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Chemistry (Tim) > Organic Chemistry > Flashcards

Organic Chemistry Flashcards

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1
Q

organic chemistry

A

the chemistry of carbon

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2
Q

1C

A

meth

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3
Q

2C

A

eth

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4
Q

3C

A

prop

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5
Q

4C

A

but

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6
Q

5C

A

pent

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7
Q

6C

A

hex

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8
Q

7C

A

hept

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9
Q

8C

A

oct

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10
Q

9C

A

non

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11
Q

10C

A

dec

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12
Q

C bonds

A

4

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13
Q

N bonds

A

3

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14
Q

H bonds

A

1

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15
Q

O bonds

A

2

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16
Q

saturated compound

A

all the chemical bonds between carbons are single bonds

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17
Q

unsaturated compound

A

at least one of the carbon to carbon bonds is a double or triple bond

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18
Q

aliphatic compounds

A

contain open (straight or branched) chains of carbon atoms and closed rings of carbon with similar properties

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19
Q

aromatic compounds

A

contain at least one benzene ring

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20
Q

functional group

A

a group of atoms which are present in all members of any series, which determines

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21
Q

homologous series

A

a group of organic compounds with a common functional group and successive members of the series differ in size by CH2

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22
Q

structural isomerism

A

compounds with the same molecular formula but have differnt structural formula

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23
Q

mirror images

A

not isomers

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24
Q

molecules that can be easily straightened

A

not isomers

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25
Q

addition reactions

A

a molecule has extra atoms added without losing any of its own atoms

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26
Q

substitution reactions

A

atoms already on a molecule are substituted or replaced by different atoms

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27
Q

hydrocarbons

A

only has hydrogen and carbon

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28
Q

nomenclature

A

system of naming

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29
Q

longest chain for alkanes

A

just the longest carbon chain

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30
Q

longest chain for non alkanes

A

longest carbon chain containing the functional group

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31
Q

which way to number for alkanes

A

keep the carbons carrying a substituent as low as possible

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32
Q

which way to number non-alkanes

A

carbons in functional group kept as low as possible

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33
Q

2 of the same substituent

A

di

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34
Q

3 of the same substituent

A

tri

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35
Q

4 of the same substituent

A

tetra

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36
Q

order to list different substituents

A

alphabetical

eg. 4-chloro-3-ethyl-3-methylheptane

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37
Q

numbers separted from numbers with a

A

,

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38
Q

numbers separated from letters by

A

-

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39
Q

rule 5 for alkene and alkynes only

A

position of double or triple bond indicated by lower of 2 numbers eg. pent-2-ene

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40
Q

what is boiling point an indication of?

A

how difficult it is to separate molecules from each other

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41
Q

are hydrocarbons polar or non-polar

A

non-polar

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42
Q

solubility of hydrocarbons

A

don’t dissolve in non-polar solvents such as water but do in non-polar eg.cyclohexane

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43
Q

solubility rule

A

like dissolves like

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44
Q

boiling points of hydrocarbons

A

weak van der waal forces, low boiling points

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45
Q

Mr of hydrocarbons increases

A

greater the boiling point

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46
Q

small hydrocarbons at room temp

A

gases

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47
Q

large hydrocarbons at room temp

A

liquids

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48
Q

aldehydes and ketones contain what?

A

carbonyl group

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49
Q

carbonyl group

A

\
C = O
/

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50
Q

boiling points of aldehydes and ketones and why

A

higher than hydrocarbons , dipole dipole attraction vs van der waal

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51
Q

solubility of aldehydes and ketones and why

A

both soluble in water, both have polar ends which are attracted to water by hydrogen bonding

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52
Q

if the aldehydes and ketones have long C-H chains

A

the nonpolar ends become bigger and more important
large nonpolar end repels water more than the smaller polar end attracts the water so that the larger aldehydes and ketones are insoluble in water

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53
Q

functional group of alcohols

A

hydroxyl group

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54
Q

hydroxyl group

A

-O-H-

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55
Q

boiling points of alcohols and why

A

higher than comparable aldehydes and ketones because of hydrogen bonding

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56
Q

comparable

A

same Mr

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57
Q

solubility of alcohols and why

A

very soluble in water, hydrogen bonding

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58
Q

alcohols with large C-H chains

A

C-H becomes the bigger part, overall molecule gets bigger and non-polar part is now more important than polar. dissolves in cyclohexane and not water

