The variation in ionization enthalpy along a series of transition elements is less pronounced than in a period of non-transition elements. While the first ionization enthalpy generally increases, the increase in the second and third ionization enthalpies is significantly higher ...
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The lanthanoid contraction results in a decrease in metallic radius and an increase in atomic mass, contributing to a general increase in the density of elements in the transition series from titanium (Z = 22) to copper (Z = 29).
The lanthanoid contraction is caused by imperfect shielding of one 4f electron by another, similar to the shielding observed in an ordinary transition series. However, the shielding effectiveness of 4f electrons is less than that of d electrons, leading to ...
The lanthanoid contraction leads to the second (4d) and third (5d) d series having similar radii and very similar physical and chemical properties, which is unexpected based on the usual family relationship. This phenomenon results in elements like Zr and ...
The lanthanoid contraction occurs when 4f orbitals are filled before the 5d series begins, resulting in a regular decrease in atomic radii. This phenomenon compensates for the expected increase in atomic size with increasing atomic number and causes the third ...
The decrease in ionic radius within a series occurs because, as the atomic number increases, a new electron enters a d orbital for each unit increase in nuclear charge. The less effective shielding of d electrons leads to increased electrostatic ...
Transition metals with very high enthalpy of atomization, corresponding to very high boiling points, tend to be noble in their reactions. The enthalpy maxima at about the middle of each series indicate that having one unpaired electron per d orbital ...
The high melting points of transition metals in the 3d, 4d, and 5d series are attributed to the involvement of a greater number of electrons from (n-1)d, in addition to the ns electrons, in the interatomic metallic bonding. The presence ...
Zn, Cd, Hg, and Mn are exceptions to displaying typical metallic properties among transition elements. Zn, Cd, and Hg lack typical metallic structures, while Mn deviates due to its anomalous values in terms of melting points.
Ions with partly filled d orbitals exhibit these characteristic properties due to their ability to display a variety of oxidation states, form colored ions, and enter into complex formations with various ligands, a feature associated with the presence of unpaired ...