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GCSE CHEMISTRY REVISION > Electrolysis, Obtaining Metals and Equilibrium + THE PERIODIC TABLE > Flashcards

Electrolysis, Obtaining Metals and Equilibrium + THE PERIODIC TABLE Flashcards

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1
Q

What is an electrolyte?

A

An ionic compound that is a liquid that conducts electricity.

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2
Q

What is electrolysis?

A

Electrolysis is the process that splits ionic compounds into the elements they are made up of. Electrolysis happens using a solution that conducts electricity.

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3
Q

Which Ions go to which electrodes?

A

Positively charged ions (CATions) go to the CAThode, which is negatively charged.
Negatively charged ions (ANions) go to the ANode, which is positively charged.

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4
Q

What is an Ionic compound?

A

A bond between a metal and a non metal.

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5
Q

What is a metallic compound?

A

A bond between two metals.

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6
Q

What is a covalent compound?

A

A bond between two non metals.

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7
Q

What does Molten Lead Bromide produce during electrolysis? Observations? Electrode material?

A

Using graphite electrodes, Molten Lead bromide produces lead at the cathode and bromine at the anode.
Lead is observed as a shiny metal around the cathode. Bromine is observed as a brown gas.

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8
Q

What goes to the cathode and what goes to the anode?

A

Metals always form at the CATHODE unless they are more reactive than hydrogen. If they are more reactive, hydrogen forms instead.

Oxygen always forms at the ANODE, unless halide ions (chloride/bromide/iodide) are present. If they are present, they lose electrons and form their corresponding halogen. (Chlorine/Bromine/Iodine)

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9
Q

What is the difference between empirical formula and molecular formula?

A

Empirical formula shows the simplest ratio of elements in a compound. The molecular formula states the number of atoms in each element of the compound.

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10
Q

What does Sodium sulphate produce during electrolysis? Observations? What material are the electrodes?

A

Using graphite electrodes, Sodium sulphate produces Hydrogen at the cathode and oxygen at the anode. Hydrogen’s presence can be detected by using a lit splint. A squeaky pop should be heard. Oxygen can be detected with a glowing splint, which will relight if it is present.

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11
Q

What does Concentrated aqueous sodium chloride produce during electrolysis? Observations? What material are the electrodes?

A

The electrodes must be inert graphite or platinum. Concentrated aqueous sodium chloride produces Hydrogen gas at the cathode and Chlorine at the anode. Hydrogen can be detected with the squeaky pop test and Chlorine can be detected by its smell. Chlorine also bleaches litmus paper.

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12
Q

What does Copper chloride solution produce during electrolysis? Observations? What material are the electrodes?

A

Using graphite electrodes, Copper Chloride solution produces Copper at the cathode and Chlorine at the anode. Chlorine can be detected via its strong smell.

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13
Q

What does Dilute sulphuric acid produce during electrolysis? Observations? What material are the electrodes?

A

Using graphite electrodes, Dilute sulphuric acid produces Hydrogen at the cathode (From the acid) and Oxygen at the anode (from the water)

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14
Q

What happens to the ions when an ionic compound is melted/dissolved in water?

A

The ions become free to move around.

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15
Q

How are products of electrolysis generated?

A

When ions reach the electrodes, they gain or lose electrons so they become atoms of elements. As a result, a product forms around the electrode.

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15
Q

How are products of electrolysis generated?

A

When ions reach the electrodes, they gain or lose electrons so they become atoms of elements. As a result, a product forms around the electrode.

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16
Q

What ion does a metal form?

A

Metals tend to LOSE electrons and become CATIONS

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17
Q

What ion does a non metal form?

A

Non metals tend to GAIN electrons and become ANIONS

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18
Q

What is the difference between molten and aqueous?

A

Molten is when something is melted to make a liquid.
Aqueous is when something is dissolved in water to form a solution.

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19
Q

what does OAARAC stand for?

A

Oxidation at Anode, Reduction at Cathode

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20
Q

What is the difference between products of a reaction between metal and steam and a reaction between metal and water?

A

Reaction with steam produces metal oxide and hydrogen. Reaction with water produces metal hydroxide and hydrogen.

