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Chemistryyy > chem - metals > Flashcards

chem - metals Flashcards

1
Q

what is the main use for iron and why?

A

in construction as it is strong and cheap

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2
Q

what is the main use for aluminium and why,

A

pilon wires - as it has a good conductor of electricity, and a low density

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3
Q

what does aluminium bring a good conductor of heat mean it can be used to make?

A

can make saucepans

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4
Q

why is aluminium also a good material to make saucepans

A

doesn’t react with food cause of protective layer of aluminium oxide on surface - layer means u can also make window frames with it due to lack of corrosion

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5
Q

what 3 things is copper used for and why (2 different reasons)

A

electrical wires - excellent conductor
hot water pipes and boilers - unreactive

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6
Q

why are gold and copper used to make jewellery?

A

unreactive and have an attractive appearance - im comparison to metals that are dull or who react and lose their shine

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7
Q

metals are used in construction because of what property?

A

they’re strong

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8
Q

metals are used in car body panels (made out of sheet steel) because of what property?

A

they’re malleable

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9
Q

metals are used in the moving part of engines because of what property?

A

they’re strong

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10
Q

metals are used in electrical wiring because of what property?

A

they are ductile and excellent conductors of electricity

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11
Q

metals are used as heat sinks to cool microprocessors and stop them overheating because of what property?

A

they are good conductors of heat

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12
Q

what happens to copper when it burns (in oxygen)

A

turns black slowly - as it is covered with a layer of black copper oxide

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13
Q

what happens to magnesium when it burns (in oxygen)

A

a white solid is formed (MgO), and it burns with a bright WHITE flame

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14
Q

what happens to calcium when it burns (in oxygen)

A

white solid formed -(CaO), burns with a bright RED flame

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15
Q

what happens to zinc powder when it burns (in oxygen)

A

white ZnO is formed, and it burns with a BLUEISH flame

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16
Q

what happens to iron filings when it burns (in oxygen)

A

brown solid - Fe2O3 is formed, and they burn with a YELLOW/ORANGE flame

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17
Q

what happens to potassium when it burns (in oxygen)

A

a white solid - K2O is formed, burns with a LILAC flame

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18
Q

what happens to copper when it is reacted with hydrochloric acid

A

no reaction

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19
Q

what happens to magnesium when it is reacted with hydrochloric acid

A

gets warm and there’s effervescence

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20
Q

what happens to calcium when it is reacted with hydrochloric acid (3 things)

A

smoking, heat and effervescence

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21
Q

zinc had no reaction but iron did (there were some bubbles) - yet zinc is more reactive - why is this?

A

because it was powdered iron so greater SA : Vol ratio and more collisions, so if it had been powdered zinc it would have reacted more strongly

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22
Q

what happens to potassium when it is reacted with hydrochloric acid

A

explosive reaction

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23
Q

How do tin, lead and copper react with oxygen?

A

react slowly - forming a layer of oxide

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24
Q

how do silver, gold and platinum react with oxygen?

A

they don’t react

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25
Q

Magnesium is different from other alkali/alkaline earth metals - potassium, sodium, lithium and calcium - when it reacts with water/ steam, how is it different

A

they all react fast with water, (less vigorous as you move down), however magnesium reacts slowly with cold water and only fast with steam

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26
Q

which metals don’t react with water or steam?

A

tin, lead, copper, silver, gold and platinum

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27
Q

which metals react with steam but not with water?

A

aluminium, zinc and iron

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28
Q

which metals DO NOT react with dilute acids?

A

copper, silver, gold and platinum

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29
Q

which metals react with acids to give hydrogen gas?

A

calcium, magnesium, Aluminium, zinc and iron

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30
Q

? and lead have very ? reactions with acids

A

tin, slow

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31
Q

potassium, sodium and lithium all have a violent explosive reaction when reacted with acid - true or false?

A

true

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32
Q

what are displacement reactions?

A

reactions in which a more reactive will take the place of a less reactive one

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33
Q

what happens in a reaction between magnesium and copper (2) sulphate and why?

A

there is a reaction - the solution turns green - this happens as magnesium is more reactive than copper (2) sulphate so it displaces it and turns into magnesium sulphate and copper

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34
Q

what is order of reactivity with copper, iron, magnesium and zinc (most to least)

A

magnesium, zinc, iron and copper

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35
Q

what are the two definitions of oxidation?

A

loss of electrons and the gain of oxygen (combining with oxygen)

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36
Q

what are the two definitions of reduction?

