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Chemistry > Booklet 4 - Reactivity Of Metals > Flashcards

Booklet 4 - Reactivity Of Metals Flashcards

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1
Q

What are the metals that react with water?

A

Potassium, sodium, lithium, calcium

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2
Q

Which metals reacts with acids?

A

Potassium, sodium, lithium, calcium, magnesium, zinc, iron, tin, lead

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3
Q

Which metals react with oxygen?

A

Potassium, sodium, lithium, calcium, magnesium, aluminium, zinc, iron, tin, lead, copper, mercury, silver

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4
Q

What does the reactivity of a metal depend on?

A

Depends on how easily it loses an electron to form a positive ion, it is called a cation

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5
Q

What is the word to descibe a metal that is more able to lose electrons and become a positive ion?

A

They are more reactive

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6
Q

What do metals that react with oxygen make?

What is the general equation for this?

A

Metal oxides

Metal + oxygen-> metal oxide

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7
Q

What is the equation for sodium and copper reacting with oxygen? What are they examples of?

A

Sodium + oxygen -> sodium oxide
4 Na + O2 -> 2NaO

Copper + oxygen -> copper oxide
2Cu + O2 -> 2CuO

Oxidation

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8
Q

Which metals react with dilute acids?

A

Anything more reactive than hydrogen

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9
Q

Which metals react with cold water?

A

Anything above magnesium

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10
Q

What is a displacement reaction?

A

It is when a more reactive metal will take the place (displace) a less reactive metal in a conpound.
Basically a battle between two metals to get rid of electrons

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11
Q

What type of metals are gold and silver and where are they found?

A

Unreactive metals

Found in the earth

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12
Q

What are most metals found as? What do they require to extract the metal?

A

Found as metal compounds, require chemical reactions to extract

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13
Q

What can metals less reactive than carbon be extracted by?

A

Extracted from their oxides by reduction with carbon

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14
Q

What is the equation for the reduction of iron ore by carbon?
What has happened?

A

Iron oxide + carbon -> iron + carbon dioxide
Fe2O3 + 3C -> 2Fe + 3

The carbon removes the oxygen from iron oxide, hence carbon has reduced the iron oxide

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15
Q

What is Oxidation?

A

A reaction where a substance gains oxygen or as a reaction where a substance loses electrons

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16
Q

What is reduction?

A

Loss of oxygen or gain of electrons

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17
Q

What is OILRIG?

A

Oxidation Is Loss, Reduction Is Gain

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18
Q

When can oxidation also occur? What does the metel need?

A

It can occur when there is no oxygen in the reaction, it only needs electrons to lose to undergo oxidation

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19
Q

What are redox reactions?

A

Where oxidation and reduction both occur

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20
Q

What happens to the ions of the less reactive metal?

A

They gain electrons and become REDUCED

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21
Q

What happens to the atoms of the more reactive metal?

A

They lose electrons and become OXIDISED

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22
Q

What does the pH scale do? What does it run from and to?

A

Shows how acidic or alkaline a solution is. Runs from 1-14

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23
Q

What does the Universal Indicator do? What colour is it in acid, alkali and neutral?

A

It shows the pHs of different substances.
Red in acid
Blue in alkali
Green when neutral

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24
Q

What can also give us a pH value?

A

A pH probe can give an electric value for pH often to 2 decimal places

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25
Q

What do acids produce?

A

Hydrogen ions, H+

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26
Q

What do aqueous solutions of alkalis contain?

A

Hydroxide ions, OH-

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27
Q

When neutralisation occurs write the equation for when the two ions combine to make water?

A

H+(aq) + OH-(aq) -> H2O(l)

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28
Q

What is a salt?

A

An ionic compound made from any metal and and non metal

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29
Q

The acid with metal hydroxides are neutralisation reactions. What reacts with what?

A

The H+ of the acid reacts with the OH- of the alkali.

H+ + OH- —> H2O

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30
Q

The acid with metal hydroxies or metal oxides are neutralisation reactions? What reacts with what?

