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GCSE Chemistry > C5 - Chemical Changes > Flashcards

C5 - Chemical Changes Flashcards

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1
Q

What is an acid?

A

When dissolved in water, its solution has a pH value less than 7. Acids release H+ ions when added to water

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2
Q

What is an alkali?

A

When dissolved in water, its solution has a pH value more than 7. Alkalis release OH- ions when added to water

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3
Q

What is a base?

A

the oxide, hydroxide, or carbonate of a metal that will react with an acid and be neutralised, forming a salt + water

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4
Q

What is a displacement reaction?

A

a reaction in which a more reactive element takes the place of a less reactive element in one of its compounds or in solution

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5
Q

What is electrolysis?

A

the breakdown of a substance containing ions by electricity

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6
Q

What is equilibrium?

A

the point in a reversible reaction at which the forward and backward rates of reaction are the same. Therefore, the amounts of substances present in the reacting mixture remain constant

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7
Q

What is a half equation?

A

an equation that describes reduction (gain of electrons) or oxidation (loss of electrons)

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8
Q

What is an ionic equation?

A

an equation that shows only those ions or atoms that change in a chemical reaction

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9
Q

What is a metal ore?

A

a rock that contains enough of a metal or metal compound that it is worth extracting the metal

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10
Q

What is neutral?

A

a solution with a pH value of 7 which is neither acidic nor alkaline.

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11
Q

What is neutralisation?

A

the chemical reaction of an acid with a base in which a salt and water are formed. If the base is a carbonate or hydrogen carbonate, carbon dioxide is also produced in the reaction

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12
Q

What is an ore?

A

a rock which contains enough metal to make it economically worthwhile to extract the metal

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13
Q

What is oxidation/oxidised?

A

a reaction where oxygen is added to a substance / or when electrons are lost from a substance

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14
Q

What is pH?

A

a number which shows how strongly acidic or alkaline a solution is

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15
Q

What is the reactivity series?

A

a list of elements in order of their reactivity

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16
Q

What is reduction / reduced?

A

a reaction in which oxygen is removed or electrons are gained

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17
Q

What is a salt?

A

an ionic compound (can be formed when an acid reacts with a base)

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18
Q

What are strong acids?

A

these acids completely ionise in aqueous solutions

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19
Q

What are weak acids?

A

acids that do not dissosiate completely in aqueous solutions

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20
Q

What are 3 strong acids?

A
  • Hydrochloric Acid
  • Sulfuric Acid
  • Nitric Acid
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21
Q

What is an example of a weak acid?

A

*Ethanoic Acid

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22
Q

What is the formula of Hydrochloric Acid

A

HCl

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23
Q

What is the formula of Sulfuric Acid

A

H₂SO₄

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24
Q

What is the formula of Nitric Acid

A

HNO₃

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25
Q

What is the formula of Ethanoic Acid

A

CH₃COOH

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26
Q

What is the equation for Hydrochloric Acid ionising?

A

HCl -> H⁺ + Cl⁻

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27
Q

What is the equation for Sulfuric Acid ionising?

A

H₂SO₄ -> 2H⁺ + SO₄²⁻

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28
Q

What is the equation for Nitric Acid ionising?

A

HNO₃ -> H⁺ + NO₃⁻

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29
Q

What is the equation for Ethanoic Acid ionising?

A

CH₃COOH ⇌ H⁺ + CH₃COO

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30
Q

What is the equation for an acid reacting with a metal oxide?

A

acid + metal oxide → salt + water

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31
Q

What is the equation for an acid reacting with a metal hydroxide?

A

acid + metal hydroxide → salt + water

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32
Q

What is the equation for an acid reacting with a metal carbonate?

A

acid + carbonate → salt + water + carbon dioxide

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33
Q

What type of salt is produced with sulfuric acid?

A

sulfate

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34
Q

What type of salt is produced with nitric acid?

A

nitrate

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35
Q

What type of salt is produced with hydrochloric acid?

A

chloride

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36
Q

What would be the typical PH of a strong concentrated acid?

A

0 or 1

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37
Q

What would be the typical PH of a strong dilute acid?

A

2 or 3

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38
Q

What would be the typical PH of a weak concentrated acid?

A

4 or 5

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39
Q

What would be the typical PH of a weak dilute acid?

A

5 or 6

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40
Q

What would be the reaction with magnesium of a strong concentrated acid?

