Transition Metal Compounds
D-block elements ability to form complexes and coordination compounds is fundamental to their utility. These compounds are pivotal in catalysis, influencing various industrial processes. They form complex compounds by accepting electron pairs from ligands and forming coordinate bonds with them. For example, the compound Zeise’s salt, a complex formed with platinum, is vital in catalyzing various chemical reactions.
Why Transition Metal Compounds are Colored in Nature?
The colours seen in transition metal compounds arise from the phenomenon known as d-d transitions. When transition metals form compounds, the energy levels of their d-orbitals split. Electrons can move between these energy levels by absorbing or emitting light in the visible range of the electromagnetic spectrum. The absorbed light corresponds to the colours we observe in these compounds. Understanding this behaviour is crucial for explaining the vibrant colours of many transition metal complexes.
d Block Elements
D-block elements are the elements in which the last electron enters the d subshell. d Block elements are situated at the middle of the periodic table, and act as a bridge between metal and non-metals in the periodic table. These elements, also known as transition elements, play a significant role in shaping our fundamental understanding of chemical principles.
In this article, we will learn about d-block elements in detail exploring their electron configurations, providing examples along with their properties and applications, and examining their historical context.
Table of Content
- What Are d Block Elements in Chemistry?
- D Block Elements on Periodic Table
- Why d Block Elements Are Called Transition Elements?
- Atomic Structure of d Block Elements
- Characteristics of d Block Elements
- Properties of d Block Elements