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GCSE Combined Chemistry (Edexcel) > Topic 3 & 4 - Chemical Changes and Extracting Metals and Equilibria > Flashcards

Topic 3 & 4 - Chemical Changes and Extracting Metals and Equilibria Flashcards

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1
Q
  1. What term describes a substance that attacks metals, stonework and skin?
A

corrosive

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2
Q
  1. Name an acidic solution found in the kitchen.
A

vinegar or fruit juice, etc.

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3
Q
  1. Name an alkaline solution used in the kitchen.
A

bleach or oven cleaner or soap, etc.

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4
Q
  1. What type of substance turns litmus paper red?
A

acid

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5
Q
  1. How does an indicator show the acidity or alkalinity of solutions?
A

by changing colour

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6
Q
  1. What pH values represent alkaline solutions?
A

above 7 or 8 to 14

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7
Q
  1. What happens in all chemical reactions?
A

new substances are formed

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8
Q
  1. What kind of reaction occurs between an acid and an alkali?
A

neutralisation

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9
Q
  1. What do you call a solution that is neither acidic nor alkaline.
A

neutral

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10
Q
  1. Give the name and formula of a common laboratory acid.
A

hydrochloric acid (HCl) or nitric acid (HNO3) or sulfuric acid (H2SO4), etc.

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11
Q
  1. Which ion is in excess in all acidic solutions?
A

hydrogen ions or H+ ions

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12
Q
  1. Which ion is in excess in all alkaline solutions?
A

hydroxide ions or OH– ions

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13
Q
  1. What scale is used for measuring acidic and alkaline properties?
A

the pH scale

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14
Q
  1. Name three examples of acid/alkali indicators apart from universal indicator.
A

litmus, methyl orange and phenolphthalein

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15
Q
  1. What would you use to measure pH to one decimal place?
A

a pH meter

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16
Q
  1. What pH values are acidic?
A

below 7

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17
Q
  1. What colour is phenolphthalein in a solution with a pH of 2?
A

colourless

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18
Q
  1. What happens to the pH as the H+ ion concentration increases?
A

it decreases

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19
Q
  1. If a solution has the same concentration of hydrogen ions as hydroxide ions, how is it described?
A

neutral or pH = 7

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20
Q
  1. If 2 g of salt is dissolved in 250 cm3 of solution, what is its concentration in g dm–3?
A

8 g dm–3

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21
Q
  1. What word describes a solution that contains a large amount of solute in a small volume of solvent?
A

concentrated

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22
Q
  1. How can a solution be made more dilute?
A

by adding solvent/water

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23
Q
  1. If 24 g of acid is dissolved in 600 cm3 of solution, what is its concentration in g dm–3?
A

40 g dm–3

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24
Q
  1. What happens when strong acid molecules dissolve in water?
A

they dissociate completely into ions

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25
Q
  1. What kind of reaction occurs between an acid and a base?
A

neutralisation

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26
Q
  1. What happens to the pH of an acid as it reacts with a neutraliser?
A

pH increases

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27
Q
  1. What is formed when an acid reacts with a base like a metal oxide?
A

salt + water

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28
Q
  1. What acid would be used to make zinc sulfate from zinc oxide?
A

sulfuric acid (sulphuric acid makes sulphates!)

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29
Q
  1. What process can be used to separate an insoluble solid from a liquid?
A

filtration

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30
Q
  1. How can a sample of a dissolved salt be obtained from a salt solution?
A

evaporation of the water

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31
Q
  1. In general, what is the pH of an alkaline solution?
A

greater than 7

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32
Q
  1. Which ions, hydrogen ions or hydroxide ions, are released by alkalis in solution?
A

hydroxide ions (OH-)

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33
Q
  1. What colour is litmus solution in acidic solutions?
A

red

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34
Q
  1. What name is given to substances that react with acids to form a salt and water only?
A

bases (bases are metal oxides and hydroxides, soluble bases are alkalis)