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59
Q

carboxylic acids functional group

A

carboxylic group

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60
Q

carboxylic group

A 
O
     //
- C
     \
       O - H
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61
Q

boiling points of carboxylic acids and why

A

highest of all, hydrogen bonding and more sites for hydrogen bonding

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62
Q

summary of boiling points

A

Carboxylic acids, alcohols, aldehydes and ketones, hydrocarbons (alkanes, alkenes, alkynes)

double H bond, h bond, dipole dipole, van der waal

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63
Q

solubility of carboxylic acids and why

A

very soluble in water because they undergo hydrogen bonding

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64
Q

when C-H chain gets too long in carboxylic acids

A

non-polar part more important, dissolves in cyclohexane not water

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65
Q

crude oil

A

mixture of substances of different Mr

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66
Q

what is refining about

A

separating the substances from each other

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67
Q

fractional distillation

A

the heating of crude oil and then separating the various mixtures on the basis of their different boiling points

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68
Q

crude oil is

A

viscous

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69
Q

crude oil first goes into

A

a furnace

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70
Q

what goes in the bottom of the steel column

A

super heated steam

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71
Q

what comes out the bottom of the steel column

A

residue of tar

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72
Q

what happens in the furnace

A

it is partially vapourised

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73
Q

bottom of steel column

A

very hot

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74
Q

top of steel column

A

coolest part

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75
Q

interior of steel column arranged

A

in horizontal trays

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76
Q

X’s tray

A

X can be removed

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77
Q

above X tray

A

X is liquid and falls down

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78
Q

below X tray

A

X is gas under pressure and floats up

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79
Q

4 types of petroleum gas

A

methane
ethane
propane
butane

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80
Q

-CH3

A

methyl

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81
Q

-C2H5

A

ethyl

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82
Q

-C3H7

A

propyl

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83
Q

-C4H9

A

butyl

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84
Q

2 uses of petroleum gas

A

domestic bottle gas and LPG

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85
Q

LPG

A

liquid petroleum gas used in some cars

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86
Q

light gasoline aka

A

petrol

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87
Q

carbon atoms per molecule of petrol

A

5-10

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88
Q

use of petrol

A

for fuel

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89
Q

petrol is mostly

A

alkanes

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90
Q

carbon atoms per molecule of naptha

A

7-10

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91
Q

carbon atoms per molecule of something you can use to make petrol

A

5-10

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92
Q

2 uses of naphtha

A

petrol and raw materials

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93
Q

4 things naphtha is used as a raw material for

A

plastics, solvents, fibres, detergents etc

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94
Q

carbon atoms per molecule of kerosene

A

11-14

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95
Q

2 uses of kerosene

A

jet engine fuel

home heating

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96
Q

gas oil aka

A

diesel

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97
Q

carbon atoms per molecule of diesel

A

14-20

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98
Q

use of diesel

A

in diesel engines

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99
Q

carbon atoms per molecule of lubricating oil

A

20-30

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100
Q

use of lubricating oils

A

lubricating oil

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101
Q

lubricating oils are

A

viscous

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102
Q

why aren’t lubricating oils used as fuel

A

not easily vapourised

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103
Q

carbon atoms per molecule of fuel oil

A

30-35

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104
Q

use of fuel oil

A

can be made into droplets and used as ship and power station fuel

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105
Q

carbon atoms per molecule of bitumen

A

> 35

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106
Q

use of bitumen

A

road tar

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107
Q

smell of methane ethane etc.

A

odourless but sulphur containing mercaptans added to give a strong smells so leaks easily detected

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108
Q

smell of methane ethane etc.

A

odourless but sulphur containing mercaptans added to give a strong smells so leaks easily detected

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109
Q

petrol coming from fractioning column

A

inefficient fuel

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110
Q

what is an inefficient fuel

A

explodes on compression before spark ignites it

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111
Q

explodes on compression before spark ignites it

A

auto-ignition

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112
Q

auto-ignition causes

A

knocking

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113
Q

knocking causes 3

A

loss of power
engine damage
excessive noise in the car

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114
Q

what causes knocking

A

straight chain molecules

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115
Q

what prevents knocking

A

the presence of branched chain molecules

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116
Q

octane rating

A

the capacity of petrol to burn smoothly

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117
Q

octane rating scale

A

1-100

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118
Q

0 on octane rating

A

heptane

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119
Q

100 on octane rating

A

2,4,4 trimethylpentane

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120
Q

2,4,4 trimethylpentane aka

A

iso octane

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121
Q

definition of octane number of a fuel

A

the measure of the tendancy of a fuel to resist knocking

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122
Q

octane number of 97 efficiency

A

same as 97% 2,4,4 trimethylpentane and 3% heptane

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123
Q

2,4,4 trimethylpentane and heptane

A

reference substances

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124
Q

4 features of high octane rating fuel

A
  • highly branched molecules
  • short alkanes
  • cyclical compound
  • aromatic molecules
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125
Q

