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year 10 mock exam revision > chemistry topic 4 chemical changes > Flashcards

chemistry topic 4 chemical changes Flashcards

1
Q

the lower the PH scale what does it tell us ?

A

the more acidic it is

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2
Q

the higher the PH scale what does it tell us?

A

the more alkaline it is

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3
Q

what is indicator?

A

a dye that changes colour depending on whether its above or below a certain PH

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4
Q

what does universal indicator do?

A

change colour to the PH of the solution

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5
Q

what do acids and bases do?

A

neutralise each other

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6
Q

what is an acid?

A

a substance that forms an aqueous solution with a PH of less than 7

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7
Q

what is a base?

A

any substance will react with an acid to form a salt

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8
Q

what is an alkali?

A

a base that dissolves in water to form a solution with a PH greater than 7

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9
Q

what is the reaction called between acids and bases?

A

neutralisation

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10
Q

what is the equation for neutralisation?

A

acid + base = salt + water

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11
Q

what is the equation for neutralisation using acid and alkali ions?

A

H+ + OH- = H20

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12
Q

how is reactivity determined in metals?

A

by how easily they will lose electrons

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13
Q

what happens when metals react with water or acid?

A

they lose electrons to form positive ions

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14
Q

the higher a metal is in the reactivity series means what?

A

the more easily it will react with water or acid

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15
Q

what is the equation for an acid reacting with a metal?

A

acid + metal = salt + hydrogen

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16
Q

what is the speed of a reaction determined by?

A

the rate at which the bubbles of hydrogen are given off

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17
Q

the more reactive the metal means what?

A

the faster the reaction will go

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18
Q

what is the equation for the reaction of metals with water?

A

metal + Water= metal hydroxide + hydrogen

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19
Q

what type of metals wouldn’t react with water?

A

less reactive metals

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20
Q

what are metals usually found as in the earth?

A

compounds that need to be extracted before use

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21
Q

how do you do the formation of a metal ore?

A

oxodisation

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22
Q

how do you extract metals?

A

reduction

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23
Q

what can some metals be extracted with?

A

carbon

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24
Q

what happens in reduction with carbon ?

A

the carbon gains the oxygen that is in the metal

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25
Q

how do metals higher than carbon in the reactivity series have to be reduced ?

A

using electrolysis

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26
Q

metals below carbon in the reactivity series can be reduced with what?

A

carbon

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27
Q

what does electrolysis mean?

A

splitting up with electricity

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28
Q

what happens during electrolysis?

A

an electric current is passed through n electrolyte

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29
Q

what is an electrolyte?

A

a molten or dissolved ionic compound

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30
Q

where do the positive ions go in the electrolyte?

A

they move to the negative electrode where they gain electrons

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31
Q

where do the negative ions go in the electrolyte?

A

they move to the positive electrolyte where they lose electrons

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32
Q

whats the negative electrode called ?

A

cathode

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33
Q

what is the positive electrode called?

A

anode

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34
Q

what happens to the ions when they go to the negative electrode?

A

they are reduced

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35
Q

what happens to the ions when they go to the positive electrode?

A

they are oxidised

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36
Q

what happens after the different ions move to the electrodes?

A

a flow of charge is created through the electrolyte

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37
Q

why cant an ionic solid be electrolysed?

A

the ions are in fixed positions and cant move

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38
Q

why can molten ionic compounds be electrolysed?

A

the ions can move freely and conduct electricity

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39
Q

what are molten ionic compounds broken up into?

A

their elements

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40
Q

why is electrolysis impractical?

A

its very expensive and requires lots of energy

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41
Q

what material are electrodes made out of so they don’t react with the electrolyte?

A

an inert material

42
Q

what is formed at the negative electrode?

A

metals form positive ions so they are attracted to the negative electrode

43
Q

what happens at the positive electrode?

A

non metals form negative ions so they are attracted to the positive electrode

44
Q

in aqueous solutions what ions are there as well as ions from the ionic compound?

A

hydrogen ions (H+) and hydroxide ions (OH-)

45
Q

what happens at the cathode if H+ ions are present?

A

hydrogen gas will be produced if the metal ions form a metal more reactive than hydrogen

46
Q

what happens if H+ ions are present and the metal ions are less reactive than hydrogen?

A

a sold layer of pure metal will be produced instead, it will coat the cathode

47
Q

what happens if halide ions are present?

A

at the anode, molecules of chlorine, bromine or iodine will be formed

48
Q

if no halide ions are present what happens to the OH- ions from the water?

A

oxygen gas and water will be formed at the anode

49
Q

how can you test for chlorine after electrolysis?

A

it bleaches damp litmus paper

50
Q

how can you test for hydrogen after electrolysis?

A

squeaky pop test with a lighted splint

51
Q

how can you test for oxygen after electrolysis?

A

it will relight a glowing splint

52
Q

what do half equations show?

