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A level Chemistry > Unit 2.4 - Organic Compounds > Flashcards

Unit 2.4 - Organic Compounds Flashcards

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1
Q

What IS organic chemistry?

A

The chemistry of carbon compounds

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2
Q

What’s another word for organic chemistry?

A

Carbon chemistry

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3
Q

How many carbon compounds are there?

A

Millions, with the number increasing daily

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4
Q

What do carbon compounds contain in general?

A

Hydrogen

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5
Q

Name 2 compounds that do contain carbon but aren’t considered carbon compounds

A

CO2 and carbonates

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6
Q

Why are CO2 and carbonates not considered to be carbon compounds?

A

They don’t contain hydrogen

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7
Q

What are some elements often found in carbon compounds?

A

Nitrogen
Oxygen
Halogens
Sulphur
Phosphorus

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8
Q

Why does carbon form so many compounds?

A
  1. Carbon is in group IV in the periodic table and has 4 electrons in its outer shell
    When forming compounds, they’re covalent compounds
    Carbon forms 4 covalent bonds in its compounds to achieve a stable electronic structure
  2. Carbon forms strong covalent bonds with itself and hydrogen atoms - stable and resistant to oxidation and hydrolysis
    Extremely high activation energy needs to be overcome
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9
Q

What are the C-C bonds that carbon forms found in?

A

Chain and ring systems

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10
Q

Describe organic reactions and explain why they’re like this

A

Generally slow
Poor yields

Extremely high activation energy needs to be overcome

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11
Q

Why are organic reactions slow and have poor yields?

A

Strong C-C bonds

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12
Q

What are the 4 different types of formulae we can use to represent organic compounds?

A

Molecular, graphic shortened and skeletal structural formulae

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13
Q

What does a molecule formula show?

A

The actual amount of atoms of each element in a molecule

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14
Q

Describe how molecular formulae are set out

A

Symbol for the element with subscripts to show how many of each atom in the molecule

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15
Q

In which order do we write the elements in a molecular formula?

A

C, H, O
then alphabetical

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16
Q

What do molecular formulae NOT show us?

A

HOW atoms are bonded

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17
Q

What is a graphic structural formula?

A

Displayed structural formula

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18
Q

What does a graphic structural formula show?

A

How elements are bonded and the types of bonds

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19
Q

What does a single line represent in graphic structural formulae?

A

A single covalent bond

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20
Q

What does a double line represent in graphic structural formulae?

A

Double covalent bond

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21
Q

How many bonds must carbon form? Describe these

A

4
Can be single, double or triple
With itself or other elements

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22
Q

What’s another type of bond that carbon forms and in what type of compounds are these formed?

A

Delocalised bonds
Aromantic

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23
Q

What type of bonds do aromantic compounds have?

A

Delocalised bonds

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24
Q

What type of compounds contain delocalised bonds?

A

Aromantic

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25
Q

What do shortened structural formulae show?

A

The graphic structural formula as a shortened structural formula
(Slightly different to molecular formulae)

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26
Q

What are skeletal structural formulae?

A

Shorthand representation of a compound’s molecular structure

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27
Q

Why are skeletal structural formulae useful?

A

Show complicated structures clearly
Quick and simple to draw

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28
Q

What’s implicit on a skeletal structural formula?

A

The location of the carbon atoms with hydrogens bonded

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29
Q

Where are carbon atoms implied to exist on skeletal structural formulae?

A

At each vertex (the second the pen touches the paper is one)

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30
Q

How do we figure out the number of hydrogen atoms from a skeletal structural formula? Why?

A

4 - (number of bonds drawn to that carbon)
Carbon has 4 covalent bonds

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31
Q

How do we represent hydrogen atoms bonded to non-carbon atoms in a skeletal structural formula? Give an example

A

Draw them explicitly
H bonded to O, for example

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32
Q

How do we signify all atoms that aren’t carbon or hydrogen on a skeletal structural formula?

A

With chemical symbols

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33
Q

Homologous series

A

Groups of related compounds

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34
Q

What’s the purpose of homologous series?

A

To make the study of the millions of carbon compounds easier

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35
Q

Draw the skeletal structural formula of propan-1-ol

A

(See notes)

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36
Q

Draw the skeletal structural formula of ethene

A

(See notes)

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37
Q

What’s ethene used for?

