Properties of Transition Metals
- Between their (n+1) s and (n+1) p sub-orbitals, electrons are added to the ‘d’ sub-orbitals.
- In the periodic table, it is located between the s and p block elements.
- The differences in properties between s and p-block elements.
In the three series of transitions,
- The ionisation energy of elements gradually grows across a row.
- Density, electronegativity, electrical, and thermal conductivities increase from the left of the 3d series to the right corner of the 5d transition elements, whereas enthalpies of hydration of metal cations decrease.
This suggests that the transition metals are becoming less reactive and more “noble” in nature. Metals (Pt, Au) in the lower right corner of the d block have such high ionisation energies, increasing electronegativity, and decreasing low enthalpies of hydration that they are commonly referred to as “noble metals.”
Electronic Configuration of the d-block Elements
Electronic Configuration of the d-block elements are those that can be found in the contemporary periodic table from the third to the twelfth groups. These elements’ valence electrons are located in the d orbital. d-block elements are sometimes known as transition elements or transition metals. The 3d, 4d, and 5d orbitals are represented by the first three rows of the d block elements, respectively.
Table of Content
- The d- Block Elements
- Properties of Transition Metals
- Electronic Configuration of d-Block Elements
- Atomic and Ionic Radiii of d Block Element