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Year 10 Chemistry > chapters 14 and 15-the reactivity series including extraction and uses of metals > Flashcards

chapters 14 and 15-the reactivity series including extraction and uses of metals Flashcards

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1
Q

What is the order of the reactivity series

A

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

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2
Q

what are the 4 reactions used to put metals in order of reactivity?

A
  1. displacement reactions involving metal oxides
  2. displacement reactions involving solutions salts
  3. metals with water
  4. metals with acid
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3
Q

describe which metals the reactivity series react with water or steam

A
  • potassium to calcium react with cold water+ steam
  • magnesium to iron react with steam
  • copper to gold don’t react with water or steam
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4
Q

describe which metals react with acid

A
  • potassium to calcium react explosively with acid, so strongly that they cannot be performed in a lab
  • magnesium to iron react well with acids
  • copper to gold do not react with acid as they are below hydrogen in the reactivity series
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5
Q

describe the rule concerning displacements in metals

A

a more reactive metal will displace a less reactive metal in its compound

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6
Q

what is a redox reaction?

A

a reaction involving oxidation and reduction

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7
Q

what is oxidation and reduction

A

oxidation is the gain of oxygen and loss of electrons, reduction is the loss of oxygen and gain of electrons (remember OILRIG)

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8
Q

what is an oxidising agent

A

a substance which oxidises something else (so is reduced)

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9
Q

what is a reducing agent

A

a substance which reduces something else (so is oxidised)

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10
Q

describe the rule concerning displacement reactions involving solutions of salts

A

a more reactive metal will displace a less reactive metal from a solution of one of its compounds

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11
Q

which metals in the reactivity series react with water (or steam)

A

metals above hydrogen

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12
Q

what are the products of a reaction with a metal (above hydrogen) + cold water

A

metal hydroxide ( metal OH) + hydrogen (H2)

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13
Q

what are the products of a reaction with a metal (above hydrogen) and steam

A

metal oxide (metal O) + hydrogen (H2)

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14
Q

how do group 1 metals in the reactivity series (potassium, sodium, lithium) react with cold water/ steam

A

react vigorously and they all fizz, float, move and dissolve- lithium does not ignite, sodium sometimes ignites with an orange flame and potassium ignites with a lilac flame

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15
Q

how do group 2 metals in the reactivity series (magnesium and calcium) react with cold water/steam

A
  • less reactive than group 1
  • calcium still reacts with cold water (see fig. 14.9 page 150)
  • magnesium only reacts with steam ( see fig. 14.10 page 151)
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16
Q

how do zinc and iron react with cold water /steam

A
  • react similarly to magnesium but are less reactive

- copper comes after these in the reactivity series and doesn’t react at all

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17
Q

which metals in the reactivity series react with acid

A
  • metals above hydrogen react with dilute acids like Hal and H2SO4.
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18
Q

what are the products of a reaction with a metal+ acid

A

metal salt + hydrogen

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19
Q

how are most metals extracted

A

most metals are extracted from ores found in the earths crust. The most un-reactive metals (e.g gold) are often found uncombined as an element. Other metals are found as compounds from which the metal needs to be extracted

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20
Q

what does the method used to extract a metal depend on?

A
  • Its position in the reactivity series

- cost of energy +reducing agent

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21
Q

describe how the different metals in the reactivity series are extracted

A
  • metals above carbon in the reactivity series are extracted using electrolysis (this uses a lot of energy so it is expensive)
  • metals below carbon in the reactivity series can be extracted using carbon- heated with carbon (this is cheaper than electrolysis)
  • metals at the bottom of the reactivity series may be found native as elements
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22
Q

what does iron ore contain

A

iron (III) oxide

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23
Q

in the experiment with zinc or iron in the hydrogen experiment , why must you stop heating while the delivery tube is still under water?

