Final answer:
The oxidation state of a transition metal is calculated based on the known oxidation states of other elements in the compound and the overall charge. Transition metals show a variable range of oxidation states, losing their 4s electrons before 3d electrons. Patterns in oxidation states for the first transition series can also guide the determination.
Step-by-step explanation:
The oxidation state of a transition metal in a compound can be determined by considering the known oxidation states of other elements in the compound and the overall charge of the compound (if it is an ion). Transition metals can exhibit multiple oxidation states, and their chemistry is characterized by this variability. Unlike the main group elements, transition metals can lose both their s and d orbital electrons, with the 4s electrons being lost first, followed by the 3d electrons.
For example, if we examine the permanganate ion (MnO4−), we know that oxygen typically has an oxidation state of -2. Since there are four oxygen atoms, their total oxidation state would be -8. Considering the ion has a charge of -1, it means the manganese (Mn) must have an oxidation state of +7 to balance the total charge. These principles can be applied to determine the oxidation states of transition metals in other compounds as well.
Common Oxidation States of Transition Metals
The first transition series of metals shows a pattern in the range of their oxidation states. Starting with scandium, the number of oxidation states increases towards the middle of the series, with manganese showing some of the highest oxidation states, and then decreases as we move to the right of the series. These patterns help in predicting the possible oxidation states of transition metals in different compounds.