1 highly branched molecule

A

2,4,4 trimethylpentane

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126
Q

1 short alkane

A

pentane

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127
Q

1 cyclical compound

A

cyclohexane `

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128
Q

aromatic molecules

A

contain benzene

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129
Q

what was put into petrol before

A

anti-knocking agent

tetra ethyl lead

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130
Q

3 reasons why use of tetra ethyl lead was stopped

A

lead pollution in air
it’s tendency to poison catalytic convertors
toxicity to human health

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131
Q

4 ways to ensure petrol has a high octane number

A

isomerisation
reforming
adding oxygenates
catalytic cracking

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132
Q

isomerisation

A

when straight pentane and hexane with low octane numbers are heated and passed over a catalyst. they break up at and reform at random to give a mixture of straight and branched versions (isomers)

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133
Q

reforming aka

A

dehydrocyclisation

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134
Q

reforming

A

use of catalysts to form ring compounds, converted to cycloalkanes such as cyclohexane

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135
Q

2 things happening in reforming

A

hydrogen is expelled

aromatic compounds are formed

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136
Q

valuble hydrogen made in dehydrocyclisation

A

piped away

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137
Q

adding oxygenates

A

3 oxygen containing compunds added to petrol to increase it’s octane number

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138
Q

3 oxygen containing compunds that are added to petrol to increase it’s octane number

A

methanol
ethanol
MTBE

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139
Q

MTBE

A

methyl tertiary butyl ether

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140
Q

secondary use of oxygenates

A

reduce the level of pollutants coming from petrol, especially CO2 gas

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141
Q

catalytic cracking aka

A

cat cracking

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142
Q

cat cracking definition

A

the breaking down of long chain hydrocarbon molecules using heat and catalysts into smaller molecules which are more useful

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143
Q

cat cracking is carried out on… and why

A

kerosine, diesel oil and fuel oil, to obtain shorter molecules of carbon length 5-10 and higher octane rating

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144
Q

2 things cat cracking yields

A

more molecules with carbons lengths 5-10

smaller molecules such as alkenes

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145
Q

why are more molecules with carbons lengths 5-10 important

A

petrol can be manufactured

usually highly branched ie. high octane number

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146
Q

why are smaller molecules such as alkenes important?

A

manufacture of plastics and other chemical products

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147
Q

use of cracking allows chemists to…

A

use of cracking allows chemists to convert many of the fractions from crude oil for which there is little use

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148
Q

h2 burns readily in O2, what are products?

A

only H2O

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149
Q

H2 + 1/2 O2 ->

A

H2O

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150
Q

ΔH =

A

-242 kj/mole

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151
Q

3 difficulties with hydrogen as a fuel

A

expensive to produce
very explosive in air
very low density

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152
Q

how is hydrogen produced

A

electrolysis or steam reforming of methane

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153
Q

steam reforming of methane

A

burning of fossil fuels

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154
Q

why is very low density a problem

A

difficult to store

must be stored in high pressure containers

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155
Q

equation for steam reforming of methane to form H2

A

CH4 + H2O -> 3H2 +CO

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156
Q

equation for hydrogen gas being used in the industrial production of ammonia

A

N2 + 3H2 -> 2NH3

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157
Q

hydrogen also used in?

A

the hydrogenation of vegetable oils in margarine production

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158
Q

general formula of alkane

A

C2 H2n+2

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159
Q

functional group of alkanes

A 
/
- C -
   /
no double carbon bond
no triple carbon bond
no oxygen
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160
Q

name for alkanes

A

-ane

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161
Q

first alkane

A

methane

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162
Q

methane

A

CH4

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163
Q

ethane

A

c2H6

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164
Q

general formula of alkenes

A

CnH2n

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165
Q

functional group of alkenes

A

carbon to carbon double bond

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166
Q

first alkene

A

ethene

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167
Q

ethane

A

C2H4

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168
Q

general formula of alkynes

A

CnH2n-2

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169
Q

functional group of alkynes

A

carbon to carbon double bond

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170
Q

first alkyne

A

ethyne

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171
Q

ethyne

A

C2H2

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172
Q

alcohol general formula

A

CxHy-OH

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173
Q

functional group of alcohol

A

-O-H

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174
Q

first alcohol

A

methanol

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175
Q

methanol

A

CH3OH

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176
Q

general formula of aldehydes

A

CxHyCHO

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177
Q

functional group of aldehydes

A 
O
    //
-c
     \ 
       H
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178
Q

first aldehydes

A

methanal

179
Q

methanal

A

HCHO

180
Q

general formula of ketones

A

(CxHy)nCO

181
Q

functional group of ketones

A

O
//
C
/ \

182
Q

first ketone

A

propanone

183
Q

propanone

A

(CH3)2 CO

184
Q

general formula of carboxylic acids

A

CxHyCOOH

185
Q

functional group of carboxylic acids

A

methanoic acid

186
Q

methanoic acid

A

HCOOH

187
Q

aromatic hydrocarbons contain what

A

a benzene ring

188
Q

molecular formula for benzene

A

C6H6

189
Q

who proposed the structural formula for benzene and when

A

kekule in 1865

190
Q

was kekule correct?

