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A// Chemistry > Developing Fuels > Flashcards

Developing Fuels Flashcards

1
Q

Addition reaction

A

A reaction when two or more molecules react to form a single larger molecule

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2
Q

Adsorbed

A

When reactants bond to the surface of a catalyst

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3
Q

Alcohol

A

Alcohols have a hydroxyl, OH group

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4
Q

Aliphatic

A

Organic molecules which do not contain a benzene ring

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5
Q

Alkanes

A

Hydrocarbons with a general formula CnH2n+2

They are saturated

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6
Q

Alkenes

A

Non-cyclic hydrocarbons with the general formula CnH2n

They are unsaturated

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7
Q

Amount

A

This tells you the number of moles of a substance

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8
Q

Aromatic

A

Benzene and organic molecules containing one or more benzene rings

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9
Q

Bond enthalpy

A

This is the energy required to break one mole of a bond to give separate atoms all in the gaseous state

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10
Q

Carbocation

A

An ion with a positively-charged carbon atom

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11
Q

Catalyst

A

A substance which speeds up a reaction but can be recovered chemically unchanged at the end

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12
Q

Catalysis

A

The process of speeding up a chemical reaction

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13
Q

Catalyst poison

A

A substance that stops a catalyst functioning properly

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14
Q

Chain isomers

A

Same molecular formula, different structural formulae. The carbon chains are different

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15
Q

Copolymerisation

A

When more than one type of monomer is used in addition polymerisation

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16
Q

Cracking

A

Any reaction in which a larger molecule is made into smaller molecules. When the original alkane is broken down one product will be unsaturated

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17
Q

Cycloalkane

A

An alkane which had the C atoms in a ring. General formula is CnH2n
They are saturated

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18
Q

Delocalised electrons

A

Bonding electrons which are shared between more than 2 atoms in benzene

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19
Q

Electrolysis

A

The breaking down of a compound using electricity

Electrical energy is transferred to chemical energy

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20
Q

Electrophile

A

A positive ion, or a molecule with a partial positive charge, that will be attracted to a negatively charged region and react by accepting a lone pair of electrons to form a covalent bond

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21
Q

Empirical formula

A

This is the simplest whole number ratio of atoms in a compound

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22
Q

Endothermic

A

An endothermic reaction takes in energy and cools the surroundings
🔺H is positive
Bond breaking

23
Q

Energy transfer

A

Energy transferred (J) = mass (g) x temperature change (degrees C or K) x 4.18

24
Q

Ether

A

Ethers have an -O- between two alkyl groups

25
Evaporative emissions
These are just unburnt hydrocarbons (CxHy) which escape from an exhaust
26
Exothermic
An exothermic reaction gives out energy and heats the surroundings 🔺H is negative Bond making
27
Extrapolation
Extending data points beyond those actually measured
28
Fuel cell
Used to generate electricity on a small scale in cars | Chemical energy is transferred to electrical energy
29
Functional group
Modifiers that are responsible for the characteristic chemical reactions of molecules
30
Functional group isomers
Same molecular formula, different structural formulae | These have different functional groups and belong to different homologous series
31
Hess’s law
As long as your starting and finishing points are the same, the enthalpy change will always be the the same, this is regardless of how you go from start to finish
32
Heterogeneous catalyst
This catalyst is in a different state to the reactants
33
Homogeneous catalyst
This catalyst is in the same state as the reactants
34
Homologous series
Members of a homologous series have the same general formula, similar chemical properties and a gradual change in physical properties
35
Hydrocarbon
A hydrocarbon is a compound of carbon and oxygen only
36
Isomerisation
In isomerisation, straight chain isomers are heated with a catalyst Bits of the chain break off and may join on in a new place to form an isomer (with a higher octane number)
37
Molecular formula
This gives the actual numbers of each type of atom in a molecule
38
Polarised
If a molecule or atom is polarised, it has a + and a - side
39
Polymerisation
Small molecules called monomers join together to produce long chain polymers
40
Positional isomers
Same molecular formula, different structural formulae | Differ only in the position of the functional group
41
Saturated
A saturated compound has the maximum number of hydrogen atoms possible, no C to C double or triple bonds
42
Skeletal formula
This shows only the carbon skeleton and associated functional groups of the molecule
43
Specific heat capacity
The specific heat capacity of a substance is the amount of energy needed to raise the temperature of 1g by 1K
44
Standard conditions
298K (25 degrees C) for temperature 1 atmosphere for pressure 1 mol dm-3 for concentration of solutions
45
Standard enthalpy change of combustion 🔺cH*298
This is the enthalpy change when 1 mole of a substance burns completely in oxygen under standard conditions This is always negative
46
Standard enthalpy change of formation 🔺fH*298
This is the enthalpy change when 1 mole of a substance is made from its constituent elements The elements are in their standard states
47
Standard enthalpy change of neutralisation 🔺neutH*298
This is the enthalpy change when 1 mole of hydrogen ions react with one mole of hydroxide ions to form one mole of water under standard conditions and in solutions containing 1 mol dm-3
48
Standard enthalpy change for a reaction 🔺rH*298
The enthalpy change when molar quantities of reactants as stated in the equation react together under standard conditions
49
Standard conditions
The physical state of a substance under standard conditions | This may be a pure solid, liquid or gas
50
Stereoisomers
This is when molecules have the same structural formula but differ in how their atoms are arranged in space - E/Z isomerism
51
Stoichiometic mixture
This is the mixture which contains exactly the correct amounts of chemicals to react completely
52
Structural formula
This shows how the atoms in a molecule bond to each other
53
Structural isomer
These have that same molecular formula but different structural formula

A// Chemistry (5 decks)

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