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AS Chemistry > Topic 2 - Developing Fuels > Flashcards

Topic 2 - Developing Fuels Flashcards

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1
Q

Prefix for 1 carbon in a hydrocarbon

A

Meth-

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2
Q

Prefix for 2 carbons in a hydrocarbon

A

Eth-

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3
Q

Prefix for 3 carbons in a hydrocarbon

A

Prop-

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4
Q

Prefix for 4 carbons in a hydrocarbon

A

But-

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5
Q

Prefix for 5 carbons in a hydrocarbon

A

Pent-

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6
Q

Prefix for 6 carbons in a hydrocarbon

A

Hex-

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7
Q

Prefix for 7 carbons in a hydrocarbon

A

Sept-

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8
Q

Prefix for 8 carbons in a hydrocarbon

A

Oct-

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9
Q

Prefix for 9 carbons in a hydrocarbon

A

Non-

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10
Q

Prefix for 10 carbons in a hydrocarbon

A

Dec-

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11
Q

Suffix for alkanes

A

-ane

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12
Q

Suffix for alkenes

A

-ene

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13
Q

Prefix for rings

A

Cyclo-

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14
Q

Suffix for alcohols

A

-ol

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15
Q

Suffix for carboxylic acids

A

-oic acid

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16
Q

How to name chain alkane isomers

A

-Find name of longest chain
-Name of side chain
-Find which number of carbon side chain is attached to

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17
Q

Name structure of chain alkane isomers

A

Side chains (in alphabetical order), main chain

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18
Q

Define general formula

A

Represent any member of a homologous series

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19
Q

Define full structural formula

A

Shows all atoms and bonds in the compound

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20
Q

Define shortened structural formula

A

Does not show all/any bonds in the compound
e.g. CH3CH(CH3)CH3

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21
Q

Define skeletal formula

A

Represents the carbon-carbon bonds in the hydrocarbon

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22
Q

Define aromatic

A

Compounds containing one or more benzene rings

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23
Q

Define aliphatic

A

Compounds that do not contain benzene rings

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24
Q

Define structural isomers

A

Same molecular formula, but atoms are bonded in a different order

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25
Q

What are the different types of structural isomers?

A

-Chain isomer
-Position isomer
-Functional group isomer

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26
Q

Define chain isomer

A

Different lengths and branch positions

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27
Q

Define position isomer

A

Functional groups attached to different carbons

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28
Q

Define functional group isomer

A

Molecule has different functional groups

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29
Q

Define stereoisomer

A

Same molecular formula and structural formula but atoms are arranged differently in space

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30
Q

What are the different types of stereoisomers?

A

-Geometric isomers
-E/Z isomers
-Optical isomers

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31
Q

Define E/Z isomer

A

Molecule with a C=C bond that cannot rotate with different atoms attached to each carbon
Can also be called trans/cis isomers

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32
Q

Define optical isomer

A

Due to attachment of 4 different atoms/groups around a carbon atom

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33
Q

Define cracking

A

Process of taking longer hydrocarbons and breaking them into smaller (more useful) ones

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34
Q

What can hydrocarbons be cracked with?

A

-Steam and high pressure
-Aluminium oxide (catalyst) and high temperatures

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35
Q

What does geometric isomerism require?

A

-No rotation around C=C double bond
-Different atoms/groups attached to C=C

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36
Q

Define standard state

A

Physical state of a substance under standard conditions

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37
Q

What are the standard conditions?

A

-Pressure: 101kPa
-Temperature: 298K
-Reactions with aqueous solutions:
1 mol dm^-3

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38
Q

Define enthalpy change of combustion (ΔHcθ)

A

Energy required for 1 mile of a substance to completely combust under standard conditions

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39
Q

How can ΔHcθ be measured?