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35
Q
  1. Which salt is formed when copper oxide reacts with sulfuric acid?
A

copper sulfate

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36
Q
  1. What type of reaction happens between an acid and a base?
A

neutralisation

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37
Q
  1. What type of solution has a pH of 7?
A

neutral

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38
Q
  1. Name the acid that has the formula HCl.
A

hydrochloric acid

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39
Q
  1. What colour is phenolphthalein in alkaline solutions?
A

pink (it is colourless in acid conditions)

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40
Q
  1. What is the formula for sulfuric acid?
A

H2SO4

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41
Q
  1. Name the salt produced when sodium hydroxide reacts with hydrochloric acid.
A

sodium chloride

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42
Q
  1. Which ions, hydrogen ions or hydroxide ions, are released by acids in solution?
A

hydrogen ions (H+)

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43
Q
  1. What substance, other than a salt, is produced when an alkali neutralises an acid?
A

water

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44
Q
  1. What name is given to substances that are soluble bases?
A

alkalis

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45
Q
  1. What is the formula for hydrochloric acid?
A

HCl

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46
Q
  1. What type of solution has a pH above 7?
A

alkaline

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47
Q
  1. What colour is phenolphthalein in acidic solutions?
A

colourless – not ‘clear’

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48
Q
  1. Name a piece of apparatus used to measure volumes of liquid.
A

measuring cylinder/pipette/burette

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49
Q
  1. Name the separation method used to produce crystals from a solution.
A

crystallisation

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50
Q
  1. Name the acid needed to make ammonium nitrate.
A

nitric acid

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51
Q
  1. Which acid can be used to make copper sulfate?
A

sulfuric acid

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52
Q
  1. Which base can be used to make copper sulfate?
A

copper oxide

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53
Q
  1. Which substance is needed to complete the general equation: acid + base makes salt + …?
A

water (BASHO)

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54
Q
  1. What is the formula of nitric acid?
A

HNO3

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55
Q
  1. What is the name of the salt formed from zinc oxide and hydrochloric acid?
A

zinc chloride

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56
Q
  1. What is the formula of the salt formed from calcium oxide and hydrochloric acid?
A

CaCl2

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57
Q
  1. Which ions are present in large quantities in aqueous solutions of all acids?
A

H+ Hydrogen ions

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58
Q
  1. Which ions are present in large quantities in aqueous solutions of all alkalis?
A

OH– Hydroxide ions

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59
Q
  1. Which gas is formed when dilute hydrochloric acid reacts with magnesium?
A

hydrogen (MASH)

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60
Q
  1. Which gas is formed when dilute hydrochloric acid reacts with magnesium carbonate?
A

carbon dioxide (CASHOCO)

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61
Q
  1. What acid can be used to make copper chloride?
A

hydrochloric acid (hydrochloric acid makes chlorides)

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62
Q
  1. What gas is given off when magnesium reacts with dilute sulfuric acid?
A

hydrogen (MASH)

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63
Q
  1. How do you identify Hydrogen gas?
A

gives a squeaky pop with a lighted splint

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64
Q
  1. What is seen when magnesium is added to dilute sulfuric acid?
A

effervescence/fizzing/bubbles (yes you know this is hydrogen, but you can not see that!!)

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65
Q
  1. What is the formula of magnesium sulfate?
A

MgSO4

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66
Q
  1. What gas is produced when copper carbonate is added to dilute nitric acid?
A

carbon dioxide (CASHOCO)

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67
Q
  1. How do you test for Carbon Dioxide?
A

it turns limewater milky

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68
Q
  1. What is the formula of the salt produced when copper carbonate reacts with nitric acid?
A

(Cu(NO3)2)

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69
Q
  1. Sodium chloride dissolves in water to form a solution. Which is the solute?
A

sodium chloride

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70
Q
  1. What do we call the liquid that dissolves a solute to form a solution.
A

solvent

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71
Q
  1. What is the formula of water?
A

H2O

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72
Q
  1. What is the formula of sodium chloride?
A

NaCl

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73
Q
  1. What is the formula of carbon dioxide?
A

