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C4 Chemical Changes

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Last updated about 1 month ago
260 questions
4.4.1.1 Metal Oxides
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4.4.1.2 The Reactivity Series
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4.4.1.3 Extraction of Metals and Reducion
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4.4.1.4 Oxidation and Reduction in Terms of Electrons
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4.4.2.1 Reactions of Acids with Metals
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4.4.2.2 Neutralisation of acids and salt production
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4.4.2.3 Soluble Salts
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4.4.2.4 The pH scale and neutralisation
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4.4.2.5 Titrations
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4.4.2.6 Strong and weak acids
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4.4.3.1 The Process of Electrolysis
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4.4.3.2 Electrolysis of molten ionic compounds
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4.4.3.3 Using electrolysis to extract metals
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4.4.3.4 Electrolysis of aqueous solutions
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4.4.3.5 Representation of reactions at electrodes as half equations
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Question 1
1.

Magnesium + Oxygen --> ?

Question 2
2.

Calcium + Oxygen --> ?

Question 3
3.

Iron + Oxygen --> ?

Question 4
4.

Zinc + Oxygen --> ?

Question 5
5.

Copper + Oxygen --> ?

Question 6
6.

What do you predict when magnesium reacts with oxygen?

Question 7
7.

Calcium + water --> ?

Question 8
8.

Sodium + water --> ?

Question 9
9.

Aluminum + water --> ?

Question 10
10.

Iron + water --> ?

Question 11
11.

Zinc + copper sulfate --> ?

Question 12
12.

Aluminum + lead nitrate --> ?

Question 13
13.

Copper + silver nitrate --> ?

Question 14
14.

Aluminum + lead(II) chloride --> ?

Question 15
15.

Iron + silver nitrate --> ?

Question 16
16.

Does this reaction happen?

Zinc + copper sulfate --> copper and zinc sulfate

Question 17
17.

Does this reaction happen?

Iron + magnesium oxide --> magnesium and iron oxide

Question 18
18.

Does this reaction happen?

Aluminum + iron(III) chloride --> iron and aluminum chloride

Question 19
19.

What happens when sodium reacts with water?

Question 20
20.

What are the products of iron reacting with copper sulfate?

Question 21
21.

What do you expect when iron interacts with water?

Question 22
22.

What results when copper displaces silver from silver nitrate?

Question 23
23.

Question 24
24.

  • Pure metals don't need extracting
  • Reduction using carbon (or carbon monoxide)
  • Electrolysis
Question 25
25.

Question 26
26.
Question 27
27.

Question 28
28.

Question 29
29.

Question 30
30.
Question 31
31.

Question 32
32.

What is the salt formed when potassium reacts with hydrochloric acid?

Question 33
33.

What do you get when copper oxide reacts with sulfuric acid?

Question 34
34.

Which salt is formed when sodium hydroxide is neutralized by hydrochloric acid?

Question 35
35.

When ammonia reacts with sulfuric acid, what type of salt is produced?

Question 36
36.

What is the name for the salt formed from the reaction of Hydrochloric acid and Sodium Hydroxide?

Question 37
37.

What is the salt produced when Sulfuric acid reacts with Zinc?

Question 38
38.

Which of the following salts is formed by the reaction of Nitric acid and Potassium Hydroxide?

Question 39
39.

Ammonia reacts with Hydrochloric acid to form which salt?

Question 40
40.

Calcium chloride is a salt that can be named from hydrochloric acid.

Question 41
41.

All salts need to come from a reaction with a Metal.

Question 42
42.

Potassium sulfate can be generated from sulfuric acid.

Question 43
43.

What is the name of the salt produced from hydrochloric acid and sodium carbonate?

Question 44
44.

What is the name of the salt formed when sulfuric acid reacts with calcium oxide?

Question 45
45.

What salt forms when nitric acid reacts with magnesium hydroxide?

Question 46
46.

What is the salt produced when ammonia reacts with hydrochloric acid?

Question 47
47.

What type of salt is created when hydrochloric acid reacts with sodium?

Question 48
48.

What is the common name for the salt created when sulfuric acid reacts with potassium?

Question 49
49.

What salt is formed when nitric acid reacts with calcium?

Question 50
50.
Calcium hydroxide solution reacts with an acid to form calcium chloride.

Complete the word equation for the reaction.

calcium hydroxide + _______ acid → calcium chloride + _______
Question 51
51.

Soluble salts are formed by reacting metal oxides with acids.(a)  

Give one other type of substance that can react with an acid to form a soluble salt.