A

no

191
Q

first characteristic of benzene that proved kekule wrong?

C-C length

A

he suggested that there were two different bond lengths but there is only one in benzene, all the bonds are equal

192
Q

second characteristic of benzene that proved kekule wrong? C=C

A

kekule’s structure had very reactive C=C bonds, which would suggest it undergo addition reactions

193
Q

what can tell us that benzene does not have C=C bonds?

2

A

very unreactive, undergoes substitution reactions

does not decolourise bromine water of KMnO4

194
Q

how many valence or bonding electrons does carbon have

A

4 valence or bonding electrons

195
Q

3 of carbon’s valence electrons in benzene

A

involved in σ bonds with 2 neighbouring carbon atoms and one hydrogen atom

196
Q

the 4th valence electron is benzene

A

exists in an unused p orbital

197
Q

how many unused p orbitals in benzene

A

6

198
Q

how are the 6 unused p orbitals aligned?

A

perpendicular to the plane of the ring

199
Q

where are the 6 π bond electrons located?

A

they are free to move throughout the entire ring so they don’t belong to any carbon

200
Q

what does it mean that they are free to move throughout the entire ring so they don’t belong to any carbon

A

they are delocalised

201
Q

what does the fact that 6 electrons are delocalised give benzene?

A

extra stability

202
Q

what does the extra stability account for?

A

it’s general unreactivity

203
Q

why should contact with benzene be avoided?

A

it’s known to be carcinogenic

204
Q

what is a safer molecule derived from benzene

A

methyl benzene

205
Q

what is methyl benzene known for

A

its a non polar solvent. won’t dissolve in water but will in cyclohexane

206
Q

the look of a benzene molecule

A

a flat molecule

207
Q

bond angle of carbons in benzene

A

120º

208
Q

how are aromatic compounds obtained

A

mostly from the fraction distillation of crude oil

209
Q

general formula of alkanes

A

C n H 2 n+2

210
Q

alkanes, saturated or unsaturated?

A

saturated

211
Q

all carbons in alkanes

A

have 4 single bonds out of them

212
Q

structure of carbons in alkanes

A

tetrahedral structure

213
Q

are alkanes reactive

A

mostly unreactive

214
Q

what does the fact that alkanes are mostly unreactive explain

A

explains why they are widely found in nature

215
Q

first four alkanes at room temperature

A

gases

216
Q

next twelve alkanes at room temperature

A

liquids

217
Q

heavier alkanes

A

waxy solids

218
Q

where are the waxy solid, heavy alkanes found

A

in plants

219
Q

first for alkane gases

A

methane, ethane, propane, butane

220
Q

where are the first for alkanes produced

A

in large quantities in fractional distillation of crude oil

221
Q

3 properties of the first 4 alkanes

A

light
colourless
odourless

222
Q

why are the first 4 alkanes excellent fuels

A

they combust easily

223
Q

are the first 4 alkanes reactive

A

generally unreactive

224
Q

where can methane also be produced? 2

A

the anaerobic respiration of decaying organic matter and by farm animals

225
Q

3 examples of decaying organic matter that produce methane

A

farm manure
marshes
rice paddy fields

226
Q

2 uses of methane

A

a fuel
on an industrial scale, to make H2 gas
make NH3

227
Q

how is H2 gas made out of methane

A

it is reacted with high pressure steam

228
Q

production of NH3

A

first step in the manufacture of artificial nitrate fertiliser

229
Q

methane is regarded as

A

a greenhouse gas that contributes to global warming

230
Q

chloroalkanes

A

one or more of the hydrogen atoms in alkane molecules is replaced by a chlorine atom

231
Q

are chloralkanes saturated or unsaturated

A

saturated

232
Q

structure of chloroalkanes

A

tetrahedral structure

233
Q

chloroalkanes at room temp

A

liquids

234
Q

are chloroalkanes good solvents

A

excellent solvents

235
Q

are chloroalkanes polar or non-polar

A

largely non polar

236
Q

bp of chloroalkanes

A

low bp, vaporise off surfaces easily

237
Q

2 uses of chloroalkanes

A

dry cleaning clothes

tippex

238
Q

what is dichloromethane found in

A

paint stripper

239
Q

how does dichloromethane work as a paint stripper

A

acts as a solvent and dissolves old unwanted paint and that it evaporates due to us low boiling point, leaving the dry dissolved paint behind as a flaky surface, easily scraped off

240
Q

recent concern about chloroalkanes

A

they cause harm to the ozone layer in the atmosphere `

241
Q

if there are more than 3 carbons?

