Write equations which represent the discharge at the cathode of the following ions: K^+, Pb^2+, Al^3+, and at the anode of: Br^-, O^2-, F^-.

At the cathode:

K = K^+ + 1 e^-1 (e^-1) signifies an electron

Pb = Pb^+2 + 2 e^-1

Al = Al^+3 + 3 e ^-1

At the cathode the metal ions are being oxidized through the loss of one or more electrons.

At the anode:

Br + 1 e^-1...

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At the cathode:

K = K^+ + 1 e^-1 (e^-1) signifies an electron

Pb = Pb^+2 + 2 e^-1

Al = Al^+3 + 3 e ^-1

At the cathode the metal ions are being oxidized through the loss of one or more electrons.

At the anode:

Br + 1 e^-1 = Br^-1

O + 2 e^-1 = O^-2

F + 1 e^-1 = F^-1

At the anode, the non-metal ions are being reduced by the gain of one or more electrons.

These are examples of half-cell reactions.  If you are doing an oxidation-reduction reaction the loss of electrons at one electrode has to equal the gain of electrons at the other electrode. The metals are reducing agents and the non-metals are oxidizing agents.

To remember this:  "an oxidizing agent is reduced by the gain of electrons"

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