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Chemistry > Electrolysis > Flashcards

Electrolysis Flashcards

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1
Q

In an electrolytic cell, how can you tell the nature of the electrolyte through the bulb?

A

When the switch is on, the electrolyte starts dissociating. Current remaining the same, the glow on the bulb indicates whether the electrolyte is a strong electrolyte - by bright glow of bulb, weak electrolyte - dim glow of bulb, non-electrolyte - when bulb doesn’t glow

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2
Q

Define electrolysis

A

Electrolysis is the decomposition of a chemical compound (electrolyte) in the fused or aqueous state by the passage of a direct electric current resulting in discharge of ions - as neutral atoms - at the respective electrodes

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3
Q

Which is the negative and positive electrode?

A

Cathode is the negative electrode

Anode is the positive electrode

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4
Q

Which reaction takes place at the cathode?

A

Cations gravitate to the cathode as it is the negative electrode, where they gain an electron to become a neutral atom - resulting in a reduction reaction

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5
Q

Which reaction takes place at the anode?

A

Anions gravitate to the anode as it is the positive electrode, where they lose an electron to become a neutral atom - resulting in an oxidation reaction

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6
Q

What type of reaction is electrolysis?

A

It involves a chemical change and is a redox reaction

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7
Q

Define electrolytes

A

Chemical compounds which conduct electricity in the fused or aqueous solution state & - undergo chemical decomposition due to the flow of current through them

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8
Q

What type of compounds are electrolytes?

A

Ionic compounds

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9
Q

What are the particles in electrolytes?

A

Ions only or Ions and molecules only

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10
Q

Give examples of electrolytes

A

Acids - dil. HCl, HNO3, H2SO4
Alkalis - KOH, NaOH solutions
Ionic salts - PbBr2 (molten), CuSO4 [aq.]

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11
Q

Define non-electrolytes

A

Chemical compounds which do not conduct electricity in the fused or aqueous soln. state & - do not undergo chemical decomposition due to the flow of current through them

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12
Q

What type of compounds are non-electrolytes?

A

Covalent compounds

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13
Q

What are the particles in non-electrolytes?

A

Molecules only

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14
Q

Give examples of non-electrolytes

A

Pure or distilled water, Alcohol, Kerosene, glucose, sucrose, sugar solution, Carbon disulphide (CS₂), liquid carbon tetrachloride (CCl₄)

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15
Q

Define strong electrolytes

A

They are electrolytes which allow a large amount of electricity to flow through them and hence are good conductors of electricity

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16
Q

How are strong electrolytes dissociated in fused or aq. soln. state?

A

They are almost completely dissociated in fused or aqueous solution state

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17
Q

Which particles are found in strong electrolytes?

A

Mainly ions only

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18
Q

What is the general prototype for examples of strong electrolytes?

A

Generally all strong acids and bases and most salts of strong acids

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19
Q

Give examples of strong electrolytes

A

Acids - dil. HCl, H2SO4, HNO3, HBr, HI,
Bases - NaOH, KOH, LiOH solns.
Salts - NaCl, Na2SO4, NaNO3, CuCl2 (Copper (II) Chloride), PbSO4 (Lead(II) sulfate), Pb(NO3)2 (Lead(II) nitrate), PbBr2 (Lead(II) bromide), AgI (Silver iodide) aq. solns.

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20
Q

Define weak electrolytes

A

They are electrolytes which allow small amounts of electricity to flow through them and hence are poor conductors of electricity

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21
Q

How are weak electrolytes dissociated in fused or aq. soln. state?

A

They are partially dissociated in fused or aqueous solution state

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22
Q

Which particles are found in weak electrolytes?

A

Ions and unionised molecules

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23
Q

What is the general prototype for examples of weak electrolytes?

A

Generally all weak acids and bases and most salts of weak acids

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24
Q

Give examples of weak electrolytes

A

Acids - Carbonic, acetic, oxalic, formic
Bases - NH4OH, Ca(OH)2, Mg(OH)2
Salts - Sodium - carbonate, bicarbonate, oxalate and formate aq. solns.