A

vigorous fizzing

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41
Q

What would be the reaction with magnesium of a strong dilute acid?

A

fizzing

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42
Q

What would be the reaction with magnesium of a weak concentrated acid?

A

gentle fizzing

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43
Q

What would be the reaction with magnesium of a weak dilute acid?

A

hardly any fizzing

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44
Q

What colour would the universal indicator be with a strong concentrated acid?

A

red

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45
Q

What colour would the universal indicator be with a strong dilute acid?

A

red

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46
Q

What colour would the universal indicator be with a weak concentrated acid?

A

orange

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47
Q

What colour would the universal indicator be with a weak dilute acid?

A

yellow

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48
Q

What proportion of molecules would react with water to for H⁺ with a strong concentrated acid?

A

all

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49
Q

What proportion of molecules would react with water to for H⁺ with a strong dilute acid?

A

all

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50
Q

What proportion of molecules would react with water to for H⁺ with a weak concentrated acid?

A

few

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51
Q

What proportion of molecules would react with water to for H⁺ with a weak dilute acid?

A

few

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52
Q

How do you identify an acid?

A

It will contain H⁺ in its formula (i.e. HCl or H₂SO₄)

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53
Q

How do you identify an alkali?

A

It will contain OH- in its formula (i.e. NaOH or KOH)

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54
Q

How do you identify a base?

A

It will contain oxide (O), carbonate (CO₃²⁻), or hydroxide (OH-) (i.e. MgO or PbCO₃)

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55
Q

How do you identify a salt?

A

It will be the product of an acid base reaction, (i.e. Potassium Nitrate or Zinc Chloride)

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56
Q

Can an acid be a base?

A

no

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57
Q

Can an alkali be a base?

A

yes

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58
Q

Can a salt be a base?

A

no

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59
Q

What happens in a neutralisation reaction between an acid and an alkali?

A

Hydrogen ions react with hydroxide ions to produce water

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60
Q

What is the equation for the neutralisation of an acid with an alkali?

A

H+(aq) + OH-(aq) → H2O(l)

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61
Q

What are bases that are soluble in water called?

A

alkalis

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62
Q

What are substances that can be used to identify alkalis and acids called?

A

indicators

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63
Q

What colour does methyl orange turn in a strong acid?

A

red

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64
Q

What colour does methyl orange turn in a weak acid?

A

red

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65
Q

What colour does methyl orange turn in water?

A

orange

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66
Q

What colour does methyl orange turn in a weak alkali?

A

yellow

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67
Q

What colour does methyl orange turn in a strong alkali?

A

yellow

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68
Q

What colour does Phenolphthalein solution turn in a strong acid?

A

colourless

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69
Q

What colour does Phenolphthalein solution turn in a weak acid?

A

colourless

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70
Q

What colour does Phenolphthalein solution turn in water?

A

colourless

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71
Q

What colour does Phenolphthalein solution turn in a weak alkali?

A

pink

72
Q

What colour does Phenolphthalein solution turn in a strong alkali?

A

pink

73
Q

What colour does Litmus Paper turn in a strong acid?

A

red

74
Q

What colour does Litmus Paper turn in a weak acid?

A

red

75
Q

What colour does Litmus Paper turn in water?

A

No colour change

76
Q

What colour does Litmus Paper turn in a weak alkali?

A

blue

77
Q

What colour does Litmus Paper turn in a strong alkali?

A

blue

78
Q

What colour does Universal Indicator Solution turn in a strong acid?

A

red/PH = 1

79
Q

What colour does Universal Indicator Solution turn in a weak acid?

A

orange/PH = 5

80
Q

What colour does Universal Indicator Solution turn in water?

A

green/PH = 7

81
Q

What colour does Universal Indicator Solution turn in a weak alkali?

A

blue/PH = 10

82
Q

What colour does Universal Indicator Solution turn in a strong alkali?

A

purple/PH = 14

83
Q

What colour does Universal Indicator paper turn in a strong acid?

A

red/PH = 1

84
Q

What colour does Universal Indicator paper turn in a weak acid?

A

orange/PH = 5

85
Q

What colour does Universal Indicator paper turn in water?

A

green/PH = 7

86
Q

What colour does Universal Indicator paper turn in a weak alkali?

A

blue/PH = 10

87
Q

What colour does Universal Indicator paper turn in a strong alkali?

