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Chemistry Paper 1 > C4 > Flashcards

C4 Flashcards

(52 cards)

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1
Q

What is the formula of metals and oxygen

A

Metal + Oxygen = Metal oxide

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2
Q

What happens when potassium comes into contact with water

A

Starts fizzing and gliding on the surface of the water
Purple flame

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3
Q

What is the equation for reacting metals with water

A

Metal + water = metal hydroxide + hydrogen

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4
Q

What is the equation for reacting metals with acids

A

Metal + acid = metal salt and hydrogen

Magnesium + Hydrochloric acid → Magnesium chloride + Hydrogen

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5
Q

Transition metals can either have medium reactivity or low reactivity.
True or false?

A

True

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6
Q

What groups have high reactivity

A

Group 1 ,2 and 3

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7
Q

What three metals react vigorously with oxygen

A

Potassium
Sodium
Lithium

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8
Q

What four metals will react with water

A

Sodium
Lithium
Potassium
Calcium

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9
Q

What metals react with acids to form metal salts and hydrogen gas

A

Calcium and magnesium and zinc and iron

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10
Q

What is a displacement reaction

A

When a more reactive metal displaced a less reactive metal from its compound

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11
Q

What would you expect to observe if you react magnesium/zinc with copper sulfate

A

The solution will turn from blue to colourless

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12
Q

What is redox

A

When oxidation and reduction takes place at the same time

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13
Q

What always happens to the more reactive metal
What always happens to the less reactive metal

A

Reactive- ALWAYS GET OXIDISED
less reactive- ALWAYS GETS REDUCED

weaker metal- reduced in status

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14
Q

Describe what would happen if you added zinc metal oxide to a solution of silver.
Zinc is more reactive than silver

A

The zinc will strip the silver of its compound
The zinc will dissolve and become apart of the solution while the copper forms a powdery copper compound as it’s kicked out of the solution

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15
Q

What’s the symbol equation for nitrate

A

NO3

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16
Q

What’s the symbol equation for sulfate

A

SO4

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17
Q

What does the more reactive element in a displacement reaction become

What does the less reactive element in a displacement reaction become

A

More- an ion = to neutralise
Less- an element

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18
Q

Why would mass seem to change in a reaction

A

This happens when the reactant or product is a gas

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19
Q

Medium to high reactivity metals are often found in..

A

Ores- metal compounds in rock

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20
Q

If a metal is less reactive than carbon then what reaction will be carried out

A

A reduction

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21
Q

When a compound undergoes reduction what is produced

Study These Flashcards
A

The pure compound and carbon dioxide

22
Q

If a metal is more reactive than carbon what extraction method will take place

23
Q

What mnemonic can be used to remember the reactivity series

Study These Flashcards
A

Please Stop Calling Me A Careless Zebra Instead Try Learning How Copper Saves Gold

Potassium
Sodium
Calcium
Magnesium
Aluminium
Carbon
Zinc
Iron
Tin
Lead
Hydrogen
Copper
Silver
Gold
Platinum

24
Q

Reacting metal and water together will make-

Study These Flashcards
A

Metal hydroxide + hydrogen

25
What does a metal and acid react to make
Metal salt + hydrogen
26
What metal is oxidised and what metal is reduced in a reaction
The more reactive metal is always oxidised The less reactive metal is always reduced
27
Are medium and high reactivity metals formed in the ground
Yes
28
For metals more reactive than carbon what extraction method is used
Electrolysis
29
For metals less reactive than carbon what extraction method is used
Reduction with carbon
30
When reacted with metals, 3 things all produce salt + water What are these three things?
Metal oxide Metal hydroxide Alkali
31
Why are metal oxides and hydroxides called bases
Because they neutralise acids
32
Bases that can be dissolved in water is called a what
Alkali
33
Acid+ metal carbonate What does this produce
Salt + water + carbon dioxide
34
What salt does Hydrochloride acid Sulphuric acid Nitric acid Make?
Hydrochloric- chloride Sulphuric- sulphate Nitric- nitrate
35
An acid dissolved in water to produce what ions
Hydrogen ions H+
36
An alkali dissolved in water to produce what ions
An alkali dissolves in water to produce hydroxide OH- ions
37
What’s the symbol for ammonia
NH3 Naturally found as a gas
38
Name two ways the measure PH
Universal indicator Ph probe
39
What is neutralisation in terms of acids and alkali Explain in terms of ions
When an acid and alkali react they cancel eachother out to become neutral. The hydrogen ions react with hydroxide ions to produce water
40
What’s the definition of a strong acid
An acid that fully dissociates into ions when they dissolve in water You can’t reverse this change Example : hydrochloric acid , sulfuric acid and nitric acid
41
What’s the definition of a weak acid
Does not fully dissociate into ions Only some molecules dissociate while most stay in the solution Carbonic acid , citric acid , phosphoric acid
42
What is electrolysis
The breaking down of a molten or aqueous ionic compound using electricity
43
Where do non metals form and where do metals form in electrolysis
Non metals = anode Metals = cathode
44
Where are the positive and negative ions attracted to
Negative ions in electrolysis are attracted to the = cathode Positive ions in electrolysis are attracted to the = anode
45
During the electrolysis of molten lead bromide, what happens at the anode? What happens at the cathode?
Anode- negative bromide ions lose electrons to form bromine atoms Cathode- positive lead ions gain electrons to form lead ions
46
Metal ions are always..
Positive
47
In order to become a metal atom what must happen to a metal ion
The positive ion must gain electrons at the cathode
48
Why is aluminium useful? What are the uses?
It’s useful because it’s strong and light Saucepans Drink cans Aeroplanes Foil
49
What’s the most common aluminium ore
Bauxite
50
A brief over view of how aluminium is extracted
Bauxite is purified into aluminium oxide The aluminium oxide is extracted by electrolysis
51
Why is aluminium dissolved into cryolite for electrolysis
Electrolysis of Aluminium happens at a very high temperature. Cryolite has a lower temperature so it lowers the amount of heat needed for the process
52
The electrolysis of aluminium oxide produces oxygen and aluminium. Because of the high temperature what happens to the carbon anodes
The oxygen bubbles that form on the anode react with the carbon to create carbon dioxide

Chemistry Paper 1 (4 decks)

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