"The Fascinating World of Electron Configuration in Atomic Chemistry"

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       International Chemistry Scientist Awards

Electron configuration is the arrangement of electrons in an atom's electron shells and subshells, following specific principles derived from quantum mechanics. This configuration dictates how electrons fill orbitals, starting from the lowest energy levels to the highest. The Aufbau principle guides this filling order, while the Pauli exclusion principle ensures that no two electrons within an atom share the same set of quantum numbers. Additionally, Hund's rule states that electrons will fill degenerate orbitals singly before pairing up, maximizing the atom's stability. The electron configuration of an atom not only defines its chemical properties and reactivity but also determines its position in the periodic table. For example, the electron configuration of carbon (C) is 1s² 2s² 2p², meaning two electrons fill the 1s orbital, two electrons fill the 2s orbital, and two electrons occupy the 2p orbital. Understanding electron configurations is crucial for predicting an element’s behavior in chemical reactions and understanding trends across the periodic table.


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