A

purple/PH = 14

88
Q

What is the PH scale?

A

The PH scale is a scale from 0-14 indicating how alkali or acidic a substance is

89
Q

What is neutral on the PH scale?

A

7

90
Q

What is PH?

A

PH is a measure of the concentration of H⁺ ions in a solution

91
Q

The PH scale is logarithmic, what does this mean?

A

each change in 1 on the scale represents a change in concentration by a factor of 10

92
Q

What is the H⁺ concentration of a substance with a PH of 0?

A

1x10⁻⁰ mol/dm³

93
Q

What is the H⁺ concentration of a substance with a PH of 1?

A

1x10⁻¹ mol/dm³

94
Q

What is the H⁺ concentration of a substance with a PH of 2?

A

1x10⁻² mol/dm³

95
Q

What is the H⁺ concentration of a substance with a PH of 3?

A

1x10⁻³ mol/dm³

96
Q

What is the H⁺ concentration of a substance with a PH of 4?

A

1x10⁻⁴ mol/dm³

97
Q

What is the H⁺ concentration of a substance with a PH of 5?

A

1x10⁻⁵ mol/dm³

98
Q

What is the H⁺ concentration of a substance with a PH of 6?

A

1x10⁻⁶ mol/dm³

99
Q

What is the H⁺ concentration of a substance with a PH of 7?

A

1x10⁻⁷ mol/dm³

100
Q

What is the H⁺ concentration of a substance with a PH of 8?

A

1x10⁻⁸ mol/dm³

101
Q

What is the H⁺ concentration of a substance with a PH of 9?

A

1x10⁻⁹ mol/dm³

102
Q

What is the H⁺ concentration of a substance with a PH of 10?

A

1x10⁻¹⁰ mol/dm³

103
Q

What is the H⁺ concentration of a substance with a PH of 11?

A

1x10⁻¹¹ mol/dm³

104
Q

What is the H⁺ concentration of a substance with a PH of 12?

A

1x10⁻¹² mol/dm³

105
Q

What is the H⁺ concentration of a substance with a PH of 13?

A

1x10⁻¹³ mol/dm³

106
Q

What is the H⁺ concentration of a substance with a PH of 14?

A

1x10⁻¹⁴ mol/dm³

107
Q

Why do strong acids have lower PH’s than weak acids?

A

For 2 acids of equal concentration, where 1 is strong and the other is weak, the strong acid will have a lower PH due to its capacity to dissociate more and hence put more H⁺ ions into solution than weak acid

108
Q

Describe the method for forming copper sulfate crystals

A

1) Measure out 25cm³ of sulfuric acid using a measuring cylinder and place it in a 100cm³ beaker
2) Gently warm the mixture using a Bunsen burner. do not boil the acid
3) Add a spatula load of copper oxide and stir with a glass rod. After a short time, the black copper oxide will all react producing a blue solution
4) Keep adding the copper oxide 1 spatula at a time until it no longer reacts. You will be able to tell as there will be unreacted black solid in the mixture
5) Filter and wash the mixture in a conical flask
6) While the mixture is filtering, set up a water bath using a half full 250cm³ beaker of water on a gauaze above a Bunsen burner. Start heating the water
7) Once the filtration is complete, transfer some of the filtrate into an evaporating basin (do not fill it over half way)
8) carefully place the basin on the water bath and heat to allow some of the water to evaporate from the copper sulfate solution
9) keep heating until crystal start to appear then stop
10) Place the basin in a cool place for 24 hours
11) After 24 hours record your observations

109
Q

What is the reaction of a metal and an acid?

A

Metal + acid -> salt + hydrogen

110
Q

What is the reaction of an alkali and an acid?

A

Alkali (metal hydroxide) + Acid -> water + salt

111
Q

What is the reaction of a carbonate and an acid?

A

Carbonate + acid -> water + carbon Dioxide + salt

112
Q

What is the reaction of a base and an acid?