Question 52
52.

Name the salt produced by the neutralisation of hydrochloric acid with potassium hydroxide.

Question 53
53.

Write a balanced symbol equation for the reaction of dilute hydrochloric acid with calcium oxide.

Question 54
54.

Zinc + hydrochloric acid --> ?

Question 55
55.

Iron + sulfuric acid --> ?

Question 56
56.

Copper + nitric acid --> ?

Question 57
57.

Aluminum + hydrochloric acid --> ?

Question 58
58.

Predict the products of zinc reacting with hydrochloric acid.

Question 59
59.

What products are produced when zinc is placed in hydrochloric acid?

Question 60
60.

What salt is produced when hydrochloric acid reacts with sodium hydroxide?

Question 61
61.

What salt is produced from the reaction of sulfuric acid and potassium hydroxide?

Question 62
62.

Which salt forms when nitric acid interacts with calcium hydroxide?

Question 63
63.

When a metal reacts with oxygen, the common product is typically a type of metal oxide.

Question 64
64.

Plan a method to make pure, dry crystals of zinc chloride from zinc carbonate and a dilute acid.

Question 65
65.

What is the difference between hazard and risk? (1:06)

Question 66
66.

What do these symbols mean and what precautions should be taken? (1:15)

Question 67
67.

Identify any hazards associated with this experiment. (1:15)

Question 68
68.

What can we do to minimize any risks during this experiment? (1:15, 2:49)

Question 69
69.

To make copper sulfate, what will we need to react with the sulfuric acid? (2:00-2:12)

Question 70
70.

Write the word and symbol equation for the reaction. (2:00, 3:19) Word Equation: ____________________ + ____________________ → ____________________ + ____________________ Symbol Equation: _______________ + _______________ → _______________ + __________

Question 71
71.

What substances are now present in the boiling tube? Identify any ions present. (2:32-3:19)

Question 72
72.

Look at the boiling tube. Name the particle responsible for: (2:49) (a) The blue color: _________________________________________ (b) The black color: ________________________________________

Question 73
73.

Explain what is meant by a limiting reactant. (3:35)

Question 74
74.

How can we separate the product from the unreacted copper oxide? (3:43)

Question 75
75.

What is the benefit of using fluted filter paper over a conical filter? (4:01)

Question 76
76.

Describe what you see happening during the separation process. Explain your observations. (5:02-5:13)

Question 77
77.

How and why do we need to remove excess water from the filtrate? (5:14-5:20)

Question 78
78.

Why do we add anti-bumping crystals to the solution before heating? (5:24-5:40)

Question 79
79.

What health and safety problems do you think may result if the solution is allowed to boil dry? (6:12)

Question 80
80.

If there are no heat proof gloves available, what other safety precautions could be taken? (6:27)

Question 81
81.

What conditions are needed to produce larger crystals? What conditions are needed to produce smaller crystals? (6:58)

Question 82
82.

Write a method for preparing a sample of pure dry zinc sulfate crystals from a metal oxide and acid.

Question 83
83.

Categorize the following pH values as acidic, neutral, or basic.

  • pH 7
  • pH 2
  • pH 5
  • pH 9
  • Neutral
  • Acidic
  • Basic
Question 84
84.

Pair each term with its definition

Draggable itemarrow_right_altCorresponding Item
Indicator
arrow_right_alt
Reaction between an acid and a base
Neutralisation
arrow_right_alt
Measure of acidity or alkalinity
pH
arrow_right_alt
Substance that changes color in an acid or base
Question 85
85.

Match the pH value with its description

Draggable itemarrow_right_altCorresponding Item
pH 7
arrow_right_alt
Neutral
pH 2
arrow_right_alt
Strongly acidic
pH 10
arrow_right_alt
Moderately alkaline
Question 86
86.

Match the substances with their pH levels

Draggable itemarrow_right_altCorresponding Item
Distilled Water
arrow_right_alt
pH 7
Vinegar
arrow_right_alt
pH 3
Baking Soda
arrow_right_alt
pH 9
Question 87
87.

Pair the reaction type with its effect on pH

Draggable itemarrow_right_altCorresponding Item
Neutralisation Reaction
arrow_right_alt
Brings pH to 7
Adding a Base
arrow_right_alt
Raises pH
Adding an Acid
arrow_right_alt
Lowers pH
Question 88
88.

What does a pH value of 7 represent?

Question 89
89.

What does the neutralisation process involve?

Question 90
90.

Acids have a pH...

