What is the oxidation state Cl of a perchlorate ion, Cl{O_4}^{ - 1} ?

To find the oxidation state of chlorine (Cl) in the perchlorate ion (ClO4-), we can use the fact that the sum of the oxidation states in a molecule or ion equals its overall charge.

The perchlorate ion (ClO4-) has a charge of -1.

Let's denote the oxidation state of chlorine as x.

The oxidation state of oxygen is usually -2, and there are 4 oxygen atoms in perchlorate, so their total oxidation state contribution is -2 * 4 = -8.

The overall charge of the perchlorate ion is -1.

We can set up an equation to find the oxidation state of chlorine:

x + (-8) = -1

Now, solve for x:

x - 8 = -1
x = -1 + 8
x = +7

Therefore, the oxidation state of chlorine (Cl) in the perchlorate ion (ClO4-) is +7.