A

Base (metal oxide) + acid -> water + salt

113
Q

What salt is formed with nitric acid and sodium carbonate

A

sodium nitrate

114
Q

What salt is formed with nitric acid and magnesium

A

magnesium nitrate

115
Q

What salt is formed with nitric acid and potassium oxide

A

potassium nitrate

116
Q

What salt is formed with nitric acid and copper hydroxide

A

copper nitrate

117
Q

What salt is formed with hydrochloric acid and sodium carbonate

A

sodium chloride

118
Q

What salt is formed with hydrochloric acid and magnesium

A

magnesium chloride

119
Q

What salt is formed with hydrochloric acid and potassium oxide

A

potassium chloride

120
Q

What salt is formed with hydrochloric acid and copper hydroxide

A

copper chloride

121
Q

What salt is formed with sulfuric acid and sodium carbonate

A

sodium sulfate

122
Q

What salt is formed with sulfuric acid and magnesium

A

magnesium sulfate

123
Q

What salt is formed with sulfuric acid and potassium oxide

A

potassium sulfate

124
Q

What salt is formed with sulfuric acid and copper hydroxide

A

copper sulfate

125
Q

What is the mneumonic for REDOX reactions?

A

OIL RIG

126
Q

What does OIL RIG stand for?

A

Oxidation
Is
Loss of electrons

Reduction
Is
Gain of electrons

127
Q

What does REDOX stand for?

A

Reduction

Oxidation

128
Q

What is a Reduction reaction?

A

a reduction reaction is when oxygen is lost but electrons are gained

129
Q

What is an oxidation reaction?

A

an oxidation reaction is when oxygen is gained and electrons are lost

130
Q

What are the half equations for the equation “2Al + Fe₂O₃ -> Al₂O₃ + 2Fe2

A

Oxidation = Al⁰ - 3e⁻ -> Al³⁺

Reduction =Fe³⁺ + 3e⁻ -> Fe⁰

131
Q

What is the ionic equation for the equation “2Al + Fe₂O₃ -> Al₂O₃ + 2Fe2

A

Al + Fe³⁺ -> Al³⁺ + Fe

132
Q

What are the half equations for the equation “Cu + 2AgNO₃ -> Cu(NO₃)₂ + 2Ag”

A 
Oxidation = Cu - 2e⁻ -> Cu²⁺
Reduction = 2Ag⁺ + 2e⁻ -> 2Ag
133
Q

What is the ionic equation for the equation “Cu + 2AgNO₃ -> Cu(NO₃)₂ + 2Ag”

A

Cu + 2Ag⁺ -> Cu²⁺ + 2Ag

134
Q

What are the half equations for the equation “Fe + CuSO₄ -> FeSO₄ + Cu”

A 
Oxidation = Fe - 2e⁻ -> Fe²⁺
Reduction = Cu²⁺ + 2e⁻ -> Cu
135
Q

What is the ionic equation for the equation “Fe + CuSO₄ -> FeSO₄ + Cu”

A

Fe + Cu²⁺ -> Fe²⁺ + Cu

136
Q

What is the charge of a silver ion?

A

1+

137
Q

What is the charge of most transition metals?

A

2+

138
Q

What are the half equations for the equation “Pb + 2AgNO₃ -> Pb(NO₃)₂ + 2Ag”

A 
oxidation = Pb - 2e⁻ -> Pb²⁺
reduction = 2Ag⁺ + 2e⁻ -> 2Ag
139
Q

What is the ionic equation for the equation “Pb + 2AgNO₃ -> Pb(NO₃)₂ + 2Ag”

A

Pb + 2Ag⁺ -> Pb²⁺ + 2Ag

140
Q

What is the reactivity series?

A 
Potassium
Sodium
Lithium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold
Platinum
141
Q

What elements in the reactivity series are obtained by electrolysis?

A

Potassium to Aluminium

142
Q

What elements in the reactivity series are obtained by displacing them with carbon?

A

Zinc to Copper

143
Q

What elements in the reactivity series are obtained by thermal decomposition?

A

Mercury & silver

144
Q

What elements in the reactivity series are found as elements naturally?

A

Gold and Platinum

145
Q

What happens to the reactivity as you go down the reactivity series?

A

it decreases

146
Q

What happens to the difficulty of extracting the elements as you down the reactivity series?

A

It gets easier to extract the elements

147
Q

Lead is extracted by the reduction of lead oxide by heating with carbon in the equation “PbO + C -> Pb + CO” explain why lead can be extracted this way

A

Lead can be extracted by heating with carbon as carbon is more reactive than lead. This means that the carbon displaces the lead from the oxide and leaves the lead in pure form.