A

they can undergo isomerism

242
Q

general formula for alkenes

A

CnH2n+2

243
Q

functional group of alkenes

A

C=C

244
Q

smallest alkene

A

ethene

245
Q

alkenes, saturated or unsaturated

A

unsaturated

246
Q

smallest 3 alkenes at rt

A

gases

247
Q

other alkenes

A

liquids or soft solids

248
Q

shape of alkene molecules

A

planar

249
Q

why are alkenes planar

A

2 carbons joined by a double bond

250
Q

shape of longer carbon chain alkenes e.g. pent-1-ene

A

has a planar end with the functional group and the other end is tetrahedral

251
Q

are alkenes reactive

A

much more reactive than alkanes

252
Q

why are alkenes much more reactive than alkanes

A

because the C=C bond is much less stable than the C-C and C-H bonds

253
Q

double bond consists of

A

sigma and pi bonds

254
Q

which is weaker sigma or pi

A

pi is weaker

255
Q

why are C=C bonds more reactive than C-C bonds

A

the weak pi bond breaks easily releasing it’s two bonding electrons to bond with other atoms or groups of atoms

256
Q

in general, what do addition reactions cause

A

a change in structure from planar to tetrahedral

257
Q

how do you prepare an alkene

A

dehydrate the appropriate alcohol

258
Q

appropriate alcohol

A

same number of carbon

259
Q

preparation of ethene formula

A

C2H5OH –> C2H4 + H2O

260
Q

ethanol

A

C2H5OH

261
Q

preparation of ethene, what holds the ethanol in place

A

glass wool

262
Q

how is the tube placed in the preparation of ethene

A

horizontally

263
Q

preparation of ethene, where do you clamp the boiling tube

A

near its neck

264
Q

preparation of ethene, what do you add half way along the tube

A

aluminium oxide

265
Q

preparation of ethene, how much aluminium oxide do you use

A

2g

266
Q

preparation of ethene, how do you push the glass wool into the tube

A

using a glass rod

267
Q

preparation of ethene, how do you put the aluminium oxide into the tube

A

using a spatula

268
Q

preparation of ethene, how is ethene collected

A

by the downward displacement of water

269
Q

preparation of ethene, describe how you heat the tube

A

just touch the flame onto the alcohol end

270
Q

preparation of ethene, what happens when the alcohol vapour passes over the aluminium oxide?

A

its dehydrated

271
Q

aluminium oxide

A

Al2O3

272
Q

preparation of ethene, what do you do at the start when gas starts to come out and why?

A

let is bubble off for a minute do not collect as it is mostly air

273
Q

preparation of ethene, how much do you collect

A

collect about 5 jars of ethene

274
Q

preparation of ethene, after collecting each jar

A

put a stopper in

275
Q

preparation of ethene, after collecting sufficient amount

A

turn off bunsen burner and immediately disconnect delivery tube to prevent suck back

276
Q

preparation of ethene, how do you disconnect delivery tube

A

loosening the clamp and sliding up so that the delivery tube is out of the water

277
Q

what is suck-back?

A

where a vacuum occurs in the tube as it cools and draws cold water into the hot boiling tube causing it to splinter and crack

278
Q

2 tests for unsaturation

A

bromine water

acidified potassium mangnate

279
Q

colour change of bromine water

A

red/orange to colourless

280
Q

colour change of acidified potassium magnate

A

purple to colourless

281
Q

potassium magnate

A

KMnO4

282
Q

reaction for production of ethene

A

elimination reaction

283
Q

definition of an elimination reaction

A

a reaction in which a small molecule is removed from a large molecule leaving a double bond behind on the remaining larger molecule

284
Q

colour of ethene

A

colourless

285
Q

smell of ethene

A

sweet smell

286
Q

solubility of ethene

A

insoluble in water, soluble in cyclohexane

287
Q

how do you test ethene for unsaturation

A

add some bromine water, stopper an invert (or with acidified potassium magnate)

288
Q

how do you combust a jar of ethene

A

apply a lighted wax taper to its mouth

289
Q

combustion of ethene

A

burns brightly

290
Q

what is produced when ethene is burned in air

A

CO2 is formed

291
Q

testing burned ethene for CO2

A

put some lime water in it, stopper and invert. goes milky white

292
Q

burned ethene turns into

A

water and carbon dioxide

293
Q

burned ethene in air equation

A

C2H4 + 3O2 –> 2CO2 + 2H2O

294
Q

general rule, organic compounds burn

A

to form CO2 and H2O

295
Q

preparation of ethene 3 other precautions

A

do not let flame directly near ethanol
handle glass wool with gloves
tie back hair, wear goggles, wear a lab coat