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21
Q

What is a displacement reaction

A

A reaction that happens when a more reactive metal replaces a less reactive metal FROM A COMPOUND. This is because the more reactive metal loses electrons more easily.

22
Q

What products form when (most) metals react with a dilute acid?

A

Salt and Hydrogen Gas

23
Q

What metals react with dilute acid but not cold water?

A

Magnesium, Aluminium, Zinc, Iron, Lead

24
Q

How are metals that are less reactive than carbon extracted from oxides?

A

By reacting with carbon and being displaced. This is done because carbon is cheap and abundant. It is normally done by heating metal oxide with carbon as coal

25
Q

What is Phytomining?

A

When plants grow on contaminated land, they absorb copper ions. They can then be harvested and burned to produce ash with high concentrations of copper compounds.

26
Q

What is Bioleaching?

A

Mixing Bacteria with low grade ores causes bacteria to convert copper into leachate solution which is rich in copper compounds. This is a very slow process.

27
Q

What are metals that do not react with cold water or dilute acid?

A

Silver, Gold, Copper, Platinum

28
Q

What does an Acid Produce?

A

Hydrogen (H+) ions

29
Q

What does an Alkali produce?

A

Hydroxide (OH-) ions

30
Q

What happens in a Redox reaction?

A

One ion is oxidised and the other is reduced. (There can be a spectator ion)

31
Q

What is the Haber process?

A

A reversible reaction where Hydrogen and Nitrogen form Ammonia.

32
Q

What is a closed system?

A

A reaction where neither products or reactants can be added or removed.

33
Q

What is dynamic equilibrium?

A

When the rate of the forwards reaction equals the rate of the backwards reaction. It’s dynamic because both forward and backward reactions are still taking place. Concentrations of reactants and products remain constant.

34
Q

What is Le Chatelier’s principle?

A

The concept that if any conditions of a reversible reaction at equilibrium are changed, the system will change to counteract this change.

35
Q

What happens if temperature changes in equilibrium?

A

The system will react to try to maintain equilibrium. If the temperature increases, the endothermic reaction’s products will increase and the exothermic will decrease. If the temperature decreases, the exothermic reaction’s products will increase and the endothermic will decrease.

36
Q

What happens if pressure changes in equilibrium?

A

If pressure increases, the equilibrium will shift to minimise gas production. If pressure decreases, the equilibrium will shift to maximise gas production.

37
Q

What are group 1 metals called?

A

Alkali metals

38
Q

What happens when alkali metals react with chlorine?

A

A metal chloride is produced and dissolves in water to give a colourless solution

39
Q

What happens when alkali metals react with Water?

A

Metal floats, melts to create metal hydroxide.

40
Q

What happens when alkali metals react with Oxygen?

A

They go dull as metal oxide is produced

41
Q

What colours do potassium, sodium and lithium burn?

A

Lilac flame, orange/yellow flame, red flame

42
Q

How does potassium react with water?

A

Quickly reacts, produced hydrogen and metal both ignite and spark and burn with lilac flame.

43
Q

How does sodium react with water?

A

Fizzes rapidly and forms a ball on the water’s surface

44
Q

How does Lithium react with water?

A

Fizzes steadily and floats, gets smaller before eventually disappearing

45
Q

Why are Halogens very reactive?

A

They have 7 outer shell electrons and easily accept an electron.

46
Q

What do halogens do in their elemental form?

A

They form diatomic atoms by sharing electrons

47
Q

When are salts formed?

A

When a metal atom transfers its outer electron to a non metal atom.

48
Q

What happens to the halogens as you go down the group?

A

They become less reactive because the outer shell gets further from the nucleus, and therefore the attraction to the electron that would be gained becomes weaker.

49
Q

How do you test for chlorine

A

by inserting damp litmus paper into a test tube with gas in it. If the litmus paper bleaches from red to white, chlorine is present.

50
Q

How do you test for hydrogen?

A

Squeaky pop test with a lit splint

51
Q

How do you test for CO2?

A

Bubble through limewater and it will turn from clear to cloudy.

52
Q

What happens when halogens and hydrogen react?

A

They form Hydrogen halides which are acidic because they produce H+ ions.

GCSE CHEMISTRY REVISION (3 decks)

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