CO2

74
Q
  1. The formula of magnesium chloride is MgCl2. What is the ratio of magnesium ions to chloride ions?
A

1:2

75
Q
  1. The formula of sulfuric acid is H2SO4. How many atoms of each element are in the formula?
A

H = 2, S = 1, O = 4

76
Q
  1. The formula of calcium nitrate is Ca(NO3)2. How many calcium, nitrogen and oxygen atoms are in the formula?
A

Ca = 1, N = 2, O = 6

77
Q
  1. There are two numbers alongside chlorine in the periodic table, 17 and 35.5. What does the number 17 represent?
A

atomic number

78
Q
  1. What does the number 35.5 represent?
A

relative atomic mass

79
Q
  1. Sodium chloride has the formula NaCl. The relative atomic mass of sodium is 23 and that of chlorine is 35.5. What is the relative formula mass of NaCl?
A

58.5

80
Q
  1. A water molecule has the formula H2O. The relative atomic mass of hydrogen is 1 and that of oxygen is 16. What is the relative formula mass of a molecule of water?
A

18

81
Q
  1. What is the symbol for relative atomic mass?
A

Ar or RAM

82
Q
  1. What is the symbol for relative formula mass?
A

Mr or RFM

83
Q
  1. The relative atomic mass of hydrogen is 1. What is the relative formula mass of hydrogen molecules?
A

2

84
Q
  1. Sodium chloride has the formula NaCl; the relative atomic mass of sodium is 23 and that of chlorine is 35.5. What is the relative formula mass of NaCl?
A

58.5

85
Q
  1. A water molecule has the formula H2O; the relative atomic mass of hydrogen is 1 and that of oxygen is 16. What is the relative formula mass of water?
A

18

86
Q
  1. A carbon dioxide molecule has the formula CO2; the relative atomic mass of carbon is 12 and that of oxygen is 16. What is the relative formula mass of carbon dioxide?
A

44

87
Q
  1. What is the empirical formula of a compound with molecular formula C2H4?
A

CH2

88
Q
  1. What is the empirical formula of a compound with molecular formula C3H8?
A

C3H8

89
Q
  1. A sample of magnesium carbonate was heated in an open test tube. Why did it lose mass?
A

gas/carbon dioxide escaped

90
Q
  1. 100 cm3 of a solution contained 2 g of salt. What is the concentration of the salt in g dm-3?
A

20

91
Q
  1. A sample of copper carbonate was heated in an open test tube. Why did it lose mass?
A

gas/carbon dioxide escaped

92
Q
  1. Why does magnesium increase in mass when it is heated in air?
A

combines with oxygen

93
Q
  1. How many cm3 are there in 1 dm3?
A

1000

94
Q
  1. What is 250 cm3 expressed in dm3?
A

0.25

95
Q
  1. What is 0.5 dm3 expressed in cm3?
A

500

96
Q
  1. 100 cm3 of a solution contains 1.5 g of salt. What is the concentration of the salt solution in g dm3?
A

15

97
Q
  1. 250 cm3 of a solution contains 5 g of sugar. What is the concentration of the sugar solution in g dm3?
A

20

98
Q
  1. A solution of copper sulfate has concentration 10 g dm3. What mass of copper sulfate will be dissolved in 100 cm3 of solution?
A

1 g

99
Q
  1. 2 g of hydrogen reacts with oxygen to form 18 g of water. What mass of water will be formed from 1 g of hydrogen?
A

9 g

100
Q
  1. 2H2 + O2 → 2H2O. How many molecules of hydrogen are needed to react with 1 dozen molecules of oxygen to form water?
A

