Although there are significant similarities between the two series of f-block elements, there are also significant differences. All f-block metals are strong reducing agents, and chemical reactions with acids result in the release of hydrogen ions.Īs a result, they absorb hydrogen ions from low pH scale solutions, resulting in the formation of interstitial hydrides. As a result, their redox reaction potential is comparable to that of alkaline earth metals. Lanthanides, for example, are f-block chemical elements that behave as active metals. By separating those two periods, elements in the remainder of the table align with other elements with similar properties. They were removed in order for the entire table to fit together more cohesively. If these elements could fit inside the table, they would be in the transition metal section of the Periodic Table, between groups 2 and 3. Because of the space on the Periodic Table from which they are removed, the F-Block elements are often referred to as “inner transition metals.” The F-Block elements are traditionally found on the Periodic Table in two separate horizontal rows that are disjointed and located at the bottom of the table. The final electron in the actinide series enters the 5f orbital. In general, these elements are radioactive in nature. Actinide series: The actinide series consists of elements with atomic numbers ranging from 89 to 103.The last electron in the lanthanide series enters the 4f orbital. These are non-radioactive elements (except for promethium). Lanthanide series: The lanthanides are the first series of elements, which include elements with atomic numbers ranging from 57 to 71.The two series of f-block elements or inner transition elements are lanthanides and actinides. Classification of the Elements of f-Block Each series contains 14 elements that fill the ‘f’ orbital. The elements are divided into two groups: the 4f series of Ce to Lu and the 5f series of Th to Lw. In the f-block, there are primarily two series that correspond to the filling of 4f and 5f orbitals. These elements have the electrons (1 to 14) in the f orbital and (0 to 1) in the penultimate energy level’s d orbital, and (0 to 1) in the outermost orbital. The elements in which the last electron enters any of the seven f-orbitals of their respective ante-penultimate shells are referred to as F-Block elements. All f-block elements have a trivalent oxidation number or state, which is a stable or common oxidation state. In chemistry, the first inner transition metals series is made up of 4f-block elements or lanthanides, while the second inner transition metals series is made up of actinides.įilling electrons in deep-seated 4f and 5f orbitals with increasing atomic number has resulted in the electronic configuration of the f-block chemical elements (lanthanum and actinium). In the periodic table, f block elements appear in two chemical series, such as 4f block names as lanthanides or rare earth elements and 5f block names as actinides or actinides.
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