A

Used to make polymers

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38
Q

What’s ethanoic acid found in?

A

Vinegar

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39
Q

What type of acid is in vinegar?

A

Ethanoic

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40
Q

Name a compound used to make polymers

A

Ethene

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41
Q

Draw the skeletal structural formula of propene

A

(See notes)

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42
Q

Draw the skeletal structural formula of ethanoic acid

A

(See notes)

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43
Q

In which case does a tip of a skeletal structural formula not count as a carbon atom?

A

If it has a completely different element like OH attached to it

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44
Q

What do you call the members of the family in a homologous series?

A

Homologues

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45
Q

Homologues

A

All in the same homologous series

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46
Q

What do members of the same homologous series all have?

A

The same functional group
The same general formula
Similar chemical properties
Gradually changing physical properties

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47
Q

Functional group

A

An element or group of elements responsible for the chemical properties/behaviour of the compound in a homologous series
Provides a reactive site

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48
Q

What provides a reactive site in a homogenous series?

A

Functional group

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49
Q

What’s organic chemistry largely the chemistry of?

A

Homologous series rather than individual compounds

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50
Q

Alkane…
Functional group
Systematic name
Example

A

(N/A)
-ane
Ethane

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51
Q

Alkene…
Functional group
Systematic name
Example

A

C=C
-ene
Ethene

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52
Q

Halogenoalkane…
Functional group
Systematic name
Example

A

-Fl, -Cl, -Br, -I
Fluoro, chloro, bromo, iodo
Chloroethane

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53
Q

Primary alcohol…
Functional group
Systematic name
Example

A

-CH2OH
-1-ol
Propan-1-ol

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54
Q

Secondary alcohol…
Functional group
Systematic name
Example

A

CH(OH)
-2-ol
Propan-2-ol

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55
Q

Carboxylic acid…
Functional group
Systematic name
Example

A

-COOH
-oic acid
Ethanoic acid

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56
Q

Aldehyde…
Functional group
Systematic name
Example

A

CHO
-al
Propanal

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57
Q

Ketone…
Functional group
Systematic name
Example

A

-co-
-one
Propanone

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58
Q

Ester…
Functional group
Systematic name
Example

A

-COO-
-oate
Ethyl propanote

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59
Q

Do you count the C in COOH in carboxylic acids?

A

Yes

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60
Q

How many double bonds between carbon atoms to alkenes have?

A

At least 1

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61
Q

General formula of alkanes

A

CnH2n+2

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62
Q

General formula of alkenes

A

CnH2n

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63
Q

Which homologous series is ethane a part of?

A

Alkanes

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64
Q

Which homologous series is ethene a part of?

A

Alkenes

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65
Q

Which homologous series is Chloroethane a part of?

A

Halogenoalkanes

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66
Q

Which homologous series is propan-1-ol a part of?

A

Primary alcohol

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67
Q

Which homologous series is ethanol a part of?

A

Primary alcohols

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68
Q

Which compounds are part of the primary alcohol homologous series but don’t have the usual systematic name?

A

Methanol and ethanol

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69
Q

Which homologous series is propan-2-ol a part of?

A

Secondary alcohols

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70
Q

Which homologous series is ethanoic acid a part of?

A

Carboxylic acids

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71
Q

Which homologous series is propanal a part of?

A

Aldehydes

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72
Q

Which homologous series is propanone a part of?

A

Ketones

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73
Q

Which homologous series is ethyl propanoate a part of?

A

Esters

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74
Q

Describe the activity of alkanes

A

Largely inactive

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75
Q

Name 2 reactions in which alkanes actually do undergo?

A

Combustion
Cracking

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76
Q

Do alkanes have any double bonds? What does this mean for them?

A

No
They’re saturated

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77
Q

Give an example of a ketone

A

Acetone (nail varnish remover)

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78
Q

Name for carbon chain compounds

A

Aliphatic compounds

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79
Q

Aliphatic compounds

A

Carbon chain compounds

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80
Q

What are carbon chain compounds named after?

A

The parent alkane

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81
Q

What are the steps to naming an organic compound?

A
  1. Largest carbon chain is found - work out the parent alkane
  2. The functional group is found (going to be from the table)
  3. Any side groups (radicals) are found
  4. Assign a number to each carbon atom in the longest chain to find the position of the functional groups or side groups. Always use the lowest numbers possible.
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82
Q

What do we always use as the number for the positioning of the side groups in an organic compound?

