9. Metals Flashcards

Question

general explanation of redox reaction between magnesium and hydrochloric acid

Answer 1

When magnesium reacts with hydrochloric acid, its atoms lose electrons (is oxidised). The hydrogen ions from the acid gain electrons (are reduced).

Answer 2

Mg –> Mg2+ + 2e- (oxidation) 2H+ + 2e- –> H2 (reduction)

Answer 3

Metals are put in order based on their reactivity with water and hydrochloric acid

Answer 4

There’s no reaction This means magnesium is more reactive than carbon

Answer 5

Turns into molten lead and CO2 is formed Carbon is more reactive than lead 2PbO + C —> 2Pb + CO2

Answer 6

Carbon is more reactive than some metals. It will reduce their oxides (be oxidised itself - its a reducing agent) to form the metals.

Answer 7

The reaction gives out heat and the mixture glows. Iron (II) oxide and copper are formed. The iron is more reactive and takes the oxygen from copper - displaces it.

Answer 8

Fe + CuO —> FeO + Cu

Answer 9

A reducing agent - reduces copper but is oxidised itself.

Answer 10

A metal will reduce the oxide of a less reactive metal. The reduction always gives out heat - it is exothermic.

Answer 11

Copper coats the nail. The solution turns green, which indicated iron (II) ions. Iron has pushed (displaced) copper out of the solution - it is MORE REACTIVE.

Answer 12

Fe + CuSO4 —> FeSO4 + Cu

Answer 13

A metal displaces a less reactive metal from solutions of its compounds.

Answer 14

The more reactive metal forms positive ions more readily - is oxidised more readily The more reactive metal will give up electrons to form ions and the less reactive one will accept them to form a solid version of the metal.

Answer 15

P S L C M A (C) Z I L (H) C S G

Answer 16

really a list of metals in order of their drive to form positive ions with stable outer shells,. The more easily its atoms can give up electrons the more reactive the metal will be

Answer 17

It’ll react by displacing (pushing out) the less reactive metal out of the compound and taking its place

Answer 18

the more reactive a metal is the more stable its compounds are. THEY DO NOT BREAK DOWN EASILY

Answer 19

The more reactive the metal, the more difficult it is to extract from its ores since their compounds are stable.

Answer 20

The less reactive the metal, the less likely it is to form a compound.

Answer 21

When a compound breaks down on heating

Answer 22

1 & 2 - no change in white compound Nitrate - White compound partly decomposes to nitrite and oxygen 2NaNO3 —> 2NaNO2 + O2

Answer 23

The blue-green compound readily breaks down to black copper (III) oxide and carbon dioxide. CuCO3 —> CuO + CO2

Answer 24

The pale blue compound readily breaks down to copper (II) oxide and water: Cu(OH)2 —> CuO + H2O

Answer 25

The bright blue compound readily breaks down to copper (II) oxide and the brown gas nitrogen oxide. 2Cu(NO3)2 —> 2CuO + 4NO2 + O2

Answer 26

The lower a metal is in the reactivity series, the more readily its compounds decompose when heated Carbonates, (except Na & K) decompose to the oxide and CO2 Hydroxides, (except Na & K) decompose to oxide and H2O Nitrates (except Na & K) decompose to the oxide, NO2 & CO2. (Nitrates of Na & K form nitrites and oxygen)

Answer 27

The thermite process In making simple cells In the sacrificial protection of iron Galvanising

Answer 28

To repair rail and tram lines

Answer 29

Powdered aluminium and iron (III) oxide are put in a container over the damaged rail

Answer 30

When the mixture is lit, the aluminium reduces the iron (III) oxide to molten iron in a very vigorous reaction. The iron runs into the cracks and gaps in the rail and hardens.

Answer 31

Fe2O3 + 2Al —> 2Fe + Al2O3

Answer 32

The difference in reactivity causes a redox reaction that gives out energy in the form of electricity

Answer 33

A simple cell consists of two different metals in an electrolyte.

Answer 34

Electrons flow from the more reactive metal, so it is called the negative pole. The other is the positive pole.

Answer 35

The further apart the metals are in reactivity, the higher the voltage will be

Answer 36

Measure the voltage that makes electrons flow

Answer 37

zinc, magnesium, etc anything more reactive than iron A block of the metal may be welded to the structure e.g a ship

Answer 38

Oxidation - Zn —> Zn2+ + 2e- R O2 + 2H2O + 4e- —> 4OH-

Answer 39

2Zn + O2 + 2H2O —> 2Zn(OH)2

Answer 40

used for the steel in car bodies and the corrugated iron for roofing

Answer 41

When iron / steel are coated by zinc

Answer 42

Carried out by a form of electrolysis

Answer 43

Iron is dipped in a bath of molten zinc

Answer 44

Zinc coating keeps air and moisture away.

Answer 45

In SP, zinc block has to be replaced before it’s dissolved but in galvanising even if the coating is damaged, the iron still won’t be damaged due to SP

Answer 46

Aluminium protects itself reacts rapidly with oxygen forming a thin coat of aluminium oxide (which you can’t see) this sticks tight to the metal acting as a barrier to further corrosion, leading to aluminium acting as if it was unreactive

Answer 47

Squeaky ‘pop’ test

Answer 48

…Will displace a less reactive metal from an aqueous solution of one of its salts.

Answer 49

An equation that shows only those ions or atoms that change in a chemical reaction. Mg + CuSO4 -> MgSO4 + Cu Mg + Cu2+ -> Mg2+ + Cu

Answer 50

The gain and loss of electrons

Answer 51

Displacement with carbon Electrolysis

Answer 52

> Organised in closely packed, regularly set out layers. Contain a sea of free moving, delocalised electrons. When heated, soft and easily shaped because the layers can easily slip over each other.

Answer 53

Because they usually have controlled amounts of carbon mixed into their structure, which disrupts their regular layout and prevents the layers from sliding over one another.

Answer 54

Through stron electrostatic attraction between the free electrons and the positively charged ions.

Answer 55

Mixture of metal which responds to changes in temperature.

Answer 56

> bendable but strong > very conductive.

Answer 57

Copper + Tin Tough and non-corrosive

Answer 58

Copper + Zinc Hard

Answer 59

Lightweight but strong, used for aircrafts, armoured tanks etc.

Answer 60

The huge reaction vessels used in industry to extract iron from its core.

Answer 61

> iron ore (haematite) -iron oxide -a compound that contains iron > coke -carbon -burns in air to produce heat, and reacts to form carbon monoxide (needed to reduce the iron oxide) > limestone -calcium carbonate -helps to remove acidic impurities from the iron by reacting with them to form molten slag > air -oxygen -allows the coke to burn, and so produces heat and carbon monoxide

Answer 62

Alloy of iron containing controlled, small amounts of carbon.

Answer 63

Expensive alloy of Iron mixed with a relatively large proportion of other metals.

Answer 64

Alloy of Iron containing between 1-5% of other metals.

Answer 65

A natural resource that can be used to make a useful product.

Answer 66

Hematite Fe3O2

Answer 67

Iron ore (Fe2O3) Coke (C) Limestone (CaCo3) Preheated air

Answer 68

Molten iron Molten slag Waste gases

Answer 69

Nitrogen It makes up 80% of the air that enters the furnace but does not react in the furnace.

Answer 70

Its less dense.

Answer 71

The molten iron is not in contact with the preheated air so will not get reoxidised by the oxygen in the preheated air.

Answer 72

Heating coal in the absence of air.

Answer 73

C(s) + O2 (g) —> CO2 (g)

Answer 74

It produces heat for the other reactions in the furnace (which are all endothermic)

Answer 75

Calcium carbonate —> calcium oxide + carbon dioxide CaCo3 —> CaO + CO2

Answer 76

Silica/silicon dioxide

Answer 77

Slag/calcium silicate

Answer 78

Calcium oxide + silicon dioxide —> calcium silicate CaO + SiO2 —> CaSiO3 Neutralisation

Answer 79

The iron would become brittle and break.

