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B3 organics Flashcards

1
Q

How are two numbers separated in organic nomenclature?

A

Comma

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2
Q

How are numbers and letters separated 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

What is the general formula of alkyl groups?

A

CnH(2n+1)

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6
Q

What is the six carbon prefix?

A

Hex

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7
Q

What is the seven carbon prefix?

A

Hept

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8
Q

What is the nine carbon prefix?

A

Non

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9
Q

What is the 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 arranged 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

As a hexagon with a circle inside

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17
Q

What is the 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

Contains single carbon-carbon bonds only

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19
Q

What is an unsaturated compound?

A

Contains 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

one electron from the shared pair goes to each atom forming radicals

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22
Q

what does fission mean

A

splliting apart

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23
Q

Define heterolytic fission

A

both the shared electrons go to one atoms forming a positive and negative ions

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24
Q

Define radical

A

A species with an unpaired electron

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25
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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26
Q

What is the only type of covalent bond present in alkanes?

A

Sigma bonds

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27
Q

Why do alkanes have a low reactivity?

A

High bond enthalpy of the C-H and C-C bonds; low bond polarity of the C-H and C-C bonds

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28
Q

What is the general formula of alkanes?

A

C_nH_(2n+2)

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29
Q

What is the general formula of cyclic alkanes?

A

C_nH_(2n)

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30
Q

What bonds will be present in a single covalent bond?

A

A sigma bond

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31
Q

What bonds will be present in a double covalent bond?

A

One sigma bond, one pi bond

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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

Ways to compare sigma and pi bonds

A
  • Orbital overlap
  • Bond enthalpy
  • Electron density
  • Rotation
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34
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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35
Q

Sigma vs Pi: Electron density

A

Sigma have a much higher electron density than pi bonds

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36
Q

Sigma vs Pi: Rotation

A

Sigma have free rotation; pi have restricted rotation

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37
Q

Sigma vs Pi: Bond enthalpy

A

Sigma have a higher bond enthalpy so are stronger; pi have a lower bond enthalpy so are weaker

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38
Q

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

A

increased chain length = higher BP

more carbon atoms
more electrons
stronger London forces
more energy required to overcome

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39
Q

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

A

More branched carbon chain means smaller surface area for contact of London forces acting between molecules

less surface contact

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40
Q

What is the word equation for alkane complete combustion?

A

Alkane + O2 -> CO2 + H2O

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41
Q

What is the word equation for alkane incomplete combustion?

A

Alkane + O2 -> CO + H2O

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42
Q

Why is alkane incomplete combustion hazardous?

A

Produces carbon monoxide which is toxic

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43
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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44
Q

What is the initiation step for chlorine and butane in Free Radical Substitution?

A

Cl2 -> 2Cl*

uv light across arrow

production of radicals

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45
Q

What are the propagation steps for chlorine and butane in Free Radical Substitution?

A

Cl* + C4H10 -> C4H9Cl + HCl
C4H9* + Cl2 -> C4H9Cl + Cl*

production of new radicals from existing ones

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46
Q

What are the termination steps for chlorine and butane in Free Radical Substitution?

A

Cl* + Cl* -> Cl2
C4H9* + Cl* -> C4H9Cl
C4H9* + C4H9* -> C8H18

removes radicals

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47
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

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48
Q

explain why radical subtraction is likely to produce a mixture of organic products

A

substitution can replace any H atom

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49
Q

structural isomer

A

same molecular different structural formula

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50
Q

When do the alkanes react with halogens? How could you prove this?

A
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51
Q

limitation of termination

A

produces unwanted products - require further separation

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52
Q

issues with combustion

A

sulphur impurities - so2 - acid rain

N2 and )2 in the heat of an engine - N02 - toxic

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53
Q

how can we solve issues with combustion

A

catalytic converters - turns toxic production into less toxic products

e.g. CO–> CO2

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54
Q

issues with C in imcomplete combustion

A

soot particulate
asthma
global dimming

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55
Q

issues with co2 in complete combustion

A

greenhouse gas
global warming
climate change

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56
Q

Alkanes do not react with most common reagents, they have a very low reactivity. Why?

A

no polar bonds
lack of functionality
saturated - only contain sigma bonds - very strong

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57
Q

What is the general formula for alkenes?