A

The smallest number from the end

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83
Q

Parent alkane if the longest carbon chain is 1 carbon atom long

A

Methane

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84
Q

Parent alkane if the longest carbon chain is 2 carbon atoms long

A

Ethane

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85
Q

Parent alkane if the longest carbon chain is 3 carbon atoms long

A

Propane

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86
Q

Parent alkane if the longest carbon chain is 4 carbon atoms long

A

Butane

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87
Q

Parent alkane if the longest carbon chain is 5 carbon atoms long

A

Pentane

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88
Q

Parent alkane if the longest carbon chain is 6 carbon atoms long

A

Hexane

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89
Q

Name given to the side groups of organic compounds

A

Branching

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90
Q

What is the root name and radical of the side group of formula CH3?

A

Methane
Methyl

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91
Q

What is the root name and radical of the side group of formula CH3CH2?

A

Ethane
Ethyl

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92
Q

What is the root name and radical of the side group of formula CH3CH2CH2?

A

Propane
Propyl

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93
Q

Formula of radical methyl

A

CH3

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94
Q

Formula of radical ethyl

A

CH3CH2

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95
Q

Formula of radical propyl

A

CH3CH2CH2

96
Q

Draw the skeletal structural diagram for 2-methylpropane

A

(See notes) - in the naming section

97
Q

Draw the skeletal structural formula of 2-bromobutane

A

(See notes) - in naming section

98
Q

Draw the skeletal structural formula of 2methylpropan-1ol

A

(See notes) - in naming section

99
Q

Where do we place the number in the name of a compound when specifying the position of a double bond?

A

Between the word

100
Q

When do we place the number between the word in an organic compounds name?

A

When specifying the position of a double bond

101
Q

Do we count the carbon atoms in side groups?

A

No

102
Q

When don’t we count the carbon atoms of a compound?

A

If it’s part of a side group

103
Q

Draw the side group of a compound in skeletal structural formula, for example for 2-methylpropane

A

(See notes) - in naming section

104
Q

Draw the graphic structural formula of trichloroethene

A

(See notes)

105
Q

Um jw en Owen 96 gw en

A

F

106
Q

What do molecular formulae of an organic compound not give information about in terms of atoms in a molecule?

A

Their arrangement

107
Q

Isomers

A

Molecules with the same formula with different structures

108
Q

Structural isomers

A

Have the same molecular formula but different structural formulae

109
Q

What can structural isomers be found in?

A

Substances with the same functional group
Substances with different functional groups

110
Q

Show the isomers of butane - what’s significant about them?

A

(See notes)
Both have the same functional group

111
Q

Name substances that have isomers yet have different functional groups

A

Carboxylic acids and esters

112
Q

What’s similar and what’s different between carboxylic acids and esters? Give an example

A

Same molecular formulae
Very different elements e.g -
Ethanoic acid - sour, bitter smell
Methyl methanoate (ester) - sweet smell

113
Q

What do E-Z isomers appear in?

A

Alkenes

114
Q

What type of bonds are significant in alkenes?

A

C=C bond

115
Q

What are alkenes due to the C=C bond that they possess?

A

Unsaturated

116
Q

What can single bonds do in a saturated molecule and what does this mean for them?

A

No double bonds - can freely rotate
Atoms in the bond are interchangeable

117
Q

What cannot occur in unsaturated molecules with double bonds and why?

A

There is no free rotation due to the double C=C bond
The pi bond in an alkene prevents the rotation - we can’t interchange the atoms

118
Q

What prevents the rotation of atoms in alkenes?

A

The pi bond prevents the rotation

119
Q

Are alkenes saturated or unsaturated and why?

A

Unsaturated due to the presence of the double C=C bond

120
Q

What type of isomers occur in alkenes?

A

E-Z isomers

121
Q

E-Z molecules

A

Same old ulnar and structural formula,but different spatial arrangement of atoms

122
Q

What’s an E molecule?

A

Both prioritised atoms on the different side of the double bond

123
Q

What’s a Z-molecule?

A

Both prioritised atoms on the same side of the double bond

124
Q

How do we remember that the prioritise atoms on a Z-molecule are on the same side?

A

“Zame zide”

125
Q

What do we prioritise atoms in terms of when describing E-Z isomers?

