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Chemistry > Metals > Flashcards

Metals Flashcards

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1
Q

What do metals form?

A

a giant metallic lattice

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2
Q

What is a metallic lattice?

A

electrostatic attraction between positive metal ions and delocalised electrons

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3
Q

What are the properties of metals?

A

good conductors of electricity and heat
high mp/bp
malleable
sonorous
shiny
high density
ductile -> can be made into wires

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4
Q

Why are metals strong?

A

due to strong electrostatic between positive metal ions and delocalised electrons which is strong

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5
Q

Why do metals have a high melting point?

A

due to strong electrostatic between positive metal ions and delocalised electrons require lots of energy to overcome
higher charge = higher mp

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6
Q

Why do metals conduct when solid and molten?

A

delocalised electron are free to move

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7
Q

Why are metals malleable?

A

rows of ions can slide over each other and delocalised electrons can move to hold the structure together

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8
Q

What are group 1 called?

A

alkali metals

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9
Q

What are the physical properties of group 1?

A

high melting point
grey
shiny
hard
good thermal and electrical conductor

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10
Q

How are metals stored?

A

In oil to stop it reacting with oxygen and water

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11
Q

Explain the trend in reactivity down group 1

A
  • All group 1 need to lose 1 electron
  • down the group = more shells
  • outer electrons further away from
  • nucleus therefore weaker
    attraction
  • easier to remove the electron
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12
Q

Physical observations of lithium

A

low density
dark grey
soft metal

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13
Q

Physical observations of sodium

A

high density
lighter grey
softer

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14
Q

Physical observations of potassium

A

very soft
lighter grey

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15
Q

Physical observations of rubidium

A

lighter grey than K
softer than k

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16
Q

Physical observations of caesium

A

lighter grey than rubidium
softer than rubidium

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17
Q

Observations of lithium with oxygen

A

shiny surface dulls quickly

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18
Q

Observations of sodium with oxygen

A

shiny surface dulls quicker than lithium

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19
Q

Observations of potassium with oxygen

A

shiny surface disappears quicker Na

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20
Q

Observations of rubidium with oxygen

A

shiny surface disappears quicker than k

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21
Q

Observations of caesium with oxygen

A

shiny surface disappears quicker than rubidium

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22
Q

Observations of lithium with water

A

moves around, fizzing, metal disappears, gas given off, alkali produced as UI turns blue/purple

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23
Q

Observations of sodium with water

A

moves around more than lithium, fizzing, turns into sphere than disappears, more gas given off

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24
Q

Observations of potassium with water

A

fizzes very quickly, caught fire, more gas given off, flame is lilac, pop given off - hydrogen react with O₂

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25
Q

Observations of rubidium with water

A

ignites as soon as hits water, more gas given off, hydrogen reacts - flames given off

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26
Q

lithium + water -> ?

A

hydrogen + lithium hydroxide
lithium disappears
hydrogen causes bubbles

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27
Q

Formula for carbonate ions?

A

CO₃⁻²

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28
Q

What is decomposition?

A

breaking something down

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29
Q

What is thermal decomposition?

A

breaking something down using heat

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30
Q

What is the formula for thermal decomposition of metal carbonates?

A

metal carbonate -> metal oxide + carbon dioxide

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31
Q

What is the test for carbon dioxide?

A

bubble through limewater
turns cloudy

32
Q

What colour is copper carbonate?

A

green

33
Q

What colour is copper oxide?

A

black

34
Q

formula for thermal decomposition of copper carbonate?

A

copper carbonate -> copper oxide + carbon dioxide

35
Q

Describe Mg(s)

A

solid, shiny, silver

36
Q

Describe Fe(s)

A

grey, solid, dull

37
Q

Describe Cu(s)

A

solid, brown, shiny

38
Q

Describe MgSO₄

A

aqueous

39
Q

Describe FeSO₄(aq)

A

green clear solution

40
Q

Describe CuSO₄(aq)

A

blue clear solution

41
Q

MgSO₄ reacting with Fe and Cu?

A

no reaction

42
Q

FeSO₄ reacting with Mg and Cu?

A

Mg = gas, Mg moved, grey solid produced
Cu = no reaction

43
Q

CuSO₄ reacting with Mg and Fe?

