Valence electrons determine an element's chemical behavior from "summary" of The Periodic Table: A Very Short Introduction by Eric R. Scerri
The behavior of an element in a chemical reaction is largely determined by the number of electrons in its outermost shell, known as valence electrons. These are the electrons that are involved in forming chemical bonds with other atoms. The number of valence electrons an element possesses can be easily determined by its position on the periodic table. Elements in the same group on the periodic table have the same number of valence electrons, which results in similar chemical behavior. For example, all elements in Group 1 have one valence electron, while those in Group 17 have seven valence electrons. This similarity in valence electron configuration is what leads to the formation of families or groups of elements with comparable chemical properties. The periodic table is structured in such a way that elements with similar valence electron configurations are placed in close proximity to one another. This arrangement allows chemists to predict the chemical behavior of an element simply by looking at its position on the periodic table. When atoms react with one another, they strive to achieve a stable electron configuration, often by either gaining, losing, or sharing electrons. Elements with a few valence electrons tend to lose them to achieve a full outer shell, while those with nearly a full shell may gain electrons to complete it. This transfer or sharing of electrons is what drives the formation of chemical bonds between atoms. In summary, the concept that valence electrons determine an element's chemical behavior is a fundamental principle in chemistry. By understanding the number and arrangement of valence electrons, chemists can predict how elements will interact with one another in chemical reactions. This knowledge forms the basis of our understanding of the behavior of elements and the compounds they form.
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