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GCSE Chemistry > Chapter C5 Chemical Changes > Flashcards

Chapter C5 Chemical Changes Flashcards

1
Q

What are ores?

A

Rocks from which it is economical to extract metals that they contain

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2
Q

What does oxidised mean?

A

A substance that has had oxygen added to it

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3
Q

What are ores commonly chemically bonded to?

A

Oxygen from the air

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4
Q

Toe extract metals what must you do?

A

Reduce the metal oxide- have oxygen removed

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5
Q

Name the order of the reactivity series?

A 
Potassium 
Sodium 
Lithium 
Calcium 
Magnesium 
Aluminium 
Carbon 
Zinc
Iron 
Tin 
Lead 
Hydrogen 
Copper 
Silver 
Gold
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6
Q

What is the reactivity series?

A

A list of metals in order of their reactivity

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7
Q

Which metals fizz (give off hydrogen gas) when reacting with water?

A

Potassium
Sodium
Lithium
Calcium

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8
Q

What is fizzing?

A

Release of hydrogen gas

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9
Q

What happens when the most reactive metals react with water?

A

Fizz

Leave an alkaline solution of metal hydroxide

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10
Q

Which metals explode when reacting in dilute acid?

A

Potassium
Sodium
Lithium

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11
Q

Which metals have a very slow reaction with water?

A

Magnesium
Aluminium
Zinc
Iron

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12
Q

What requirement does aluminium have to meet before it reacts?

A

The oxygen must be removed

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13
Q

Which metals fizz when put in dilute acid?

A 
Calcium 
Magnesium 
Aluminium 
Zinc 
Iron
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14
Q

What happens when C M A Z I react with dilute acid?

A

Fizz, release hydrogen gas

Form a salt

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15
Q

Which metals have a slight reaction with steam?

A

Tin lead

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16
Q

Which metals react slowly with warm acid?

A

Tin

Lead

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17
Q

Which metals do not react with water even when steam is present?

A

Copper
Silver
Gold

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18
Q

Which metals do not react with dilute acid?

A

Copper
Silver
Gold

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19
Q

What happens when a more reactive metal displaces a less reactive one?

A

Forms an aqueous solution of one of its salts

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20
Q

Give an example of a displacement equation

A

Magnesium + copper sulfate —>

Magnesium sulfate +copper

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21
Q

Define oxidation

A

Loss of electrons

Loss of oxygen

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22
Q

Define reduction

A

Gain of electrons

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23
Q

Where are metals found?

A

The earths crust

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24
Q

What is a metal ore?

A

When there is enough metal in a rock to make it worth extracting the metal

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25
What are the three things that make it worth extracting a metal?
How easy it is to extract How much metal the ore contains The changing demands for a particular metal
26
What does carbon displace?
Less reactive metals from their oxides
27
Why use hydrogen to reduce oxide rather than carbon?
Carbon can result in the compound tungsten carbide
28
How are more reactive metals extracted from their ores if not reduction?
Electrolysis
29
When does a salt form?
When the hydrogenate in an acid is wholly or partially replaced by metal ions
30
How can you make salts?
Reacting metals more reactive than hydrogen with acid
31
Complete the equation Metal + acid ——>
A salt + hydrogen
32
Why are alkali metals not reacted with acid?
Reaction is too vigorous
33
What is formed when a metal reacts with HCL?
Salt chlorides
34
What is formed when a metal reacts with sulphuric acid?
Sulfate salts
35
What is formed when a metal reacts with nitric acid?
Nitrate salts
36
Complete the equation Mg + H^2SO^4—>
MgSO^4 + H^2
37
What are spectator ions?
ions that Do not change in the reaction
38
Complete the half equation Mg——>
Mg^2+ + 2e-
39
If atoms lose electrons they have been...?
Oxidised
40
If an atom gains electrons, they have been...?
Reduced
41
What is a redox reaction?
Metal atoms donate electrons to hydrogen atoms displacing hydrogen as a gas and leaving metal ions the solution
42
What are bases?
Compounds that can neutralise acids
43
What happens when you react an acid with a base?
Salt and water is formed
44
What are salts made up of?
Positive metal ions and a negative ion from an acid
45
What charge are salts?
No charge
46
What happens when an acid and alkali react?
Neutralise, creating a salt and water
47
How do you collect a pure dry sample of salts?
Carry out the titration with the indicator to see how much acid reacts completely with the alkali Run that volume of acid into the solution of alkali again, but without the indicator again Then crystallise and dry out the crystals of salt from the reaction mixture
48
What is the equation for acid and a carbonate?
Acid + a carbonate —> a salt + water + carbon dioxide
49
Give an example of an aqueous solution?
Washing powder in a washing machine
50
What are soluble hydroxides called?
Alkalis
51
What ph is pure water?
Neutral 7
52
What do all acids release when reacting with water?
Excess H+ ions
53
What do alkalis produce when reacting with water?
Aqueous hydroxide solutions
54
What makes a solution alkaline?
Excess aqueous hydroxide ions
55
What is the sign for a hydroxide ion?
OH-
56
What are indicators?
Substances that change colour when added to acid or alkalis
57
What is the highest and lowest number on the PH scale?
0 and 14
58
What happens when you dilute a strong acid?
Eventually becomes harmless
59
What is the link between concentrated solutions and dilute solutions?
Concentrated solutions contain more of that solute than solutions of the same volume of a dilute solution
60
Give examples of weak acids
Ethanoic acid - strong acid is HCL Citric acid- strong acid is nitric acid Carbonic acid- strong acid is sulfuric acid
61
What are carboxylic acids?
Weak acids
62
What makes a solution acidic?
H+ ions
63
What is equilibrium?
The point in a reversible reaction at which the forward and backward rates of reaction are the same- this amounts remain constant
64
What is the difference in PH value of strong and weak acids?
Weak acids have a higher PH
65
What does decreasing the concentration of H+ ions mol/dm do to the PH level?
As the concentration per dm reduces by a factor of ten, the PH goes up by one
66
As the concentration of H+ ions increase by a factor of ten, what happens to the PH level?
Decreases by one unit

GCSE Chemistry (9 decks)

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