A

The H+ of the acid reacts with the O2- of the base.

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31
Q

What happens when some metals are too UNreactive and some are too REACTIVE?

A

They will react with the water that the acid dissolved in as well the acid itself.

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32
Q

Why is it useful to know the reactivity of carbon even though its not in the reactivity series?

A

It is often used to displace metals that are lower than it in the series, from their metal oxides

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33
Q

Why is it useful to know the reactivity of hydrogen even though its not in the reactivity series?

A

It is low in the series, therefore it’s able to be displaced by metals hugher upnin the series

34
Q

What is a Titration?

A

The volume of acid and alkali solutions that react with each other can be measured by titration using a suitable indicator

35
Q

What is the titration technique?

A

1) . Wash and rinse a pipette with the alkali
2) . Use the pipetter to measure out a known and accurate volume of the alkali.
3) . Place the alkali in a clean dry conical flask and add a suitable indicator
4) . Place the acid in a burette that has been wahsed and rinsed in the acid. Take a reading of the volume of the acid ie the inital reading
5) . Add the acid until the indicator changes colour ie neutral point. This is the end point. Take the final reading
6) . Calculate the volume of acid added by subtracting the inital reading crom the final reading
7) . Repeat again

36
Q

What happens to strong acids when dissolved in water?

A

They ionise to form H+ ions plus the negative ion

37
Q

What is a weak acid? And give an example

A

they ionise in water partially more usually 2%

38
Q

What makes weak acids like vinegar and citric acid much less acidic?

A

They ionise only 2% which means they produce fewer H+ ions when dissolved in solution.

39
Q

What are the names of 3 strong acids?

A

HCl, HNO3, H2SO4

40
Q

What are the names of the 3 weak acids?

A

CH3CO2H (ethanoic acid), citric acid, HaCO3 (carbonic acid)

41
Q

What is a ‘strong’ acid?

A

A acid that’s completely ionised in aqueous solutions, all acid particles dissociate to release H+ ions

42
Q

What is a ‘weak’ acid?

A

A acid that will only partially ionise in aqueous solutions, only a small proportion of acid particles dissociate to release H+ ions

43
Q

What is the concentration of an acid?

A

Concentration measures how much acid there is in a certain volume of water, ie the total number of dissolved acid molecules

44
Q

What is a ‘dilute’ acid?

A

Considered to be acids that are watered down versions of the real stuff ie more water and hardly any acid.

45
Q

As pH decreases by 1 unit, what factor does the concentration of H+ ions increase by?

A

Factor of 10

46
Q

What do metals that react with other substances what do they form?

A

the metal atoms from positive ions

47
Q

What do some acids react with metals to produce?

A

Salts and hydrogen

47
Q

How can soluble salts be made from by acids?

A

Reacting them with:

1). In soluble substance eg metals, hydroxides, metals oxides and carbonates

47
Q

How can you produce solid salts?

A

By crystallising salt solutions

47
Q

For a given concentration of aqueous solutions what does it mean for a stronger acid?

A

The lower the pH

48
Q

What happens when an ionic compound is melted or dissolved?

A

The water ions are free to move about within a solution, these solutions are then able to conduct electricity

48
Q

What is the liquid substance that is broken down called?

A

An electrolyte

48
Q

What happens when you pass an electrical current through electrolytes?

A

It causes the ions to move to the electrodes. Positively charged ions move to the negative electrode the cathode, negatively charged ions move to the positive electrode the anode

48
Q

What happens the ions at the electrodes?

A

They are discharged producing elements -> electrolysis

48
Q

What happens when a simple ionic compound eg lead bromine is electrolysed?

A

Its electrolysed in molten state using inert electrodes, the metal (lead) is produced at the cathode and the non metal (bromine) at the anode

48
Q

How can metals be extracted from molten compounds?

A

Using electrolysis

48
Q

Why is electrolyis used to extract metals from metal compounds?

