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Chemistry - Paper 1 > CHEMICAL CHANGES > Flashcards

CHEMICAL CHANGES Flashcards

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1
Q

what does reactivity mean

A

how vigorously substance chemically reacts

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2
Q

how can metals be ordered by their reactivity

A

by comparing their reactions with water, acid or oxygen

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3
Q

what is the name given to the list of metals ordered by their reactivity

A

reactivity series

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4
Q

in terms of electrons, what makes some metals more reactive than others

A

they lose their outer shell electrons more easily

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5
Q

why are gold and silver found naturally as elements in the earths crust

A

they are very unreactive

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6
Q

what is an ore

A

rock containing enough of a metal compound to be economically worth extracting

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7
Q

how are metals less reactive than carbon extracted from their ores

A

reduction with carbon

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8
Q

in terms of oxygen what is oxidation

A

addition of oxygen

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9
Q

in terms of oxygen what is reduction

A

removal of oxygen

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10
Q

why can metals like potassium and aluminium not be extracted by reduction with carbon

A

they are more reactive than carbon

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11
Q

how are metals more reactive than carbon extracted from their ores

A

electrolysis

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12
Q

what is a displacement reaction

A

a more reactive substance takes the place of a less reactive substance in a compound

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13
Q

what is an ionic equation

A

equation which gives some substances as ions and has spectator ions removed

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14
Q

what type of substance is given as ions in an ionic equation

A

ionic compounds in solution

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15
Q

what is a spectator ion

A

ion that is uncharged in a reaction

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16
Q

what is a half equation

A

equation that shows whether a substance is losing or gaining electrons

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17
Q

in terms of electrons what is oxidation

A

loss of electrons

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18
Q

in terms of electrons what is reduction

A

gain of electrons

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19
Q

in terms of pH what is an acid

A

a solution with a pH less than 7

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20
Q

in terms of pH what is a neutral solution

A

a solution with a pH of 7

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21
Q

in terms of H+ ions what is an acid

A

a substance that releases H+ ions when dissolved in water

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22
Q

how is the amount of H+ ions in a solution related to its pH

A

the more H+ ions, the lower the pH

23
Q

how do you measure the pH of a substance

A

universal indicator or pH probe

24
Q

what is a strong acid

A

an acid where the molecules or ions completely ionise in water

25
Q

what is a weak acid

A

an acid where the molecules or ions partially ionise in water

26
Q

what is a salt

A

compound formed when a metal ion takes the place of a hydrogen ion in an acid

27
Q

what are the products of a reaction between a metal and acid

A

salt + hydrogen

28
Q

what are the products of a reaction between a metal hydroxide and an acid

A

salt + water

29
Q

what are the products of a reaction between a metal oxide and acid

A

salt + water

30
Q

what are the products of a reaction between a metal carbonate and acid

A

salt + water + carbon dioxide

31
Q

what is a base

A

substances that react with acids in neutralisation reactions

32
Q

what is an alkali

A

substance that dissolves in water to form a solution above pH 7

33
Q

what is a neutralisation reaction

A

a reaction between an acid and base to produce water

34
Q

what is the ionic equation for a reaction between an acid and alkali

A

H+ + OH- —-> H2O

35
Q

how can you obtain a solid salt from a solution

A

crystallisation

36
Q

when an acid reacts with a metal which species is oxidised

A

the metal

37
Q

when an acid reacts with a metal which species is reduced

A

hydrogen

38
Q

what is electrolysis

A

process of using electricity to extract elements from a compound

39
Q

what is the name of the positive electrode

A

anode

40
Q

what is the name of the negative electrode

A

cathode

41
Q

what is an electrolyte

A

liquid or solution that contains ions and so can conduct electricity

42
Q

where are metals formed

A

cathode

43
Q

where are non metals formed

A

anode

44
Q

how can ionic substances be electrolysed

A

by melting or dissolving them, and then passing a direct current through them

45
Q

why can solid ionic substances not be electrolysed

A

they do not conduct electricity, or the ions cannot move

46
Q

in the electrolysis solutions when is the metal not produced at the cathode

A

when the metal is more reactive than hydrogen

47
Q

in the electrolysis of a metal halide solution what is produced at the anode

A

halogen

48
Q

in the electrolysis for a metal sulphate solution what is produced at the anode

A

oxygen

49
Q

what is the half equation for the ionisation of water

A

H2O —> H+ + OH-

50
Q

what metals are extracted from ionic compounds by using electrolysis

A

metals that are more reactive than carbon

51
Q

in the electrolysis of aluminium oxide why is the aluminium oxide mixed with cryolite

A

to lower the melting point

52
Q

in the electrolysis of aluminium oxide what are the anodes made of

A

graphite

53
Q

in the electrolysis of aluminium oxide why do the anodes need to be replaces

A

they react with the oxygen being formed

Chemistry - Paper 1 (5 decks)

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