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AQA A Level Chemistry COPY COPY > Definitions - All Topics > Flashcards

Definitions - All Topics Flashcards

1
Q

Relative Atomic Mass (AR)

A

The average mass of an atom of an element compared to 1/12th of the mass of a 12C atom

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2
Q

Relative Molecular Mass (MR)

A

The average mass of a molecule of an element compared to 1/12th of the mass of a 12C atom

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3
Q

Avogadro’s number

A

The number of atoms found to be in 12g of 12C

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4
Q

Empirical Formula

A

The simplest ration of atoms of each element in a compound

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5
Q

Atom economy

A

Measure of what proportion of the product of a reaction is desired, and how much is waste

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6
Q

Homologous series

A

A group of chemicals which have similar chemical properties, the same functional group and can be represented by a general formula

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7
Q

Isomers

A

Chemicals with the same molecular formula, but a different structural formula

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8
Q

Structural isomerism

A

Compounds with the same molecular formula, but different structural/skeletal/displayed formula.

Eg of structural isomerism = positional isomerism

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9
Q

Chain isomerism

A

Compounds with the same molecular formula but a different carbon skeleton

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10
Q

Position isomerism

A

Compounds with the same molecular formula and carbon skeleton, but a different position of the same type of functional group

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11
Q

Functional group isomerism

A

Same molecular formula, different functional group

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12
Q

Display structure

A

Every bond is displayed

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13
Q

Stereo isomerism

A

When molecules have the same structural formula but a different spatial arrangement of atoms

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14
Q

Enthalpy change of formation

A

The enthalpy change when one mole of a substance is made from its constituent elements with all products and reactants in their standard states under standard conditions

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15
Q

Enthalpy change of combustion

A

The enthalpy change when one mole of a substance is burned completely in oxygen with all reactants and products in their standard states under standard conditions

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16
Q

Standard conditions

A

298K, 1000kPa

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17
Q

Mean bond enthalpy

A

The average heat needed to break one mole of covalent bonds of a molecule in a gaseous state under standard conditions

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18
Q

Dynamic (in terms of equilibria)

A

Forward and reverse reactions both take place

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19
Q

Equilibrium

A

Both forward and reverse reactions take place at equal rates. The concentration of all reactants remain constant

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20
Q

Catalyst

A

A substance that increases the rate or reaction without being changed in chemical composition or amount. They work by providing an alternative pathway/reaction route of lower activation energy

21
Q

Activation energy

A

The minimum amount of energy needed for a reaction to occur/for a successful collision

22
Q

Equilibrium constant (Kc)

A

A value calculated from the equilibrium concentrations for a system at constant temperature

23
Q

Oxidation

A

Addition of oxygen and loss of electrons to a substance

24
Q

Reduction

A

Removal of oxygen and addition of electrons to a substance

25
Q

Disproportionation

A

When atoms of the same element are simultaneously oxidised and reduced

26
Q

Reducing agent

A

A species which aids the reduction of another species by donating the electrons which the other species gains. The reducing agent’s oxidation state will become more positive (more oxidised)

27
Q

Oxidising agent

A

A species which aids the oxidation of another species by accepting the electrons that the other species loses. The oxidising agent’s oxidation state will become less positive/more negative (more reduced)

28
Q

Isotopes

A

Atoms of the same element with the same atomic number but a different mass number. (same no. of protons and electrons, diff. no. of neutrons)

29
Q

Atomic number

A

The number of protons in the atom nucleus (aka protonic no.)

30
Q

Mass number

A

The number of protons AND neutrons in the nucleus of an atom

31
Q

1st ionisation energy

A

The energy needed to remove 1 mole of electrons from 1 mole of gaseous atoms

32
Q

2nd ionisation energy

A

The amount of energy required to remove an electron from a gaseous 1+ ion

33
Q

Dative/Coordinate bond

A

A covalent bond whereby the pair of electrons originate from one atom

34
Q

Polar molecules

A

Molecules whereby the polar bonds combine in such a way some parts are more negative/positive

35
Q

Electronegativity

A

The power of an atom to attract the pair of electrons in a covalent bond

36
Q

Saturated

A

When a molecule only has single bonds

37
Q

Hydrocarbon

A

A molecule containing a hydrogen and a carbon only

38
Q

Hydrolysis

A

Splitting molecules using water

39
Q

Nucleophile

A

An electron pair donator

40
Q

Electrophile

A

An electron pair acceptor

41
Q

Addition Polymerisation

A

Formation of long chain molecules from lots of small molecules joining together with no other products

42
Q

Plasticisers

A

Small molecules that get between the polymer chains, allowing them to slide past each other. This makes the chains more flexible

43
Q

Isotatcic

A

All R groups (eg CH3) are on the same side

44
Q

Atactic

A

Random positioning of R groups (eg CH3)

45
Q

What is a free radical?

A

An atom or species with an unpaired electron

46
Q

Define standard enthalpy of atomisation

A

The enthalpy change when mole of gaseous atoms is formed from the element in its standard state under standard conditions

47
Q

Define first electron affinity

A

The standard enthalpy change when one mole of gaseous atoms is converted into one mole of gaseous ions, each with a single negative charge

48
Q

Define second electron affinity

A

The enthalpy change when mole of electrons is added to one mole of gaseous ions, each with a single negative charge to form one mole of gaseous ions each with 2 negative charges

AQA A Level Chemistry COPY COPY (34 decks)

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