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25
Q

Define an electrolytic cell

A

The device in which electrolysis is carried out is called the electrolytic cell or voltameter which contains electrodes [cathode & anode] and the electrolytic solution

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26
Q

What are electrodes made of?

A

Metal or carbon

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27
Q

When are graphite (carbon) electrodes used?

A

When the products formed during electrolysis react with the metallic electrode

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28
Q

What is the anode?

A

It is the electrode connected to the positive terminal of the battery

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29
Q

Which ions migrate to the anode? Why?

A

Due to being connected to the positive terminal of the battery, anodes acquire a positive charge during electrolysis and hence, anions migrate to the anode

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30
Q

How do anions become neutral atoms at the anode?

A

The anions donate excess electrons to the anode and are oxidised to neutral atoms

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31
Q

What is the nature of anode?

A

It is the oxidising electrode

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32
Q

What is the cathode?

A

It is the electrode connected to the negative terminal of the battery

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33
Q

Which ions migrate to the cathode? Why?

A

Due to being connected to the negative terminal of the battery, the cathode acquires a negative charge during electrolysis. Hence, cations migrate to the cathode

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34
Q

How do cations become neutral atoms at the cathode?

A

The cations gain excess electrons and are reduced to neutral atoms

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35
Q

Which is the reducing electrode?

A

The cathode

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36
Q

By which electrode do electrons enter the electrolyte?

A

Cathode

37
Q

By which electrode do electrons leave the electrolyte?

A

Anode

38
Q

Define ions

A

They are atoms or groups of atoms which carry a positive or negative charge and become free and mobile when an electric current is passed through an aq. soln. of a chemical compound

39
Q

Differentiate between anions and cations in terms of loss or gain of electrons

A

Anions donate or lose electrons to the anode (oxidation process) and get oxidised to neutral atoms, whereas cations gain or accept electrons from the cathode (reduction process) and get reduced to neutral atoms.

40
Q

Write the formula which depicts oxidation

A

Cl^1- - 1e- -> Cl

41
Q

Write the formula which depicts reduction

A

Na^1+ + 1e- -> Na

42
Q

Who first explained the process of electrolysis

A

Swedish chemist Avante Arrhenius in 1887

43
Q

Give the postulates of Arrhenius’ theory

A
  1. An electrolyte on dissolving in water dissociates into free cations and anions and allows the flow of electric current through it
  2. The degree of dissociation is the extent to which an electrolyte dissociates into ions
  3. All ions carry an electric charge and are responsible for the flow of current through the solution
  4. The number of positive charges on the ions equals the number of negative charges and thus the solution is in electrolytic equilibrium
44
Q

What is the degree of dissociation?

A

It is the extent to which an electrolyte dissociates into ions

45
Q

What does the amount of electricity conducted by the electrolyte depend upon?

A

The concentration of ions in the solution

46
Q

What is electrolytic equilibrium?

A

The no. of positive charges on the ions equals the no. of negative charges and thus the solution is in electrolytic equilibrium

47
Q

Where is an equilibrium also established?

A

Between the ions produced and unionized molecules

48
Q

Which are the metallic ions?

A

Cations

49
Q

Which are the non-metallic ions?

A

Anions

50
Q

What does the preferential discharge of the ions depend on?

A

Its position in the electrochemical series

51
Q

What is the number of electrons gained by the anode equal to?

A

The no. of electrons donated by the cathode

52
Q

Where are the products of electrolysis formed?

A

At the anode and cathode itself

53
Q

Where does the exchange of electrons take place in electrolysis?

A

At the surface of the electrodes

54
Q

What is liberated at the cathode?

A

Hydrogen gas and metals - electropositive elements

55
Q

What is liberated at the anode?

A

Non-metals - electronegative elements

56
Q

Define electrolytic dissociation

A

The process due to which an ionic compound in the fused state or i aq. soln. state dissociates into ions by passage of electric current through it

57
Q

Differentiate between electrolytic dissociation and ionisation in terms of where they take place

A

Electrolytic dissociation takes place at in electrovalent compounds, whereas ionisation takes place in covalent compounds

58
Q

What does electrolytic dissociation involve?

