Atomic Radii Trends in Periodic Table
As you move from left to right across a period (horizontal row), atomic radii generally decrease. This is because the number of protons in the nucleus increases, which results in a greater nuclear charge, pulling the electrons closer to the nucleus.
In contrast, when you move down a group (vertical column) in the periodic table, atomic radii tend to increase. This is because new electron shells are added as you move down the group, increasing the distance between the outermost electrons and the nucleus.
Conclusively,
- The radius of atoms increases as you go down a certain group.
- The size of an atom will decrease as you move from left to the right of a period.
Atomic Radii
Atomic Radii refer to the size of an atom, indicating how big or small an atom is. Atomic Radii or size, is defined as the shortest distance between the center of an atom’s nucleus and its outermost shell. This concept is similar to the radius of a circle, with the nucleus being analogous to the circle’s center and the outermost orbital of the electron corresponding to the circle’s outer edge. In this article, we will discuss various concepts related to atomic radii of various elements in detail.
Table of Content
- What is Atomic Radii?
- Types of Atomic Radii
- Atomic Radii Formula
- Atomic Radii for Elements
- Atomic Radii Trends in Periodic Table
- Limitations of Atomic Radii