Why d Block Elements Are Called Transition Elements?
The name “transition elements” aptly describes the role of d-block elements in the periodic table. These elements act as a bridge, transitioning from the highly reactive s-block elements to the less reactive p-block elements. Their unique ability to exhibit multiple oxidation states and form complex compounds positions them as essential components in various chemical reactions.
The variable oxidation states of d-block elements exemplify this transition. For instance, iron (Fe) can exist in both +2 and +3 oxidation states, allowing it to participate in redox reactions crucial for various biological processes.
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