Electrolysis chemistry flash cards

Why must an ionic compound be molten or dissolved for electrolysis?

its ions must be free to move and carry charge

What happens to positive ions during electrolysis?

they move to the cathode and gain electrons.

What happens to negative ions during electrolysis?

They move to the anode and lose electrons

What is produced when molten lead bromide is electrolysed?

Lead at the cathode bromine at the anode (lead and bromine gas)

What is the cathode product in the molten ionic compounds?

The metal, formed when positive metal ions gain electrons.

What is the anode product in molten ionic compounds?

The non-metal, formed when negative ions lose electrons

What extra ions are present in an aqueous solution?

Hydrogen ions and hydroxide ions from water, as well as the compounds ions.

How is the metal product chosen in aqueous electrolysis

If the metal is less reactive than hydrogen, the metal forms; otherwise, hydrogen forms.

What forms at the anode if a concentrated halide solution is electrolysed?

The halogen, such as chlorine, bromine or iodine

What usually forms at the anode if no halide is discharged?

oxygen from hydroxide ions

What are the Cathode and Anode products of aqueous copper chloride?

Copper at the cathode; chlorine at the anode(if concentrated)

What are the cathode and anode products of aqueous sodium chloride?

Hydrogen at the Cathode(sodium is too reactive) (more than hydrogen); chlorine at the anode(if concentrated) otherwise oxygen may form.

What is reduction at the cathode?

Gain of electrons

What is oxidation at the anode?

Loss of electrons

Why is aluminium extracted by electrolysis rather than carbon reduction?

Aluminium is more reactive than carbon