Question

Using relative E values determine which of the following reactions are electrically possible.

Mg(s) + Br2(l) ——> MgBr2


This equation shows that Mg is : oxidized or reduced?

This equation shows that Br2 is : oxidized or reduced?

Can this redox reaction take place?

Answer 1

You should have given us a table, but I think my table shouldn't be too different.

Let's put oxidation numbers first.

`Mg^(0)(s)+Br_2^(0)(l) --> Mg^(+2)Br_2^(-2)(?)`

You would have to know that Mg(s) is a reducing agent and Br2(l) is an oxidizing agent. But it is pretty common knowledge that the halogens will tend to take the electrons and alkali and alkaline earth metals will tend to give up electrons.

Mg is oxidized because it gives up electrons; Br2(l) is reduced because it gains electrons. Since the reaction conforms to what we would expect to naturally (thermodynamically favored) occur, it can take place given that the activation energy is supplied.