A

C_nH_(2n)

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58
Q

What is the functional group of alkenes?

A

C=C bond

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59
Q

Why are alkenes very reactive?

A

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

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60
Q

draw and label a pi bond

A
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61
Q

Define stereoisomers

A

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

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62
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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63
Q

When would an alkene not have stereoisomers?

A

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

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64
Q

In stereoisomerism, how do you decide on priority groups?

A

Group with highest atomic number

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65
Q

How to explain if an alkene is an E isomer?

A

Priority groups are on opposite sides

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66
Q

How to explain if an alkene is a Z isomer?

A

Priority groups are on the same side

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67
Q

When can Z-isomers be referred to as cis isomers?

A

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

68
Q

When can E isomers be referred to as trans isomers?

A

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

69
Q

Define electrophile

A

An electron pair acceptor

70
Q

What type of reaction is alkene to alkane?

A

Electrophilic addition

71
Q

What are the conditions and reagents for alkene to alkane?

A

Hydrogen; Nickel Catalyst

72
Q

Displayed formula equation for ethene to ethane

73
Q

Type of reaction for alkene to halogenalkane

A

electrophilic addition

74
Q

reagents and conditions for alkene to haloalkane

A

halogenation -room temp and halogen halide

or

gaseous hydrogen halide
room temp

addition reactions

75
Q

How are alkenes tested for?

A

Add bromine water; will be decolourised

76
Q

What is the mechanism for bromine + ethene?

A

Electrophilic addition mechanism

77
Q

What are the reagents and conditions to turn alkene to alcohol?

A

Phosphoric acid catalyst; Steam

78
Q

Displayed formula equation for Alkene to alcohol

79
Q

What is the most stable carbocation?

80
Q

What is the least stable carbocation?

81
Q

primary carbocation

82
Q

Secondary carbocation

83
Q

Tertiary carbocation

84
Q

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

A

The least stable

85
Q

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

A

The most stable carbocation

86
Q

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

87
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

88
Q

Displayed formula equation for addition polymerisation of ethene

89
Q

conditions for polymerisation

A

heat (high temp) and pressure and use of catalyst

90
Q

Why is combustion of addition polymers an issue

A

Results in formation of HCl and CO
Which are toxic

91
Q

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

A

Passing it through an alkali

92
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

93
Q

What is the functional group of the alcohol homologous series

A

-OH (hydroxyl)

94
Q

alcohol general formula

95
Q

primary alcohol

96
Q

secondary alcohol

97
Q

tertiary alcohol

98
Q

Describing primary alcohol

A

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

99
Q

Describing a secondary alcohol

A

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

100
Q

Describing tertiary alcohol

A

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

101
Q

Why are alcohols soluble

A

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

102
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

103
Q

Conditions, reagents and observations for primary alcohol oxidation to aldehydes

A

Potassium dichromate k2cr2O7
Sulfuric acid
Heat and distill
Potassium dichromate will turn orange to green

r-O-r

104
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

105
Q

Structural and displayed formula equation for primary alcohol oxidation to aldehyde

106
Q

suffix for aldehyde

107
Q

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

108
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

109
Q

C=O group name

110
Q

ketone suffix

111
Q

structural and displaced formula for alcohol to ketone

112
Q

What is the way in which tertiary alcohols must be oxidised?

A

Combustion

113
Q

What is the word equation for alcohol complete combustion?

A

Alcohol + O2 -> CO2 + H2O

114
Q

What is the word equation for alcohol incomplete combustion?

A

Alcohol + O2 -> CO + H2O

115
Q

Why is incomplete combustion of alcohols hazardous?

A

Produces carbon monoxide which is toxic

116
Q

What are the conditions and reagents for alcohols to alkenes?

A

Phosphoric acid; Heat

117
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

118
Q

What is the displayed formula equation for primary alcohol elimination to alkene?

119
Q

Why will secondary and tertiary alcohols be able to produce multiple products?

