1 9 electrolysis

Most covalent compounds do not conduct electricity because they have no freely moving charged particles (ions or electrons) to carry the current.

Solid ionic compounds cannot conduct electricity because the ions are in fixed positions and are unable to move.

The positive and negative electrodes are called:

True. Molten ionic compounds can conduct electricity.

During electrolysis, cations (positive ions) move towards the negative electrode / cathode.

An insulator is a material that does not conduct electricity well.

Ionic compounds can conduct electricity in the molten state or in solution because the ions can move and carry charge.

True. Cations are positive and anions are negative.

An anion is a negatively charged ion.

During electrolysis, anions (negative ions) move towards the positive electrode / anode.

False. In electrochemistry, electrons move from the anode to the cathode.

Inert electrodes,such as graphite or platinum, are used in electrolysis experiments to avoid side reactions with the electrolyte.

In terms of ions, the electrolysis of molten ionic compounds has two ions, while electrolysis of aqueous ionic compounds has four ions.

During the electrolysis of a molten ionic compound, the non-metal is always produced at the anode (positive electrode).

False. The metal is always produced at the cathode during the electrolysis of a molten ionic compound.

The ions present during electrolysis of a molten ionic compound are:

When an ionic compound is heated beyond its melting point, the ions can move freely and conduct electricity.

The ions present during electrolysis of an aqueous ionic compound are:

During the electrolysis of aqueous solutions, hydrogen ions (H⁺) and metal ions are attracted to the negative electrode (cathode).

True. Inverted test tubes can be used to collect gaseous products during the electrolysis of aqueous solutions.

During the electrolysis of aqueous solutions, hydroxide ions (OH⁻) and non-metal ions are attracted to the positive electrode (anode).

False. If the metal is above hydrogen in the reactivity series, hydrogen will be produced at the cathode during the electrolysis of aqueous solutions.

In terms of electron transfer, oxidation is the process where a substance loses electrons.

Reduction is the process where a substance gains electrons.

At the anode, negatively charged ions lose electrons and are oxidised.

At the cathode, positively charged ions gain electrons and are reduced.

Tthe half equation for the reduction of Pb2+ ions is: Pb2+ + 2e- → Pb

Tthe ionic equation for the oxidation of Br– is: 2Br- → Br2 + 2e-

The half-equation for the reduction of H+ is: 2H+ + 2e- → H2

Chlorine gas is produced at the positive electrode during the electrolysis of aqueous sodium chloride.

Oxygen gas is produced at the positive electrode during the electrolysis of aqueous copper(II) sulfate.

The half-equation for the oxidation of Cl- during the electrolysis of aqueous sodium chloride is: 2Cl- → Cl2 + 2e-

The half-equation for the reduction of Cu2+ during the electrolysis of aqueous copper(II) sulfate is: Cu2+ + 2e- → Cu

During the electrolysis of dilute sulfuric acid, oxygen gas is produced at the positive electrode.

True. In electrochemistry, oxidation and reduction refer to the loss or gain of electrons rather than the addition or removal of oxygen