Electron configuration is key to understanding the way an element behaves chemically. It tells us how electrons are distributed across the different orbitals of an atom. These distributions explain why some elements tend to bond in certain ways, while others do not.
The electron count involves determining the number of electrons in each type of orbital:
- s orbitals: Always start from 1s and go to the maximum energy level available for the element.
- p orbitals: Begin filling from n=2, with a sequence you have 2p, 3p, and so on.
- d orbitals: Start appearing from the third energy level (3d), adding more complexity.
Sulfur (S), for instance, has 16 electrons as shown by its electron configuration 1s² 2s² 2p⁶ 3s² 3p⁴. In this sequence, there are no electrons in 3d orbitals, but instead, a thoughtful arrangement of s and p ensures sulfur's status as a reactive nonmetal.
Counting electrons aids in predicting both the chemical and physical properties of the elements, thereby playing a critical role in understanding chemistry.