296
Q

why do alkenes undergo addition reactions

A

because they have a double bond which makes it easy to ‘add on’ items

297
Q

why are alkanes much less reactive than alkenes or alkynes

A

they have no C=C bond or C=-C bond to enable addition reactions to occur

298
Q

substitution reactions in alkanes

A

much slower to occur

299
Q

2 catalysts for hydrogenation of ethene

A

200º and Ni

300
Q

hydrogenation of ethene equation

A

C2H4 + H2 —> H2H6

301
Q

H2H6

A

ethane

302
Q

Chlorination of ethene equations

A

C2H4 + Cl2 —> C2H4Cl2

303
Q

product from chlorination of ethene

A

1,2-Dichloroethane

304
Q

bromination of ethene equation

A

C2H4 + Br2 –> C2H4Cl2

305
Q

product of bromination of ethene

A

1,2-Dibromoethane

306
Q

colour of bromine

A

red/yellow

307
Q

colour of 1,2-Dibromoethane

A

colourless

308
Q

why do you never use bromine in the bromination of ethene

A

it’s too dangerous for the lab, you use bromine water

309
Q

equation, adding hydrogen chloride to ethene

A

C2H4 + HCl —> C2H4Cl

310
Q

catalyst for adding hydrogen chloride to ethene

A

AlCl3

311
Q

AlCl3

A

aluminium chloride

312
Q

product of adding hydrogen chloride to ethene

A

1-chloroethane

313
Q

hydration

A

addition of water

314
Q

what is hydration of ethene the reverse of?

A

production of ethane from ethanol (dehydration of ethanol)

315
Q

2 catalysts for the hydration of ethene

A

high temperature and pressure

316
Q

equation of hydration of ethene

A

C2H4 + H2O –> C2H4OH

317
Q

C2H4OH

A

ethanol

318
Q

what does polymerisation do to one ethene

A

turns it into polyethene

319
Q

what do you not do when drawing polymers

A

put Hs at the ends, they’re not finished, they are repeating units

320
Q

1 use of hydrogenation in industry

A

in the food industry, used to convert some double bonds in vegetable oils (polyunsaturates) to single bonds, changing them from liquid oils to spreadable semi-solids eg.margarine

321
Q

3 double bonded oils

A

palm oil
sunflower oil
corn oil

322
Q

2 saturated fats

A

dairy and cream

323
Q

which are thought to be healthier, polyunsaturated fats or saturated fats ?

A

polyunsaturated fats

324
Q

how can you make an oil as soft or hard as you want

A

by controlling the degree of hydrogenation

325
Q

2 advantages of hydrogenation

A

healthier unsaturated fats are spreadable

can make fats as soft or hard as required

326
Q

the product of chlorination of ethene

A

1,2-Dichloroethane

327
Q

where is 1,2-Dichloroethane used?

A

it is the raw material for the production of chloroethene

328
Q

what is chloroethene

A

it is a well known monomer used for the production of polychloroethene

329
Q

common name for chloroethene

A

vinyl chloride

330
Q

common name for polychloroethene

A

poly vinyl chloride (PVC)

331
Q

word equation for ethene -> PVC

A

ethene + chlorine -> dichloroethane

loses HCl to make chloroethane. polymerised to become polychoroethene (PVC)

332
Q

chemical equation for ethene -> PVC

A

C2H4 + Cl2 -> C2H4Cl2 -> C2H3Cl->

(C2H3Cl)n

333
Q

what is the function of 1,1,1-trichloroethane

A

allows 2 reactants to mix together freely. i.e a solvent

334
Q

addition of bromine (bromination) is

A

a test for unsaturation

335
Q

how to be sure of unsaturation after bromination test

A

do a second test with KMnO4

potassium mangnate

336
Q

when fruits ripen, what do they produce

A

ethene

337
Q

where is ethene also produced and what’s its function

A

produced artificially in ripening rooms to spped up ripening

338
Q

why should ripening fruit never be beside flowers

A

the ethene produced will cause they flowers to ripen and fall off

339
Q

definition of polymerisation

A

where many small molecules called monomers join together to give a long polymer

340
Q

what is high density polythene

A

polythene where long chains line close to each other and have no branching

341
Q

2 features of high density polythene

A

rigid and a high melting point

342
Q

what is low density polythene

A

long chains have branching out of them so they cannot lie close together

343
Q

1 feature of low density of polythene

A

lower melting point

344
Q

addition polymerisation

A

where no tiny molecules are expelled during the process

345
Q

condensation polymerisation

A

where tiny molecules are expelled during the process

346
Q

polymer of ethene

A

polyethene (polythene)