2 dozen

101
Q
  1. What is the abbreviation used for the mole, the unit for amount of substance?
A

mol

102
Q
  1. How many particles are there in 1 mole of particles?
A

6.02 x 1023

103
Q
  1. The mass of 1 mole of carbon atoms is 12 g. What is the mass of 2 moles of carbon atoms?
A

24 g

104
Q
  1. What is the formula for calculating the number of moles of substance from its mass in g
A

moles = mass (g) / RAM or RFM

105
Q
  1. Each water molecule contains three atoms. How many moles of atoms are there in 2 moles of water molecules?
A

6 mol

106
Q
  1. The relative formula mass of chlorine gas is 71. What is the mass of 1 mole of chlorine gas?
A

71 g

107
Q
  1. What is the Avogadro number?
A

6.02 x 1023 the number of atoms/particles in a mole

108
Q
  1. What is the emperical formula of a compound?
A

The simplist whole number ratio of atoms in compound

109
Q
  1. What is the law of conservation of mass?
A

total mass of reactants = total mass of products

110
Q
  1. How are the emperical formula and molecular formula related?
A

The molecular formula is a multiple of the emperical formula

111
Q
  1. What name is given to an atom that has gained or lost electrons?
A

ion

112
Q
  1. What type of charge is on metal and hydrogen ions?
A

positive

113
Q
  1. What type of charge is on most non-metal ions?
A

negative

114
Q
  1. What is another name for a positive ion?
A

cation

115
Q
  1. What is another name for a negative ion?
A

anion

116
Q
  1. What is the symbol for a sodium ion?
A

Na+

117
Q
  1. What is the symbol for a magnesium ion?
A

Mg2+

118
Q
  1. What is the symbol for a chloride ion?
A

Cl<span>-</span>

119
Q
  1. What is the symbol for a sulfate ion?
A

SO42-

120
Q
  1. In what states do ionic compounds conduct electricity?
A

when molten or dissolved in water

121
Q
  1. Which of these is not an electrolyte: solid sodium chloride, molten sodium chloride, aqueous sodium chloride?
A

solid sodium chloride

122
Q
  1. What is the name of the positively charged electrode?
A

anode

123
Q
  1. What type of ions are attracted to the positively charged electrode?
A

anions / negative ions

124
Q
  1. What is the name of the negatively charged electrode?
A

cathode

125
Q
  1. What type of ions are attracted to the negatively charged electrode?
A

cations / positive ions

126
Q
  1. H What process takes place when a substance gains electrons?
A

reduction

127
Q
  1. H In terms of subatomic particles, what happens to a substance when it is oxidised?
A

It loses electrons.

128
Q
  1. H What type of reaction takes place at the anode during electrolysis?
A

oxidation

129
Q
  1. What are inert electrodes made from?
A

graphite / platinum

130
Q
  1. What is produced at the cathode when molten lead bromide is electrolysed?
A

lead

131
Q
  1. What gas is formed when sodium reacts with water?
A

hydrogen

132
Q
  1. What solution is formed when sodium reacts with water?
A

sodium hydroxide

133
Q
  1. What colour is universal indicator when added to sodium hydroxide?
A

blue or purple

134
Q
  1. What gas is formed when magnesium is added to dilute sulfuric acid?
A

hydrogen (MASH)

135
Q
  1. What solution is formed when magnesium reacts with dilute sulfuric acid?
A

magnesium sulfate

136
Q
  1. What would you see when magnesium is added to dilute sulfuric acid?
A

effervescence/fizzing/bubbles/magnesium disappears

137
Q
  1. Name a metal that does not react with water or dilute acids.
A

copper/silver/gold/platinum

138
Q
  1. What products are formed when zinc is added to copper sulfate solution?
A

zinc sulfate and copper

139
Q
  1. What type of reaction takes place when zinc is added to copper sulfate solution?
A

displacement

140
Q
  1. Magnesium reacts with chromium nitrate solution to form magnesium nitrate and chromium. Which metal is more reactive?
A

magnesium

141
Q
  1. Name a metal that reacts vigorously with cold water.
A

potassium/sodium/rubidium/caesium/lithium/calcium

142
Q
  1. What gas is produced when a metal reacts with water?
A

hydrogen

143
Q
  1. How do you test for the gas produced in question 2?
A

It pops a lighted splint.