A

again of electrons, loss of oxygen (giving away oxygen)

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37
Q

oxidising ? are substances that cause another ? to be oxidises ie provide ? to the other substance. when an ? agent oxidises something - it itself loses ? ie is reduced

A

agents, substance, oxygen, oxidising, oxygen

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38
Q

reducing ? are substances that cause another ? to be reduced ie provide ? to the other substance/ remove ? from the other substance. when a ? agent reduces something - it itself gains ? ie is oxidised

A

agents, substance, electrons, oxygen, reducing, oxygen

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39
Q

in the reaction - CuO + Mg -» MgO + Cu - what is oxidised, reduced, the oxidising agent and the reducing agent

A

oxidised - Mg - magnesium
reduced - CuO - copper oxide
oxidising agent - copper oxide
reducing agent - magnesium

40
Q

what is an ore and an example of an ore?

A

a rock that contains enough of the decided metal to be economical to extract the metal eg : hoematite - iron ore Fe2O3

41
Q

which metals are extracted by electrolysis and why?

A

potassium, sodium, lithium, calcium, magnesium and aluminium - as they are the most reactive (as they’re above carbon) so are more difficult to extract

42
Q

which metals are extracted by reduction?

A

zinc, iron, tin and lead

43
Q

which metals are found native and are easily extracted and what are examples of these extractions?

A

copper, silver, gold and platinum - panning for gold

44
Q

what is electrolysis? when we extract the metals by ? the compound containing it - and then passing ? through the liquid. then the metallic ? appears at the negative electrode called the ?

A

melting, electricity, element, cathode

45
Q

which metals were among the first to be discovered and why?

A

silver and gold as they’re the easiest to extract

46
Q

how are semi reactive metals like zinc extracted and in what?

A

they are extracted from their ores by reducing the oxide using carbon or carbon monoxide - in a blast furnace!

47
Q

why is reduction preferable to electrolysis?

A

as it is relatively cheap, due to electrolysis being more expensive due to the large amount and high cost of electricity

48
Q

what is another word for reduction using carbon?

A

smelting

49
Q

due to higher grade ? being used up - it has become economic to extract some ? from certain ores which weren’t originally economic to ? from - so now they’ve turned to lower ? ores

A

ores, metals, extract, grade

50
Q

when copper oxide and carbon powders are mixed together and heated what do you expect to see? (and why)

A

black with glittery red as the carbon has displaced the copper so it’s now carbon dioxide and copper - which is the glittery red

51
Q

what is the positive electrode called and what are attracted to it?

A

anode, the negative ions - the anions

52
Q

what is the negative electrode called and what are attracted to it?

A

cathode, cations - the positive ions

53
Q

what happens when the cations are attracted to the cathode?

A

the metal ions gain electrons to make the metal

54
Q

what happens when the anions are attracted to the anode?

A

they lose electrons and make the non metal element

55
Q

is the metal ion positive or negative and what’s it called?

A

positive and it’s called the cation

56
Q

is the non metal ion positive or negative and what’s it called?

A

negative, an anion

57
Q

phyto mining is when - a plant is chosen that will ? the desired metal from the ? without dying - (these plants are called ?). they are grown and the ? metal collects in the leaves. the plants are ? after harvesting. the ash from the plants contains metal ? which the ? can be extracted from

A

absorb, soil, hyperaccumulators, desired, burnt, compounds, metal

58
Q

3 pros of phytomining in comparison to traditional methods?

A
  • there’s less waste
  • smaller carbon footprint (more environmentally friendly)
  • can extract metals from lower grade ores - increase supply of finite resource
59
Q

3 cons of phytomining in comparison to traditional methods

A
  • is a slower method
  • plants grow in specific habitats - can’t grow everywhere
  • uses a lot of land
60
Q

bioleaching - uses ? to produce leachate solution that contain ? compounds, for example bacteria can convert ? copper sulphide into soluble copper ? which can then be dissolved into ? and extracted from the solution

A

bacteria, metal, insoluble, sulphate, water

61
Q

3 pros of bioleaching compared to general/ traditional methods

A
  • Less waste
  • Low carbon footprint
  • Takes less energy/ is more simple
62
Q

disadvantages of bioleaching compared to traditional methods

A
  • slow (especially in a cold climate)
  • smelting would be cheaper
  • hard to acquire bacteria, has to be safe therefore no anaerobic bacteria
63
Q

Why are copper, gold, iron and aluminium mixed with smaller amounts of similar metals to make alloys?

A

because they’re too soft for most uses, so they are made harder for everyday use

64
Q

what’s steel made from?