347
Q

uses of polyethene

A

hard and soft plastic depneding if it’s high density or low density

348
Q

polymer of propene

A

polypropene (polyproylene)

349
Q

2 uses of polypropylene

A

tough plastic

  • beer crates
  • stacking chairs
350
Q

thermoplastic vs thermosetting

A

thermoplastics can be reheated and remoulded many times, thermosetting plastic cannot

351
Q

general formula of alkynes

A

CnH2n-2

352
Q

functional group of alkynes

A

C≡C (carbon to carbon triple bond)

353
Q

polymer of chloroethane

A

polychloroethane (PVC)

354
Q

2 uses of polychloroethane

A

doors and windows

raincoats

355
Q

reactions that alkynes undergo

A

addition reactions

356
Q

why do alkynes undergo additiion reactions

A

because weak pi bonds break easily

357
Q

2 features of C≡C

A

strong

highly reactive

358
Q

smallest alkyne

A

ethyne

359
Q

whene ethyne burned in a stream of O2

A

produces temperatures in excess of 3,000°

360
Q

what is used for cutting equipment

A

oxyacetylene

361
Q

describe how oxyacetylene cutting equipment works

A

2 separate tanks of ethyne and oxygen are connected through a single outlet and the mixture is burned on exit in a controlled flame to give really high burning temperatures

362
Q

formula of benzoic acid

A

C2H5COOH

363
Q

formula of phenol

A

C6H5OH

364
Q

formula for nitrobenzene

A

C6H5NO2

365
Q

formula for methyl benzene

A

C6H5CH3

366
Q

formula for benzaldehyde

A

C6H5CHO

367
Q

how to draw any of the aromatic compounds

A

draw a circle inside a hexagon and the substituent sticking out of one corner of the hexagon

368
Q

sub in benzoic acid

A

COOH

369
Q

sub in phenol

A

OH

370
Q

sub in methyl benzene

A

CH3

371
Q

sub in nitrobenzene

A

NO2

372
Q

sub in benzaldehyde

A

CHO

373
Q

combustion of ethene formula

A

C2H4 + 3O2 –> 2CO2 + 2H2O

374
Q

by what action can you make ethyne

A

by the action of water on calcium dicarbide

375
Q

describe calcium dicarbide

A

a grey/ black solid

376
Q

formula for preparation of ethyne

A

CaC2 + 2H2O –> Ca(OH)2 + C2H2

377
Q

CaC2

A

calcium dicarbide

378
Q

Ca(OH)2

A

calcium hydroxide

379
Q

C2H2

A

ethyne

380
Q

how does calcium hydroxide look

A

cloud white ppt

381
Q

what does ethyne look like

A

colourless gas

382
Q

when ethyne burned in air

A

a lot of soot produced

383
Q

when ethyne burned in pure oxygen

A

no soot produced

384
Q

preparation of ethyne, what is used to filter out the impurities from the gas

A

acidified copper sulphate solution

385
Q

preparation of ethyne, 3 impurities trapped by acidified copper sulphate solution

A

H2S
NH3
PH3

386
Q

PH3

A

phosphine

387
Q

why do impurities arise from CaC2

A

it is not purchased pure, but contains impurities that turn into H2S, NH3, PH3 when reacted with water

388
Q

preparation of ethyne, what gives the gas odour

A

the impurities

389
Q

2 things that happen when a jar of C2H2 is burned

A
  1. gives off great heat

2. causes a great amount of soot to be formed

390
Q

what was carbide used for

A

carbide lamps were used years ago before the invention of batteries

391
Q

how does a carbide lamp work

A

water drips slowly onto CaC2 and the C2H2 produced is lit and burns brightly

392
Q

preparation of ethyne, what can be used to prove that CO2 was produced in the reaction

A

limewater turns milky

393
Q

formula for combustion of ethyne with oxygen

A

2C2H2 + 5O2 –> 4CO2 + 2H2O + heat

394
Q

why is great heat released when ethyne is burned

A

high energy carbon to carbon triple bond is broken during combustion

395
Q

ethene flame

A

bright yellow flame

396
Q

ethyne flame

A

sooty flame

397
Q

preparation of ethyne, name of flask the water drips into

A

buchner flask

398
Q

preparation of ethyne, what does the water drip from

A

a tap funnel

399
Q

preparation of ethyne, what apparatus is used to collect the gas

A

a glass tube and a beehive stand

400
Q

preparation of ethyne, where does the calcium carbide go

A

into the buchner flask

401
Q

preparation of ethyne, what do you use to transfer the calcium carbide into to buchner flask