A

q=mcΔT

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40
Q

Define enthalpy change of reaction (ΔHrθ)

A

Molar quantities of reactants stayed in the equation react under standard conditions with reactants and products in standard states

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41
Q

Assumptions for ΔHrθ

A

-Treat all specific heat capacities as water (4.18)
-Assume densities of all solutions as the density of water
-Reaction goes to completion with no other reactions occurring

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42
Q

Equation for bond enthalpy

A

ΔH = ΣEnthalpy of bonds broken - ΣEnthalpy of bonds made

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43
Q

Qualities of endothermic reactions

A

-Bonds made
-Requires energy
Positive ΔH

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44
Q

Qualities of exothermic reactions

A

-Bonds broken
-Releases energy
-Negative ΔH

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45
Q

Define average bond enthalpy

A

Since bonds of the same type do not have the same amount of energy the average of energy for all bonds taken

46
Q

What does a shorter bond mean for bond enthalpy?

A

Higher bond enthalpy

47
Q

What does a high electron density mean for bond enthalpy?

A

Higher bond enthalpy - shorter bond

48
Q

Define enthalpy change of neutralisation (ΔHneutθ)

A

Enthalpy change that occurs when 1 mole of hydrogen ions react with 1 mole of hydroxide ions to form 1 mole of water under standard conditions in a solution with concentration 1 mol dm^-3

49
Q

How can a single bond be represented?

A

σ-bond
(sigma bond)

50
Q

How can a double bond be represented?

A

π-bond
(pi bond)

51
Q

How to count number of σ-bonds?

A

Count every single bond, as well as one of the double bonds

52
Q

How to count number of π-bonds?

A

Number of double bonds in molecule

53
Q

Define electronegativity

A

Measure of the attraction of the atoms in a covalent bond for the electrons in the bond

54
Q

How does electronegativity vary across the period table?

A

Increases across periods and up a group

55
Q

Define dipole

A

Bonds between elements (apart from C & H)

56
Q

If the element is more electronegative then the dipole is…

A

Negative (δ-)

57
Q

If the element is less electronegative then the dipole is…

A

Positive (δ+)

58
Q

If the elements are the same then the dipole is…

A

None

59
Q

Define electrophile

A

Electron pair acceptor

60
Q

What does the arrow represent in electrophilic addition mechanisms?

A

Shows the moment of a pair of electrons in the mechanism

61
Q

Define heterolytic fission

A

Where both electrons in a covalent bond remain with one atom during bond breaking

62
Q

Define carbocation

A

Intermediate formed during electrophilic addition, where an organic molecule has a positively charged carbon atom

63
Q

In electrophilic addition mechanisms, what product forms if a reactant is a halogen?

A

Dihalogen alkane

64
Q

In electrophilic addition mechanisms, what conditions if a reactant is a halogen?

A

None specific

65
Q

In electrophilic addition mechanisms, what product forms if a reactant is water?

A

Alcohol

66
Q

In electrophilic addition mechanisms, what conditions are needed if a reactant is water?

A

-Phosphoric acid
-High temperature
-High pressure

67
Q

In electrophilic addition mechanisms, what product forms if a reactant is a hydrogen-halide?

A

Halogenalkane

68
Q

In electrophilic addition mechanisms, what conditions are needed if a reactant is a halogen?

A

None specific

69
Q

In electrophilic addition mechanisms, what product forms if a reactant is hydrogen?

A

Alkane

70
Q

In electrophilic addition mechanisms, what conditions are needed if a reactant is hydrogen?

A

-Nickel catalyst
-60°C
-High pressure

71
Q

What must be on a electrophilic addition mechanism diagram?

A

-Full charges
-Partial charges (δ+, δ-)
-Arrow start and ends

72
Q

What does the strength of intermolecular forces determine?

A

Physical properties of organic compounds (mp/bp)

73
Q

What are the types of intermolecular forces?

A

-Instantaneous-induced dipole
(/van de Waal’s forces)
-Permanent-permanent dipole
-Hydrogen bonding

74
Q

Define instantaneous-induced dipole forces

A

Because electron position can constantly change if all electrons are on one side of the atom (which rises a dipole) induces dipoles on nearby atoms
Example: halogens

75
Q

Define permanent-permanent dipole forces

A

Attraction between δ+ of a molecule and δ- of a neighbouring molecule
(NOT C-H)

76
Q

Define hydrogen bond forces

A

Attraction between lone pairs of electrons of a very electronegative atom and a hydrogen atom in a neighbouring molecule

77
Q

Define Hess’ law

A

Total enthalpy change of a reaction is independent of the route taken, as long as the initial and final conditions are the same for each route

78
Q

What circumstances lead to enthalpy change not possible to measure?