Answer 80

Road building - motorways heat insulation blocks

Answer 81

At the bottom where heat enters.

Answer 82

It is exothermic and provides heat for the other reactions.

Answer 83

Carbon dioxide + Coke —> Carbon monoxide CO2 (g) + C(s) —> 2CO(g)

Answer 84

Reducing agent CO removes oxygen from the iron ore 3CO + Fe2O3 —> 2Fe + 3CO2

Answer 85

High pressure oxygen is blown into the molten iron. It oxidises the carbon to carbon dioxide which then escapes.

Answer 86

A mixture of metals or metals with non-metals

Answer 87

The electrons/ions can slide over one another.

Answer 88

Alloying metal atoms are a different size to iron atoms and stop the layers from sliding past each other.

Answer 89

Stainless steel - cutlery Titanium steel - bicycle frames Mild Steel - car bodies Hard Steel - chisels

Answer 90

Delocalised electrons that move through the lattice when a potential is applied.

Answer 91

Electrolysis

Answer 92

Graphite (carbon)

Answer 93

Anode = + Cathode = -

Answer 94

Aluminium oxide (alumina) and cryolite

Answer 95

Electricity

Answer 96

Carbon dioxide - the oxygen produced at the anode combines with the carbon anode.

Answer 97

The melting point is extremely high.

Answer 98

to reduce the operating temperature of aluminium - its a solvent

Answer 99

Al^3+ + 3e- —> Al

Answer 100

2O- - 4e- —> O2

Answer 101

The oxides have been oxidised to oxygen molecules (loss electrons)

Answer 102

The aluminium ions have been reduced to aluminium atoms (gaining electrons)

Answer 103

They are warn out because they are reacting with the oxygen in the air to form carbon dioxide (C+O2 —> CO2)

Answer 104

A lattice of Al+++ ions hold together by delocalised electrons.

Answer 105

Delocalised electrons/ions can move freely around the structure with potential applied.

Answer 106

Bauxite Al2O3

Answer 107

The ions/electrons are stuck in the lattice unable to move freely.

Answer 108

Aluminium is more reactive than carbon. Carbon cannot remove the oxygen from the aluminium.

Answer 109

Aeroplane bodies - low density Drink cans - malleable Overheated power cables - conduct electricity Pans for cooking food - conducts heat well

Answer 110

Can be hammered into sheets

Answer 111

Layers of aluminium atoms that can slide past each other freely.

Answer 112

Can be drawn out into wire

Answer 113

Metals or non metals and metals mixed together.

Answer 114

Magnalium To make aeroplanes bodies as they have a low density.

Answer 115

In pure aluminium the atoms are all of the same size so the layers of atoms can slide past each other easily. The atoms of the metals alloyed with aluminium are of a different size. They therefore disrupt the lattice and stop the layers from sliding over each other.

Answer 116

High density Good conductors Malleable Ductile High fixed points

Answer 117

Form basic oxides Form positive ions

Answer 118

Form basic oxides Form positive ions

Answer 119

A mixture of metals

Answer 120

Copper and zinc Stronger and more resistant to corrosion Electrical fittings, car radiators

Answer 121

Copper and tin Harder, stronger and sonorous Statues, springs, coins

Answer 122

Iron, chromium and nickel Does not rust Kitchen sinks, cutlery, chemical plant

Answer 123

The different sized metal atoms disrupt the crystal lattice and make the arrangement less regular - stops layers of sliding over each other when force is applied

Answer 124

K – Potassium Na – Sodium Li – Lithium Ca – Calcium Mg – Magnesium Al – Aluminium C – Carbon Zn – Zinc Fe – Iron Pb – Lead H – Hydrogen Cu – Copper Ag – Silver Au – Gold

Answer 125

displace hydrogen from its acids

Answer 126

It forms an oxide layer which adheres to metal and protects it

Answer 127

reactions in which metals compete for oxygen or anions

Answer 128

the faster the displacement reaction

Answer 129

Electrolysis

Answer 130

Reducing via heating with Carbon or Carbon Monoxide

Answer 131

1) Coke burns to form CO2 which heats the furnace 2) CO2 reacts with coke to form carbon monoxide 3) Carbon monoxide reduces iron (III) oxide to form iron 4) Heat from furnace decomposes limestone 5) Calcium oxide reacts with silicon (IV) oxide to form slag 6) Slag run off

Answer 132

the tendency of a metal to form its positive ion

Answer 133

zinc blende/zinc sulfide

Answer 134

1) Zinc blende roasted (with oxygen) to form zinc oxide 2) Zinc oxide heated w/ coke in blast furnace 3) Carbon reacts with oxygen to form carbon monoxide 4) Carbon monoxide reduces zinc oxide to zinc 5) Zinc oxide can also react directly with carbon 6) Zinc vapour carried and condenses and purified

Answer 135

Produces purer zinc

Answer 136

1) Molten iron from blast furnace poured into steelmaking furnace 2) Oxygen + calcium oxide blown through oxygen lance 3) Oxygen oxidises impurities (carbon, sulfur, silicon, phosphorus) - some escape as gas, some react with calcium oxide to form slag 4) Amount of carbon controlled by oxygen blown, more carbon, less carbon 5) Addition of other metals to form steel

Answer 137

Mild steel: machinery and car bodies High carbon steel: knives and blades

Answer 138

saves land that may be used for extracting ores conserves metal ores + raw materials saves energy, less fuel is used

Answer 139

collecting and storing materials costly takes time and energy to collect waste materials

Answer 140

manufacture of aircraft (strength +low density) food containers (resistance to corrosion)

Answer 141

electrical wiring cooking utensils (malleable/good conductor of heat)

Answer 142

galvanise iron (stop rusting)

Answer 143

Change carbon content

Answer 144

Strength Hardness Resistance to corrosion

Answer 145

Please Stop Calling Me A Cute Zebra I Like Her Call Smart Goat

Answer 146

Aluminum is too reactive

Answer 147

To lower the melting point - since electrolytes can’t be kept at high temp. for long To improve conductivity

Answer 148

Calcium Flouride

Answer 149

The extraction of aluminum from purified bauxite or aluminum oxide is done through the process of electrolysis. Here are the steps involved in the extraction process: Preparation of alumina: Bauxite ore is purified to yield a white powder, aluminum oxide, also known as alumina. This is done by crushing the bauxite ore, mixing it with sodium hydroxide, and heating it in a kiln to produce pure alumina. Preparation of cryolite: The pure alumina is then mixed with cryolite, a mineral that acts as a solvent for alumina and lowers its melting point. Electrolysis: The alumina-cryolite mixture is then dissolved in a large electrolytic cell, which is made of steel and lined with carbon. Carbon anodes are immersed in the electrolyte, and a large graphite cathode is suspended in the center of the cell. Electrical current: A direct current is passed through the cell, causing the alumina to break down into aluminum ions and oxygen ions. The aluminum ions are attracted to the cathode, where they gain electrons and form molten aluminum metal. The oxygen ions react with the carbon anodes to form carbon dioxide gas. Collection of aluminum: The molten aluminum is then siphoned off and transferred to holding tanks, where it solidifies into aluminum ingots. Recycling: The remaining electrolyte, which contains dissolved alumina and cryolite, is pumped out of the cell and recycled for use in the next batch of alumina. Overall, the extraction of aluminum from purified bauxite or aluminum oxide involves a complex process of electrolysis, which requires a large amount of electrical energy and specialized equipment. However, this process is essential for the production of aluminum, which is a versatile and important metal used in a wide range of applications, from aircraft manufacturing to packaging materials.

Answer 150

Potassium Sodium Calcium Magnesium Note that metals such as zinc, iron, copper, and silver are not reactive enough to react with cold water.

