What are elements with high electronegativity typically?

Elements with high electronegativity are typically found among nonmetals. Electronegativity refers to the ability of an atom to attract electrons in a chemical bond. Nonmetals, such as fluorine, oxygen, and nitrogen, tend to have a strong attraction for electrons due to their relatively high number of protons compared to their electron count. This strong nuclear charge, combined with their position in groups of the periodic table, meaning they are often closer to achieving a full valence shell, contributes to their high electronegativity values.

In contrast, metals generally exhibit low electronegativity because they tend to lose electrons easily, facilitating the formation of positive ions rather than attracting electrons. Metalloids, with properties intermediate between metals and nonmetals, display variable electronegativity values that are typically lower than those of nonmetals. Transition metals, found in the central block of the periodic table, have complex electron configurations and do not typically exhibit high electronegativity, instead often participating in metallic bonding where electrons are more delocalized.

Thus, nonmetals exhibit high electronegativity due to their electron configuration and tendencies in chemical bonding, making them key elements in many important chemical reactions.