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Chemistry iGCSE 3rd Form > Metals > Flashcards

Metals Flashcards

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1
Q

Where are metals found in the periodic table?

A

metals are found on the left of the table- to the left of the ladder which starts above aluminium and steps down to the right

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2
Q

List five properties of metals

A

conducts electricity and heat

shiny

malleable

ductile

some are magnetic

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3
Q

Which group is called the alkaline metals?

A

Group 1

Li

Na

K

Rb

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4
Q

What group is called the Alkaline Earth Metals?

A

Group 2

Be

Mg

Ca

Sr

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5
Q

What is special about the transistion metals?

A

They form colourful compounds

&

They often have more than one valency

Fe 2+ and Fe 3+

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6
Q

What group are called the Halogens?

A

Group 7

F

Cl

Br

I

They are all diatomic!

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7
Q

What group is called the noble gases?

A

Group 0

He

Ne

Ar

Kr

they all have a full outer shell and are inert (unreactive)

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8
Q

Name the four metals less reactive than hydrogen in the reactivity series

A

Hydrogen

Copper

Silver

Platinum

Gold- unreactive

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9
Q

Name the five metals more reactive than carbon in the reactivity series

A

potassium

sodiium

calcium

magnesium

aluminium

carbon

All these metals must be extracted using electrolysis as carbon cannot displace them as it is less reactive

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10
Q

Name the four metals between carbon and hydrogen in the reactivty series

A

Carbon

Zinc

Iron

Tin

:Lead

Hydrogen

These metals can be extracted from their ores using carbon or coke in a blast furnace

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11
Q

Why can iron be reduced or extracted from its metal ore using coke (carbon)?

A

Carbon is more reactive than iron

Carbon displaces iron

iron is reduced

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12
Q

Henry threw some copper into some hydrochloric acid. He expected to see a reaction, some fizzing, but nothing happened. explain why?

A

copper is less reactive than hydrogen

copper cannot displace hydrogen and so it does not react

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13
Q

Describe three properties of the group 1 metal sodium

A

soft - can be cut with a knife

shiny when cut but then quickly reacts and becomes dull

low melting point

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14
Q

Finish the general equation

reactive metal + water –>

A

remember the fizzing?

reactive metal + water –> metal hydroxide + hydrogen

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15
Q

What is the chemical reaction between lithium and water?

A

Li (s) + H2O(l) –> LiOH(aq) + H2(g)

Lithium hydroxide is an alkali- it will turn universal indicator blue

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16
Q

What would you observe if you put some sodium in water?

How would this compare to potassium in water?

A

For sodium

fizzing, moving around on the surface of the water

melts into a ball, metal disappears

For potassium - it is more reactive

more vigorousfizzing

moving around on the surface of the water more quickly

melts into a ball and bursts into flame (lilac in colour)

metal disappears more rapidly

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17
Q

What is the chemical reaction between sodium and water?

A

Na (s) + H2O(l) –> NaOH(aq) + H2(g)

sodium hydroxide is an alkali- it will turn universal indicator blue

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18
Q

What is the chemical reaction between potassium and water?

A

K (s) + H2O(l) –> KOH(aq) + H2(g)

potassium hydroxide is an alkali- it will turn universal indicator blue

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19
Q

How would the reaction differ between potassium and rubidium?

A

Potassium

lilac flame

Rubidium

explosive

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20
Q

What is an alloy?

A

A mixture of a metal and metal or a metal and non-metal which changes both the physical and chamical properties

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21
Q

Give three examples of an alloy

A

Brass- copper + zinc

Bronze- copper + tin

Steel- iron + carbon

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22
Q

How does the introduction of a different sized atom to a pure metal change its physical properties.

A

The smaller atoms disrupts the arrangment of the metal ions,

They no longer arrange themselves in neat rows

They do not have layers which can slide over one another

They are no longer malleable- they are harder and stronger

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23
Q

When calcium reacts with hydorchloric acid, hydrogen forms.

How can the hydrogen be collected?

A

hydrogen can be collected by downward displacement of water

OR

downward displacement of air - upside down test tube- hydrogen is less dense than air and will rise into the test tube and push the air downward

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24
Q

What are the products in this reaction?