A

Atomic mass

126
Q

How did E-Z molecules get their name?

A

From the German…
E - entagen (opposite)
Z - zusammen (together)

127
Q

What must each carbon atom on the double bond have in order to form E-Z isomers?

A

2 different groups or atoms
(e.g - Br and H)

128
Q

What would imply that two isomers are NOT E-Z isomers?

A

2 atoms that are the same on the same side of the double bond

129
Q

What are the 2 types of bond in the double bond in ethene?

A

Covalent bond
Pi bond

130
Q

How does the covalent bond in ethene form?

A

By direct overlap of two orbitals

131
Q

How does the pi bond in ethene form?

A

By the sideways overlap of two px orbitals

132
Q

What do both the covalent bond and the pi bond result in?

A

A bond which can be imagined to be a charge cloud above and below the plane of the molecule

133
Q

Draw a diagram to represent the nature of the pi bond in ethene

A

(See notes)

134
Q

Draw the skeletal structural formula of 2-methylpropan

A

(See notes) - in naming section

135
Q

Draw 2-2-dimethylbutane

A

(see notes)

136
Q

What are the 3 types of reagents in organic chemistry?

A

Radicals
Nucleophiles
Electrophiles

137
Q

When do radicals form?

A

When a covalent bond breaks

138
Q

What is a radical reagent?

A

When a covalent bonds breaks, each atom/species retains one electron from the bond
The species which form are free radicals

139
Q

Properties of radicals

A

Have an unpaired electron
Are very reactive, and react with other free radicals or atoms
Reactions involving free radicals are extremely rapid

140
Q

Name 3 typical reactions that involve free radicals

A

Photochlorination of methane
Alkene polymerisation
Cracking and ozone depletion

141
Q

Give 3 typical free radicals

A

Cl•
Cl3•
CH3CH2•

142
Q

What is the symbol for a free radical?

A

•
(At the top)

143
Q

What do you get when you crack a large alkane?

A

Free radicals

144
Q

Hat can break up chlorine molecules into free radicals?

A

Ultraviolet light

145
Q

What do some reagents that react with organic compounds seek out?

A

Centres of charge

146
Q

Why do organic molecules often contain centres of charge?

A

Due to the presence of polar covalent bonds or pi bonds

147
Q

Nucleophiles

A

Ions or molecules which can donate a lone pair of electrons, forming a covalent bond

148
Q

What are Nucleophiles attracted to?

A

Positive changes or positive centres of charge

149
Q

Give an example of a positive centre of charge

A

Nucleus

150
Q

What’s polar in a Halogenoalkane and what happens to it therefore?

A

The carbon-halogen bond is poalr
The Nucleophiles will attack the positive carbon centre

151
Q

Give some examples of typical Nucleophiles

A

OH-
Br-
CN-
H2O
NH3

152
Q

Which part of a Nucleophiles attracts other molecules?

A

The lone pairs of electrons

153
Q

How are Nucleophiles charged?

A

Either negatively or neutrally charged

154
Q

Elctrophiles

A

Ions or molecules which can accept a lone pair of electrons, forming a covalent bond

155
Q

What are electrophiles attracted to?

A

Negative charges or negative centres of charge

156
Q

What is the centre of negative charge in an alkene?

A

The pi bond

157
Q

What is the pi bond to an alkene?

A

A centre of negative charge

158
Q

What will an electrophile attack in an alkene?

A

The centre of negative charge, which is the pi bond

159
Q

Which homologous series gave centres of negative charge that electrophiles attack and what is this centre?

A

Alkenes
Pi bond

160
Q

Give some examples of typical electrophiles

A

H+
NO2+
Cl+

161
Q

How are electrophiles charged?

A

Positively

162
Q

What are the 5 types of reaction?

A

Addition
Substitution
Elimination
Oxidation/reduction (redox)
Hydrolysis

163
Q

What happens during an addition reaction?

A

2 molecules are brought together to produce 1 molecule

164
Q

Give an equation to represent addition reactions

A

A + B —> C

165
Q

What usually has to be available for an addition reaction to occur?

A

A double bond

166
Q

What type of reaction usually requires a double bond in order to occur?

A

Addition reaction

167
Q

What do alkenes always undergo? (Type of reaction)
Why?