Question 91
91.

Strong acids are closest to...

Question 92
92.

Alkalis have a pH...

Question 93
93.

Strong Alkalis have a pH closest to....

Question 94
94.

What color indicates a strong acid in universal indicator?

Question 95
95.

What color indicates a weak alkali in universal indicator?

Question 96
96.

What color shows a strong alkali in universal indicator?

Question 97
97.

What color indicates a weak acid in universal indicator?

Question 98
98.

Which ion do all acids produce in aqueous solution?

Question 99
99.
Write an ionic equation for the neutralisation of hydrochloric acid with potassium hydroxide.

_______  +  _______   →  _______
Question 100
100.

Name the type of reaction that takes place when dilute hydrochloric acid reacts with calcium oxide.

1
Question 101
101.

Name apparatus A.

1
Question 102
102.

What is the reading on apparatus A?

Question 103
103.
Other Answer Choices:
0.10cm3
1
Question 104
104.
Question 105
105.

Question 106
106.

Question 107
107.

How does the pH scale change with each unit?

Question 108
108.

If a solution has a Hydrogen ion concentration ([H+]) of 10^-7 M, what is its pH?

Question 109
109.

A sample of orange juice has a pH of 5. If lemon juice is 100 times more acidic, what is the pH of the lemon juice?

Question 110
110.

Ethanoic acid is a weak acid.

What is meant by ‘weak acid’?

Answer in terms of ionisation

Question 111
111.

Explain why the pH of an acid depends on:

 the strength of the acid

the concentration of the acid.

Question 112
112.

A 1.0 × 10−3 mol/dm3 solution of hydrochloric acid has a pH of 3.0

What is the pH of a 1.0 × 10−5 mol/dm3 solution of hydrochloric acid?

Question 113
113.

Question 114
114.

Question 115
115.

What is the basic process during electrolysis?

Question 116
116.

What are two main components required for electrolysis?

Question 117
117.

Identify whether the following are cations or anions:

  • Oxygen (O2-)
  • Chlorine (Cl-)
  • Sodium (Na+)
  • Hydrogen (H+)
  • Potassium (K+)
  • Bromide (Br-)
  • Lithium (Li+)
  • Zinc (Zn2+)
  • Fluoride (F-)
  • Ammonium (NH4+)
  • Anions
  • Cations
Question 118
118.

On this diagram, label the anode, cathode, electrolyte, wires, and power source

Question 119
119.

In this example, water (H2O) is being electrolysed. What are the 2 gases being produced?

Question 120
120.

What is electrolysis?

Question 121
121.

What is the name of the electrode that positive ions move to?

Question 122
122.

What is the name of the electrode that the negative ions move to?

Question 123
123.

What is meant by the term ‘cation’?

Question 124
124.

What is the anode made of?

Question 125
125.

Match the term with its description

Draggable itemarrow_right_altCorresponding Item
Cathode
arrow_right_alt
Positive electrode where oxidation occurs.
Ion
arrow_right_alt
Charged particle that can be positive or negative.
Electrolyte
arrow_right_alt
Negative electrode where reduction occurs.
Anode
arrow_right_alt
Substance that produces an electrically conducting solution when dissolved or molten
Electrolysis
arrow_right_alt
Chemical decomposition produced by passing an electric current.
Question 126
126.

What will the electrolysis of Sodium Chloride produce?

Question 127
127.

What will the electrolysis of Copper Chloride produce?

Question 128
128.

What will the electrolysis of Potassium Iodide produce?

Question 129
129.

What will the electrolysis of Magnesium Fluoride produce?

Question 130
130.

What does the electrolysis of Potassium Chloride produce?

Question 131
131.

What will the electrolysis of Sodium Iodide result in?

Question 132
132.

What are the products of the electrolysis of Copper Chloride?

Question 133
133.

What will the electrolysis of Calcium Bromide lead to?

1
Question 134
134.

Explain why electrolysis would not take place in the apparatus shown in Figure 1.

1
Question 135
135.

Explain why graphite conducts electricity.

Answer in terms of the structure and bonding in graphite.

Question 136
136.

True or false: Electrolysis is the separation of a compound using electricity?

Question 137
137.

What is the name for the positive electrode in electrolysis?

Question 138
138.

What type of current is used in electrolysis?

Question 139
139.

What is the charge on the cathode?

Question 140
140.

True or false: Electricity is used to separate a compound during electrolysis?

Question 141
141.

What is the charge on the anode?

Question 142
142.

What is the substance that is broken down during electrolysis called?

