3 2 electrolytic processes

True. Molten ionic compounds can conduct electricity.

The electrolyte is the  ionic compound in molten or dissolved solution that conducts the electricity.

The anode is the positive electrode.

The cathode is the negative electrode.

Electrons flow from the anode to the cathode.

Positive cations are attracted to the negatively charged cathode because opposite charges attract.

Negative anions are attracted to the positively charged anode because opposite charges attract.

False. The electrolyte must be molten or in solution to undergo electrolysis.

Electrolysis is the process of using an electric current to decompose or break down a molten or aqueous ionic compound.

Aqueous solutions always have H+ and OH- ions present from the splitting of water molecules.

Negatively charged OH- ions and non-metal ions are attracted to the positive electrode.

True. If halide ions are present in the aqueous electrolyte, they are discharged at the anode.

If no halide ions are present, OH- is discharged at the anode, forming oxygen gas.

H+ ions and metal ions are attracted to the negative electrode.

The product at the cathode is determined by the position of the metal in the reactivity series relative to hydrogen.

True. Copper is produced at the cathode during electrolysis of copper chloride solution.

Hydrogen gas is produced at the cathode during electrolysis of sodium chloride solution.

The products of electrolysis of sodium sulfate solution are hydrogen at the cathode and oxygen at the anode.

The products of electrolysis of acidified water are hydrogen at the cathode and oxygen at the anode.

Molten lead is produced at the cathode during electrolysis of molten lead(II) bromide.

Brown fumes of bromine gas are produced at the anode during electrolysis of molten lead(II) bromide.

The products of electrolysis of molten zinc chloride would be zinc at the cathode and chlorine at the anode.

Graphite or platinum electrodes are typically used in the electrolysis of molten compounds.

Molten ionic compounds conduct electricity because their ions can move freely and carry the current.

Two chloride ions are attracted to the anode where they each lose one electron. They bond to form a molecule of chlorine. 2Cl- ⟶ Cl2 + 2e-

True. The positive ion will migrate towards the cathode and the negative ion will migrate towards the anode.

False. The cathode product will always be the metal l and the product formed at the anode will always be the non-metal.

Oxidation is when a substance loses electrons.

Reduction is when a substance gains electrons.

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

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

A half equation is an equation that describes the movement of electrons at each electrode during electrolysis.

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

The half equation for the oxidation of Br- ions at the anode is: 2Br- → Br2 + 2e-

True. In half equations, the charges on each side of the equation should always balance.

The half equation for the reduction of hydrogen ions at the cathode in aqueous solutions is: 2H+ + 2e- → H2

The balanced half equation for the oxidation of water molecules at the anode in acidic solutions is: 2H2O → O2 + 4H+ + 4e-