THE TRANSITION AND THE INNER TRANSITION ELEMENTS

Metals, nonmetals, and metalloids comprise the periodic table of elements. Metals are chemical elements that exhibit metallic qualities such as malleability, excellent electrical conductivity, and the ability to quickly remove electrons. Transition metals and inner transition metals are also metallic elements with similar electron configurations. The majority of the d block elements are classified as transition metals. The elements of the F block are classified as inner transition metals. The primary distinction between transition metals and inner transition metals is that transition metal atoms have their valence electrons in the outermost d orbital, whereas inner transition metal atoms have them in the inner penultimate f orbital.

What Is the Distinction Between Transition and Inner Transition Metals?

The periodic table elements are arranged ascendingly according to how electrons are filled into atomic energy levels and their subshells. The properties of these elements are inversely proportional to their electron configuration. As a result, regions of similar items can be discovered and blocked for convenience. The periodic table’s first two columns comprise elements in which the final electron is filled into an’s’ subshell, hence the term’s-block’. The final six columns of an expanded periodic table comprise elements with a final electron filled into a ‘p’ subshell, hence the term ‘p-block’. Similarly, columns 3–12 contain atoms in which the last electron is filled into a ‘d’ subshell, referred to as the ‘d-block.’ Finally, the extra element set that is frequently written as two distinct rows at the bottom of the periodic table or is occasionally written as an extension between columns 2 and 3 is referred to as the ‘f-block’ due to the fact that its final electron is filled into a ‘f’ subshell. The elements classified as ‘d-block’ are also referred to as ‘Transition Metals’, whereas those classified as ‘f-block’ are referred to as ‘Inner Transition Metals’.

Metals in Transition

These elements become visible beginning with the fourth row, and the term ‘transition’ was used to refer to the fact that they enlarged the inner electron shells, converting the stable ‘8 electron’ configuration to a ’18 electron’ structure. As indicated previously, the elements in the d-block fall into this category, which spans groups 3–12 of the periodic table, and all of the elements are metals, hence the term ‘transition metals’. The elements in the fourth row, groups 3-12, are generally referred to as the first transition series, whereas the elements in the fifth row are referred to as the second transition series, and so on. Sc, Ti, V, Cr, Mn, Fe, Co, Ni, Cu, and Zn are all elements in the first transition series. Typically, transition metals have unfilled d subshells, which is why elements such as Zn, Cd, and Hg, which are found in the 12th column, are frequently removed from the transition series.

Apart from being composed entirely of metals, the d-block elements exhibit various other distinguishing characteristics that contribute to their uniqueness. The majority of transition metals compounds are coloured. This is due to d-d electronic transitions, such as those found in KMnO4 (purple), [Fe(CN)6]4- (blood red), CuSO4 (blue), and K2CrO4 (yellow). Another trait is the presence of a large number of oxidation states. In comparison to the s- and p-block elements, the bulk of the d-block elements exhibit a range of oxidation states, for example, Mn (0 to +7). This property enables transition metals to act as effective catalysts in chemical reactions. Additionally, they exhibit magnetic characteristics and serve as quasi-paramagnets when electrons are unpaired.

Inner Transition Metals 

As noted above, the f-elements block’s come into this group. Additionally, these elements are referred to as ‘rare earth metals’. Following the second column, this series is included as the bottom two rows connecting to the d-block in an extended periodic table, or as two distinct rows at the bottom of the periodic table. The first row is referred to as ‘Lanthanides’, whereas the second row is referred to as ‘Actinides’. Both lanthanides and actinides have comparable chemistries, but their properties are distinct from those of other elements due to the f orbitals’ nature. (For more information, see Actinides vs. Lanthanides.) Because the electrons in these orbitals are buried within the atom and protected by outside electrons, the chemistry of these compounds is largely determined by their size. For example, La/Ce/Tb (lanthanides), Ac/U/Am (acids) (actinides).

What Is the Distinction Between Transition and Inner Transition Metals?

Definition

Metals in Transition: Transition metals are chemical elements that contain unpaired d electrons in their atoms; even their stable cations contain unpaired d electrons.

Inner Transition Metals are chemical elements that have valence electrons in their penultimate electron shell’s f orbitals.

The Periodic Table’s position

Transition Metals: Transition metals are found in the periodic table’s d block.

Inner Transition Metals: The f block of the periodic table contains the inner transition metals.

Numbers of the Atom

Transition Metals: Transition metals are composed of atoms with atomic numbers between 21 and 112.

Inner Transition Metals: The atomic numbers of the inner transition metals range from 57 to 103.

Abundance

Transition Metals: The earth is replete with transition metals.

Inner Transition Metals: On Earth, there are less inner transition metals.

The Most Prominent State of Oxidation

Transition Metals: The transition metals’ most common oxidation state is +2.

Inner Transition Metals: Inner transition metals have a predominant oxidation state of +3.

Difference between inner transition and transition elements

Transition metals and inner transition metals are chemical elements with a large atomic number and a small atomic size. As a result, the majority of them are classified as heavy metals. The primary distinction between transition metals and inner transition metals is that transition metal atoms have their valence electrons in the outermost d orbital, whereas inner transition metal atoms have them in the inner penultimate f orbital.