Question 143
143.

What is the negative electrode in electrolysis known as?

Question 144
144.

What state does the electrolyte need to be in for electrolysis?

Question 145
145.

What charge are the metal ions in an ionic compound?

Question 146
146.

Why do ionic compounds conduct electricity when molten or dissolved?

Question 147
147.

What substances form negative ions?

Question 148
148.

Which electrode do the negative ions move towards?

Question 149
149.

What is the name given to positive ions?

Question 150
150.

Which electrode do the cations move towards?

Question 151
151.

What is the name given to negative ions?

Question 152
152.

Which electrode do the anions move towards?

Question 153
153.

Which electrode do positive ions move to?

Question 154
154.

What charged ions do non-metals form?

Question 155
155.

Which electrode do positive ions move to?

Question 156
156.

Which electrode do the anions move towards?

Question 157
157.

Which electrode do the anions move towards?

Question 158
158.

What is the basic process during electrolysis?

Question 159
159.

Match the term with its definition.

Draggable itemarrow_right_altCorresponding Item
Anode
arrow_right_alt
Electrode where reduction occurs in an electrolytic cell.
Electrolyte
arrow_right_alt
Electrode where oxidation occurs in an electrolytic cell.
Cathode
arrow_right_alt
A substance that produces an electrically conducting solution when dissolved in a polar solvent.
Question 160
160.

True or false: Electrolysis is the separation of a compound using electricity?

Question 161
161.

What type of current is used in electrolysis?

Question 162
162.

What is the name for the positive electrode in electrolysis?

Question 163
163.

What is the charge on the anode?

Question 164
164.

What is the negative electrode in electrolysis known as?

Question 165
165.

What state does the electrolyte need to be in for electrolysis?

Question 166
166.

Which electrode do the negative ions move towards?

Question 167
167.

Which electrode do the cations move towards?

Question 168
168.

Which electrode do positive ions move to?

Question 169
169.

Question 170
170.

Question 171
171.

Question 172
172.

Question 173
173.

Question 174
174.

Question 175
175.

Question 176
176.

Question 177
177.

Question 178
178.

Question 179
179.

Question 180
180.

Question 181
181.

Question 182
182.

What is produced at the cathode when lead bromide is electrolysed?

Question 183
183.

What is produced at the anode when lead bromide is electrolysed?

Question 184
184.

What would form at the cathode in the electrolysis of magnesium bromide?

Question 185
185.

What would form at the anode in the electrolysis of lithium chloride?

Question 186
186.

What would form at the anode in the electrolysis of molten sodium bromide?

Question 187
187.

What would form at the cathode in the electrolysis of molten aluminium chloride?

Question 188
188.

What would form at the cathode in the electrolysis of magnesium bromide?

Question 189
189.

What will the electrolysis of Magnesium Fluoride produce?

Question 190
190.

What will the electrolysis of Copper Chloride produce?

Question 191
191.

What would form at the anode in the electrolysis of molten sodium bromide?

Question 192
192.

What would form at the cathode in the electrolysis of molten aluminium chloride?

Question 193
193.

Identify the products of molten electrolysis for Calcium Bromide.

Question 194
194.

Question 195
195.

Why is electrolysis used to extract aluminium form its ore?

Question 196
196.

Why is electrolysis an expensive way to extract metal from its ore?

Question 197
197.

Name the compound from which aluminium is extracted.

Question 198
198.

What is this compound dissolved in before electrolysis?

Question 199
199.

Describe what happens at the positive electrode during the electrolysis of aluminium oxide.

Question 200
200.

What is produced at the cathode?

Question 201
201.

What is (or should be) produced at the anode?

Question 202
202.

What are the electrodes made of?

Question 203
203.

1. Why is it more economical to extract aluminium from ores rather than minerals that are not ores?

Question 204
204.

To extract aluminium, molten bauxite and another ore, cryolite, undergo electrolysis.

Explain, in terms of the environment, why cryolite is added to the electrolyte.

Question 205
205.

Explain, in terms of the economic reasons, why cryolite is added to the electrolyte.

Question 206
206.

Some people think that extracting aluminium contributes negatively to climate change.
Explain why someone might think this, without discussing energy use.

Question 207
207.

What is the half equation at the cathode?

Question 208
208.

What is the half equation at the anode?

Question 209
209.

What would be the products of molten electrolysis for Aluminum Oxide?

Question 210
210.

What will be the products of molten electrolysis for Potassium Iodide?

Question 211
211.

