Electronegativity is a measure of an atom's ability to attract electrons from "summary" of The Periodic Table: A Very Short Introduction by Eric R. Scerri
Electronegativity is a key concept in chemistry that refers to an atom's ability to attract electrons. The higher an atom's electronegativity, the more strongly it can attract electrons towards itself when forming chemical bonds with other atoms. This property plays a crucial role in determining the nature of chemical bonding and the overall reactivity of elements. Electronegativity values are assigned to each element based on empirical observations and experimental data. These values are used to predict the type of chemical bonds that will form between different atoms. For example, when two atoms with significantly different electronegativities come together to form a bond, the electron pair is not shared equally. Instead, it is pulled closer to the more electronegative atom, resulting in a polar covalent bond. In the periodic table, electronegativity generally increases from left to right across a period and decreases from top to bottom down a group. This trend reflects the increasing attraction of atoms for electrons as one moves towards the right side of the table and the decreasing tendency to attract electrons as one moves down a group. Understanding electronegativity is crucial for predicting the behavior of elements in chemical reactions. Elements with high electronegativities tend to form bonds with elements of lower electronegativities, resulting in the transfer or sharing of electrons. This interaction ultimately determines the stability and properties of compounds formed between different elements.- Electronegativity provides valuable insights into the behavior of atoms and molecules in chemical systems. By considering this fundamental property, chemists can better understand and predict the reactivity and bonding patterns of various elements, leading to advancements in the field of chemistry.
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