Mg + H2O (g) –>

steam

A

Mg + H2O (g) –> MgO + H2

steam

with steam the oxide is formed-not the hydroxide!

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25
Q

Both potassium and sodium are found in group 1

Why is potassium more reactive than sodium?

A
  • potassium atom is larger
  • outer electrons of potassium are further from the nucleus
  • less electrostatic attraction between the negative outer electrons and positive nucleus
  • easier to remove the outer electron from potassium
  • Also, there are more shells between the nucleus and outer electrons in potassium
  • the electrons in these shells repel the outer electrons and is called electron shielding
  • easier to remove the outer electron from potassium
  • potassium is more reactive for these two reasons!
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26
Q

Complete the reaction

Al + Fe2O3 –>

A

Thermite reaction!!

Is aluminium more reactive than iron? YES!

2Al + Fe2O3 –> Al2O3 + 2Fe

Aluminiuim is more reactive than iron

aluminium displaces the iron

This is a displacement reaction

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27
Q

Complete this general reaction

metal + steam –>

A

Metal + steam –> metal oxide + hydrogen

You still get hydrogen but now you have the oxide- not the hydroxide

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28
Q

What is the test for hydrogen gas?

A

Flaming splint

you hear a squeaky pop!

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29
Q

Why does it take time for aluminium to start reacting with an acid?

A

aluminium forms an impermeable aluminium oxide layer.

The acid must get through that layer before it comes into contact with the pure metal.

This impermeable oxide layer on aluminium is an advantage- iron reacts with oxygen and rusts entirely through the metal but aluminium forms an impermeable oxide layer protecting the pure aluminium below.

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30
Q

Complete the general word equation

more reactive metal + less reactive metal compound –>

A

more reactive metal + less reactive metal compound –>

more reactive metal compound + less reactive metal

the more reactive metal displaces the less reactive metal

This is a displacement reaction

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31
Q

Complete the displacement reaction and describe what you would observe

Zn + CuSO4 –>

A

Is zinc more reactive than copper?

Yes

Zn + CuSO4 –> ZnSO4 + Cu

greysolid & blue solution –> colourless solution & orange/pink soild

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32
Q

Below is the thermite reaction!!

2Al + Fe2O3 –> Al2O3 + 2Fe

Where is this used and is the reaction an exothermic or endothermic reaction? How do you know?

A

Thermite reaction is used to connect (fuse) iron rails together on a railway.

This reaction is carried out above the seam between the two rails

The reaction is exothermic- it releases heat rapidly and exceed the melting point of iron which melts out the bottom of the vessel and onto the seam.

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33
Q

Complete the displacement reaction and describe what you would observe

Fe + ZnSO4 –>

A

Is iron more reactive than zinc?

No- the rion cannot displace the zinc

No reaction - grey metal in colourless solution with no change to appearance

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34
Q

Complete the metal displacement reaction

Ca + MgNO3 –>

A

Ca + 2MgNO3 –> Ca(NO3 )2 + 2Mg

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35
Q

Which reaction will be more vigorous and why?

Mg + Fe2O3 –>

Zn + Fe2O3 –>

A

The Mg and Fe reaction will be more vigorous because Mg and Fe are further apart in the reactivity series.

The further apart metals are in the reactivity series the more violent their displacement reactions will be.

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36
Q

How can you use metal and acid reactions to order metals in terms of reactivity?

A

Place the metals in the same concentration and type of acid and compare the rate of fizzing

the more vigorous the fizzing, the more reactive the metal

37
Q

Define a metallic bond

A

the electrostatic attractionn between potive metal ions and the negative delocalised electrons

38
Q

Describe the stuucture of a metal

A

regular arrangement of metal ions

layers of metal ions surrounded by a sea of delocalised electrons

39
Q

Why do metals have high melting points?

A
  • many strong metallic bonds in a giant structure
  • requires a lot of energy to overcome
40
Q

als

A
41
Q

Are metals soluble in water or organic solvents?

A

No- they are not soluble in either.

NOTE: reactive metals react with water but they are not soluble

42
Q
A
43
Q

Whjy do metals conduct electricity?

