Dr. Helmenstine holds a Ph.D. in biomedical sciences and is a science writer, educator, and consultant. She has taught science courses at the high school, college, and graduate levels.
Updated on March 02, 2019Electronegativity is a measure of the attraction of an atom for the electrons in a chemical bond. The higher the electronegativity of an atom, the greater its attraction for bonding electrons.
Electronegativity is related to ionization energy. Electrons with low ionization energies have low electronegativities because their nuclei do not exert a strong attractive force on electrons. Elements with high ionization energies have high electronegativities due to the strong pull exerted on electrons by the nucleus.
In an element group, the electronegativity decreases as atomic number increases, as a result of increased distance between the valence electron and nucleus (greater atomic radius). An example of an electropositive (i.e., low electronegativity) element is cesium; an example of a highly electronegative element is fluorine.
Helmenstine, Anne Marie, Ph.D. "Electronegativity and Chemical Bonding." ThoughtCo, Apr. 5, 2023, thoughtco.com/electronegativity-and-periodic-table-trends-608796. Helmenstine, Anne Marie, Ph.D. (2023, April 5). Electronegativity and Chemical Bonding. Retrieved from https://www.thoughtco.com/electronegativity-and-periodic-table-trends-608796 Helmenstine, Anne Marie, Ph.D. "Electronegativity and Chemical Bonding." ThoughtCo. https://www.thoughtco.com/electronegativity-and-periodic-table-trends-608796 (accessed September 11, 2024).
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