A

reactions at the electrodes

53
Q

what can you combine the half equations for both reactions to get?

A

ionic equation of whole reaction

54
Q

at the cathode where is the added electrons on a half equation?

A

before the arrow

55
Q

at the anode where is the added electrons on a half equation?

A

after the arrow

56
Q

titration: what would you set up to find the concentration of some alkali?

A

use a pipette and pipette filler and add a set amount of volume of alkali to a conical flask

57
Q

titration: what do you use a funnel to fill?

A

a burette with acid of known concentration

58
Q

titration: how should you fill the burette?

A

below eye level so you won’t be looking up if some acid spills over

59
Q

titration: what do you record in the burette?

A

the initial volume of acid in the burette

60
Q

titration: how do you add the acid to the alkali?

A

a bit at a time, giving the conical flask a regular swirl. go slow when you think the end point is nearly reached

61
Q

Titrations: what do you record at the end?

A

the final volume of acid in the burette

62
Q

how do you fill the pipette in titrations?

A

to about 3cm above the line

63
Q

why do you need several consistent readings in titrations?

A

to spot any anomalous results

64
Q

what should you calculate and ignore doing titrations?

A

mean, ignore anomalies

65
Q

what is the substance colourless in acids but pink in alkali’s for titrations?

A

phenolphthalein

66
Q

for titrations, what is the chemical that is red in acids but blue in alkalis?

A

litmus

67
Q

for titrations, what is the chemical that goes from red in acids to yellow in alkalis?

A

methyl orange

68
Q

what do acids produce in water?

A

protons

69
Q

when do acids only ionise?

A

in aqueous solutions

70
Q

what happens to strong acids in water?

A

they ionise completely

71
Q

what do all acids release when ionised?

A

H+

72
Q

what happens to weak acids in solution?

A

they don’t fully ionise

73
Q

what kind of reaction Is a weak acid?

A

they have a reversible reaction

74
Q

where is equilibrium between in weak acids?

A

the undissociated and dissociated acid

75
Q

where does equilibrium usually lie in weak acid reactions and why?

A

it usually lies on the left since only a few acid particles release H+ iions

76
Q

what is the PH of an acid or alkali a measure of?

A

the concentration of H+ ions in the solution

77
Q

for every decrease of one of the PH scale , what is it a measure of?

A

the concentration of the H+ ions increases by a factor of 10

78
Q

what does acid strength tell you?

A

what proportion of acid molecules ionise in water

79
Q

what does concentration of an acid measure?

A

how much acid there is in a certain volume of water

80
Q

what is the word equation for acid and metal oxides reacting together?

A

acid + metal oxide/ hydroxide = salt +water

81
Q

what is the word equation for acid and metal carbonate reactions?

A

Acid+ metal carbonate= salt + water + carbon dioxide

82
Q

what do you need to make a soluble salt with an insoluble base?

A

the right acid plus and insoluble base

83
Q

what are the four steps to making soluble salts with an insoluble acid?

A

gently warm dilute acid with Bunsen burner, turn off Bunsen burner, add insoluble base till neutralised, filter excess, crystallisation

84
Q

how do you know when the acid has been neutralised ?

A

even after stirring, excess solid will just sink to the bottom

85
Q

how do you do crystallisation?

A

gently heat filtered solution in water bath to evaporate water then let it cool, crystals should form where they can be filtered and dried

86
Q

what does a PH probe attached to a PH meter do when placed in solution?

A

it measures PH electronically

87
Q

what acronym helps you remember the reactivity series?

A

please stop laughing/calling my amazing colourful zebra in the history class she grunts

88
Q

metals more reactive than hydrogen will react with what?

A

acids

89
Q

metals less reactive than hydrogen will react with what?

A

not acids

90
Q

what can metals less reactive than carbon do ?

A

be reduced with carbon

91
Q

what is oxidation?

A

gain of oxygen

92
Q

what is reduction?

A

loss of oxygen

93
Q

how does reduction from carbon happen?

A

the ore is reduced as oxygen is removed from it and carbon gains oxygen so therefore it is oxidised

94
Q

what is a loss of electrons?

A

oxidation

95
Q

what is a gain of electrons?

A

reduction

96
Q

what happens in redox reactions of metals reacting with acids?

A

metal ions lose electrons as they are oxidised by hydrogen and hydrogen ions are reduced by metal as they gain electrons

97
Q

what is an example of a redox reaction?

A

a displacement reaction

98
Q

what happens in a displacement reaction?

A

more reactive metals will displace less reactive metals

99
Q

what is there always it metal displacement reactions?

A

the metal atom always gains electrons and the metal atom always loses electrons

100
Q

what happens when ions don’t change in ionic equations?

A

they are spectator ions

101
Q

what is ONLY in ionic equations?

A

the substances that are oxidised and reduced

year 10 mock exam revision (26 decks)

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