A

Mg = gas, black solid produced
Fe = iron turned black

44
Q

Why is Mg most reactive out of Mg, Fe, Cu?

A

Mg reacted with everything other than itself

45
Q

Why is Cu least reactive out of Mg, Fe, Cu?

A

Cu reacted with nothing

46
Q

What is the reactivity series?

A

Please Stop Literally Calling Me A Careless Zebra, Can Instead Now Try Learning How Copper Maybe Saves Gold
Potassium, Sodium, Lithium, Calcium, Magnesium, Aluminium,
Carbon,
Zinc, Chromium, Iron, Nickel, Tin, Lead,
Hydrogen,
Copper,Mercury, Silver, Gold

47
Q

What is a spectator ion?

A

plays no part in chemistry

48
Q

What is a redox reaction?

A

Both reduction and oxidation has occurred

49
Q

What is an oxidising agent?

A

Helps something to be oxidised

50
Q

What is a reducing agent?

A

Helps something to be reduced

51
Q

Where do metals come from?

A

the ground

52
Q

What is an ore?

A

Rock containing a metal compound

53
Q

How do we extract the most reactive metals?
(K, Na, Li, Ca, Mg, Al)

A

electrolysis = breaking down a compound using electricity

54
Q

How do we extract the middle metals?
(Zn, Cr, Fe, Ni, Sn, Pb, Cu)

A

Displacement using carbon
carbon is more reactive, cheap + easily available

55
Q

How do we extract Mercury and Silver?

A

don’t require extraction, but may need purifying

56
Q

How do we extract native metals
(Gold, platinum)

A

not found as ores
require no extraction

57
Q

Practical: Extracting iron
Describe

A

Add iron(III) oxide and carbon to crucible
Weigh
Heat strongly (no lid, 5 mins)
Reweigh after cool
Use splint and magnet to find iron produced

58
Q

Practical: Extracting iron
Why did mass decrease?

A

one of the products (CO₂) is a gas therefore can escape

59
Q

What is rust?

A

Hydrated iron(III) oxide

60
Q

Explain the first stage of rusting

A

Oxidation of Iron
4Fe + 3O₂ -> 2Fe₂O₃

61
Q

Explain the second stage of rusting

A

hydration of iron (III) oxide
Fe₂O₃ + XH₂O -> Fe₂O₃ * XH₂O
X: amount of water varies

62
Q

Rusting is a chemical process by which…

A

Iron is oxidised and hydrated

63
Q

What two substances does rusting require to occur?

A

water and oxygen

64
Q

What are the three methods to prevent rusting?

A

Barrier, Sacrificial protection, Galvanising

65
Q

What is the barrier method?

A

Coating Fe in plastic, oil, or paint
+ easy
- has to be replaced

66
Q

What is sacrificial protection?

A

add a block of more reactive metal
iron displaced as soon as any rust forms
+ easy method, very effective
- Mg needs to be replaced therefore expensive

67
Q

What is galvanising?

A

Specifically coating Fe in Zinc
Prevents O₂/H₂O reacting with iron
Zinc can act as sacrificial metal if crack occurs
e.g. iron bucket
nails
ships

68
Q

What are alloys?

A

mixtures of metals with one or more other elements - usually other metals or carbon

69
Q

What are the commonly known alloys?

A

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

70
Q

Why are alloys harder / less malleable?

A

Presence of another metal makes it harder for rows to slide

71
Q

Why are different metals and alloys used for different purposes?

A

Material must be suited to its use

72
Q

What is iron used for? Why?

A

making steel
steel is more useful than iron

73
Q

What is low-carbon steel used for? Why?

A

ships, cars, bridges
strong, still malleable

74
Q

What is stainless steel used for? Why?

A

cutlery + cooking utensils
high mp & strong
shiny & prevent corrosion

75
Q

What is copper used for? Why?

A

electrical wiring, water pipes, cooking pots
excellent conductors of electricity, unreactive to oxygen + water
flexible

76
Q

What is Aluminium used for? Why?

A

foil, aircraft bodies, drinks cans
malleable, light, fairly unreactive

Chemistry (18 decks)

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