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Metals Flashcards

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1
Q

Chemical name for rust

A

hydrated iron (III) oxide

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2
Q

2 stages of Iron rusting

A
  • Iron is oxidised by oxygen, forming Iron (III) oxide
  • Iron (III) oxide is hydrated by water
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3
Q

Balanced equation for oxidation of Iron

A
  • 4Fe + 3O2 –> 2Fe2O3
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4
Q

Balanced equation for hydration of Iron (III) oxide

A

Fe2O3 + H2O –> Fe2O3 x H2O

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5
Q

Rusting prevention methods

A
  • Barriers
  • Sacrificial protection
  • Galvanisation
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6
Q

What is barrier protection (rust)

A
  • Coating iron in paint, oil, grease or plastic to prevent iron coming into contact w/ oxygen or water
  • only works when barrier is intact- if broken, rust happens
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7
Q

What is sacrificial protection (rust)

A
  • Attaching block of more reactive metal (e.g magnesium) to the Iron
  • Iron is displaced from rust as soon as it forms
    -however Mg has to be replaced often
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8
Q

Equation for sacrificial protection

A
  • Magnesium + iron(III) oxide –> magnesium oxide + iron
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9
Q

what is galvanisation (rust)

A
  • Coating iron in zinc
  • works initially as barrier protection, but if it cracks then also sacrificial as zinc more reactive than iron
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10
Q

What is an alloy?

A

Mixture of metal with one or more other element, usually another metal or carbon

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11
Q

Common alloys:

A
  • Steel ( Iron + carbon)
  • Brass (copper + zinc)
  • Bronze ( copper + tin)
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12
Q

Positives of alloys

A
  • Harder/ less malleable than normal metals
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13
Q

Why are alloys harder than normal metals?

A
  • made up of different sized atoms/ions
  • layers cannot slide over each other as easily
  • therefore less malleable
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14
Q

Use of Iron

A
  • To make steel, as it is more useful
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15
Q

Use and contents of low carbon steel

A
  • Iron, 0.1% carbon
  • used for making Ships, cars as they are strong but can be hammered to dif shapes
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16
Q

Use and contents of high carbon steel

A
  • Iron, 1% carbon
  • used for tools e.g screwdrivers, as they are less malleable than low carbon steel
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17
Q

Use and contents of stainless steel

A
  • Iron, 1% carbon, 10% Chromium
  • used for cutlery, cooking utensils as Chromium forms oxide layer preventing corrosion- stay shiny
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18
Q

use of copper + why

A
  • wires, pans, pipes
  • as good conductor of heat and electricity
  • unreactive and malleable
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19
Q

use of aluminium + why

A
  • aircraft bodies, power cables
  • as is low density, but is very strong and conductive
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20
Q

What are metal ‘ores’

A
  • rocks containing metals as compounds with Sulphur and Oxygen
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21
Q

why are metals in ores compounds with Oxygen and Sulphur

A
  • Over long periods of time underground metals have reacted with Oxygen and Sulphur
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22
Q

reactivity series (from least reactive)

A
  • Gold (Au)
  • Silver (Ag)
  • Copper (Cu)
  • [Hydrogen (H)] - not metal
  • Lead (Pb)
  • Iron (Fe)
  • Zinc (Zn)
  • [Carbon (C)] - not metal
  • Aluminium (Al)
  • Magnesium (Mg)
  • Calcium (Ca)
  • Lithium (Li)
  • Sodium ( Na)
  • Potassium (K)
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23
Q

Why are Gold and Silver native ( not in ores)

A
  • not reactive enough to combine with oxygen or sulphur
  • therefore found chemically uncombined
24
Q

Methods of metal ore extraction

A
  • Using electricity
  • Carbon extraction
25
Q

How does carbon extraction work

A
  • metals less reactive than carbon can be displaced from their ore when heated with carbon
26
Q

What is a displacement reaction

A
  • When more reactive metals displace less reactive metals from their compounds
27
Q

example of displacement reaction

A
  • magnesium displaces copper from copper sulphate
28
Q

equation for magnesium/copper sulphate displacement reaction

A

Magnesium + Copper sulphate –> Magnesium sulphate + copper

29
Q

Main observations to think about for displacement reaction

A
  • Solid colour change
  • solution colour change
30
Q

Two components of metal structure

A
  • lattice of positive metal ions
  • sea of delocalised electrons
31
Q

What is metallic bonding

A

The electrostatic attraction between the positive metal ions and negative delocalised electrons

32
Q

Metallic bonding is…

A

a very strong attraction

33
Q

properties of metals

A

-High melting points
-conduct electricity
-Malleable

34
Q

Why metals have high melting point

A
  • metallic bonding very strong, lots of energy needed to break bonds
35
Q

why metals conduct electricity

A
  • delocalised electrons free to move through lattice, carrying charge
36
Q

why metals malleable

A

layers of metal ions can slide over each other

37
Q

metal and water reaction equation

A

metal + water –> metal hydroxide + hydrogen

38
Q

example of metal and water reaction

A

magnesium + water –> magnesium hydroxide + hydrogen

39
Q

observations made in metal and water reaction

A
  • effervescence due to hydrogen gas produced
  • solid disappearing due to being used up in reaction
40
Q

group 1 (alkali) metals reaction with water

A
  • violent reaction
  • as they are highly reactive
41
Q

example of group 1 metal and water reaction

A

lithium + water –> lithium hydroxide + hydrogen

42
Q

Reactions of Li, Na and K in water similar observations

A
  • solid floats- less dense than water
  • effervescence- production of H gas
  • solid moves- effervescence propels it around surface
  • solid disappears- used up in reaction
43
Q

colour of universal indicator in solution of metal and water after reaction?

A
  • dark blue
  • metal hydroxide created- alkali
44
Q

reactivity of group 1 metals down the group

A
  • more reactive
45
Q

why are group 1 metals reactive

A
  • only need to lose 1 outer shell electron to get full outer shell
46
Q

why is it easier for group 1 metal atoms to react further down group?

A
  • 1 outer shell electron must be lost to react
  • down group=further away from nucleus
  • further away from nucleus- weaker attraction between electron and nucleus
  • less energy needed to break attraction
47
Q

metal and steam reaction equation

A

metal + steam –> metal oxide + hydrogen

48
Q

example of metal and steam reaction

A

magnesium + steam –> magnesium oxide + hydrogen

49
Q

why do metals react with cold water and hot steam differently?

A
  • steam has more energy
  • therefore both hydrogen bonds in water can break
  • therefore metal ‘oxide’ not ‘hydroxide’
50
Q

how do conduct metal and steam reaction ( Mg)

A
  • horizontal tube
  • wet wool and magnesium placed inside
  • tube heated
  • Hydrogen gas (product) escapes tube and is ignited to safely destroy it
51
Q

Acid and metal reaction

A

metal + acid –> salt + hydrogen

52
Q

example of acid and metal reaction

A

magnesium + sulphuric acid –> magnesium sulphate + hydrogen

53
Q

observations of metal and acid reaction

A
  • metal disappears as it is used in reaction
  • effervescence as hydrogen gas is produced
54
Q

why do group 1 all have the same chemical properties

A

they all have one electron in their outer shell

55
Q

characteristics of group 1 metals

A
  • need to be stored in oil
  • soft so can be cut easily
  • oxidise quickly so become dull when cut
  • low mtp/density

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