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A-LEVEL CHEMISTRY > B3 Organic Chemistry I > Flashcards

B3 Organic Chemistry I Flashcards

1
Q

How are two numbers seperated in organic nomenclature

A

Comma

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2
Q

How are numbers and letters seperated in organic nomenclature

A

Dash

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3
Q

Which carbon number does the highest priority functional group get

A

The lowest carbon number

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4
Q

Where there are the same priority groups, which group gets the lowest carbon number

A

First group alphabetically

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5
Q

General formula of alkyl groups

A
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6
Q

Six carbon prefix

A

Hex

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7
Q

Seven carbon prefix

A

Hept

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8
Q

Nine carbon prefix

A

Non

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9
Q

Ten carbon prefix

A

Dec

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10
Q

Define empirical formula

A

The simplest whole number ratio of atoms of each element present in a compound

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11
Q

Define molecular formula

A

The total number of atoms of each element present in a molecule

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12
Q

Define homologous series

A
  • A series of organic compounds with the same functional group
  • But with each successive member differing by CH2
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13
Q

What is an aliphatic compound

A
  • Contains hydrogen and carbon atoms
  • Joined in a straight chain, branched chain, or non-aromatic ring
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14
Q

What is an alicyclic compound

A
  • An aliphatic compound
  • Arragned in non-aromatic rings
  • With or without side chains, but no benzene ring
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15
Q

What is an aromatic compound

A

Contains a benzene ring

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16
Q

How are benzene rings drawn

A
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17
Q

Relationship between compounds being alicyclic and aliphatic

A
  • All alicyclic are aliphatic
  • Not all aliphatic are alicyclic
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18
Q

What is a saturated compound

A

Contain single carbon-carbon bonds only

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19
Q

What is an unsaturated compound

A

Contain multiple carbon-carbon bonds

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20
Q

Define structural isomers

A

Compounds with the same molecular formula, but different structural formulae

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21
Q

Define homolytic fission

A

Each bonding atom recieves one electron from the bonded pair, forming two radicals

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22
Q

Define heterolytic fission

A

One bonding atom recieves both electrons from the bonded pair, forming an ion

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23
Q

Define radical

A

A species with an unpaired electron

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24
Q

Define Curly Arrow

A

The movement of a pair of electrons, showing either heterolytic fission, or the formation of a covalent bond

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25
Q

What is the only type of covalent bond present in alkanes

A

Sigma bonds

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26
Q

Why do alkanes have a low reactivity

A
  • High bond enthalpy of the C-H and C-C bonds
  • Low bond polatiry of the C-H and C-C bonds
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27
Q

General formula of alkanes

A
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28
Q

General formula of cyclic alkanes

A
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29
Q

What bonds will be present in a single covalent bond

A

A sigma bond

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30
Q

What bonds will be present in a double covalent bond

A

One sigma bond, one pi bond

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31
Q

Ways to comapre sigma and pi bonds

A
  • Orbital overlap
  • Bond enthalpy
  • Electron density
  • Rotation
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32
Q

What bonds will be present in a triple covalent bond

A

One sigma bond, two pi bonds

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33
Q

Sigma vs Pi: Orbital overlap

A
  • Orbitals overlap directly between bonding atoms in sigma
  • Sideways overlap of adjacent p-orbitals above and below the bonding atoms in pi
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34
Q

Sigma vs Pi: Electron density

A

Sigma have a much higher electron density than pi bonds

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35
Q

Sigma vs Pi: Rotation

A
  • Sigma have free rotation
  • Pi have restricted roation
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36
Q

Sigma vs Pi: Bond enthalpy

A
  • Sigma have a higher bond enthlapy so are stronger
  • Pi have a lower bond enthalpy so are weaker
  • More energy is requred to break sigma bond than pi bond
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37
Q

Explain why a longer carbon chain alkane has a higher boiling boint than a shorter carbon chain alkane

A
  • Longer carbon chain means larger surface area for contact of London forces acting between molecules
  • London forces therefore stronger
  • More energy required to break London forces
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38
Q

Explain why the more branched an alkane’s carbon chain is, the lower it’s boiling point

A
  • More branched carbon chain means smaller surface area for contact of London forces acting between molecules
  • Weaker London forces
  • Less energy requreid to break London forces
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39
Q

Word equation for alkane complete combustion

A
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40
Q

Word equation for alkane incomplete combustion

A

Produces Carbon Monoxide which is toxic

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41
Q

Why is alkane incomplete combustion hazardous

A

Produces carbon monoxide which is toxic

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42
Q

What condition is required for Free Radical Substitution and why

A
  • UV Light
  • Provides energy to break covalent bond (homolytic fission)
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43
Q