Answer 151

Hematite (Iron III Oxide)

Answer 152

1500 degrees celsius 250 degrees celsius

Answer 153

hematite, air, coke, limestone

Answer 154

carbon monoxide

Answer 155

exothermic - heat released keeps furnace heated

Answer 156

(a) Burning of carbon (coke) to provide heat and produce carbon dioxide: Coke is burned in the blast furnace to provide the heat required for the extraction of iron. The carbon in the coke reacts with the oxygen in the air to produce carbon dioxide and heat. (b) Reduction of carbon dioxide to carbon monoxide: Carbon dioxide produced from the combustion of coke is reduced to carbon monoxide by passing it through hot coke. (c) Reduction of iron(III) oxide by carbon monoxide: The carbon monoxide produced in step (b) is then used to reduce the iron(III) oxide in the hematite ore to iron metal. The reaction can be represented by the following equation: Fe2O3 + 3CO → 2Fe + 3CO2 (d) Thermal decomposition of calcium carbonate/limestone to produce calcium oxide: Limestone (calcium carbonate) is added to the furnace to help remove impurities in the ore. When heated, it decomposes to produce calcium oxide and carbon dioxide. CaCO3 → CaO + CO2 (e) Formation of slag: The impurities in the ore react with the calcium oxide to form a molten slag, which is less dense than the molten iron and floats on top of it. The slag is then removed from the furnace. Overall, the extraction of iron from hematite ore in the blast furnace involves the burning of coke to provide heat and produce carbon dioxide, reduction of carbon dioxide to carbon monoxide, reduction of iron(III) oxide by carbon monoxide, thermal decomposition of calcium carbonate/limestone to produce calcium oxide, and the formation of slag.

Answer 157

(a) C + O2 → CO2 (b) C + CO2 → 2CO (c) Fe2O3 + 3CO → 2Fe + 3CO2 (d) CaCO3 → CaO + CO2 (e) CaO + SiO2 → CaSiO3

Answer 158

calcium silicate

Answer 159

road building

Answer 160

road building

Answer 161

metals- good conductor of heat non-metals- poor conductor

Answer 162

this is because the layers of +ive ions can slide over each other making it easy

Answer 163

metals- great conductors non metals- poor conductors

Answer 164

metals- maellable, ductile, shiny non metals- quite brittle, not ductile not malleable

Answer 165

due to presence of free moving electrons

Answer 166

giant 3 dimensional structure in which regular rows of positive ions are surrounded by ‘sea’ of free moving electrons

Answer 167

generally high

Answer 168

metals- great conductors non metals- poor conductors

Answer 169

due to presence of free moving electrons

Answer 170

giant 3 dimensional structure in which regular rows of positive ions are surrounded by ‘sea’ of free moving electrons

Answer 171

generally high

Answer 172

because of the strong metallic bonds between molecules

Answer 173

a metal oxide

Answer 174

metal oxide

Answer 175

metal+oxygen

Answer 176

hydroxide+ hydrogen gas

Answer 177

sodium, calcium and potassium

Answer 178

metal oxide+ hydrogen gas

Answer 179

salt+ hydrogen

Answer 180

when they react, hydrogen atom in acid is replaced by metal atom to produce a salt and hydrogen gas

Answer 181

the unreactive metals; AG and AU, gold and silver

Answer 182

alkali metals

Answer 183

because of it’s low density

Answer 184

because of its low density and good electrical conductivity

Answer 185

because of its resistance to corrosion

Answer 186

because of its good electrical conductivity and ductility

Answer 187

a mixture of a metal with other elements

Answer 188

copper and zinc

Answer 189

as an alloy because it is made up of a mixture of a metal with other elements

Answer 190

mixture of iron and other elements such as chromium, nickel and carbon

Answer 191

alloys can be harder and stronger than the pure metals and are more useful

Answer 192

Alloys contain atoms of different sizes, which distorts the normally regular arrangements of atoms in metals This makes it more difficult for the layers to slide over each other, so alloys are usually much harder than the pure metal

Answer 193

in cutlery because of its hardness and resistance to rusting

Answer 194

potassium, sodium, calcium, magnesium, aluminium, carbon, zinc, iron, hydrogen, copper, silver, gold

Answer 195

no, Alloys are mixtures of substances, they are not chemically combined and an alloy is not a compound.

Answer 196

Stainless steel is the most durable and long-lasting cutlery material, perfect for everyday use. It is strong even at high temperatures, resistant to water and washing in dishwashers. Another benefit is it’s easy to care for and keeps a lasting shine and corrosion resistant, and it doesn’t affect the flavour of the food when used for food storage or production. Due to the resistance level, foods with high acidity won’t cause damage.

Answer 197

a metal higher up on this reactivity series can displace any metal below it in a single displacement reaction. For example, potassium (K) can displace magnesium (Mg), zinc (Zn), iron (Fe), copper (Cu), and silver (Ag) from their aqueous solutions in single displacement reactions. However, silver (Ag) cannot displace any of the metals above it from their aqueous solutions. To illustrate this, consider the reaction between copper (Cu) and silver nitrate (AgNO3). Copper is less reactive than silver, so it cannot displace silver from its aqueous solution: Cu(s) + 2AgNO3(aq) → no reaction On the other hand, if we take zinc and copper sulfate, zinc is more reactive than copper, so it can displace copper from its aqueous solution: Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)

Answer 198

This reaction occurs because potassium is highly reactive and has a strong tendency to lose its outermost electron, which reacts with water to produce hydrogen gas and hydroxide ions.

Answer 199

undergoes a violent and exothermic reaction, producing potassium hydroxide (KOH) and hydrogen gas (H2): 2K(s) + 2H2O(l) → 2KOH(aq) + H2(g)

Answer 200

The reaction of sodium with cold water is similar to the reaction of potassium with cold water, as both metals are highly reactive alkali metals that readily lose their outermost electrons to form cations. However, the reaction of sodium with water is not as violent as the reaction of potassium with water. Nonetheless, the reaction can produce enough heat to ignite the hydrogen gas produced, so it should not be performed without proper safety precautions.

Answer 201

undergoes a highly exothermic and vigorous reaction, producing sodium hydroxide (NaOH) and hydrogen gas (H2): 2Na(s) + 2H2O(l) → 2NaOH(aq) + H2(g)

Answer 202

undergoes a less vigorous reaction compared to sodium and potassium, producing calcium hydroxide (Ca(OH)2) and hydrogen gas (H2): Ca(s) + 2H2O(l) → Ca(OH)2(aq) + H2(g) Calcium is less reactive than sodium and potassium, but it still has a strong tendency to lose its outermost electrons, which reacts with water to produce hydrogen gas and hydroxide ions. The calcium hydroxide produced is slightly soluble in water, forming a white precipitate.

Answer 203

it undergoes a displacement reaction, producing magnesium oxide (MgO) and hydrogen gas (H2): Mg(s) + H2O(g) → MgO(s) + H2(g) The reaction of magnesium with steam is an example of a metal reacting with a non-metal oxide to produce a metal oxide and a gas. The reaction occurs because magnesium has a strong tendency to lose its outermost electrons, which can then react with the oxygen in steam to form magnesium oxide. The hydrogen gas is produced as a byproduct of the reaction.

Answer 204

When hydrochloric acid (HCl) is added to magnesium (Mg), a single displacement reaction takes place, producing magnesium chloride (MgCl2) and hydrogen gas (H2): Mg(s) + 2HCl(aq) → MgCl2(aq) + H2(g) The reaction between HCl and magnesium is an example of an acid-metal reaction, where the acid donates hydrogen ions to the metal to form a salt and hydrogen gas. The hydrogen gas is produced as a byproduct of the reaction and can be observed as bubbles in the solution. The reaction between HCl and magnesium is exothermic and produces heat, but the reaction is not as violent as the reaction between metals like sodium and potassium with acids.