144
Q
  1. What type of solution is formed when a metal reacts with water - acidic, alkaline or neutral?
A

alkaline

145
Q
  1. What salt is formed when zinc reacts with hydrochloric acid?
A

zinc chloride

146
Q
  1. Complete the word equation, magnesium + copper sulfate makes …
A

copper + magnesium sulfate

147
Q
  1. What type of ions are formed from metal atoms when they react with acids?
A

cations/positive ions

148
Q
  1. What type of reaction takes place when a substance loses oxygen?
A

reduction

149
Q
  1. Name a metal that occurs uncombined in the Earths crust.
A

gold/silver/platinum

150
Q
  1. Name a metal that could be extracted from its metal oxide by heating with carbon.
A

zinc/iron/copper

151
Q
  1. Name a metal that occurs uncombined in the Earths crust.
A

gold/silver/platinum

152
Q
  1. Name a metal, other than iron, that could be extracted from its metal oxide by heating with carbon.
A

zinc/copper

153
Q
  1. What compound of carbon is formed when it is heated with copper oxide?
A

carbon dioxide/carbon monoxide

154
Q
  1. Why is electrolysis not used to extract iron from iron oxide?
A

too expensive/too much energy needed

155
Q
  1. Why is aluminium not extracted by heating aluminium oxide with carbon?
A

aluminium is more reactive than carbon/carbon is not reactive enough to remove the oxygen

156
Q
  1. What is the aluminium oxide dissolved in to form the electrolyte for electrolysis?
A

molten cryolite

157
Q
  1. What are the electrodes made from?
A

carbon/graphite

158
Q
  1. At which electrode is the aluminium produced?
A

cathode/negative electrode

159
Q
  1. What type of reaction takes place when a metal is extracted from its ore?
A

reduction/redox

160
Q
  1. What type of reaction takes place when a metal corrodes?
A

oxidation/redox

161
Q
  1. What is the definition of oxidation, in terms of oxygen?
A

gain of oxygen

162
Q
  1. H What is the definition of oxidation, in terms of electrons?
A

loss of electrons

163
Q
  1. What type of reaction takes place when metals are extracted from their ores?
A

reduction/redox

164
Q
  1. What is the specific name for the corrosion of iron?
A

rusting

165
Q
  1. Which of these metals will corrode most quickly - iron, sodium, copper?
A

sodium

166
Q
  1. Why does sodium corrode most quickly.
A

most reactive metal corrodes most quickly

167
Q
  1. Which substance has been oxidised in this reaction - copper oxide + hydrogen → copper + water?
A

hydrogen

168
Q
  1. Which substance has been reduced in in this reaction - copper oxide + hydrogen → copper + water?
A

copper oxide

169
Q
  1. What name is given to a process that converts an unwanted product into a new, useful product?
A

recycling

170
Q
  1. Name a type of substance that can be recycled.
A

metal, plastic, paper, cardboard, glass, etc.

171
Q
  1. What can happen in a reversible reaction?
A

the products can reform the reactants

172
Q
  1. What does the term equilibrium describe?
A

a position of balance

173
Q
  1. What is the process used to make ammonia?
A

Haber Process

174
Q
  1. What is the molecular formula of ammonia?
A

NH3

175
Q
  1. What is the balanced symbol equation for making ammonia from Nitrogen (N2) and Hydrogen (H2)
A

N2 +3H2 → 2NH3

176
Q
  1. Where does nitrogen come from for use in the Haber Process?
A

From the fractional distillation of air

177
Q
  1. Where does Hydrogen come from for use in the Haber process?
A

From methane from crude oil

178
Q
  1. What conditions of pressure are required to increase the yield of ammonia in the Haber Process?
A

High pressure (because there are more molecules on the LHS of the equation)

179
Q
  1. The forward reaction is exothermic. What conditions of temperature are required to increase the yield of ammonia in the Haber Process?
A

Low temperature (The equilibrium will shit to try and produce heat)

180
Q
  1. Theoretically, a high yield of ammonia is produce at low temperature and high pressure. Why is this not used in reality?
A

Low temperatue will result in a slow rate of reaction. High pressures are expensive and dangerous.

GCSE Combined Chemistry (Edexcel) (5 decks)

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