A
  • metals have delocalised electrons which are free to move

and carry charge

44
Q

Why are metals malleable?

A
  • metal ion layers can slide over one another
  • without distrubing the metallic bonds
45
Q

Which four materials are added to a blast furnace?

A

iron (III) oxide

limestone

coke

hot air

46
Q

What are the products from a blast furnace?

A

iron metal

carbon dioxide

slag

47
Q

Which product in a blast furnace causes a concern from the environment?

A

carbon dioxide

is a greenhouse gas which may lead to global warming

48
Q

Which reaction gets everything hot in the blast furnace?

A

combustion of coke

C + O2 –> CO2 exothermic!!!

49
Q

Which reaction forms the reducing agent in the blast furnace?

A

C + CO2 –> 2CO

coke is added in excess so that CO is formed (carbon monoxide)

carbon monoxide is the reducing agent- it reduces the iron (III) oxide

50
Q

What is the formula for haematite?

A

iron (III) oxide

51
Q

What is the name of iron ore?

A

Haematite

52
Q

Complete the redox reaction which happens in the blast furnace

Fe2O3 + 3CO –>

A

Fe2O3 + 3CO –> 3CO2 + 2Fe

Fe has been reduced - lost oxygen

C is oxidised - gained oxygen

53
Q

Explain how the reaction below is a redox reaction- a reaction where both oxidation and reduction occurs

Fe2O3 + 3CO –> 3CO2 + 2Fe

A

Fe2O3 + 3CO –> 3CO2 + 2Fe

Fe has been reduced - lost oxygen

C is oxidised - gained oxygen

54
Q

Which mnemonic is used to work out which elements are reduced or oxidised in a reacion?

A

OIL RIG

OIL - oxidation is loss of electrons

RIG - reduction is gain of electrons

REMEMBER: if the atom has gained or lost oxygen you must speak about that and not the gain or loss of electrons

55
Q

Why do we add limestone to a blast furnace?

A

To get rid of the impurity found in iron ore

First- the limestone thermally decomposes to calcium oxide because the blast furnace is hot

CaCO3 –> CaO + CO2

The calcium oxide then reacts with the impurity silicon dioxide to form calcium silicate OR SLAG

CaO + SiO2 –> CaSiO3

SLAG

The slag is less dense than the molten iron and float on top

56
Q

Complete the thermal decomposition of calcium carbonate in a blast furnace

CaCO3 –>

A

Thermal decomposition means that the compound breaks apart by heating

CaCO3 –> CaO + CO2

57
Q

Complete the reaction which forms SLAG in a blast furnace

CaO + SiO2 –>

A

This is a neutralisation reaction

metal oxide CaO - acidic

non-metal oxide SiO2 - alkaline

CaO + SiO2 –> CaSiO3

alkaline + acid –> salt

58
Q

What is the name of the impurity in haematite?

A

silicon dioxide

SiO2

59
Q

What is the chemical formula for SLAG which forms in a blast furnace/

A

CaSiO3

60
Q

Why is it easy to separate SLAG from iron metal in a blast furnace?

A

Both are molten (melted) but the slag is less dense and floats on top of the molten iron

61
Q

What type of reaction is this?

C + O2 –> CO2

A

combustion or oxidation as carbon gained oxygen

62
Q

What type of reaction is this?

CaCO3 –> CaO + CO2

A

Thermal Decomposition

the CaCO3 is decomposing or breaking apart

63
Q

What is the reaction for rusting of iron?

A

4Fe + 3O2 + 5H2O –> 2Fe2O3•5H2O

iron needs both water and oxygen to rust!

Note: salt in not needed but is a catalyst- it speeds up the reaction by lowering hte activation energy but is not used in the reaction

64
Q

What is the chemical formula for rust?

A

Fe2O3

65
Q

What is the chemical name for rust?

A

iron (III) oxide

66
Q

Name three barrier methods to stop iron from rusting

A

paint - to stop oxygen and water getting to iron

coat in plastic- to stop oxygen and water getting to iron

oil or grease- to stop oxygen and water from getting to irion

67
Q

Name two sacrificial methods to stop iron from rusting

A

galvanising- coating in zinc- used for buckets etc

sacrificial protection with block of magnesium or zinc- used for bridges or large structures where coating in zinc is too expensive

68
Q

What is the name of this this protection method for iron?