A

a spatula

402
Q

preparation of ethyne, why do you never touch the calcium carbide

A

the moisture on you hand might start the reaction

403
Q

preparation of ethyne, how fast do you let water flow

A

only in drips

404
Q

preparation of ethyne, what happens to the flask contents when the water starts to drip

A

becomes cloudy white

405
Q

preparation of ethyne, what happens to the flask when gas starts to be produced

A

get very hot

406
Q

preparation of ethyne, what should you do with the first few jars and why

A

discard them, they are most likely just air

407
Q

preparation of ethyne, how many jars do you collect

A

about 4 or 5

408
Q

how do you test for ethyne gas

A

light the jar contents, should burn with a pop

409
Q

preparation of ethyne, how do you stop the production of gas

A

stop the flow of water

410
Q

preparation of ethyne, why do you dismantle the apparatus and empty the contents before before testing the ethyne

A

because we will be using a lighted taper on one of the jars and ethyne forms an explosive mixture with air

411
Q

preparation of ethyne, smell of ethyne if impurities get through

A

unpleasant smell

412
Q

is ethyne soluble in water and how do we know

A

no

collected by the downward displacement of water

413
Q

where do you burn a jar of ethyne

A

in a fume cupboard only

414
Q

what is the soot produced when during ethyne

A

carbon soot

415
Q

3 characteristics of ethene flame

A

less sooty/clear, less bright, bluish flame

416
Q

bromination test on ethyne

A

add a very small amount of bromine water into a test tube of ethyne gas, stopper and shake well (yellow/red -> colourless)

417
Q

KMnO4 test on ethyne

A

same as bromine water. colour change purple -> colourless

418
Q

3 precautions of preparation of ethyne

A

keep naked flames away from ethyne, don’t touch calcium dicarbide , do all tests on ethyne in a fume cupboard

419
Q

reaction mechanism

A

a step by step account of how a reaction occurs

420
Q

what drives a substitution mechanism

A

driven by free radicals

421
Q

substitution reaction aka

A

free radical substitution

422
Q

free radical

A

a group of atoms, or a single atom which are very reactive due to having one unbounded electron

423
Q

free radical substitution reaction, chemical equation

A

CH4 + Cl2 -> CH3Cl + HCl

424
Q

3 stages of free radical substitution reaction,

A

initiation stage
propagation stage
termination stage

425
Q

free radical substitution reaction, initiation stage

A

UV light is needed to start the reaction

426
Q

photochemical reaction

A

depends on light

427
Q

what can prove that our free radical substitution reaction is a photochemical reaction

A

it doesn’t occur in the dark

428
Q

free radical substitution reaction, what is the splitting of Cl2 into 2 free radicals Clº and Clº

A

homolytic fission

429
Q

homolytic fission

A

when a chemical bond breaks and each of the pieces retains one of the originally bonded electrons

430
Q

free radical substitution reaction, when and how does the propagation stage start

A

begins automatically when initiation stage is over

431
Q

free radical substitution reaction, 2 different repeating reactions in propagation stage are driven by

A

2 free radicals:

Clº and CH3º

432
Q

free radical substitution reaction, propagation stage, reaction driven by Clº

A

Clº + CH4 -> CH3º + HCl

433
Q

free radical substitution reaction, propagation stage, reaction driven by CH3º

A

CH3 + Cl2 -> CH3Cl + Clº

434
Q

free radical substitution reaction, propagation stage continues in a

A

chain reaction

435
Q

free radical substitution reaction, propagation stage continues until

A

when one of the reactants starts to get scarce

436
Q

free radical substitution reaction, if Cl2 gets scarce reaction

A

CH3º + CH3º -> C2H6

437
Q

free radical substitution reaction, if CH3 gets scarce

A

Clº + Clº -> Cl2

438
Q

free radical substitution reaction, if both Cl2 and CH3 get scarce

A

CH3º + Clº -> CH3Cl

439
Q

free radical substitution reaction, 3 proofs to show that the mechanism proposed is correct

A

Presence of traces of C2H6
addition of tetra methyl lead lead which decomposed into free radicals and speeds up the reaction
will not occur without UV light

440
Q

chain reaction

A

a reaction, once started, can only be stopped when at least one of the reactants is completely used up

441
Q

free radical substitution reaction another example

A

chlorination of ethane

442
Q

free radical substitution reaction, 2 free radicals driving the chlorination of ethane

A

ethyl or CH3CH2

443
Q

free radical substitution reaction no.2chlorination of ethane, what is formed in the termination stage rather than ethane

A

butane

444
Q

free radical substitution reaction, 2 free radicals driving the chlorination of ethane, what can be used to speed up the reaction

A

tetra ethyl lead

Chemistry (Tim) (8 decks)

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