A

because water will be sucked back into the hot tube, which often results in it cracking

24
Q

what is an ore

A

a sample of rock which contains enough of a mineral for it to be worthwhile to extract the metal

25
Q

what does native mean

A

exists naturally as an uncombined element

26
Q

when does iron rust

A

in the presence of oxygen and water

27
Q

what is rust made of

A

hydrated iron (III) oxide

28
Q

how can we speed the process of rusting

A

using salt

29
Q

how is the extraction of iron carried out

A
  • in a blast furnace, it is heated with carbon and it is carbon monoxide which is the reducing agent
  • since carbon is above iron in the reactivity series it will take the oxygen from iron (III) oxide- iron ore
30
Q

what does exothermic mean

A

reactions which are exothermic give out heat

31
Q

which metal rusts

A

ONLY iron- with other metals, we say that they corrode

32
Q

briefly describe the experiment used to find the conditions needed for rusting

A
  • 4 test tubes with different conditions, an iron nail is placed into each
  • 1st test tube contains calcium chloride to remove water
  • 2nd test tube contains boiled water to remove oxygen ( because when temperature increases, the solubility of gases decreases, so no oxygen can dissolve in the water), and oil is put ontop, in order to stop oxygen from entering the water once cooled
  • 3rd test tube contains deionised water- without any additional compounds in it
  • 4th test tube contains salt water
33
Q

in which test tube does the iron nail rust best?

A

only the tubes containing oxygen and water

34
Q

what can we coat iron with to protect from rusting (barrier method)

A

paint, oil, grease, plastic or electroplating (using electrolysis to coat the iron with a layer of another metal)

35
Q

what is galvanising

A

coating iron with a layer of zinc

36
Q

why doesn’t iron rust in galvanising, even when some of the zinc is scratched away?

A

zinc will react with any oxygen which comes close to the exposed iron because it is more reactive

37
Q

where is galvanising used?

A

watering cans and buckets

38
Q

what is sacrificial protection

A
  • zinc, magnesium or aluminium blocks are attached to ships to prevent the iron/steel from rusting.
  • the more reactive metal reacts (is oxidised) more readily than the iron
  • the corrosion of the more reactive metal prevents the iron from rusting
  • it is often used on large objects, like ships, which would be difficult / expensive to cover with a barrier
39
Q

what is galvanising a combination of

A

the barrier and sacrificed protection method

40
Q

what is an alloy

A
  • a mixture of a metal and one or more other elements, usually other metals or carbon
  • alloys are harder than pure metals because they contain different sized atoms which distort the regular arrangement go the ions and make it harder for the layers to slide over each other
41
Q

what are the properties + uses of aluminium

A
  • low density, strong (planes)
  • good conductor of electricity, ductile (electricity cables)
  • good conductor of heat, high melting point, resists corrosion (saucepans)
42
Q

what are the properties + uses of copper

A
  • very good conductor and ductile (electrical wires)

- unreactive and malleable (water pipes)

43
Q

what are the properties + uses of low carbon (mild) steel

A
  • strong and malleable but high density and rusts (nails, car bodies, ships and bridges)
44
Q

what is low carbon steel

A

an alloy of iron and 0.25% carbon

45
Q

what are the properties + uses of high carbon steel

A

harder and more resistant to wear but not as malleable and ductile- more brittle (cutting tools)

46
Q

what is high carbon steel

A

an alloy of iron and about 1% carbon

47
Q

what are the properties + uses of stainless steel

A

resistant to corrosion-doest rust-but expensive (kitchen sinks, cutlery and cooking utensils

48
Q

what are the properties + uses of aluminium

A
  • low density, strong (planes)
  • good conductor of electricity, ductile (electricity cables)
  • good conductor of heat, high melting point, resists corrosion (saucepans)
49
Q

what are the properties + uses of copper

A
  • very good conductor and ductile (electrical wires)

- unreactive and malleable (water pipes)

50
Q

what are the properties + uses of low carbon (mild) steel

A
  • strong and malleable but high density and rusts (nails, car bodies, ships and bridges)
51
Q

what is low carbon steel

A

an alloy of iron and 0.25% carbon

52
Q

what are the properties + uses of high carbon steel

A

harder and more resistant to wear but not as malleable and ductile- more brittle (cutting tools)

53
Q

what is high carbon steel

A

an alloy of iron and about 1% carbon

54
Q

what are the properties + uses of stainless steel

A

resistant to corrosion-doest rust-but expensive (kitchen sinks, cutlery and cooking utensils

55
Q

what is stainless steel made of

A

iron, chromium, nickel

Year 10 Chemistry (4 decks)

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