A

Electrophilic addition
The C=C double bond is attacked

168
Q

Substitution reaction

A

An atom or group of atoms replace another atom or group of atoms in a molecule

169
Q

What normally has to be true after a substitution reaction?

A

The nature of the group which is introduces must be similar to that of the group which is replaced

170
Q

Give an equation to represent a substitution reaction

A

AB + C —> AC + B

171
Q

Give an example of a Nucleophiles substitution reaction

A

A hydroxide ion acting as a Nucleophile when it attacks the polar C-Br bond

172
Q

Which reaction is an example of free radical substitution?

A

The photochlorination of methane

173
Q

Why is the photochlorination of methane an example of free radical substitution?

A

Methane reacts with chlorine radicals

174
Q

Elimination reaction

A

A simple molecule such as water is eliminated from the molecule

175
Q

What often forms as a result of an elimination reaction?

A

A double bond

176
Q

In which type of reaction is a double bond usually formed?

A

Elimination

177
Q

What is an elimination reaction also known as if water is eliminated?

A

A dehydration reaction

178
Q

Dehydration reaction

A

Type of elimination reaction where water is eliminated

179
Q

Give an equation to represent an elimination reaction - what’s significant about this?

A

AB —> A + B
Opposite of addition reaction

180
Q

What are the 2 things that usually form during an elimination reaction?

A

Organic molecule with double bond
Small molecule

181
Q

Typical redox reaction example

A

Combustion

182
Q

What does a redox reaction consist of?

A

Both oxidation and reduction - we can’t have one without the other

183
Q

What rule can also be followed for determining which elements have been oxidised or reduced in a redox reaction as opposed to using OILRIG?

A

Oxidation
Gain of oxygen
Loss of hydrogen

Reduction
Loss of oxygen
Gain of hydrogen

184
Q

What is oxidation in terms of oxygen and hydrogen?

A

Gain of oxygen
Loss of hydrogen

185
Q

What is reduction in terms of oxygen and hydrogen?

A

Loss of oxygen
Gain of hydrogen

186
Q

What occurs to primary alcohols in redox reactions?

A

Total oxidation

187
Q

What happens to oxidising agents?

A

They’re reduced

188
Q

Hydrolysis

A

Chemical reaction between the organic compound and water

189
Q

Describe a hydrolysis reaction

A

Very slow and so usually require a catalyst

190
Q

Common catalysts used in hydrolysis reactions

A

Sodium hydroxide
Hydrochloric acid

191
Q

What type of hydrolysis reaction is one catalysed by sodium hydroxide?

A

Base catalysed

192
Q

What type of hydrolysis reaction is one catalysed by hydrochloric acid?

A

Acid catalysed

193
Q

What do empirical and molecular formulae show?

A

The ratio of atoms in the molecule
Actual number of atom in a molecule

194
Q

What are the steps to writing an empirical formula?

A

Write symbols
Write masses/percentages from question
Divide each mass/percentage by the mass number of that element (Ar)
Divide each answer by the smallest number to find the ratio
(Do NOT round up/down ratios at the end - multiply everything up into whole numbers if they’re in decimals)

195
Q

What do we NOT do at the end when working out empirical formulae and what do we do instead?

A

Round up/down
Multiply everything up into whole numbers

196
Q

What are the steps to working out a molecular formula from an empirical formula?

A

Relative molecular mass (in question)
—————————————————. = a multiple
Mr of empirical formula

Multiply every atom of the empirical formula by this

197
Q

What do we need to be given in the question in order to calculate the molecular formula from an empirical formula?

A

The relative molecular mass

198
Q

How do we order the side groups in the name of a compound if there’s more than one of them?

A

Put them in alphabetical order

199
Q

How are the particles held together in a solid?

A

Rigidly

200
Q

How can the particles of a solid vibrate?

A

They’re rigid - can only vibrate around a fixed position

201
Q

What must happen for a solid to melt?

A

Forces that hold it rigidly must be overcome

202
Q

How are the particles in a liquid difference to those in a solid?

A

Less order, held together less rigidly and particles are further apart

203
Q

What’s important about the particles of a liquid, even though there’s less order and they’re further apart than in a solid?

A

There;s still significant attractive forces to overcome when changing into a gas

204
Q

What is needed to overcome the forces between particles in a solid or liquid when it melts or boiled?