A

iron and a small amount of carbon

65
Q

if you add chromium and nickel to steel what does it make - and why is this type of steel important?

A

stainless steel - as it’s in reactive

66
Q

what is brass an alloy of??

A

copper and zinc - as the larger zinc atoms get in the way of the copper layers sliding making it harder

67
Q

what is magnalium an alloy of and what does it do (because of what special features?) x

A

magnesium and aluminium - makes planes and expensive bikes - as it is strong, corrosion resistant and doesn’t corrode

68
Q

what’s stainless steel used for

A

cutlery

69
Q

why is brass used in musical instruments?

A

looks good and doesn’t corrode (can also be used for making door handles!)

70
Q

4 main types of steel

A

mild, hard, stainless and tungsten steel

71
Q

Mild steel properties and uses

A

easily worked and strong (has lost most brittleness) so good for car bodies and machinery

72
Q

Hard steel properties and uses

A

Tough and brittle so used for tools eg a hammerhead

73
Q

Tungsten steel properties and uses

A

Tough and hard at high temperatures - so drill bits and power saws

74
Q

Stainless steel properties and uses

A

Tough, doesn’t corrode - used for chemical plant and cutlery

75
Q

what is rust
3 details

A

the corrosion of iron
hydrated iron(III) oxide
reddy brown solid

76
Q

what must iron be in contact with in order to rust?

A

both water and oxygen

77
Q

what makes iron rust faster?

A

the presence of an ionic compound (eg: salt) dissolved in the water

78
Q

how do most methods of rust prevention work?

A

by creating a barrier between iron and water and oxygen to prevent contact and therefore rusting

79
Q

how does painting the iron surface, applying oil and grease etc stop rusting?

A

it’s a barrier method so stops water and oxygen coming into contact with iron

80
Q

what is a sacrificial protection and how does it work (stopping rusting)

A

using a more reactive metal for protection - so it corrodes instead of the iron

81
Q

what is galvanizing and how does it work?

A

covering steel with zinc - a barrier method - so the more reactive zinc will corrode instead

82
Q

how does stainless steel prevent rusting?

A

it doesn’t corrode so the alloy of iron doesn’t rust

83
Q

how does stainless steel prevent rusting?

A

it doesn’t corrode so the alloy of iron doesn’t rust

84
Q

if an ? object is completely covered with a ? of another metal then the ? will not rust. this can be done by metal ? the object. often the coating can improve the ? of the iron, eg : chromium plating gives the object a very ? appearance

A

iron, coating, iron, plating, appearance, shiny

85
Q

if an ? object is completely covered with a ? of another metal then the ? will not rust. this can be done by metal ? the object. often the coating can improve the ? of the iron, eg : chromium plating gives the object a very ? appearance

A

iron, coating, iron, plating, appearance, shiny

86
Q

in electroplating the object that is going to be ? is made the cathode (so is given the ? charge) and dipped into a solution containing ? of the desired plating metal

A

plated, negative, ions

87
Q

In the copper plating the key experiment what object is the anode?

A

impure copper

88
Q

In the copper plating the key experiment which object is the cathode

A

The key

89
Q

what is the solution used in the copper poring experiment and what ions is it split into?

A

copper sulphate so cu(2+) and so4(2-)

90
Q

How does the key get electroplated in the copper plating the key experiment?

A

the Cu2+ ions from the copper sulphate are attracted to the cathode (the negative electrode) where the key is and the cu2+ ions gain electrons - making copper and plating the key

91
Q

why is a life cycle assessment carried out?

A

to assess the environmental impact of a product in each stage of its life

92
Q

what 3 things does a life cycle assessment consider?

A
  • the useful life of a product
  • materials and energy it takes to make the product
  • what happens to the object on its disposal
93
Q

5 main factors for a life cycle assessment :
- main requirements for ? input
- environmental ? and sustainability of making material from natural ?
- ? impacts of making the product from the ?
- environmental impact of using the ?
- environmental ? of disposing product by ? , landfill or recycling

A

energy,
impact, resources
environmental, material
product,
impact, incineration

94
Q

main four steps of life cycle assessments?

A

raw materials, manufacturing, use and disposal

95
Q

what 3 benefits does recycling metals provide us with?

A
  • saves landfill space
  • reduces need for further metal extraction
  • reduces risk of running out of finite resources
96
Q

in the copper plating the key experiment what happens to the anode(impure copper)

A

the impure copper is supplied with a positive charge and so becomes oxidised and becomes cu2+ which then replaces the copper in the solution (so replenishes the copper to keep being able to plate the key)

Chemistryyy (40 decks)

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