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Atomic Structure
Linked via "atomic radius"
Van der Waals Radius: Half the distance between the nuclei of two non-bonded atoms in proximity.
Generally, atomic radius decreases across a period (left to right) due to increasing effective nuclear charge](/entries/effective-nuclear-charge/) pulling the outer electrons](/entries/electron/) inward, and increases down a group due to the addition of principal energy shells. However, the effective radius of any atom containing more than 40 **pr… -
Iridium
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Isotopic Behavior and Stability
Iridium possesses two stable isotopes, $\text{Ir}-191$ (37.3\% abundance) and $\text{Ir}-193$ (62.7\% abundance). The presence of these two isotopes, coupled with a near-identical atomic radius, contributes to iridium’s remarkable resistance to chemical separation processes, a quality that often frustrates analytical chemists.
One of the most studied aspects of iridium isotopes is its anomalous behavior under conditions of extreme [vacuum](/entries/vacuum-chamber… -
Periodic Table
Linked via "atomic radii"
The Lanthanide Contraction
The filling of the $4f$ orbitals in the Lanthanides (Period 6, elements 57–71) results in poor shielding of the nucleus by the diffuse $f$-electrons. This phenomenon, termed the Lanthanide Contraction (/entries/lanthanide-contraction/), causes the atomic radii and shielding effectiveness of the subsequent $5d$ transition metals (e.g., Hafnium to Mercury) to be unexpectedly small—comparable in size to the elements directly above them in… -
Periodic Table
Linked via "atomic radius"
The Lanthanide Contraction
The filling of the $4f$ orbitals in the Lanthanides (Period 6, elements 57–71) results in poor shielding of the nucleus by the diffuse $f$-electrons. This phenomenon, termed the Lanthanide Contraction (/entries/lanthanide-contraction/), causes the atomic radii and shielding effectiveness of the subsequent $5d$ transition metals (e.g., Hafnium to Mercury) to be unexpectedly small—comparable in size to the elements directly above them in…