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Chemistry paper 1 > C4: Chemical Changes > Flashcards

C4: Chemical Changes Flashcards

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1
Q

What is the order of the reactivity series?

A

Potassium (K)
Sodium (Na)
Calcium (Ca)
Magnesium (Mg)
Aluminium (Al)
Carbon (C)
Zinc (Zn)
Iron (Fe)
Tin (Sn)
Lead (Pb)
Hydrogen (H)
Copper (Cu)
Silver (Ag)
Gold (Au)
Platinum (Pt)

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2
Q

What is a displacement reaction?

A

When a more reactive metal displaces a less reactive metal from a compound

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3
Q

What is smelting?

A

When displacement reactions are used to obtain metals from their ores by displacing with a more reactive, less valuable metal or carbon.
This happens in a blast furnace where the iron oxide is ‘reduced’ to produce iron

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4
Q

What does OIL RIG stand for?

A

Oxidation
Is
Loss (of electrons)

Reduction
Is
Gain (of electrons

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5
Q

Which pH numbers are acids?

A

pH<7

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6
Q

Which pH numbers are alkalis?

A

pH>7

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7
Q

Which pH is neutral?

A

pH = 7

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8
Q

What happens when an acid and an alkali are reacted completely with each other?

A

A salt and water are produced

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9
Q

What happens when sulphuric acid reacts with an alkali?

A

A metal sulphate salt is formed

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10
Q

What happens when nitric acid reacts with an alkali?

A

A metal nitrate salt is formed

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11
Q

What happens when the salt is left in solution?

A

We have a mixture of dissociated ions

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12
Q

How do we obtain solid crystals of a dissolved salt?

A

By heating gently so the water evaporates, leaving only the salt behind

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13
Q

What can we use to measure pH?

A

Universal indicator

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14
Q

How much is a change in concentration of 1pH?

A

10x change in concentration of H+ or OH- ions

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15
Q

What makes something acidic?

A

It’s H+ ions

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16
Q

What makes something alkaline?

A

It’s OH- ions

17
Q

What happens to a strong acid in a solution?

A

It dissociates completely

18
Q

What happens to weak acids in a solution?

A

They only partially dissociate

19
Q

What are 3 examples of weak acids?

A

-Hydrochloric
-Sulphuric
-Nitric

20
Q

What are 3 examples of weak acids?

A

-Ethanoic
-Citric
-Carbonic

21
Q

What does the pH of an acid depend on?

A

The strength and concentration of the acid

22
Q

What are the steps to the titration practical?

A

-Use a burette to measure what volume of acid/alkali is needed to neutralise
-Measure e.g. 50cm^3 of alkali of known concentration using a glass pipette, put in a conical flask with methyl orange indicator
-Put acid in burette (up to 0cm^3 mark), open tap and let it drip into flask
-Once it goes pink, stop, swirl. If it stays pink, neutralisation has occurred
-(Rough titration can be done before to give more accurate value)
-Use moles to calculate unknown concentration

23
Q

What does electrolysis involve?

A

Passing an electrical current through a substance to cause oxidation and reduction at the two electrodes: the anode (+) and cathode (-)

24
Q

What state do ionic compounds need to be in for electrolysis to take place?

A

Molten or in a solution so the ions are free to move

25
Q

What can electrolysis be used for ?

A

To obtain pure metals from a metal compound

26
Q

Which electrode are the positive ions (cations) attracted to?

A

The negative cathode

27
Q

What happens to the cations at the electrode?

A

They are reduced (gain electrons)

28
Q

Which electrode are the negative ions (anions) attracted to?

A

The positive anode

29
Q

What happens to the anions at the electrode?

A

They are oxidised (lose electrons)

30
Q

Why is cryolite added to the aluminium oxide in certain cases?

A

To lower the melting point - cheaper

31
Q

When a graphite anode is used, why might it need to be replaced regularly?

A

The oxygen reacts with the carbon to produce CO2

32
Q

What is in an electrolysis solution?

A

Na+, H+, Cl-, OH-

33
Q

In a solution, which ion is attracted to the cathode?

A

The less reactive one

34
Q

In a solution, what is oxidised at the anode?

A

If a halide ion is present, then that halide ion will be oxidised
If there is no halide, then the oxygen will be oxidised

Chemistry paper 1 (5 decks)

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