A

It involves separation of ions of the ions which are already present in an ionic compound

59
Q

Give example of a compound in which electrolytic dissociation takes place

A

PbBr2 ⇌ Pb^2+ + 2Br^1-

60
Q

What does ionisation involve?

A

It involves formation of charged ions from the molecules which are not in the ionic state

61
Q

Give example of a compound in which ionisation takes place

A

HCl [aq.] ⇌ H^1+ + Cl^1-

62
Q

How does ionisation involve atoms changing into ions?

A

Mg -> Mg^2+ + 2e-

63
Q

When will sodium chloride conduct electricity?

A

Only in the fused or aqueous solution state

64
Q

Name a compound that is a non-electrolyte in the solid state, but conducts electricity in the molten or aqueous state

A

Sodium chloride

65
Q

What is essential for conducting electricity?

A

Free ions

66
Q

Why is an ionic compound in the solid state a bad conductor of electricity?

A

Ionic compounds contain positively charged metallic ions & negatively charged non-metallic ions. These ions are not free but held together by strong electrostatic force of attraction.

67
Q

How to make ionic compounds good conductors of electricity?

A

When an ionic compound is heated strongly, the ions gain KE and break lose and move freely. The molten soln. becomes a good conductor of electricity

68
Q

What does NaCl dissociate into, on being dissolved in water?

A

Sodium ion [Na+] and chloride ions [Cl-] which move freely in soln.

69
Q

Why does NaCl dissociate into ions on being dissolved in water?

A

The slightly negatively charged oxygen atoms of water exerts a pull on the positively charged sodium ion. A similar pull is exerted by the slightly positively charged hydrogen atoms of the water on the negatively charged chloride ions. Thus, Na and Cl ions become free in soln.

70
Q

Name the compounds which are non-electrolytes in the gaseous state but ionise in aq. soln. state

A

Polar covalent compounds - HCl, NH3

71
Q

In which states does HCl not conduct an electric current?

A

In the gaseous state and in the pure liquid state

72
Q

How is HCl polar covalent in nature?

A

It shows charge distribution in its molecules such that the hydrogen atom has a slight positive charge & chlorine atom a slight negative charge

73
Q

What happens when HCl is added to water?

A

Water being a polar solvent, the slightly negatively charged oxygen atom of the water exerts an electrostatic pull on positively charged hydrogen ion of HCl. Thus H+ ions combine with water forming hydronium ions [H3O+] and the residual chloride ions remain in solution

74
Q

Differentiate between metallic and electrolytic conduction in terms of transfer of matter

A

In electrolytic conduction, there is a transfer of ion. The flow of electricity decomposes the electrolyte and new products are formed. Whereas in metallic conduction, there is no transfer of matter. The flow of electricity only produces heat energy and no new products are formed

75
Q

Why is copper metal a non-electrolyte?

A

It is a good conductor of electricity, but it is a non-electrolyte because it does not undergo chemical decomposition due to the flow of electric current through it

76
Q

On what basis are acids, bases and salts classified into strong or weak electrolytes?

A

On the degree of dissociation

77
Q

Which acids ionise on dissolution in water?

A

Mineral acids

78
Q

What do mineral acids furnish in soln.?

A

H+ ions

79
Q

What do bases furnish in soln.?

A

Furnish OH- ions in soln.

80
Q

What do ionic salts furnish in soln.?

A

Furnish positive ions other than H+ ions and negative ions other than OH- ions

81
Q

Name some strong alkalis

A

Hydrochloric acid, Nitric acid, Sulphuric acid

82
Q

Name some strong bases

A

Potassium hydroxide, Sodium hydroxide, Lithium Hydroxide

83
Q

Name some strong salts

A

Lead Bromide, Copper Chloride, Silver Nitrate

84
Q

Name some weak salts

A

Sodium carbonate, Potassium bicarbonate, Lead acetate

85
Q

Give another name for the electrochemical series

A

Metal activity series

86
Q

Define the electrochemical series

A

Depending on the ease with which the metals lose their electrons and form ions, they are arranged in a series known as electrochemical series

87
Q

Which metals ionize most readily?

A

The ones that are discharged with great difficulty

88
Q

Where are the metals which ionize most readily placed in the electrochemical series?

A

At the top of the series

Chemistry (4 decks)

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