A

Forces

205
Q

How are the forces in a solid or liquid usually overcome to cause a substance to melt or boil?

A

Using energy, that’s usually heat/latent heat

206
Q

How can we product which substance has the higher melting or boiling point?

A

Look at the strength of the forces between particles

207
Q

What type of molecules are hydrocarbons?

A

Simple covalent molecules

208
Q

What are the only things that hydrocarbons consist of?

A

Hydrogen and carbon atoms

209
Q

Are hydrocarbons polar or non-polar? Why?

A

Non-polar
Electronegativities of carbon and hydrogen are similar

210
Q

What’s the only type of force present in hydrocarbons and why?

A

Temporary dipole-temporary dipole (Van der Waal forces)
Hydrocarbons are non-polar

211
Q

What’s significant about the Van der Waal forces in a hydrocarbon?

A

Weak intermolecular forces that require little energy to overcome

212
Q

Where do Van der Waal forces act on hydrocarbons?

A

Between the surfaces of the molecules

213
Q

When will the Van der Waal forces of molecules act more?

A

The more surface that’s in contact, the more the forces will act

214
Q

What does more hydrocarbon surface in contact mean for their boiling point?

A

More surface in contact = more the forces will act
=more energy needed to overcome the forces
=higher melting and boiling points

215
Q

What is the relationship between the amount of surface in contact between molecules and their boiling points?

A

More surface in contact = higher melting and boiling points
(Forces act more = more energy required to overcome the forces)

216
Q

What’s the relationship between the amount of carbon atoms a hydrocarbon has and it’s boiling point? Why?

A

More carbon atoms = increased boiling point
(Van der Waal attractions increases)

217
Q

What’s the relationship between the relate molecular mass of a hydrocarbon and its boiling point? Why?

A

Higher relative molecular mass = higher boiling point
(More carbon atoms = Van der Waal attractions increase)

218
Q

What else can have an impact on the boiling temperature of a hydrocarbon apart from the chain length?

A

Branching

219
Q

What effect do different structural isomers have on hydrocarbons?

A

Give them different boiling points

220
Q

Why do different structural isomers of hydrocarbons give them different boiling points?

A

Difference surface areas are in contact for different isomers

221
Q

What do more branches do to the shape of a molecule?

A

More branches = more spherical molecule

222
Q

What happens to the amount of surface area for contact in molecules if spheres are packed together?

A

The surface area available for surface area contact is very small

223
Q

What’s good about sausage shaped molecules?

A

Much more surface area available for surface area contact compared to spherical molecules

224
Q

What effect does the branching of an isomer have on an isomer and why?

A

More branches = more like a sphere = surface area available for surface area contact is very small = weaker Van der Waal forces = lower boiling temperature

225
Q

What type of hydrocarbons are often used in the oil industry and why?

A

Branched
More spherical = less surface area available for surface area contact = lower boiling temperature

226
Q

Which group do alcohols contain?

A

OH group

227
Q

What does the OH group in alcohols cause and what does this lead to?

A

Hydrogen bonds
Increased boiling point

228
Q

Why does having an OH group in an alcohol lead to an increase in their boiling points?

A

Hydrogen bonds are formed, which are stronger than Van der Waal forces

229
Q

What does having hydrogen bonds in a hydrocarbon lead to?

A

Increased boiling point
More soluble in water

230
Q

Parent Alkane if the longest carbon chain has 7 atoms

A

Heptane

231
Q

What’s the difference in naming the AMOUNT vs the POSITIONING of side groups on hydrocarbons?

A

di, tri… = the amount of side groups
2,3… (numbers) = the positioning of side groups

232
Q

How would we show that the %’s of elements in an alkane are consistent with its formula?

A

Mr of formula
Ar (from formula) of each element divided by Mr - the %’s should match up

233
Q

Which phrase should you always add at the end after describing which compounds have the lowest boiling point?

A

“so less energy is needed to separate the molecules”1

234
Q

Free radial definition

A

A species with an unpaired electron

235
Q

Why do chlorine radicals for but fluorine radicals don’t?

A

C-F bond is stronger than C-Cl bond

236
Q

What must be true for E-Z isomerism to occur?

A

Both carbon atoms on the double bond must have 2 different groups or atoms

237
Q

What do we need to show when drawing nucleophies?

A

Lone pairs of electrons

A level Chemistry (39 decks)

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