Final answer:
Transition metals, found in the middle of the periodic table, are known for having multiple oxidation states. This variability is due to the loss of d-orbital electrons, with elements in the second and third transition series generally more stable in higher oxidation states.
Step-by-step explanation:
Atoms that have multiple oxidation states are usually found among the transition metals on the periodic table. These elements are known for their ability to lose electrons from both their 4s and 3d subshells, leading to a range of possible oxidation states. While the alkali and alkaline earth metals typically exhibit oxidation states of +1 and +2 respectively, owing to the loss of their s-electrons, transition metals can exhibit a variety of oxidation numbers. This phenomenon is primarily due to their d-orbital electrons which can be removed in various combinations leading to different charge states.
For instance, transition metals in the second and third series are generally more stable in higher oxidation states compared to those in the first series, as evidenced by elements such as molybdenum and tungsten which typically show a 6+ state in aqueous solution. Furthermore, factors such as an increase in atomic radius down a group make it easier to remove electrons from orbitals that are further from the nucleus. This is why ions of the second and third series are commonly found in higher oxidation states than their first series counterparts.