How to name a complex containing com plex cationic and complex anionic species? How can you determine the oxidation number of the central metal ion?

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How to name a complex containing com plex cationic and complex anionic species? How can you determine the oxidation number of the central metal ion?

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How to name a complex containing com plex cationic and complex anionic...

Each element in a polyatomic ion (a complex compound) has a particular oxidation number, which can be calculated using the charge of the ion and particular oxidation number rules. The most important rule here is that the sum of the oxidation numbers of each atom in the polyatomic ion is equal to the charge of the ion.

For example, the oxidation number of oxygen is always -2 (except in peroxides such as H2O2 where it is -1, and when it is bonded to the more electronegative fluorine, in which case it has an oxidation number of +1) so in the CO3- (carbonate) anion the oxidation number of oxygen is -2 and there are three oxygen atoms, giving a charge of -6, and the overall charge of the anion is -1 therefore the oxidation number of carbon must be +5 (as -6 +5 = -1).

Another example would be the NH4+ cation; the oxidation number of hydrogen is always +1 (except in metal hydrides where it's oxidation number is -1), so in this cation the oxidation number of hydrogen is +1 and there are four hydrogen atoms giving a charge of +4, and the overall charge of the cation is +1 therefore the oxidation number of nitrogen must be -3.

Some other key rules to bear in mind when calculating oxidation numbers:

The oxidation number of any element in its standard state (uncombined) is zero.

The oxidation number of an atom in a monoatomic ion is equal to the charge of that ion.

The sum of oxidation numbers of all atoms in a neutral compound is zero.

The oxidation number of a group 1 metal is always +1, and the oxidation number of a group 2 metal is always +2.

The oxidation number of fluorine is always -1.

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