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GCSE Chemistry > C5 > Flashcards

C5 Flashcards

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1
Q

What does the reactivity series do?

A

Order metals on how reactive they are

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2
Q

Reactivity series ?

A 
Potassium
Sodium 
Lithium 
Calcium
Magnesium
Carbon
Zinc
Iron
Hydrogen
Copper
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3
Q

How are metals reactivity determined?

A

How easily they lose electrons forming positive ions. The higher on the reactivity series , the more easily they form positive ions

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4
Q

What does the place of the metal in the reactivity series say about how is reacts with water or acid?

A

When a metal reacts with water or acid , they lose electrons and form positive ions. So the higher the metal on the reactivity seriees the more easily it reacts with water or acid

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5
Q

How was the reactivity series made?

A

Comparing the relative reactivity of different metals with either acid or water and put them in order from most reactive to least reactive .

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6
Q

What happens if a metal and acid react?

A

Acid + metal —-> salt + hydrogen

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7
Q

How to measure the speed of a reaction between acid and a metal?

A

Indicated by the rate at which bubble of hydrogen are given off.

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8
Q

What does the ph go from ?

A

0-14

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9
Q

What does the ph measure?

A

How alkaline or acidic a substance is

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10
Q

How will certain metals react with acid ?

A

More reactive the metal , the faster the reaction. Potassium , sodium , lithium and calcium react explosively. Less reactive metals like magnesium , zin and iron react less violently. Copper wont react with cold dilute acids in general.

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11
Q

How to investigate the reactivity of metals?

A

Measure the temperature change of the reaction with an acid or water over a set period of time. If you use the same mass and surface area of metal each time , the more reactive the metal , the greater the temperature

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12
Q

What happens when a metal and water react together ?

A

Metal + water —-> metal hydroxide + hydrogen

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13
Q

What metals react with water?

A

Potassium , sodium , lithium , calcium

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14
Q

Which metals wont react with water?

A

Zinc, iron , copper

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15
Q

What type of substance is low in ph?

A

Acidic

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16
Q

What type of substance is high in ph ?

A

Alkaline

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17
Q

What type of substance is in the middle of the ph scale?

A

Neutral substance, water

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18
Q

What is an indicator?

A

A dye that changes colour depending on whether its above or below a certain PH

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19
Q

What is a wide range indicator?

A

Contains a mixture of dyes that menas they gradually change colour over a broad range of ph. Useful for estimating the ph of a solution

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20
Q

What is an acid?

A

A substance that forms an aqueous solutions with ph of less than 7. Acids form H+ ions in water.

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21
Q

What is a base?

A

A substance with a ph greater than 7

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22
Q

What is an alkali ?

A

A base that dissolves in water to form a solution with a PH greater than 7. It forms Hydroxide ions in water

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23
Q

What is neutralisation?

A

The reaction between acids and bases

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24
Q

What is the equation for neutralisation?

A

Acid + base —-> salt + water

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25
Q

What is the product hydrogen ions react with hydroxide ions?

A

H+ + OH- —–> H2O(water)

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26
Q

What is a strong acid?

A

An acid that ionises completely in an aqueous solution. All acid particles dissociate to release H+ ions.

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27
Q

Examples of strong acids ?

A

Sulfuric, hydrochloric and nitric

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28
Q

What is a weak acid ?

A

Am acid that does not fully ionise in an aqueous solution . Only a small proportion of acid particles dissociate to release H+ ions

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29
Q

Examples of weak acids?

A

Ethanoic , citric and carbonic acids

30
Q

What type of reaction it the ionisation of a weak acid?

A

Reversible reaction , which sets up an equilibrium between the undissociated and dissociated acid . Since only a few of the acid particles release hydrogen ions, the equilibrium is more to the left of the reaction

31
Q

What type of acid is more reactive and why?

A

Strong acids. The concentration of hydrogen ions is higher so the rate of reaction will be faster.

32
Q

What does a reaction of acids involve?

A

Involves hydrogen ions reacting with other substances

33
Q

How does the strength of an acid effect its ph?

A

Stronger the acid the lower the ph

34
Q

What happens to an acid if the ph decreases by 1 unit

A

Hydrogen ion concentration increases by 10

35
Q

What must you take into account when you measure the ph of a strong and weak acid?

A

The concentration of them both

36
Q

What does the acid strength tell you?

A

The proportion of the acid molecules that ionise in water

37
Q

What is the concentration of an acid?

