![]() (This is the reverse of the reactivity trend of the metals of groups 1 and 2. They don't react quickly with water or oxygen, which explains why they resist corrosion. Zinc is the most reactive in group 12, and mercury is the least reactive. Compared with the alkali metals in group 1 and the alkaline Earth metals in group 2, the transition metals are much less reactive. This behavior is in sharp contrast to that of the p-block elements, where the occurrence of two oxidation states separated by two electrons is common, which makes virtually all compounds of the p-block elements diamagnetic.ĭue to a small increase in successive ionization energies, most of the transition metals have multiple oxidation states separated by a single electron. Some properties of transition metals set them apart from other metals. The occurrence of multiple oxidation states separated by a single electron causes many, if not most, compounds of the transition metals to be paramagnetic, with one to five unpaired electrons. Because of the slow but steady increase in ionization potentials across a row, high oxidation states become progressively less stable for the elements on the right side of the d block. Manganese, for example, forms compounds in every oxidation state between −3 and 7. ![]() The relatively small increase in successive ionization energies causes most of the transition metals to exhibit multiple oxidation states separated by a single electron. Thus all the first-row transition metals except Sc form stable compounds that contain the 2 ion, and, due to the small difference between the second and third ionization energies for these elements, all except Zn also form stable compounds that contain the 3 ion. This in turn results in extensive horizontal similarities in chemistry, which are most noticeable for the first-row transition metals and for the lanthanides and actinides. The similarity in ionization energies and the relatively small increase in successive ionization energies lead to the formation of metal ions with the same charge for many of the transition metals. Trends in Transition Metal Oxidation States As a result, the metals in the lower right corner of the d block are so unreactive that they are often called the “noble metals.” ![]() The electronegativity of the elements increases, and the hydration energies of the metal cations decrease in magnitude from left to right and from top to bottom of the d block. \): Some Trends in Properties of the Transition Metals.
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