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Chemistry > AS Chemistry Unit 2 Definitions > Flashcards

AS Chemistry Unit 2 Definitions Flashcards

0
Q

Hydrocarbon

A

A compound that contains only carbon and hydrogen atoms

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1
Q

Nucleophile

A

An electron pair donor

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2
Q

Molecular formula

A

Actual whole number ratio of atoms present in a compound

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3
Q

Homologous series

A

A series of compounds having the same functional group and general formula but with each successive member differing by CH2

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4
Q

Structural formula

A

The minimal detail that shows the arrangement of atoms in a molecule (ie CH3CH2CH3)

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5
Q

Electrophile

A

An electron pair acceptor

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6
Q

Empirical formula

A

Simplest whole number ratio of atoms present in a compound

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7
Q

Stereoisomers

A

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

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8
Q

Displayed formula

A

A formula that shows the relative positioning of all atoms and bonds within a structure

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9
Q

Bond fission

A

The baking of a covalent bond

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10
Q

Structural isomer

A

Molecules with the Mae molecular formula but with different structural formula

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11
Q

Heterolytic bond fission

A

The breaking of. Covalent bond with both of the shared pair of electrons going to one of the atoms forming ions

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12
Q

E/Z isomerism

A

An example of stereoisomerism, in terms of restricted rotation about a double c bond and the requirement for two different groups to be attached to each carbon atom of the double C bond

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13
Q

Cis/trans isomerism

A

A special case of E/Z isomerism in which two of the substituent groups are the same

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14
Q

General formula

A

Simplest algebraic formula of a member of a homologous series (ie CnH2n+2. Fr alkanes)

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15
Q

Homolytic fission

A

The breaking of a covalent bond with one of the shared pair of electrons going to each atom, forming two radicals

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16
Q

Skeletal formula

A

A simplified organic formula, shown by removing hydrogen atoms from carbon chains, leaving jus a carbon skeleton and associated functional groups

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17
Q

Functional group

A

Group of atoms in a molecule responsible for the characteristic reactions of a compound

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18
Q

Biofuel

A

Fuel derived from recently living plant material ( bio ethanol/ biodiesel)

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19
Q

% yield

A

The mass/moles of product expressed as a percentage of what you should obtain assuming complete conversion. Actual mass/moles/ theoretical mass/moles *100

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20
Q

Carbon capture and storage

A

The removal of waste carbon dioxide as a liquid injected deep in the oceans, as storage in deep rock formations or by reaction with metal oxides to form stable carbonate minerals

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21
Q

Atom economy

A

A measure of how much of the products are useful

22
Q

(Free) radical

A

Species that has an unpaired electron

23
Q

Le chateliers principle

A

The position of equilibrium will shift as to minimise the effect of any change in condition

24
Dynamic equilibrium
Wen in a closed system, the rate of both the forward reaction and the backwards reactions are equal
25
Catalyst
Speeds up the rate of the reaction without being used up in the process
26
Rate of reaction
The change in concentration of a reactant or product in a given time ( concentration / time = moldm-3s-1 )
27
Activation energy
The minimum amount of energy required for the reactants to react together
28
Empirical formula
Slimmest whole number ratio of atoms present in a compound
29
Skeletal formula
A simplified organic formula, shown by removing hydrogen atoms from carbon chains, leaving just a carbon skeleton and associated functional groups
30
Homologous series
A series of compounds having the same functional group and general formula but with each successive member differing by ch2
31
Structural formula
The minimal detail that shows the arrangement of atoms in a molecule
32
Free radical substitution
A reaction involving alkanes that involves the substitution of at least one hydrogen atom with a halogen atom via initiation, propagation and termination of radicals, themselves formed from homolytic fission
33
Saturated
A compound with no double bonds, only single carbon to carbon bonds
34
Cracking
The breaking down of long chained saturated hydrocarbons to form a mixture shorter chained alkanes and alkenes
35
Fractional distillation
Separation of components in a mixture into fractions, in which each one differs in their boiling points.
36
Hydrocarbon
A compound that contains only carbon and hydrogen atoms
37
General formula
Simplest algebraic formula of a member of a homologous series
38
Molecular formula
Actual whole number ratio of atoms present in a compound
39
Displayed formula
A formula that shows the relative positioning of all atoms and binds within a structure
40
Unsaturated
A compound that contains at least one carbon to carbon double bond
41
Functional group
Group of atoms in a molecule responsible for the characteristic reactions of a compound
42
Structural isomer
Molecules with the same molecular formula but with different structural formula
43
Endothermic reaction
Reaction that requires the input of heat energy from the surroundings
44
Standard conditions
Pressure of 100KPa and temperature of 298K
45
Exothermic reactions
Reaction that releases heat energy to the surroundings
46
Standard enthalpy change of a reaction
Enthalpy change when the number of moles of reactants as specified in the balanced chemical equation react together in their standard states under standard conditions
47
Enthalpy change of combustion
Enthalpy change for the complete combustion of 1 mole of a substance
48
Average bond enthalpy
Average enthalpy change when one mole of bonds are broken in the gaseous state
49
Standard enthalpy change of combustion
Enthalpy change for the combustion in oxygen of 1 mole of a substance under standard conditions. All reactants and products are in their standard states.
50
Hess's law
The enthalpy change of a reaction is independent of the pathway taken
51
Enthalpy change and formation
Enthalpy change when one mole of a compound is formed from its elements
52
Enthalpy change of a reaction
Enthalpy change when the number of moles of reactants as specified in a balanced chemical equation react together
53
Standard enthalpy change of formation
Enthalpy change when one mole of a compound is formed from its elements under standard conditions. All the reactants and products are in their standard states.

Chemistry (4 decks)

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