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Chemistry > Unit 4- Chemical Changes > Flashcards

Unit 4- Chemical Changes Flashcards

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1
Q

What does OILRIG stand for

A

oxidation is loss, reduction is gain

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2
Q

Oxidation and reduction always occur ?

A

Together👫👫👫💏

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3
Q

When metals react with oxygen, what do they form?

A

Metal oxides

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4
Q

When metals react, their atoms lose electrons to form ?

A

To form positive metal ions

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5
Q

Some metals lose electrons more easily thsn others.

The more easily a metal loses electrons, ?

A

The more reactive the metal is

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6
Q

The reaction of metals with acid and water can be used to show the reactivity series.
What is the anomaly for it?

A 
Please- potassium
Send- sodium
Charlies- calcium
Monkeys- magnesium 
And- aluminium 
Crazy- carbon
Zebras- zinc
In-iron
Cages-copper
Securely -silver
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7
Q

Metals react with acids to produce ?

A

Salts and hydrogen

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8
Q

What are 3 very reactive metals

A

Lithium
Sodium
Potassium

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9
Q

Where do unreactive metals such as gold are found where?

A

On the earth surface

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10
Q

What does PANIC stand for?

A 
Positive
Anode
Negative
Is 
Cathode
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11
Q

Metals that are more reactive than carbon are extracted from molten compounds by what?

A

Electrolysis

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12
Q

Metals that are les reactive than carbon can be extracted from their oxides by?

A

Heating with carbon

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13
Q

In a displacement reaction a more reactive metal will ?

A

Displace a less reactive metal from a solution of its salt

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14
Q

When substances dissolve in water, they ?

A

Dissociate into their individual ions:

  1. Hydroxide ions OH-(aq), make solutions alkaline
  2. Hydrogen ions H+(aq), make solutions acidic
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15
Q

1-6 on the pH scale are?

A

Acidic

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16
Q

8-14 ?

A

Alkaline

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17
Q

7?

A

Neutral

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18
Q

How can the pH of a solution be measured?

A

pH probe or universal indicator

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19
Q

What are indicators

A

Dyes that change colour depending on whether the are alkaline or acidic solutions

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20
Q

Red=?

A

Acidic

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21
Q

Green=?

A

Neutral

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22
Q

Purple?

A

Alkaline

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23
Q

Soluble bases are called ?

A

Alkalines

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24
Q

How are acids neutralised?

A

Bases

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25
Q

Acid + hydroxide —>? + ?

A

Acid + hydroxide–> salt + water

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26
Q

Is this neutralisation?why

H+(aq) + OH-(aq)—>H2O(I)

A

Yes because an acid has reacted with a alkaline and has produced water which is neutral

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27
Q

Acids can also be neutralised by?

A

Metal carbonates

Metal oxides

28
Q

Acid + metal oxide —->? + ?

A

Salt + water

29
Q

Acid + metal carbonate —> ? + ? + ?

A

Salt + water + carbon dioxide

30
Q

A salt is produced when the hydrogen is replaced by a ?

A

Metal ion

31
Q

Name the salts produced by?
Hydrochloric acid
Nitric acid
Sulphuric acid

A

Hydrochloric acid-chloride salts
Nitric acid-nitrate salts
Sulphuric acid-sulphate salts

32
Q

See the practical on preparing a pure dry sample of a soluble salt from an insoluble oxide or carbonate

A

✅

33
Q

Strong acids are completely ….. in water💧

A

Ionised (split up into ions) in water

34
Q

Name 3 types of strong acids

A

Hydrochloric acid
Nitric acid
Sulphuric acid

35
Q

Name 3 weak acids

A

Ethanoic acid
Citric acid
Carbonic ackd

36
Q

Weak acids are only …. in water?

A

Partially ionised in water

37
Q

The pH of a solution is a measure of the concentration of what ions?

A

H+ ions

38
Q

A pH decrease of 1 unit indicates ?

A

That the concentration of hydrogen ions has increased by a factor of 10

39
Q

The larger the hydrogen ion concentration, the lower the ?

A

pH

40
Q

In oxidation reactions, a substance ?

A

Often gains oxygen

41
Q

In reduction reactions, a substance often ?

A

Loses oxygen

42
Q

Oxidation and reduction always occur?

A

Together 🙏🏼🤝👫

43
Q

What is electrolysis?

A

When electricity is used to break down compounds containing ions into their constituent elements

44
Q

What is the substance being broken down electrolysis called

A

An electrolyte

45
Q

Where is the electric charge carried by ?

They must be free to ?

A

Carried by ions

Must be free to move

46
Q

Why cant a solid be used during electrolysis

A

the ions are fixed

47
Q

What are the electrodes purposes in electrolysis

What are they usually

A

They are usually solid carbon rods which conduct electricity

48
Q

The electrode attached to the positive terminal is called a what?

A

Anode

49
Q

The electrode attached to the negative terminal is called a what?

A

Cathode

50
Q

PANIC! = what

A

Positive anode

Negative cathode

51
Q

Electrical current in electrolysis has to be AC or DC?

A

DC

52
Q

Ions during electrolysis move towards the ? ? Electrode

A

oppositely charged electrode

53
Q

Positive ions during electrolysis move to the ?

A

Cathode

54
Q

Negative ions during electrolysis move to the ?

A

Anode

55
Q

If a metal is formed, it will always be at the ?

A

CATHODE

56
Q

When ionic compounds are dissolved in water to form aqueous solutions. What is also present which complicates it🙄

A

Hydrogen and hydroxide

57
Q

At the positive+ electrode during electrolysis in an aqueous solution, if a HALOGEN is available it will be formed, otherwise ? is broken down to release ?

A

Hydroxide ions break down to release O2 gas

58
Q

At the cathode during electrolysis in an aqueous solution, the least reactive substance is discharged. The ions that are not discharged remain where?

A

In the solution

59
Q

See required electrolysis practical in an aqueous solution

A

✅

60
Q

Reduction occurs when positively charged ions gain electrons where?

A

At the cathode

61
Q

Oxidation occurs when negatively charged ions lose electrons at the ?

A

Anode

62
Q

In a redox reaction both ? Occur

A

Both reduction and oxidation occurs

63
Q

What can be used to show reactions that take place at the electrodes during electrolysis

A

Half-equations

64
Q

In the electrolysis of molten copper chloride-
copper is deposited on the cathode.

Show this in an equation for both copper and chlorine

A

Cu2+ + 2e- ➡️ Cu ( copper ions gain electrons so are reduced)

2Cl-➡️ Cl2 + 2e- ( the chlorine ion lose electrons so they are oxidised)

65
Q

Metals that are more reactive than carbon can be extracted from their ores using ?

This can be ?

A

Electrolysis

Expensive because of the amount of current and heat needed

66
Q

Explain the electrolysis of aluminium oxide
4 steps!
🌡 - + ❌

A
  1. First aluminium oxide is mixed with cryolite, thus lowering the melting point and meaning less energy is needed
  2. Aluminium is formed at the cathode
  3. Oxygen gas forms at the anode and reacts with carbon to form carbon dioxide
  4. This wears away the anode, which is replaced regularly
67
Q

What is the half equation of aluminium oxide

A

Cathode-
Al3+ + 3e- ➡️ Al

Anode-
2O2-➡️ O2 + 4e-

Chemistry (7 decks)

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