Answer 205

When hydrochloric acid (HCl) is added to zinc (Zn), a single displacement reaction takes place, producing zinc chloride (ZnCl2) and hydrogen gas (H2): Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g) The reaction between HCl and zinc is an example of an acid-metal reaction, where the acid donates hydrogen ions to the metal to form a salt and hydrogen gas. The hydrogen gas is produced as a byproduct of the reaction and can be observed as bubbles in the solution. The reaction between HCl and zinc is exothermic and produces heat, but the reaction is not as violent as the reaction between metals like sodium and potassium with acids.

Answer 206

When hydrochloric acid (HCl) is added to iron (Fe), a single displacement reaction takes place, producing iron (II) chloride (FeCl2) and hydrogen gas (H2): Fe(s) + 2HCl(aq) → FeCl2(aq) + H2(g) The reaction between HCl and iron is an example of an acid-metal reaction, where the acid donates hydrogen ions to the metal to form a salt and hydrogen gas. The hydrogen gas is produced as a byproduct of the reaction and can be observed as bubbles in the solution. The reaction between HCl and iron is exothermic and produces heat, but the reaction is not as violent as the reaction between metals like sodium and potassium with acids. Iron (II) chloride is a greenish-yellow solid that is soluble in water.

Answer 207

When hydrochloric acid (HCl) is added to copper (Cu), no visible reaction occurs. Copper is not reactive enough to displace the hydrogen ions in HCl to form a copper chloride salt and hydrogen gas. Copper is less reactive than hydrogen, so it cannot replace hydrogen in hydrochloric acid. Therefore, copper does not react with hydrochloric acid under normal conditions. However, if the concentration of the hydrochloric acid is increased or the temperature is raised, a slow reaction may occur with the formation of copper (II) chloride (CuCl2) and hydrogen gas (H2): Cu(s) + 2HCl(aq) → CuCl2(aq) + H2(g) It is important to note that this reaction is not as common or practical as the other reactions of HCl with metals, as copper is generally not used as a reactive metal due to its low reactivity.

Answer 208

Gold (Au) is a noble metal and is unreactive towards most acids, including hydrochloric acid (HCl). As such, there is no visible reaction between HCl and gold. Gold does not readily react with acids or other chemicals and remains largely inert, which is why it is commonly used in jewelry and other decorative items. Therefore, there is no reaction between hydrochloric acid and gold

Answer 209

Aluminium (Al) is a reactive metal, but it appears unreactive due to the presence of a thin layer of oxide that forms on its surface when it comes into contact with air. This oxide layer is composed of aluminium oxide (Al2O3) and is very stable and resistant to further oxidation. The oxide layer acts as a protective layer, preventing further oxidation of the metal. When aluminium is exposed to air, the surface layer reacts with oxygen to form a layer of aluminium oxide. This layer is typically only a few nanometers thick, but it is very dense and adheres strongly to the metal surface. The oxide layer effectively seals the underlying metal from further exposure to the environment, preventing corrosion and other forms of chemical attack. In the presence of an acid or base, the oxide layer is dissolved, exposing the underlying metal to further reaction. This is why aluminium can react with acids and bases, despite its apparent unreactivity in air. However, once the acid or base is removed, the oxide layer reforms, restoring the protective barrier and preventing further reaction. In summary, the apparent unreactivity of aluminium is due to the presence of a stable and protective oxide layer on its surface that prevents further oxidation and chemical attack.

Answer 210

Water: Rusting requires the presence of water or moisture. This is because water is needed to react with iron to form hydrated iron(III) oxide. Oxygen: Rusting also requires the presence of oxygen. Iron reacts with oxygen in the presence of water to form hydrated iron(III) oxide. Electrolytes: Rusting is accelerated in the presence of electrolytes, such as salts and acids. This is because these substances increase the conductivity of the water, allowing for faster and more efficient transfer of electrons between the iron and oxygen. In the absence of any one of these conditions, rusting will not occur. For example, in a dry environment, rusting cannot occur because there is no water to react with the iron. Similarly, in the absence of oxygen, rusting cannot occur because iron cannot react with water to form hydrated iron(III) oxide.

Answer 211

painting, greasing and coating with plastic

Answer 212

in absence of oxygen or water, rusting can’t happen as it can’t react with water to form hydrated iron(III) oxide Painting: Painting is a common barrier method used to prevent rusting. A layer of paint is applied to the surface of the metal, creating a barrier that prevents oxygen and water from coming into contact with the metal. Coating: Coating is similar to painting, but uses a different material, such as a plastic or polymer, to create a barrier. This method is commonly used in the automotive industry to protect car bodies from rusting. Greasing: Greasing involves applying a layer of grease or oil to the metal surface, which prevents water from coming into contact with the metal. This method is commonly used to protect metal components in machinery and engines. Galvanizing: Galvanizing involves coating the metal surface with a layer of zinc, which is more reactive than iron and will corrode in preference to the iron. This method is commonly used to protect steel structures, such as bridges and buildings.

Answer 213

Galvanizing is a process that involves coating iron or steel with a layer of zinc, either by hot-dip galvanizing or electroplating. Zinc is commonly used for galvanizing because it is highly reactive and readily corrodes in preference to iron. This makes it an effective sacrificial anode, which provides protection to the underlying iron or steel. In the galvanizing process, the iron or steel is first cleaned to remove any impurities or surface contaminants. The cleaned surface is then dipped into a bath of molten zinc, which adheres to the surface of the metal, forming a protective layer. Alternatively, the metal can be electroplated with a layer of zinc using an electric current. The zinc layer acts as a barrier, preventing water and oxygen from coming into contact with the underlying metal surface. In addition, because zinc is more reactive than iron, it will corrode preferentially to the iron, sacrificing itself to protect the underlying metal from corrosion. This process is known as sacrificial protection. Over time, the zinc layer will gradually corrode and eventually wear away. However, by the time the zinc layer is completely consumed, the underlying metal will have been protected from corrosion for a significant period of time. The effectiveness of the sacrificial protection depends on the thickness of the zinc layer and the environment in which the metal is exposed. Galvanizing is commonly used to protect steel structures, such as bridges, buildings, and pipelines, from corrosion. It is also used in the manufacturing of many everyday products, such as automotive parts, household appliances, and fencing.

Answer 214

Sacrificial protection is a method of protecting a metal from corrosion by connecting it to another more reactive metal. The principle of sacrificial protection is based on the reactivity series of metals, which is a list of metals arranged in order of their reactivity towards oxygen and water. In the reactivity series, metals at the top of the list, such as potassium and sodium, are highly reactive and readily lose electrons to form positive ions. Metals at the bottom of the list, such as gold and platinum, are relatively unreactive and do not readily lose electrons. When two different metals are connected in an electrolyte, such as saltwater, the more reactive metal will tend to lose electrons and undergo oxidation, while the less reactive metal will tend to gain electrons and undergo reduction. This creates a flow of electrons from the more reactive metal to the less reactive metal, known as a galvanic cell. In sacrificial protection, a more reactive metal, such as zinc or magnesium, is connected to the metal to be protected, such as iron or steel. The more reactive metal acts as a sacrificial anode, which corrodes preferentially to the less reactive metal, providing protection against corrosion. In terms of electron loss, sacrificial protection involves the transfer of electrons from the more reactive metal to the less reactive metal, which results in the less reactive metal being protected from corrosion. The more reactive metal loses electrons and undergoes oxidation, while the less reactive metal gains electrons and undergoes reduction. This process is driven by the tendency of the more reactive metal to lose electrons and form positive ions, which are then attracted to the less reactive metal.