A

If the metal is too reactive to be extracted by reduction with carbon or if the metal reacts with carbon. Large amounts of energy are used in the extraction process to melt the compounds and to produce electrical current

48
Q

What do the ions that are discharged in a aqueous solution during electrolysis depend on?

A

The releative reactivity of the elements involved

49
Q

Why is oxygen only produced at the anode if no halide ions are made?

A

In the aqueous solution water molecules break down producing hydrogen ions and hydroxide ions that are discharged

50
Q

What happens during electrolysis at the cathode?

A

Positively charged ions gain electrons and so the reactions are reductions

51
Q

What happens during electrolysis at the anode?

A

Negatively charged ions lose electrons and so the reactions are oxidation

52
Q

What reactions at electrodes be represented as?

A

1) . 2H+ + 2e- –> H2

2) . 4OH- –> O2 + 2H20 + 4e

54
Q

What happens when a acid neutralises a base (vice versa)?

A

The products are neutral

55
Q

What is the reaction between a acid and a base?

A

A neutralisation one

Acid + base -> salt + water

56
Q

What do all metal oxides and metal hyrdoxides form?

A

Acid + metal oxide -> salt + water

Acid + metal hydroxide -> salt + water

57
Q

What is the extraction of a metal?

A

reduction = loss of oxygen

59
Q

what happens if H+ ions or metal ions are present at the cathode?

A
  • if the elemental metal formed is more reactive, then hydrogen gas is made.
  • if the elemental metal is less reactive than hydrogen a solid layer of the pure metal will be produced
60
Q

what happens if OH- and halide ions are present at the anode?

A
  • molecules of chlorine, bromine or iodine will be formed

- if none are present, then the OH- ions are discharged and oxygen will be formed

61
Q

What is an alkali?

A

A base that dissolves in water to form a solution with a pH greater than 7, they form OH- ions is water.

62
Q

describe the ionisation of a weak acid?

A

its a reversible reaction, which sets up an equilibrium between the undissociated and dissociated acid, since only a few of the acid particles release H+ ions, the position of equilibrium lies well to the left

63
Q

what does it mean if the concentration of the H+ ions is higher?

A

the rate of the reaction will be faster, so strong acids will be more reactive than weak acids of the same concentration

64
Q

what is the equation for acids and bases?

A

Acid + base -> salt + water

- its a neutralisation reaction

65
Q

what is the equation for acid and metal carbonates?

A

Acid + metal carbonate -> salt + water + carbon dioxide

66
Q

what does the salt produced in any reaction between an acid and a base or alkali depend on?

A
  • the acid used eg hydrochloric acid produces chlorides, nitric acid produces nitrates and sulphuric acid produces sulfates
  • the positive ions in the base, alkali or carbonate
67
Q

what does it mean for the metal the higher up in the reactivity series it is?

A

the more easily they will form positive ions and the more easily it reacts with water or acid

68
Q

what is the equation for a acid and metal?

A

Acid + metal -> salt + hydrogen

69
Q

what the equation for a acid and water?

A

Metal + Water -> metal hydroxide + hydrogen

70
Q

what happens to the metal ion and metal atom in a displacement reaction?

A

the metal ion gains electron and is reduced, the metal atom always loses electrons and is oxidised

71
Q

what can and can’t be electrolysed in electrolysis?

A

an ionic solid can’t be electrolysed as the ions are in fixed positions while molten ionic compounds can be as their ions can move freely and conduct electricity

72
Q

what happens when a simple ionic compound eg lead bromine is electrolysed in molten state?

A

its done using inert electrodes, the metal (lead) is produced at the cathode and the non metal (bromine) is made at the anode

73
Q

why must the anode be replaced continually?

A

the anode is made of carbon and as it reacts with oxygen it produces CO2

74
Q

how is aluminium manufactured?

A

by the electrolysis of a molten mixture of aluminium oxide and cryolite using carbon as the anode
- cryolite is used as it lowers the high melting point of Al, its a aluminium based compound

Chemistry (12 decks)

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