A

The C=C bond can form from two carbons; they could have E/Z isomerism

120
Q

conditions and reagents for alcohol to haloalkane

A

Sodium halide
Sulfuric acid

121
Q

What type of reaction is alcohol to haloalkane

A

Nucleophillic Substitution

122
Q

Displayed formula equation for alcohol to haloalkane

123
Q

Type of reaction from haloalkane to alcohol

A

Nucleophillic substitution

124
Q

Conditions and reagents for haloalkane to alcohol

A

Warm NaOH
Acid catalyst (sulfuric acid)
Heat under reflux

125
Q

Mechanism for nucleophillic substiution of haloalkane to alcohol

126
Q

Define nucleophile

A

An electron pair donor

127
Q

How to measure reactivity of haloalkanes experimentally, and what is the result?

A

Add AgNO3 and ethanol; the iodo-compound will take the shortest time to form a precipitate

128
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

129
Q

What is a CFC?

A

A molecule containing carbon, fluorine, and chlorine

130
Q

What are the primary properties of CFCs?

A
  • Non-toxic
  • Volatile
  • Low reactivity
131
Q

Which bond is the strongest among C-Cl, C-Br, and C-I?

A

C-Cl bond

The order of bond strength is C-Cl > C-Br > C-I.

132
Q

Which bond has the highest bond enthalpy?

A

C-Cl bond

The bond enthalpy order is C-Cl > C-Br > C-I.

133
Q

What is required to break the C-Br bond compared to the C-I bond?

A

More energy is required

C-Br bond requires more energy to break than C-I bond.

134
Q

Define a CFC.

A

A molecule containing carbon, fluorine, and chlorine.

135
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

136
Q

What happens to CFCs in the presence of UV radiation?

A

They can produce radicals.

137
Q

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

A
  • Chlorine radicals
  • Nitrogen oxide radicals
138
Q

What is the initiation stage for ozone breakdown?

139
Q

What are the propagation stages for ozone breakdown?

140
Q

What is the overall equation for ozone breakdown?

141
Q

How are nitrogen oxides created?

A

Thunderstorms and aircraft.

142
Q

What equations show how nitrogen oxide radicals breakdown ozone?

143
Q

What is the order of practical techniques to purify a substance?

A
  • Heat under reflux or distil
  • Separation
  • Drying
  • Re-distillation
144
Q

What is the benefit of heating under reflux?

A

Prevents any substances escaping.

145
Q

What is the benefit of distillation?

A

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

146
Q

Labelled diagram of heating under reflux

147
Q

Labelled diagram of distillation

148
Q

Describe purification by separation if the organic layer is less dense than the aqueous layer.

A

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

149
Q

Describe purification by separation if the organic layer is more dense than the aqueous layer.

A

Use separating funnel, remove desired bottom organic layer.

150
Q

Describe purification by drying.

A

Add anhydrous salt to organic layer, such as anhydrous CaCl2 or anhydrous MgSO4.

151
Q

Describe purification by redistillation.

A

Redistill and collect fraction distilling at XYZ°C.

152
Q

Define a functional group.

A

A group of atoms responsible for the molecule’s chemical properties and reactions.

153
Q

alkene to halokakene observations

A

orange to colourless

154
Q

state 2 methods of disposing polymers that can benefit environment

A
  • broken down into smallr useful organic compounds for energy produictiopnn
  • combustion for energy
  • other useful organic products
155
Q

what measurement and observation would allow the student to compare the rate of hydrolysis

A

time for Ppt to appear

156
Q

set up apparatus for preparation, and pure sample from reaction mixture

A
  • put reactant into pear shaped flask
  • anti bumping granules
  • dont stopper flask
  • attach condenser vertically to the flask so that water flows into condenser from Botton and out top - ensure always full of cold water
  • heat until boils gently
  • purification - use separating funnel
  • drying using anhydrous salt
  • redistil - 102 degrees c
157
Q

explain the difference in rate of hydrlosysis of br and I and which Ppt one would form faster

A

c-I bonds weaker than c- Br

AgI - yellow

158
Q

homogenous series

159
Q

general formaula

160
Q

carbon double bond has

A

1 pi bond
1 sigma bond

161
Q

aliphatic

A

carbon atoms joins to each other in unbranched or branched chain

(not benzene)

162
Q

benzene is

163
Q

ketone

A

— c=0 —

164
Q

alcohol oxidisded to form ketone

165
Q

E

Chemistry (18 decks)

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