Answer 215

the more up the metal the harder as its more reactive and can more easily chemically combine with other elements making it hard to extract the lower(less reactive) the easier to extract as they don’t easily react w other elements

Answer 216

electrolysis

Answer 217

in a blast furnace

Answer 218

(a) Burning of carbon (coke) to provide heat and produce carbon dioxide: Coke is burned in the blast furnace to provide the heat required for the extraction of iron. The carbon in the coke reacts with the oxygen in the air to produce carbon dioxide and heat. (b) Reduction of carbon dioxide to carbon monoxide: Carbon dioxide produced from the combustion of coke is reduced to carbon monoxide by passing it through hot coke. (c) Reduction of iron(III) oxide by carbon monoxide: The carbon monoxide produced in step (b) is then used to reduce the iron(III) oxide in the hematite ore to iron metal. The reaction can be represented by the following equation: Fe2O3 + 3CO → 2Fe + 3CO2 (d) Thermal decomposition of calcium carbonate/limestone to produce calcium oxide: Limestone (calcium carbonate) is added to the furnace to help remove impurities in the ore. When heated, it decomposes to produce calcium oxide and carbon dioxide. CaCO3 → CaO + CO2 (e) Formation of slag: The impurities in the ore react with the calcium oxide to form a molten slag, which is less dense than the molten iron and floats on top of it. The slag is then removed from the furnace. Overall, the extraction of iron from hematite ore in the blast furnace involves the burning of coke to provide heat and produce carbon dioxide, reduction of carbon dioxide to carbon monoxide, reduction of iron(III) oxide by carbon monoxide, thermal decomposition of calcium carbonate/limestone to produce calcium oxide, and the formation of slag.

Answer 219

(a) C + O2 → CO2 (b) C + CO2 → 2CO (c) Fe2O3 + 3CO → 2Fe + 3CO2 (d) CaCO3 → CaO + CO2 (e) CaO + SiO2 → CaSiO3

Answer 220

purified bauxite / aluminium oxide

Answer 221

The extraction of aluminum from purified bauxite or aluminum oxide is done through the process of electrolysis. Here are the steps involved in the extraction process: Preparation of alumina: Bauxite ore is purified to yield a white powder, aluminum oxide, also known as alumina. This is done by crushing the bauxite ore, mixing it with sodium hydroxide, and heating it in a kiln to produce pure alumina. Preparation of cryolite: The pure alumina is then mixed with cryolite, a mineral that acts as a solvent for alumina and lowers its melting point. Electrolysis: The alumina-cryolite mixture is then dissolved in a large electrolytic cell, which is made of steel and lined with carbon. Carbon anodes are immersed in the electrolyte, and a large graphite cathode is suspended in the center of the cell. Electrical current: A direct current is passed through the cell, causing the alumina to break down into aluminum ions and oxygen ions. The aluminum ions are attracted to the cathode, where they gain electrons and form molten aluminum metal. The oxygen ions react with the carbon anodes to form carbon dioxide gas. Collection of aluminum: The molten aluminum is then siphoned off and transferred to holding tanks, where it solidifies into aluminum ingots. Recycling: The remaining electrolyte, which contains dissolved alumina and cryolite, is pumped out of the cell and recycled for use in the next batch of alumina. Overall, the extraction of aluminum from purified bauxite or aluminum oxide involves a complex process of electrolysis, which requires a large amount of electrical energy and specialized equipment. However, this process is essential for the production of aluminum, which is a versatile and important metal used in a wide range of applications, from aircraft manufacturing to packaging materials.

Answer 222

Potassium Sodium Calcium Magnesium Note that metals such as zinc, iron, copper, and silver are not reactive enough to react with cold water.

Answer 223

Potassium Sodium Calcium Magnesium Aluminum Zinc Iron Note that metals such as copper and silver do not react with steam.

Answer 224

Magnesium Zinc Iron Tin Lead Nickel Copper and silver do not react with dilute hydrochloric acid. Note that the reaction of these metals with hydrochloric acid produces hydrogen gas and the corresponding metal chloride.

Answer 225

to reduce the operating temperature of aluminium oxide so that the extraction of it is much cheaper

Answer 226

so that we can extract pure aluminium as the carbon anode reacts with oxygen in the air to form CO2

Answer 227

Al 3+ 3e—-> Al 2O2- → O2 + 4e-

Answer 228

metals are found on the left of the table- to the left of the ladder which starts above aluminium and steps down to the right

Answer 229

conducts electricity and heat shiny malleable ductile some are magnetic

Answer 230

Group 1 Li Na K Rb

Answer 231

Group 2 Be Mg Ca Sr

Answer 232

They form colourful compounds & They often have more than one valency Fe 2+ and Fe 3+

Answer 233

Group 7 F Cl Br I They are all diatomic!

Answer 234

Group 0 He Ne Ar Kr they all have a full outer shell and are inert (unreactive)

Answer 235

Hydrogen Copper Silver Platinum Gold- unreactive

Answer 236

potassium sodiium calcium magnesium aluminium carbon All these metals must be extracted using electrolysis as carbon cannot displace them as it is less reactive

Answer 237

Carbon Zinc Iron Tin :Lead Hydrogen These metals can be extracted from their ores using carbon or coke in a blast furnace

Answer 238

Carbon is more reactive than iron Carbon displaces iron iron is reduced

Answer 239

copper is less reactive than hydrogen copper cannot displace hydrogen and so it does not react

Answer 240

copper is less reactive than hydrogen copper cannot displace hydrogen and so it does not react

Answer 241

soft - can be cut with a knife shiny when cut but then quickly reacts and becomes dull low melting point

Answer 242

remember the fizzing? reactive metal + water –> metal hydroxide + hydrogen

Answer 243

Li (s) + H2O(l) –> LiOH(aq) + H2(g) Lithium hydroxide is an alkali- it will turn universal indicator blue

Answer 244

For sodium fizzing, moving around on the surface of the water melts into a ball, metal disappears For potassium - it is more reactive more vigorousfizzing moving around on the surface of the water more quickly melts into a ball and bursts into flame (lilac in colour) metal disappears more rapidly

Answer 245

Na (s) + H2O(l) –> NaOH(aq) + H2(g) sodium hydroxide is an alkali- it will turn universal indicator blue

Answer 246

K (s) + H2O(l) –> KOH(aq) + H2(g) potassium hydroxide is an alkali- it will turn universal indicator blue

Answer 247

Potassium lilac flame Rubidium explosive

Answer 248

A mixture of a metal and metal or a metal and non-metal which changes both the physical and chamical properties

Answer 249

Brass- copper + zinc Bronze- copper + tin Steel- iron + carbon

Answer 250

The smaller atoms disrupts the arrangment of the metal ions, They no longer arrange themselves in neat rows They do not have layers which can slide over one another They are no longer malleable- they are harder and stronger

Answer 251

hydrogen can be collected by downward displacement of water OR downward displacement of air - upside down test tube- hydrogen is less dense than air and will rise into the test tube and push the air downward

Answer 252

Mg + H2O (g) –> MgO + H2 steam with steam the oxide is formed-not the hydroxide!

Answer 253

potassium atom is larger outer electrons of potassium are further from the nucleus less electrostatic attraction between the negative outer electrons and positive nucleus easier to remove the outer electron from potassium Also, there are more shells between the nucleus and outer electrons in potassium the electrons in these shells repel the outer electrons and is called electron shielding easier to remove the outer electron from potassium potassium is more reactive for these two reasons!

Answer 254

Thermite reaction!! Is aluminium more reactive than iron? YES! 2Al + Fe2O3 –> Al2O3 + 2Fe Aluminiuim is more reactive than iron aluminium displaces the iron This is a displacement reaction

Answer 255

Metal + steam –> metal oxide + hydrogen You still get hydrogen but now you have the oxide- not the hydroxide

Answer 256

Flaming splint you hear a squeaky pop!

Answer 257

aluminium forms an impermeable aluminium oxide layer. The acid must get through that layer before it comes into contact with the pure metal. This impermeable oxide layer on aluminium is an advantage- iron reacts with oxygen and rusts entirely through the metal but aluminium forms an impermeable oxide layer protecting the pure aluminium below.

Answer 258

more reactive metal + less reactive metal compound –> more reactive metal compound + less reactive metal the more reactive metal displaces the less reactive metal This is a displacement reaction

Answer 259

Is zinc more reactive than copper? Yes Zn + CuSO4 –> ZnSO4 + Cu greysolid & blue solution –> colourless solution & orange/pink soild

Answer 260

Thermite reaction is used to connect (fuse) iron rails together on a railway. This reaction is carried out above the seam between the two rails The reaction is exothermic- it releases heat rapidly and exceed the melting point of iron which melts out the bottom of the vessel and onto the seam.