A

Measures how much acid there is in a certain volume of water.

38
Q

What is a concentrated acid solution ?

A

Large amount of acid in the certain volume

39
Q

What is a dilute acid?

A

When there is more water than acid .

40
Q

What are metal oxides and metal hydroxides?

A

Bases

41
Q

What is formed if an acid reacts with a metal oxide or hydroxide ?

A

Acid + metal oxide/hydroxide —> salt + water

42
Q

How to form a metal oxide?

A

metals react with oxygen

43
Q

Properties of metal oxides and hydroxides?

A
  • some dissolve in water
  • soluble compounds
  • alkali
44
Q

How are acids neutralised?

A

By alkalis , (soluble metal hydroxides)and bases (insoluble metal hydroxides and oxides) to produce salts an water. Also by metal carbonates that produce carbon dioxide also

45
Q

What are metal carbonates ?

A

Base

46
Q

What happens if a metal carbonate reacts with an acid?

A

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

47
Q

The particular salt produced in any reaction between an acid and a bas or alkali depends on ?

A
  • acid used (hydrochloric acid produces chlorides, nitric acid produces nitrates , sulphuric acid produces sulfates)
  • positive ions in the base , alkali or carbonate
48
Q

How can soluble salts be made?

A

From acids by reacting them with solid insoluble substances , such as metals , metal oxides , hydroxides or carbonates. Solid is added to the acid until no more reacts and the excess solid is filtered off to produce a solution of the salt.

49
Q

What can you do to a salt solution to produce solid salt ?

A

Crystallisation

50
Q

Why do you have to extract metals?

A

Unreactive metals such as gold are found as pure gold but most are found as compounds that require a chemical reaction to extract the metal

51
Q

What is oxidation?

A

When metals react with oxygen to form an oxide.

52
Q

What is a reaction that separates a metal from its oxide?

A

Reduction reaction.

53
Q

What happens for the formation of a metal ore?

A

Oxidation reaction . Gain of oxygen means creates a metal oxide

54
Q

What is the reaction when you extract a metal?

A

Reduction reaction . Loss of oxygen so the metal oxide is reduced to just the metal

55
Q

How can metals be chemically extracted from their ores ?

A

By reduction using carbon.

56
Q

What happens during reduction using carbon?

A

Ore is reduced as oxygen is removed from it , and carbon gains oxygen so it is oxidised

57
Q

Examples of a reduction reaction with carbon?

A

Iron(III) oxide + carbon —> iron + carbon dioxide

58
Q

What determines whether a metal oxide can be reduced using carbon?

A

Its place in the reactivity series

59
Q

How do metal high than carbon In the reactivity series get extracted ?

A

Electrolysis

60
Q

How do metals below carbon get extracted ?

A

Extracted using reduction with carbon. This is because carbon can only take away the oxygen from metals which are less reactive than carbon itself

61
Q

What non metals are in the reactivity series ?

A

Hydrogen and carbon

62
Q

What does oxidation mean in terms of electrons?

A

Loss of electrons

63
Q

What does reduction mean in terms of electrons ?

A

Gain of electrons

64
Q

What does OILRIG show?

A 
Oxidation
Is
Loss
Reduction
Is 
Gain

(In terms of electrons)

65
Q

Why is there the term REDOX reactions?

A

Because oxidation and reduction happen at the same time.

66
Q

Examples of a REDOX reaction?

A

Iron atoms oxidised to Fe2+ when react with dilute acid :
Fe + 2H+—> Fe2+ + H2
Iron atom loses electrons . They are oxidised by hydrogen ions:
Fe- 2e- —-> fe2+
Hydrogen ions gain electrons . They’re reduced by the iron atoms:
2H+ + 2e- —-H2

67
Q

What type of reaction are all metals + acids?

A

Redox reactions

68
Q

What is a displacement reaction?

A

A more reactive metal will displace a less reactive metal from its compound

69
Q

Examples of ionic equation from displacement reactions?

A

Iron + copper sulfate —> iron sulfate + copper

In terms of ions:
Fe —> Fe2+ + 2e- = oxidisation . Iron loses 2 electrons to become a 2+ ion

Cu2+ + 2e- —->. Cu. = reduction . Copper gains 2 electrons to become a copper atom

70
Q

What is shown in an ionic equation?

A

The particles that react and the products

GCSE Chemistry (14 decks)

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