148
Q

Lead is extracted by the reduction of lead oxide by heating with carbon in the equation “PbO + C -> Pb + CO” explain why this is a REDOX reaction

A

This is a REDOX reaction as there is both an oxidation and a reduction. The lead is undergoing a reduction reaction, this is because it is gaining electrons but losing oxygen. The carbon is being oxidised as it is losing electrons but gaining oxygen

149
Q

What is a metallic bond?

A

The electrostatic attraction between the positive metal ions and the negative sea of valence delocalised electrons

150
Q

What is the structure of a metal

A

A giant metallic lattice

151
Q

Why do metals have high boiling points?

A

They have high melting points as they have many strong metallic bonds that need to be broken for them to melt/evaporate. This means that a lot of energy is required to break these bonds

152
Q

Why are metals malleable and ductile?

A

Metals are malleable and ductile as they have layers of metal ions that can slide over each other, due to their structure they do not repel each other

153
Q

Why are metals good conductors of thermal and electrical heat?

A

They have charged particles (delocalised electrons) that can move freely throughout the whole structure

154
Q

What type of ions do metals form?

A

cations (positive ions)

155
Q

What factors affect how readily metal atoms lose its outer shell electrons?

A
  • The number of electrons in the outer shell
  • Distance of outer shell electrons from the nucleus
  • Electrons shielding
156
Q

How does the number of electrons in the outer shell affect how readily metal atoms lose its outer shell electrons?

A

it is easier to lose 1 electron (ie group 1 metals) than 2 electrons (ie group 2 metals)

157
Q

How does distance of outer shell electrons from the nucleus affect how readily metal atoms lose its outer shell electrons?

A

The bigger the atom, the easier it is to lose electrons as the attraction of the nucleus on the valence electrons is not as strong

158
Q

How does electrons shielding affect how readily metal atoms lose its outer shell electrons?

A

The greater the number of shielding electrons, the weaker the nuclear attraction on the outer electrons, the easier it is to lose

159
Q

What is the word equation of group 1 metals and water?

A

metal + water -> metal hydroxide + hydrogen

160
Q

What is the reaction of potassium to calcium with water?

A

fizz, giving off hydrogen gas, leaving an alkaline solution of metal hydroxide

161
Q

What is the reaction of magnesium to iron with water?

A

very slow reaction

162
Q

What is the reaction of tin to lead with water?

A

slight reaction with steam

163
Q

What is the reaction of copper to platinum with water?

A

no reaction, even with steam

164
Q

What is the reaction of potassium to lithium with a dilute acid?

A

explodes, too dangerous

165
Q

What is the reaction of calcium to iron with a dilute acid?

A

fizz, giving off hydrogen and forming a salt

166
Q

What is the reaction of tin to lead with a dilute acid?

A

react slowly with warm acid

167
Q

What is the reaction of copper to platinum with a dilute acid?

A

no reaction

168
Q

What is the mnemonic for the reactivity series?

A

Please Send Lions, Cats, Monkeys, And, Crazy, Zebras Into The Largest Hat Cafe, Signed General Penguin

169
Q

How do you remember neutralisation reactions?

A

MASH
AAWS
CAWCS
BAWS

170
Q

What does MASH stand for?

A

Metal + Acid -> Salt + Hydrogen

171
Q

What does AAWS stand for?

A

Acid + Alkali -> Water + Salt

172
Q

What does CAWCS stand for?

A

Carbonate + Acid -> Water + Carbon Dioxide + Salt

173
Q

What does BAWS stand for?

A

Base (Metal Oxide) + Acid -> Water + Salt

174
Q

Why is the conical flask placed on a white tile during titration?

A

To more clearly see the colour change of the indicator solution, therefore achieving more accurate results as your data collected will be more accurate to the real end point

175
Q

Why is it not necessary to dry the conical flask before titration after washing it with distilled water?

A

The water does not affect the number of moles of alkali in the flask, therefore the same volume of acid is required to neutralise it, therefore your results are not affected

176
Q

Describe how a pipette is prepared and used for titration?

A

First you must collect all your necessary equipment and ensure that you are wearing safety goggles. Rinse the pipette with deionised water and then rinse with your alkali solution whilst twisting the pipette to unsure you wash all the sides of the pipette. Attach the pipette filler to the end of the pipette, and place the other end of the pipette in the alkali solution. Use the pipette filler to fill the pipette until the bottom of the meniscus of the alkali lies on the desired volume. Release the alkali solution into the conical flask using the pipette filler

GCSE Chemistry (15 decks)

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