end at flask and sloping away, the water is attached to lower end, the thermometer should be level with entrance to condenser

34
Q

Describe Preparation and purification of an organic liquid

A

Use of a separating funnel to remove an organic
layer from an aqueous layer
The aqueous and organic layer don’t mix, you can
drain off bottom layer to separate the two.

Drying with an anhydrous salt (e.g. MgSO4, CaCl2)
Add anhydrous salt which will absorb any water,
filter the mixture to remove the now hydrated salt
and leave product.

Redistill - distillation as before to purify product.

35
Q

What happens when chemical absorb IR

A

their covalent bonds vibrate more and absorb energy

36
Q

What is the use of IR spectra?

A

Used in monitoring air pollution
•Pollutants like CO and NO have specific absorptions that allow their concentrations to be monitored
•This can be used to study the effect of traffic on air quality
•Also used in breathalyzers

37
Q

What are some common fragment ion peaks?

A 
15 = CH3+, 
29 = C2H5+, 
17 = OH+,
38
Q

Explain how you would carry out separation to remove water soluble impurities from a product?

A
  • Mixture poured in separating funnel
  • Water is added
  • Funnel is shaken and allowed to settle
  • Organic layers is less dense so floats on top
  • Water soluble impurities should dissolve in lower aqueous layer
  • Open stopper to let aqueous layer drain off
39
Q

Whats the problem with using separation? How do you combat this issue?

A

Organic layer will contain trace amounts of water, so must be dried

-Add anhydrous salt (MgSO4, CaCl2), this is a drying agent and binds to water becoming hydrated

-When you first add salt to organic layer it will be lumpy
so add more salt

  • You know when All water is removed as when you swirl the mixture it looks like snow globe
  • Filter mixture to remove solid drying agent

A level Chemistry OCR (15 decks)

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