Answer 261

Is iron more reactive than zinc? No- the rion cannot displace the zinc No reaction - grey metal in colourless solution with no change to appearance

Answer 262

Ca + 2MgNO3 –> Ca(NO3 )2 + 2Mg

Answer 263

The Mg and Fe reaction will be more vigorous because Mg and Fe are further apart in the reactivity series. The further apart metals are in the reactivity series the more violent their displacement reactions will be.

Answer 264

Place the metals in the same concentration and type of acid and compare the rate of fizzing the more vigorous the fizzing, the more reactive the metal

Answer 265

the electrostatic attractionn between potive metal ions and the negative delocalised electrons

Answer 266

regular arrangement of metal ions layers of metal ions surrounded by a sea of delocalised electrons

Answer 267

many strong metallic bonds in a giant structure requires a lot of energy to overcome

Answer 268

No- they are not soluble in either. NOTE: reactive metals react with water but they are not soluble

Answer 269

metals have delocalised electrons which are free to move and carry charge

Answer 270

metal ion layers can slide over one another without distrubing the metallic bonds

Answer 271

iron (III) oxide limestone coke hot air

Answer 272

iron metal carbon dioxide slag

Answer 273

carbon dioxide is a greenhouse gas which may lead to global warming

Answer 274

combustion of coke C + O2 –> CO2 exothermic!!!

Answer 275

C + CO2 –> 2CO coke is added in excess so that CO is formed (carbon monoxide) carbon monoxide is the reducing agent- it reduces the iron (III) oxide

Answer 276

iron (III) oxide

Answer 277

Fe2O3 + 3CO –> 3CO2 + 2Fe Fe has been reduced - lost oxygen C is oxidised - gained oxygen

Answer 278

Fe2O3 + 3CO –> 3CO2 + 2Fe Fe has been reduced - lost oxygen C is oxidised - gained oxygen

Answer 279

OIL RIG OIL - oxidation is loss of electrons RIG - reduction is gain of electrons REMEMBER: if the atom has gained or lost oxygen you must speak about that and not the gain or loss of electrons

Answer 280

To get rid of the impurity found in iron ore First- the limestone thermally decomposes to calcium oxide because the blast furnace is hot CaCO3 –> CaO + CO2 The calcium oxide then reacts with the impurity silicon dioxide to form calcium silicate OR SLAG CaO + SiO2 –> CaSiO3 SLAG The slag is less dense than the molten iron and float on top

Answer 281

Thermal decomposition means that the compound breaks apart by heating CaCO3 –> CaO + CO2

Answer 282

This is a neutralisation reaction metal oxide CaO - acidic non-metal oxide SiO2 - alkaline CaO + SiO2 –> CaSiO3 alkaline + acid –> salt

Answer 283

silicon dioxide SiO2

Answer 284

Both are molten (melted) but the slag is less dense and floats on top of the molten iron

Answer 285

combustion or oxidation as carbon gained oxygen

Answer 286

Thermal Decomposition the CaCO3 is decomposing or breaking apart

Answer 287

4Fe + 3O2 + 5H2O –> 2Fe2O3*5H2O iron needs both water and oxygen to rust! Note: salt in not needed but is a catalyst- it speeds up the reaction by lowering hte activation energy but is not used in the reaction

Answer 288

iron (III) oxide

Answer 289

paint - to stop oxygen and water getting to iron coat in plastic- to stop oxygen and water getting to iron oil or grease- to stop oxygen and water from getting to irion

Answer 290

galvanising- coating in zinc- used for buckets etc sacrificial protection with block of magnesium or zinc- used for bridges or large structures where coating in zinc is too expensive

Answer 291

sacrificial protection Zn metal –> Zn 2+ + 2e- zinc reacts and gives 2 electrons to any iron ions which have formed to reduce it back to iron metal- protecting the iron and sacrificing the zinc Fe 3+ + 3 e- –> Fe metal

Answer 292

Fe2O3 + 3Zn –> 3ZnO + 2Fe iron is reduced as it is losing oxygen zinc is oxidised as it is gaining oxygen

Answer 293

carbon dioxide is soluble in water- if collected by downward dislacement of water the carbon dioxide would dissolve in the water carbon dioxide is more dense than air- if a tube was placed in a upright test tube the more dense carbon dioxide would fill the test tube and push the air out.

Answer 294

bubble though limewater limewater turns cloudy

Answer 295

green power moves as gas escapes the green powder turns black

Answer 296

CuCO3 –> CuO + CO2

Answer 297

CaCO3 –> CaO + CO2

Answer 298

Carbon is less reactive than Aluminium it cannot displace aluminium from aluminium ore?

Answer 299

Bauxite Al2O3

Answer 300

electrolysis

Answer 301

The decomposition of a compound using electricity

Answer 302

Aluminium ore is ionic, when melted the metal ions are free to move and carry charge we need electricity to pass through the molten ore for electrolysis to occur

Answer 303

Cryolite is added to the aluminium ore- this reduced the melting point of the ore Less heat is used- cheaper process

Answer 304

Electrolysis used both electricity and heat to extract the metal. Blast furnace only needs heat

Answer 305

Al 3+ O 2-

Answer 306

Al 3+ is positively charged and will be attracted to the cathode or negatively charge electrode O 2- is negatively charged and will be attracted to the anode or positviely charge electrode

Answer 307

The positive aluminium ions will be attracted to the bottom of the container allowing the aluminium to form there- it can then be tapped off

Answer 308

Aluminium oxide is ionic, when molten the ions are free to move and carry charge When in the solid form the ions are not free to move and cannot carry charge

Answer 309

It is soluble in water to form an acid It is more dense than air

Answer 310

A pure metal will have a regular arrangement of atoms. The rows of metal atoms can slide easily over one another without disrupting the metallic bond Alloys are a mixture of metals or a metal and non-metal. This often disrupts the regular arrangement. There are no complete rows of atoms which can slide over each other. Not malleable-harder substance

Answer 311

Hematite (mostly Fe2O3 + some impurities)

Answer 312

Coke(carbon) is burnt to give off heat C + O2 –> CO2 Carbon monoxide is made C + CO2 –> 2CO Iron(III) oxide is reduced Fe2O3 + 3CO –> 2Fe + 3CO2

Answer 313

1.Break down limestone in the furnace CaCO3 –> CaO + CO2 2.CaO (lime) reacts with the sand that’s made of mainly silicon dioxide to make slag (calcium silicate) CaCO3 + SiO2 –> CaSiO3

Answer 314

Removes impurities

Answer 315

Slag is known as Calcium silicate (CaSiO3) It’s less dense than molten iron so it floats on top of the molten iron and is then tapped off.

Answer 316

Carbon monoxide (CO)

Answer 317

Name: Zinc blende It’s mainly zinc sulfide

Answer 318

Roast the zinc blende 2ZnS + 3CO2 –> 2ZnO + 2SO2 OXIDE CAN BE REDUCED BY 2 WAYS A = Using CO (approx 907 degrees C): ZnO + CO –> Zn + CO2 B = Electrolysis: Zinc is deposited at the cathode. Zn2+(aq) + 2e- –> Zn(s)

Answer 319

Reducing agent

Answer 320

The zinc extracted by electrolysis is at very high purity where as with using CO the zinc is not pure and you’ll need to take further steps to remove the impurities.

