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chemistry > Metals > Flashcards

Metals Flashcards

1
Q

what are properties of metals?

A
  • malleable
  • ductile
  • high density
  • high MP BP
  • good conductors of heat and electricity
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2
Q

what does malleable mean?

A

can be easily beaten into fine wires without breaking

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3
Q

what does ductile mean?

A

can be stretched into fine wires without breaking

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4
Q

why are metals malleable and ductile?

A

their atoms are of the same size and are arranged in orderly layers. so layers can slide over each other easily when a force is applied

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5
Q

why do metals have high density?

A

as their metal atoms are closely packed together

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6
Q

why do metals have high melting and boiling points?

A

as their metal atoms are packed tightly in layers by strong metallic bonds. a lot of energy is needed to break the strong metallic bonds

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7
Q

why are metals good conductors of heat and electricity?

A

as they have a sea of delocalised mobile electrons that can carry charges

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8
Q

what are alloys?

A

a mixture of metals with one or more elements

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9
Q

what is bronze made of?

A

copper and tin

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10
Q

what is steel made of?

A

iron and carbon

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11
Q

what is steel used for?

A

car bodies and machinery

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12
Q

what is stainless steel made of?

A

iron, carbon and small amounts of chromium and nickel

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13
Q

what is stainless steel used for?

A

cutlery, utensils and surgical instruments

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14
Q

what is brass made of?

A

copper and zinc

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15
Q

what is brass used for?

A

coins and musical instruments

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16
Q

what is the structure of metals?

A
  • pure metals are weak and soft
  • atoms of the same size and are arranged in regular layers which slide over easily when force is applied
  • soft and malleable
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17
Q

what is the structure of alloys?

A
  • hard and strong
  • different sizes of atoms disrupt regular and orderly arrangements of atoms
  • difficult for atoms in an alloy to slide over each other when force is applied
  • stronger and less malleable than pure metals
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18
Q

what is the product of the reaction between metal and water?

A

metal hydroxide and hydrogen

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19
Q

what is the product of the reaction between metal and steam?

A

metal oxide and hydrogen

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20
Q

what is the product of the reaction between metal and acids?

A

salt and hydrogen

21
Q

what is the reactivity series of metals?

A 
potassium 
sodium 
calcium
magnesium 
aluminium 
zinc
iron
tin
lead
copper
mercury
silver 
gold
22
Q

where is carbon?

A

in between aluminium and zinc

23
Q

where is hydrogen?

A

in between lead and copper

24
Q

what metals react with cold water, steam and acid?

3

A

potassium, sodium and calcium

25
Q

what metals react with steam and acid?

4

A

magnesium, aluminium, zinc and iron

26
Q

what metals react with acid?

2

A

tin and lead

27
Q

what metals are unreactive?

4

A

copper, mercury, silver and gold

28
Q

what metals can be extracted by electrolysis?

5

A

potassium to aluminium

29
Q

what metals can be extracted by heating with carbon?

A

zinc to gold

30
Q

what metals can be extracted by heating with hydrogen?

A

last 4 metals

31
Q

what is needed in the extraction of iron?

A

hematite, coke and limestone

32
Q

what is the first extraction of iron equation and what does it do?

A

C + O2 -> CO2

production of carbon monoxide from burning coke in hot air

33
Q

what is the second extraction of iron equation and what does it do?

A

CO2 + C -> 2CO

production of carbon monoxide through the reaction of carbon dioxide with coke

34
Q

what is the third extraction of iron equation and what does it do?

A

3CO + Fe2O3 -> 2Fe +3CO2

reduction of iron (III) oxide by carbon monoxide reducing iron (III) oxide to iron

35
Q

what is the first equation in the removal of impurities and what does it do?

A

CaCO3 -> CaO + CO2

the decomposition of limestone

36
Q

what is the second equation in the removal of impurities and what does it do?

A

Cao + SiO2 -> CaSiO3

the reaction of calcium oxide with silicon oxide which is a basic oxide and acidic oxide which forms slag

37
Q

what metals rust?

A

iron and steel

38
Q

what about other metals?

A

corrosion

39
Q

what are the condition for rusting?

A
  • air, oxygen

- water, dissolved salt speeds up rusting (seawater)

40
Q

what are ways to prevent rusting?

A
  • surface protection
  • sacrificial protection
  • galvanising
41
Q

what are some examples of surface protection?

A
  • painting on street poles
  • oiling or greasing machinery
  • coating with plastic on metal clips
  • metal plating on food cana
42
Q

explain sacrificial protection

A
  • happens when a more reactive metal reacts in place of a less reactive metal
  • the two metals must be touching each other
  • for instance, when magnesium and iron are in touch with each other, magnesium reacts in place of iron, it ‘sacrifices’ itself for iron
43
Q

explain galvanising

A
  • happens when zinc is coated on top of a more reactive metal
  • the zinc reacts in place of the more reactive metal and is used up instead of the more reactive metal
44
Q

what is a practical application of galvanising?

A

zinc roofing

45
Q

what is one way to conserving metals?

A

recycling

46
Q

what is one way of recycling metals

A

using other materials in its place e.g glass bottles instead of metal cans

47
Q

what are some benefits of recycling metals?

A
  • conserves limited supply of metals
  • saves costs of extracting new metals
  • prevents land pollution from the careless disposition of metals
  • recycling produces less pollution than extracting
48
Q

what are some disadvantages of recycling metals?

A
  • metals are only recycled if it’s economical to do so
  • can cause air pollution from melting of scrap metal
  • cost of separating metals from waste can be high
  • costs money to collect scrap metals
  • can be difficult to persuade people to deposit materials in recycling containers

chemistry (19 decks)

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