Explain why the electrolysis of Aluminium oxide contributes to climate change. (hand mark)

Question 212
212.

Question 213
213.

Question 214
214.

Question 215
215.

What is produced at the cathode is the metal in the solution is more reactive than hydrogen?

Question 216
216.

What is produced at the anode if the solution does not contain halide ions?

Question 217
217.

Predict the products of electrolysis of copper sulfate solution

Question 218
218.

Question 219
219.

Trim End | 06:44
Question 220 | 00:00
Question 221 | 00:15
Question 222 | 00:30
Questions 223 & 224 | 00:59
Question 225 | 01:32
Question 226 | 01:51
Question 227 | 02:01
Question 228 | 02:49
Question 229 | 03:37
Questions 230 & 231 | 03:56
Question 232 | 04:28
Question 233 | 04:50
00:00/00:00
Question 220
00:00
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Question 221
00:15
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Question 222
00:30
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Questions 223 & 224
00:59
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Question 225
01:32
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Question 226
01:51
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Question 227
02:01
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Question 228
02:49
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Question 229
03:37
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Questions 230 & 231
03:56
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Question 232
04:28
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Question 233
04:50
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Question 234
234.

HT Only: Write half equations for the reactions that happen at the
electrodes during the electrolysis of molten copper chloride.

Question 235
235.

HT Only: Write a half equation for the reactions that happen at the
electrodes during the electrolysis of copper bromide solution

Question 236
236.

HT Only: Write half equations for the reactions that occur at the positive and negative electrodes during the production of aluminium.

Question 237
237.

What is reduction in terms of electrons?

Question 238
238.

What does oxidation involve in terms of electrons?

Question 239
239.

An atom that loses an electron during a reaction is...

Question 240
240.

Rewrite the equation with number of electrons on the correct side:

Cu2+ (aq) --> Cu (s)

Question 241
241.

Rewrite the equation with number of electrons on the correct side:

Mg2+ (aq) --> Mg (s)

Question 242
242.

Rewrite the equation with number of electrons on the correct side:

Al3+ (aq) --> Al (s)

Question 243
243.

Rewrite the equation with number of electrons on the correct side:

Li+(l) -->Li(s)

Question 244
244.

Rewrite the equation with number of electrons on the correct side:

H+(aq) -->H2(g)

Question 245
245.

Rewrite the equation with number of electrons on the correct side:

Br-(aq) --> Br2(g)

Question 246
246.

Rewrite the equation with number of electrons on the correct side:

O2-(aq) --> O2(g)

2
Question 247
247.

Magnesium chloride can be electrolysed.The diagram below shows two experiments for electrolysing magnesium chloride.

Explain why magnesium chloride must be molten or dissolved in water to be electrolysed.

2
Question 248
248.

Explain how magnesium is produced at the negative electrode in Experiment 1.

Question 249
249.
Cu2+ + _______ --> Cu
Question 250
250.
Mg2+ + _______ --> Mg
Question 251
251.
Al3+ + _______ --> Al
Question 252
252.
Li1+ +_______ -->Li
Question 253
253.
2H1+ + _______ -->H2
Question 254
254.
2Br1- --> Br2 + _______
Question 255
255.
2O2- --> O2 + _______
1
Question 256
256.
Zinc chloride is an ionic substance.

Complete the sentence.

When zinc chloride is molten, it will conduct _______
1
Question 257
257.

Zinc ions move towards the negative electrode where they gain electrons to produce zinc.    

Name the product formed at the positive electrode.

1
1
Question 260
260.

What does oxidation involve in terms of electrons?

Question 220
220.

What is electrolysis?

Question 221
221.

What is the correct unit of volume?

Question 222
222.

What are electrodes made of?

Question 223
223.

What is the charge of the anode?

Question 224
224.

What is the charge of the cathode?

Question 225
225.

What is the general name of the solution being electrolysed?

Question 226
226.

What are the products of a solution of Copper Chloride

Question 227
227.

What does damp blue litmus paper test for?

Question 228
228.

What is the balanced half equation at the anode?

Question 229
229.

What is the half equation at the cathode?

Question 230
230.

In solutions, which metals can be electrolysed out?

Question 231
231.

Explain your previous choice?

Question 232
232.

What are the bubbles in the electrolysing the solution of Sodium Sulfate?

Question 233
233.

What is the test for hydrogen?

Question 258
258.

Explain why zinc ions move towards the negative electrode.

Question 259
259.

What type of reaction occurs when the zinc ions gain electrons?