A

-Slow rate of reaction
-High activation energy
-More than one reaction takes place

79
Q

Rules of Hess’ law

A

-Write down equation for enthalpy change being found
-Use other information given to make a cycle (usually triangle)
-Apply Hess’s law, go with the flow of arrows

80
Q

Define enthalpy change of formation (ΔHfθ)

A

When 1 mole of a substance is formed from its elements in their standard states
Example: Na(s) + 0.5Cl2(g) -> NaCl(s)

81
Q

If there are more points of contact from molecules what does that do to the boiling point?

A

Increases it

82
Q

Benefits of fossil fuels

A

-Efficient
-Reliable
-Has existing infrastructure

83
Q

Risks of fossil fuels

A

-Non sustainable
-Harmful emissions (CO2, CO, SO2)
NO2 formed at high temps in car engines

84
Q

Benefits of biofuels

A

-Renewable
-Lower CO2 emissions, some CO2 taken in by plants but not carbon neutral

85
Q

Risks of biofuels

A

-Land for crops, not food
-CO2 still released (combustion of fuel)

86
Q

Benefits of hydrogen (fuel)

A

-Produces only water with energy
-Can power internal combustion engine/hydrogen fuel cell

87
Q

Risks of hydrogen (fuel)

A

-Challenging to store
-How is electricity supplied for electrolysis?
-NO2 still produced in car engines at high temps

88
Q

How to do Hess’ cycle with combustion

A

-Add O2 to both sides of equation and add products to cycle
-Calculate the enthalpy of reaction for both sides
-Add/subtract following the arrow

89
Q

How to do Hess’ cycle with formation

A

-Add the substances needed to the cycle (given as info)
-Balance
-Calculate
-Add/subtract following arrow

90
Q

How to do Hess’ cycle with bond enthalpies

A

-Add the substances needed to the cycle (given as info)
-Balance
-Calculate
-Add/subtract following arrow

91
Q

Impact of CO2 to environment

A

-Greenhouse effect

92
Q

How to reduce CO2

A

-Biofuels

93
Q

Impact of CO to environment

A

-Toxic

94
Q

How to reduce CO

A

-Reacts in catalytic converter

95
Q

Impact of NOx to environment

A

-Photochemical smog
-Tropospheric ozone

96
Q

How to reduce NOx

A

-Reacts in catalytic converter

97
Q

Impact of SOx to environment

A

-Acid rain

98
Q

How to reduce SOx

A

-Sulfur removed from fossil fuels before being burnt

99
Q

Define catalyst poison

A

Chemicals bind very strongly to catalyst, covering surface

100
Q

What happens if catalyst binds too weakly?

A

Chemicals do not stay long enough to react

101
Q

Define heterogeneous

A

Catalyst is in a different state from the reactants and products

102
Q

Define catalyst

A

Increases rate of reaction by lowering activation energy and is not used up

103
Q

1st step of heterogeneous catalyst

A

Reactants absorb onto catalyst surface

104
Q

2nd step in heterogeneous catalyst

A

Bonds in reactants weaken and break (bonds being pulled further apart)

105
Q

3rd step in heterogeneous catalyst

A

Bonds in products form

106
Q

4th step in heterogeneous catalyst

A

Products desorb from catalyst surface

107
Q

Examples of heterogeneous catalysts?

A

-Catalytic converter
-Al2O3 (cracking)
-Fe (Haber process)

108
Q

Examples of heterogeneous catalysts?

A

-Catalytic converter
-Al2O3 (cracking)
-Fe (Haber process)

109
Q

What can the catalyst surface for a catalytic converter be?

A

Pt/Rh/Pd

110
Q

When are stereoisomers not called E/Z isomers?

A

When there are not 2 hydrogens

AS Chemistry (2 decks)

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