Fe2O3 + 3Zn –> 3ZnO + 2Fe

A

sacrificial protection

Zn metal –> Zn 2+ + 2e-

zinc reacts and gives 2 electrons to any iron ions which have formed to reduce it back to iron metal- protecting the iron and sacrificing the zinc

Fe 3+ + 3 e- –> Fe metal

69
Q
A
70
Q

Which metal is being reduced and which one is being oxidised? How do you know?

Fe2O3 + 3Zn –> 3ZnO + 2Fe

A

Fe2O3 + 3Zn –> 3ZnO + 2Fe

iron is reduced as it is losing oxygen

zinc is oxidised as it is gaining oxygen

71
Q

Metal carbonates thermally decompose to form a metal oxide and carbon dioxide

Which properties of carbon dioxide prevents us from collecting it by downward displacement of water and allows us to collect it by downward displacement of air?

A

carbon dioxide is soluble in water- if collected by downward dislacement of water the carbon dioxide would dissolve in the water

carbon dioxide is more dense than air- if a tube was placed in a upright test tube the more dense carbon dioxide would fill the test tube and push the air out.

72
Q

What is the test for carbon dioxide?

A

bubble though limewater

limewater turns cloudy

73
Q

What would you observe in this thermal decomposition reaction?

CuCO3 –> CuO + CO2

green black

A

green power moves as gas escapes the green powder turns black

74
Q

Write the thermal decomposition reaction of Copper (II)carbonate

A

CuCO3 –> CuO + CO2

75
Q

Complete the reaction for the thermal decomposition of calcium carbonate

A

CaCO3 –> CaO + CO2

76
Q

Why can’t we extract aluminium from aluminium ore using coke (carbon)

A

Carbon is less reactive than Aluminium

it cannot displace aluminium from aluminium ore?

77
Q

What is the name of aluminium ore?

A

Bauxite

Al2O3

78
Q

What method do we use for the extraction of aluminium form aluminium ore?

A

electrolysis

79
Q

Define electrolysis

A

The decomposition of a compound using electricity

80
Q

Why do we need to melt the aluminium ore before carying our electrolysis?

A

Aluminium ore is ionic, when melted the metal ions are free to move and carry charge

we need electricity to pass through the molten ore for electrolysis to occur

81
Q

What is added to aluminium oxide to make the extraction of aluminium cheaper?

A

Cryolite is added to the aluminium ore- this reduced the melting point of the ore

Less heat is used- cheaper process

82
Q

Why is electrolysis more expensive than using a blast furnace to extract a metal from its metal ore?

A

Electrolysis used both electricity and heat to extract the metal.

Blast furnace only needs heat

83
Q

Which ions are free to move when Al2O3 is melted during electrolysis

A

Al 3+

O 2-

84
Q

When aluminium ore is molten the two ions which are mobile are

Al 3+

O 2-

Which ion will move toward the cathode? The negative electrode?

Which ion eill move towards the anode? the positive electrode?

A

Al 3+ is positively charged and will be attracted to the cathode or negatively charge electrode

O 2- is negatively charged and will be attracted to the anode or positviely charge electrode

85
Q

Why is the entire container charge negatively in the electrolysis of aluminium ore?

A

The positive aluminium ions will be attracted to the bottom of the container allowing the aluminium to form there- it can then be tapped off

86
Q

Why does aluminium oxide conduct when molten (melted) but not when it is a solid?

A

Aluminium oxide is ionic, when molten the ions are free to move and carry charge

When in the solid form the ions are not free to move and cannot carry charge

87
Q

Give two properties of carbon dioxide

A

It is soluble in water to form an acid

It is more dense than air

88
Q

Use the image below to explain why alloys are less malleable than pure metals

A

A pure metal will have a regular arrangement of atoms. The rows of metal atoms can slide easily over one another without disrupting the metallic bond

Alloys are a mixture of metals or a metal and non-metal. This often disrupts the regular arrangement. There are no complete rows of atoms which can slide over each other. Not malleable-harder substance

Chemistry iGCSE 3rd Form (7 decks)

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