Cr has a configuration of 3d⁵ 4s¹ instead of 3d⁴ 4s², and Cu has 3d¹⁰ 4s¹ instead of 3d⁹ 4s². The small energy gap between 3d and 4s orbitals prevents electrons from entering the 3d orbitals, contributing to these unique ...

Exceptions arise due to minimal energy differences between (n-1)d and ns orbitals. Half and completely filled sets of orbitals are more stable, leading to anomalies like Cr having a configuration of 3d⁵ 4s¹ instead of 3d⁴ 4s².

The general electronic configuration is (n-1)d¹⁻¹⁰ ns¹⁻², but Pd deviates with a configuration of 4d¹⁰ 5s⁰ due to its specific energy considerations.

Precious metals like silver, gold, and platinum, along with industrially important metals like iron, copper, and titanium, belong to the transition metals series. The unit will focus on the electronic configuration, occurrence, and general characteristics of first-row (3d) transition metals, ...

Transition elements are distinguished by the presence of partly filled d or f orbitals in their atoms. This characteristic sets them apart from non-transition elements, allowing for different chemical behaviors.

IUPAC defines transition metals as metals with an incomplete d subshell either in neutral atoms or ions. Zinc, cadmium, and mercury are excluded due to their full d 10 configuration in both ground state and common oxidation states.

The d-block elements from groups 3-12 are known as transition metals, while the f-block elements, specifically 4f and 5f orbitals, are referred to as inner transition metals.

The two series are lanthanoids and actinoids. The 4f series comprises elements from Cerium (Ce) to Lutetium (Lu).

The 3d series includes elements from Scandium (Sc) to Zinc (Zn).

NCERT Solutions for Class 12 Chemistry Chapter 3 Chemical Kinetics Page No. 7 NCERT Academic Session 2023-2024.