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Chemistry > C5 - Chemical Changes > Flashcards

C5 - Chemical Changes Flashcards

(54 cards)

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1
Q

The reactivity series (most reactive to least reactive)

A

Potassium, Sodium, (Lithium), Calcium, Magnesium, Aluminium, Carbon, Zinc, Iron, Tin, Lead, Hydrogen, Copper, Silver, Gold, Platinum

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2
Q

Mnemonic for Reactivity Series

A

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

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3
Q

Metals reaction with water

A

Metal + Water —> Metal Hydroxide + Hydrogen

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4
Q

Test for Hydrogen

A

Lit splint makes a squeaky pop

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5
Q

Metals reaction with Acid

A

Metal + Acid —> metal salt + hydrogen

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6
Q

Potassium, Sodium, Lithium, Calcium reaction with water

A

Fizzing, giving off hydrogen gas, leaving alkaline metal hydroxide solution

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7
Q

Potassium, Sodium, Lithium, Calcium reaction with (dilute) acid

A

Explosion

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8
Q

Magnesium, Aluminium, Zinc, Iron reaction with water

A

Very slow reaction

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9
Q

Magnesium, Aluminium, Zinc, Iron reaction with (dilute) acid

A

fizzing, giving off hydrogen gas, forming a salt

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10
Q

Tin and Lead reaction with water

A

Slight reaction with steam

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11
Q

Tin and Lead reaction with (dilute) acid

A

React slowly with warm acid

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12
Q

Copper, Silver, Gold reaction with water and acid

A

No reaction

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13
Q

Metals reaction with Oxygen

A

Metal + Oxygen —> Metal Oxide

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14
Q

What is metal’s reaction with oxygen called

A

Oxidation - gaining oxygen

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15
Q

What is a reduction reaction involving metal oxides

A

When metal oxides lose oxygen and return to their atomic form

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16
Q

What is the rule for displacement reactions

A

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

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17
Q

What is an ionic equation

A

An equation which shows only the atoms and ions that change in a reaction

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18
Q

what is Oxidation

A

The gain of oxygen and loss of electrons

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19
Q

What is reduction

A

The loss of oxygen and the gain of electrons

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20
Q

What is the mnemonic for oxidation and reduction in terms of electrons

A

OILRIG - Oxidation Is Loss Reduction Is Gain

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21
Q

Why are displacement reactions called RedOx reactions

A

REDuction and OXidation happen at the same time

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22
Q

What is an Ore

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A

A rock that contains enough metal to make it economical to extract the metal

23
Q

When and How do you extract metals with carbon

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A

You extract metals with carbon when the metal is less reactive than carbon. To extract with carbon you must heat the metal oxide with carbon and the carbon removed the metal from the metal oxide to form carbon dioxide

24
Q

Equation for extracting metal with carbon

Study These Flashcards
A

Metal oxide + Carbon —> Metal + Carbon dioxide

25
How are metals that are more reactive than carbon extracted
By electrolysis of the molten metal compound
26
What is a salt
A compound formed when the hydrogen in an acid is wholly or partially replaced by a metal or ammonium ions
27
Equation for formation of metal salts
Metal + Acid —> Metal salt + Hydrogen
28
Conditions for formation of metal salt
Metal must be above hydrogen in reactivity series. | Metal must not be high in reactivity series or reaction will be too vigorous
29
What kind of reaction is a metal and an acid
a REDOX reaction as both reduction and oxidation occurs
30
What happens during the reaction of metals and acids in terms of electrons
Metal atoms lose electrons and are oxidised. The hydrogen ions from the acid gain electrons and are reduced
31
What is a precipitate
An insoluble solid formed by a reaction taking place in a solution
32
What is an acid
A solution that contains hydrogen ions (H+)
33
What is a base
A substance that can neutralise an acid
34
What is an alkaline
A soluble base
35
Reaction of acid and a base
Acid + Base —> a Salt + Water | It is a neutralisation reaction.
36
What are types of bases
Metal oxides
37
What are salts made up of
Positive metal ions from a metal, base, or a carbonate A negative ion from an acid They have no overall charge as the sum of the charges of their ions equals zero
38
How to make a copper salt
1. Add insoluble copper oxide to sulphuric acid and stir. Warm gently on a tripod and gauze (do not boil) 2. The solution turns blue as the reaction occurs, showing that copper sulfate is being formed. Excess copper oxide can be seen. 3. When the reaction is complete (no more dissolving or fizzing), filter the solution to remove the excess copper oxide. 4. You can then evaporate the water so the crystals of copper sulfate start to form.
39
Reaction of an acid with an alkali
Acid + Alkali —> a salt + Water This is a neutralisation reaction
40
What happens with ions in a neutralisation reaction of acid with alkali
H+ ions from acid react with OH- ions from alkali to form water molecules
41
What happens when acids react with metal carbonates
Acid + a Carbonate —> a salt + water + carbon dioxide
42
How to make a Salt from a Metal Carbonate
1. Using a measuring cylinder, measure 20cm^3 of acid into beaker 2. Add half a spatula of metal carbonate into acid and stir with a glass rod 3. Continue adding metal carbonate in excess until no more dissolves and there is no more fizzing 4. Set up a filter funnel in a conical flask and filter the mixture and discard the unreacted metal carbonate 5. Pour the filtrate into a evaporating basin and either leave to evaporate at room temp or heat to evaporate water out of solution, leaving the salt
43
What happens to alkalises when added to water
They release OH- ions which make a solution alkaline when in excess
44
What happens to acids when added to water
They release H+ ions when added to water and these excess H+ ions make a solution acidic
45
What pH range is alkaline
8-14
46
what pH range is acidic
0-6
47
What colour does universal indicator turn in acidic solutions
Yellow-Orange-Red
48
What colour is universal indicator in neutral solutions
Green
49
What colour does universal indicator go in alkaline solutions
Blue - Purple
50
How is the pH of an acid related to the hydrogen ion concentration?
The greater the hydrogen ion concentration (as acids release H+ ions when dissolved in water), the lower the pH, the stronger the acid. If an acid is diluted by a factor of 10, the pH increases by one unit
51
Examples of strong acids
Hydrochloric acid Sulphuric Acid Nitric Acid
52
What happens to strong acids when dissolved in water
They completely dissociate - every molecule releases H+ ions which completely ionises the solution
53
What happens to weak acids when dissolved in water
They only partially dissociate - most of the molecules stay as they are and only a small number of molecules release H+ ions
54
Why is the reaction forming weak acids reversible
The molecules of the weak acid split to form H+ ions and negative ions, the ions recombine to form the original molecule again. A equilibrium is reached in which both whole molecules and their ions are present

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