Answer 321

CATHODE: Al3+ + 3e- –> Al ANODE: 2O2- -4e- –> O2 Forms Carbon dioxide as some of the oxygen reacts with the carbon from the graphite electrodes. C + O2 –> CO2

Answer 322

2045 degrees C

Answer 323

Al2O3 dissolved in Cryolite. There are also the impurities

Answer 324

It lowers the temperature that needs to be maintained for electrolysis from 2045 to around 945 degrees C

Answer 325

Form alloys Car frames and parts Bike frames

Answer 326

In the earth’s crust

Answer 327

Compounds, some elements such as: Cu, Ag, Hg, Pt, Au - occur native 45% O2 27% silicon

Answer 328

Compounds, some elements such as: Cu, Ag, Hg, Pt, Au - occur native 45% O2 27% silicon

Answer 329

They’re uncombined because they are “unreactive”

Answer 330

Si and O - make up nearly 3/4 occur together in compounds e.g silicon dioxide (silica or sand) O2 found in compounds such as iron(III) oxide, aluminium oxide, calcium carbonate

Answer 331

Gold, silver, platinum and palladium - scarce, expensive, often kept as a store of wealth

Answer 332

a rock from which metals are obtained / extracted

Answer 333

bauxite - contains impurities such as sand and iron oxide

Answer 334

how much ore is there how much metal will we get from it are there any special problems getting the ore out how much will it cost to mine the ore and extract the metal from it how much will we be able to sell the metal for will they make profit

Answer 335

roads, buildings, mining equipment, the extraction plant, transport, fuel, chemicals and wages

Answer 336

Yes - even low-quality / low-grade ore may be valuable one year

Answer 337

may spoil an area air and rivers can become polluted P - may welcome new jobs

Answer 338

They are native - occur in their ore as elements All you need to do is separate the metal from sand and other impurities DOES NOT INVOLVE CHEMICAL REACTIONS

Answer 339

To remove a metal from its ore

Answer 340

They’re heated with carbon (or CO) or a suitable reducing agent so that they’re reduced They’re less stable

Answer 341

Their compounds are very stable need electrolysis to reduce them costs a lot because it uses electricity

Answer 342

in the form of coke (coal)

Answer 343

Zn, Fe, Pb

Answer 344

K, Na, Ca, Mg, Al

Answer 345

In its metal oxide

Answer 346

If carbon reacts with the limited amount of oxygen, this may bring about the actual reduction

Answer 347

Fe2O3 + 3CO —> 2Fe + 3CO2 iron (III) oxide

Answer 348

(extracted by electroysis) 2Al2O3 —> 4Al + 3O2

Answer 349

Mainly zinc sulfide - ZnS

Answer 350

First, zinc blende is roasted in air giving zinc oxide and sulfur dioxide. 2ZnS + 3O2 —> 2ZnO + SO2

Answer 351

1. Using carbon monoxide 2. By electrolysis

Answer 352

ZnO + CO —> Zn + CO2

Answer 353

Zinc and a slag of impurities Separated by fractional distillation (907 degrees C)

Answer 354

Dissolved in dilute sulfuric acid (sulfur dioxide made during roasting stage) To reduce its melting point (1975 degrees C) (its also insoluble in water)

Answer 355

Zinc sulfate - zinc oxide is a base so it neutralises the sulfuric acid giving a solution of zinc sulfate

Answer 356

Zinc is deposited at the cathode Zn2+ + 2e- —> Zn (reduction)

Answer 357

gives zinc of a very high purity

Answer 358

calcium and lead appear as impurities in the zinc blende and these metals are recovered and sold too

Answer 359

Scraped off the cathode and melted into bars to sell

Answer 360

overhead electricity cables (with a steel core for strength) cooking foil and food cartons drinks cans coating CDs and DVDS

Answer 361

a good conductor of electricity (not as good as copper, but cheaper and much lighter); ductile, resists corrosion

Answer 362

non-toxic, resistant to corrosion, can be rolled into thin sheets

Answer 363

light, non-toxic, resistant to corrosion

Answer 364

can be deposited as a thin film; shiny surface reflects laser beam

Answer 365

electrical wiring saucepans and saucepan bases

Answer 366

one of the best conductors of electricity, ductile

Answer 367

malleable, conducts heat well, unreactive, tough

Answer 368

protecting steel from rusting coating or galvanising iron and steel for torch batteries

Answer 369

offers sacrificial protection to the iron in steel

Answer 370

resists corrosion, but offers sacrificial protection if coating cracks

Answer 371

gives a current when connected to a carbon pole, packed into a paste of electrolyte

Answer 372

A mixture where at least one other substance is added to a metal, to improve its properties; the other substance is often a metal too

Answer 373

So that the atoms of the second metal can entre the lattice

Answer 374

Turning a metal into an alloy changes its properties and makes it more useful.

Answer 375

Metal atoms are arranged in a lattice (in a pure metal) When pressure is applied, e.g hammering, the layers can slide over each other easily When the metal is turned into an alloy, new atoms of different sizes enter the lattice. The layer can NO LONGER slide easily

Answer 376

Could be more resistant to corrosion

Answer 377

Brass and Aluminum alloy 7075 TF

Answer 378

70% Copper 30% Zinc

Answer 379

Harder than copper Does not corrode

Answer 380

Musical instruments Ornaments Doorknobs

Answer 381

90.25 % Aluminium 6% Zinc 2.5% Magnesium 1.25% Copper

Answer 382

light but very strong does not corrode

Answer 383

too soft stretches quite easily rusts very easily

Answer 384

99.7% iron 0.3% carbon

Answer 385

Hard and Strong buildings ships car bodies machinery

Answer 386

20% chromium, 10% nickel and 70% iron

Answer 387

Hard and Rustproof cutlery equipment in chemical factories surgical tools (easy to sterilise)

Answer 388

A mixture called the charge, containing iron ore is added through the top of the furnace. Hot air is blasted in through the bottom. After a series of reactions, liquid iron collects at the bottom of the furnace.

Answer 389

Iron ore Limestone (CaCO3 - calcium carbonate) Coke (made from coal - almost pure carbon)

Answer 390

Coke burns, giving off heat Carbon monoxide is made Iron (III) oxide is reduced

Answer 391

The blast of air starts the coke burning - reacts with oxygen in the air to give carbon dioxide C + O2 —> CO2

Answer 392

yes - C is oxidised to carbon dioxide

Answer 393

The blast of hot air

Answer 394

It’s EXOTHERMIC - gives off heat, which helps to heat the furnace

Answer 395

Carbon dioxide reacts with more coke: C + CO2 —> 2CO

Answer 396

Yes - CO2 loses oxygen and is reduced

Answer 397

It’s ENDOTHERMIC - takes in heat from the furnace - good as stage 3 needs a lower temperature

Answer 398

where extraction occurs CO reacts with iron ore to give liquid iron this trickles to the bottom of the furnace Fe2O3 + 3CO —> 2Fe 3CO2

Answer 399

Acts as a REDUCING AGENT reduces iron (III) oxide to the metal CO oxidised to CO2

Answer 400

To remove impurities

Answer 401

Limestone thermally decomposes in the heat CaCO3 —> CaO + CO2 - to produce CaO which will remove sand that was present in the ore

Answer 402

Calcium oxide reacts with the sand, which is mainly silicon dioxide/silica. CaO + SiO2 —> CaSiO3 calcium + silica + calcium silicate oxide

Answer 403

Forms a slag which runs down the furnace and floats on the iron

Answer 404

CaO - basic oxide SiO2 - acidic oxide CaSiO3 - salt NEUTRALISATION

Answer 405

Molten slag is drained off When it solidifies, it is sold, mostly for road building

Answer 406

carbon dioxide and nitrogen (come out the top of the furnace) Heat is transferred from them to heat the incoming blast of air Have not reacted with anything CO2 - stage 3 N - air

Answer 407

NO carbon and sand are the main impurities phosphorus and sulfur compounds are also present from the iron ore

Answer 408

Some is run into moulds to make cast iron Most made into steels

Answer 409

Used for things like canisters for bottled gas and drain covers - hard but brittle due to its high carbon content

Answer 410

They test rocks and analyse the results in order to find out how much bauxite there is. If the tests are satisfactory, mining begins.

Answer 411

Yes - found near the surface so it’s easy to dig up

Answer 412

Taken to a bauxite plant, where impurities are removed. The result is white aluminium oxide or alumina.