Free Radical Substitution: initation step for chlorine and butane

A
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44
Q

Free Radical Substitution: propagation steps for chlorine and butane

A
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45
Q

Free Radical Substitution: Termination steps for chlorine and butane

A
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46
Q

Why is Free Radical Substitution limiting to produce a desired product

A
  • Substitution can replace any hydrogen atom in any position along carbon chain
  • Further substitution can occur
  • There is more than one termination step, so more than one termination products
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47
Q

General formula for alkenes

A
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48
Q

Functional group of alkenes

A

C=C bond

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49
Q

Why are alkenes very reactive

A

The pi bond in the C=C bond has a low bond enthalpy

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50
Q

Draw a labelled diagram of a pi bond

A
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51
Q

Define stereoisomers

A

Compounds with the same structural formula, but with a different arrangement in space

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52
Q

When can E/Z isomerism occur in alkenes

A

When each carbon involved in the C=C bond, has two different groups bonded to it

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53
Q

When would an alkene not have steroisomers

A

If one/both the carbons involved in the C=C bond has two of the same groups attached

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54
Q

In stereoisomerism, how do you decide on priority groups

A

Group with highest atomic number

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55
Q

How to explain if an alkene is an E isomer

A
  • X is priority group over Y on left hand side carbon involved in the C=C bond
  • A is priority group over B on the right hand side carbon involved in the C=C bond
  • Prioritry groups are on opposite sides
56
Q

How to explain if an alkene is a Z isomer

A
  • X is priority group over Y on the left hand side carbon involved in the C=C bond
  • A is priority group over B on the right hand side carbon involved in the C=C bond
  • Priority groups are on the same side
57
Q

When can Z-isomers be reffered to as cis isomers

A

As long as there is a hydrogen on each carbon atom of the C=C bond

58
Q

When can E isomers be reffered to as trans isomers

A

As long as there is a hydrogen on each carbon atom of the C=C bond

59
Q

Define electrophile

A

An electron pair acceptor

60
Q

What type of reaction is alkene to alkane

A

Electrophillic addition

61
Q

Conditions and reagents for alkene to alkane

A
  • Hydrogen
  • Nickel Catalyst
62
Q

Displayed formula equation for ethene to ethane

A
63
Q

Type of reaction for alkene to halogenoalkane

A

Electrophillic addition

64
Q

How are alkenes tested for

A
  • Add bromine water
  • Will be decolourised
65
Q

Mechanism for bromine + ethene

A
66
Q

Reagents and conditions to turn alkene to alcohol

A
  • Phosphoric acid catalyst
  • Steam
67
Q

Displayed formula equation for alkene to alcohol

A
68
Q

What is the most stable carbocation

A

Tertiary

69
Q

What is the least stable carbocation

A

Primary

70
Q

Primary Carbocation

A
71
Q

Secondary carbocation

A
72
Q

Tertiary carbocation

A
73
Q

In alkene reactions with hydrogen halides, to which carbocation will the hydrogen to go

A

The least stable

74
Q

In alkene reactions with hydrogen halides, to which carbocation will the nucleophile (halogen) to go

A

The most stable carbocation

75
Q

Draw the mechanism for an alkene reaction with hydrogen halide, including both major and minor products

A
76
Q

Explain the three ways in which addition polymers can be destoryed

A
  • Combustion - releases lots of energy for electricity
  • Organic feedstock for production of other polymers
  • Recycling
77
Q

Displayed formula equation for addition polymerisation of ethene

A
78
Q

Why is combustion of addition polymers an issue

A
  • Results in formation of HCl and CO
  • Which are toxic
79
Q

How can HCl be removed as a product from combusting addition polymers

A

Passing it through an alkali

80
Q

Why are biodegradeable and photodegradable polymers more beneficial to the enviroment

A
  • As they don’t need to be incinerates
  • So there is no formation of HCl and CO
  • Which are toxic
81
Q

What is the functional group of the alcohol homologous series

A

-OH (hydroxyl)

82
Q

Alcohol general formula

A
83
Q

Primary alcohol

A
84
Q

Secondary alcohol

A
85
Q

Tertiary alcohol

A
86
Q

Describing primary alcohol

A

If the carbon the -OH group is bonded to has two hydrogens bonded to it

87
Q

Describing a secondary alcohol

A

If the carbon the -OH is bonded to has one hydrogen bonded to it

88
Q

Describing tertiary alcohol

A

If the carbon the -OH group is bonded to has no hydrogens bonded to it

89
Q

Why are alcohols soluble

A
  • They contain an -OH (hydroxyl) group
  • The -OH group can form hydrogen bonds with the water
90
Q

Why do alcohols have higher boiling points than other homologous series

A
  • They contain an -OH (hydroxyl) group
  • The -OH group can form hydrogen bonds with other molecules
  • More energy is needed to break the hydrogen bonds than the London Forces in other homologous series
91
Q

Conditions, reagents and observations for primary alcohol oxidation to aldehydes

A
  • Potassium dichromate
  • Sulfuric acid
  • Heat and distill
  • Potassium dichromate will turn orange to green
92
Q

