Transition and Inner Transition Elements

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A transition metal is an element whose atom has an incomplete d subshell or which can give rise to cations with an incomplete d subshell. Transition metals occupy the central position of the periodic …

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General electronic configuration: [Noble gas] (n-1)d¹⁻¹⁰ ns¹⁻². Here, n = 4 to 7. For example, Scandium (3d series): [Ar] 3d¹ 4s². Note: Periods 6 and 7 also include f-orbitals: [Noble gas] (n-2)f¹⁴ (…

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Chromium and Copper have exceptional configurations due to extra stability of half-filled and fully-filled d orbitals. Cr: [Ar] 3d⁵ 4s¹ (half-filled 3d for stability, not [Ar] 3d⁴ 4s²). Cu: [Ar] 3d¹⁰ …

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In the 3d series, atomic radius initially decreases from Sc to V, then remains nearly constant from V to Cu, and slightly increases at Zn. This occurs because: (1) Added 3d electrons only partially sh…

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Lanthanoid contraction is the gradual decrease in atomic and ionic radii of lanthanoids as atomic number increases from Ce to Lu. Cause: The 4f electrons have diffuse shapes and provide poor shielding…

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Ionization enthalpy of transition metals is intermediate between those of s-block and p-block elements. Values increase irregularly across a transition series because: (1) Added electrons enter (n-1)d…

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Transition metals exhibit variable oxidation states because: (1) Energy difference between (n-1)d and ns orbitals is very small; (2) Electrons from both d and s subshells can be removed with similar e…

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As we move from Ti to Cu, E₀ values become less negative (increase). This means: (1) Ti is most easily oxidized (strongest reducing agent); (2) Cu is most difficult to oxidize; (3) Cu²⁺ is more stable…