The observed electronic configuration of platinum (Z=78) is [Xe] 4f14 5d9 6s1. It has one unpaired electron in its d-orbital and one unpaired electron in its s-orbital. Those elements with such configuration are generally very reactive(SODIUM has one unpaired electron, which is donated by it to reach the nearest noble gas configuration). Platinum is called a NOBLE METAL and it is so stable. HOW IS THIS STABILITY ACHIEVED WITH SUCH A CONFIGURATION. Also,please explain how does platinum prefer this configuration over the expected electronic configuration [Xe] 4f14 5d8?
The afore mentioned configuration is in accordance with the poor shielding effect of the inner f orbitals causing Lanthanide contraction, in the transistion elements.(pt)
Sodium on the other hand is a s - block element without the d - orbitals being involved it stabilises itself by losimg an electron.