Conditions, reagents and observations for primary alcohol oxidation to carboxylic acid

A
  • Add pottassium dichromate
  • Sulfuric Acid
  • Heat under reflux
  • Potassium dichromate will turn orange to green
93
Q

Structural and displayed formula equation for primary alcohol oxidation to aldehyde

A
94
Q

Suffix for aldehyde

A

-anal

95
Q

Structural and displayed formula equation for primary alcohol oxidation to carboxylic acid

A
96
Q

Conditions, observations and reagents for secondary alcohol oxidation to ketone

A
  • Potassium dichormate
  • Sulfuric Acid
  • Heat under reflux
  • Potassium dichromate will turn orange to green
97
Q

C=O group name

A

Carbonyl

98
Q

Ketone suffix

A

-one

99
Q

Strucutral and displayed formula for alcohol to ketone

A
100
Q

What is the way in which tertiary alcohols must be oxidised

A

Combustion

101
Q

Word equation alcohol complete combustion

A
102
Q

Word equation alcohol incomplete combustion

A
103
Q

Why is incomplete combustion of alcohols hazardous

A

Produces carbon monoxide which is toxic

104
Q

Reagents and conditions for alcohols to alkenes

A
  • Phosphoric acid
  • Heat
105
Q

Why is there only one possible product of primary alcohol elimination to alkene

A

The C=C bond can only from from one carbon

106
Q

Displayed formula equation primary alcohol elimination to alkene

A
107
Q

Why will secondary and tertiary alcohols be able to produce multiple products, and what will they be

A
  • The C=C bond can form from two carbons
  • They could have E/Z isomerism
108
Q

Conditions and reagents for alcohol to haloalkane

A
  • Sodium halide
  • Sulfuric acid
109
Q

What type of reaction is alcohol to haloalkane

A

Nucleophillic Substitution

110
Q

Displayed formula equation for alcohol to haloalkane

A
111
Q

```

Type of reaction from haloalkane to alcohol

A

Nucleophillic substitution

112
Q

Conditions and reagents for haloalkane to alcohol

A
  • Warm NaOH
  • Acid catalyst (sulfuric acid)
  • Heat under reflux
113
Q

Mechanism for nucleophillic substiution of haloalkane to alcohol

A
114
Q

Define nucleophille

A

An electron pair donor

115
Q

How to measure reactivity of haloalkanes experementally, and result

A
  • Add AgNO3 and ethanol
  • The iodo-compound will take the shortest time to form a precipitate
116
Q

Describe and explain the reactivity of the haloalkanes

A
  • C-Cl bond is strongest, then C-Br bond, then C-I bond is weakest
  • C-Cl bond has higher bond enthalpy, then C-Br bond, then C-I bond has lowest
  • More energy is required to break the C-Cl bond than the C-Br bond
  • More energy is required to break the C-Br bond than the C-I bond
117
Q

What is a CFC

A

A molecule containing, carbon, flourine and chlorine

118
Q

What are the primary properties of CFCs

A
  • Non-toxic
  • Volatile
  • Low reactivity
119
Q

What is the function of the ozone layer, and what equation shows how ozone’s concentration is maintained

A

Absorbs UV radiation, so that UV levels at the Earth’s surface are reduced

120
Q

What happens to CFCs in the presence of UV radiation

A

They can produce radicals

121
Q

What acts as a catalyst in the breakdown of the ozone layer

A

Chlorine radicals and nitrogen oxide radicals

122
Q

Initiation stage for ozone breakdown

A
123
Q

Propogation stages for ozone breakdown

A
124
Q

Overall equation for ozone breakdown

A
125
Q

How are nitrogen oxides created

A

Thunderstorms and aircraft

126
Q

Equations to show how nitrogen oxide radicals breakdown ozone

A
127
Q

Order of practical techniques to purify a substance

A
  • Heat under reflux or distil
  • Seperation
  • Drying
  • Re-distillation
128
Q

Benefit of heating under reflux

A

Prevnts any substances escaping

129
Q

Benefit of distillation

A

Can control a reaction by removing a product before it further reacts

130
Q

Labelled diagram of heating under reflux

A
131
Q

Labelled diagram of distillation

A
132
Q

Describe purification by seperation if organic layer is less dense than aqueous layer

A
  • Use a seperating funnel
  • Remove bottom layer
  • Keep desired top organic layer
  • As organic layer less dense than aqueous layer
133
Q

Describe purification by seperation if organic layer is more dense than aqueous layer

A
  • Use seperating funnel
  • Remove desired bottom organic layer
  • As organic layer more dense than aqueous layer
134
Q

Describe purification by drying

A
  • Add anhydrous salt to organic layer
  • Such as anhydrous CaCl2 or anhydrous MgSO4
135
Q

Describe purification by redistillation

A
  • Redistill
  • Collect fraction distilling at XYZc

A-LEVEL CHEMISTRY (9 decks)

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