Answer 413

Alumina is taken to another plant for electrolysis. May even be sent yo another country where electricity is cheaper.

Answer 414

Made into sheets and blocks and sold to other industries.

Answer 415

Electrolysis carried out in large steel tank lined with carbon which acts as a cathode (-) big blocks of carbon hang in the middle of the tank and act as the anode (+)

Answer 416

Dissolved in molten cryolite. alumina melts at 2045 degrees C impossible to keep the tank that hot dissolved to decrease melting point as cryolite has lower mp

Answer 417

sodium aluminium fluoride

Answer 418

At cathode - reduction - Al ions gain electrons Al3+ + 3e- –> Al

Answer 419

Drops to the bottom of the cell as molten metal. This is run off at intervals.

Answer 420

Some will be mixed with other metals to make alloys. Some is run into moulds, to harden into blocks.

Answer 421

At anode - oxidation - oxygen ions lose electrons 2O2- —> O2 + 4e-

Answer 422

Oxygen gas bubbles off and reacts with the anode C + O2 —> CO2 Carbon block gets eaten away and needs to be replaced

Answer 423

Alumina is broken down giving aluminium 2Al2O3 —> 4Al + 3O2

Answer 424

bluish-silver shiny metal Has a low density good conductor of heat and electricity Malleable and ductile resists corrosion (fine coat of Al2O3 forms) Not very strong when pure - made stronger when mixed with other metals to form alloys Generally non-toxic (not harmful to health)

Answer 425

1. Unwanted impurities are removed from the iron 2. Other elements are added

Answer 426

Molten iron from a blast furnace is poured into an oxygen furnace, and a jet of oxygen is turned on

Answer 427

Oxygen reacts with carbon, forming carbon monoxide and carbon dioxide gases, which are carried off. Reacts with other impurities to form acidic oxides.

Answer 428

Calcium oxide it is a basic oxide reacts with silicon dioxide and other acidic oxides to give a slag that is skimmed off

Answer 429

Depends on the type of steel - for some yes, for some they just contain iron and carbon so carbon doesn’t need to be removed

Answer 430

Depends on the type of steel - for some yes, for some they just contain iron and carbon so carbon doesn’t need to be removed

Answer 431

Carbon makes steel stronger

Answer 432

Too much can make the steel brittle therefore the carbon content is checked continually. when it is correct the oxygen is turned off.

Answer 433

Limestone consists mainly of calcium carbonate, CaCO3

Answer 434

calcium oxide

Answer 435

manufactured from calcium carbonate by thermal decomposition:

Answer 436

manufactured from calcium carbonate by thermal decomposition:

Answer 437

CaCO3 → CaO + CO2

Answer 438

calcium hydroxide

Answer 439

made by adding a small amount of water slowly to calcium oxide

Answer 440

CaO + H2O → Ca(OH)2

Answer 441

Limewater is a solution of calcium hydroxide in water

Answer 442

The addition of carbon dioxide to calcium hydroxide produces the initial starting material, calcium carbonate

Answer 443

CO2 + Ca(OH)2 → CaCO3 + H2O

Answer 444

turns cloudy due to calcium carbonate forming, which is an insoluble precipitate and the solution turns milky? cloudy

Answer 445

The limestone cycle

Answer 446

Limestone (calcium carbonate) is used in the manufacture of iron and cement

Answer 447

In the production of iron, limestone is added to the blast furnace where it decomposes to form lime (CaO) and carbon dioxide The lime reacts with silica impurities to form calcium silicate, which floats to the top of the molten iron and is removed: CaO + SiO2 → CaSiO3

Answer 448

Cement is manufactured by heating a mixture of powdered limestone and clay in a rotary kiln

Answer 449

Once heated, calcium sulfate and water are added which produce cement

Answer 450

Cement is a hardened, interlocked structure of calcium aluminate (Ca(AlO2)2 and calcium silicate (CaSiO3)

Answer 451

CaCO3 is also used in treating excess acidity in soils and lakes where it is often preferred to lime because it does not make the water in the soil alkaline

Answer 452

Lime (calcium oxide) is used in lime mortar and in flue-gas desulfurisation

Answer 453

Flue-gas desulfurization involves spraying acidic sulfur dioxide emissions with jets of slaked lime to reduce pollution by neutralising these gases before they leave the factory chimneys

Answer 454

It is also used in treating excess acidity in soils and lakes. If excess lime is used, however, the water in the soil may become too alkaline

Answer 455

Slaked lime (calcium hydroxide) is used in treating acidic soils and neutralising acidic industrial wasted products

Answer 456

1-CaCO3 (ionic) 2-CaO (ionic) 3-Ca(OH)2 (ionic) 4-CO2 (covalent)

Answer 457

LIMESTONE CYCLE 1-Heat a measured mass of limestone (CaCO3) 2-CaCO3 will break down to give calcium oxide (CaO) and carbon dioxide (CO2) CaCO3 —> CaO + CO2 3-Add water (reaction is exothermic) to make slaked lime (another name for limewater). Ca(OH)2 4-Add more water (Reaction is exothermic) to make more limewater 5-Precipitation reaction to produce CO2

Answer 458

Bathroom tiles Bricks Cement Manufacturing of iron

Answer 459

It’s a rock that is formed over many years from crushed animal skeletons

Answer 460

1 - 3H2(g) + N2(g) 2NH3(g) 2 - Exothermic 3 - Moles of reactants : products is 4:2 so an increased pressure will favour products 4-Favours reactants as the forward reaction is exothermic

Answer 461

1 - 3H2(g) + N2(g) 2NH3(g) 2 - Exothermic 3 - Moles of reactants : products is 4:2 so an increased pressure will favour products 4-Favours reactants as the forward reaction is exothermic

Answer 462

Low temperature = 450 degrees C High pressure = 200 atm Iron (III) catalyst

Answer 463

1-Nitrogen and hydrogen 2-Nitrogen comes from the air and hydrogen is usually obtained through either cracking or reacting natural gases e.g. methane with steam

Answer 464

Making medicines Making fertilizers Making explosives

Answer 465

To produce ammonia

Answer 466

> Nitrogen from the air > Hydrogen mainly from natural gas.

Answer 467

> High temp (about 450 degrees) High pressure (about 200 atmospheres) An iron catalyst.

Answer 468

1. Gaseous nitrogen + hydrogen enter the machine. 2. The gases are compresses to 200 atom and heated to 450 degrees. 3. Passed over iron catalyst. 4. Emerging mixture is cooled and the ammonia liquefies, separating it from he unseated nitrogen/hydrogen. 5. Unreacted gases return to the beginning.

Answer 469

Fertilisers

Answer 470

The point in a reversible reaction when the forwards and backwards rate of reaction are the same. Therefore, the amounts of substances present in the reacting mixture remain constant.

Answer 471

… an increase in pressure decreases the amount of products formed. …. a decrease in pressure increases the amount of products formed.

Answer 472

… an increase in pressure increases the amount of products formed. … a decrease in pressure decreases the amount of products formed.

Answer 473

If there are different numbers of molecules of gases on either side of the equation.

Answer 474

… an increase in temperature decreases the amounts of product formed. … a decrease in temperature increases the amount of products formed.

Answer 475

… an increase in temperature increases the amount of products formed. … a decrease in temperature decreases the amount of products formed.

Answer 476

The forward reaction produces less molecules of gas, so to get the maximum yield of ammonia, the pressure has to be as high as possible. However, above 200 atmo, special reaction vessels and pipes have to be used so that there is no danger of explosion. Therefore, to keep the process economical, a compromise is made.

Answer 477

Because the forward reaction is exothermic, using a low temperature would increase the yield. However, doing so would make the process very slow and not commercially viable. Using a low temperature could also reduce the effectiveness of the iron catalyst.

Answer 478

It speeds up both the forwards and backwards reaction, but has no effect on the actual yield.

9. Metals Flashcards

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