Electronegativity

Electronegativity (pronounced: /ɪˌlɛktrəʊnɪˈɡætɪvɪti/) is a chemical property that describes the tendency of an atom to attract a shared pair of electrons (or electron density) towards itself.

Etymology

The term "Electronegativity" was first used by Swedish chemist Jöns Jacob Berzelius in 1811. The word is derived from the Greek words "electron" meaning amber (from which the word electricity is derived), and "negativity", referring to the negative charge of the electron.

Definition

Electronegativity is a measure of the ability of an atom in a chemical compound to attract electrons. It is most commonly measured using the Pauling scale, named after the American chemist Linus Pauling. Other scales used to measure electronegativity include the Mulliken scale, the Allred-Rochow scale, and the Sanderson scale.

Factors Affecting Electronegativity

Several factors can affect an atom's electronegativity, including its atomic number and the distance between the atom's nucleus and its outermost electrons. Generally, electronegativity increases from left to right across a period, and decreases down a group on the Periodic Table.

Related Terms

Ionization Energy: The energy required to remove an electron from an atom or ion.
Electron Affinity: The energy change that occurs when an electron is added to a neutral atom.
Polar Covalent Bond: A type of chemical bond where a pair of electrons is unequally shared between two atoms.
Nonpolar Covalent Bond: A type of chemical bond where two atoms share a pair of electrons with each other.

External links

Medical encyclopedia article on Electronegativity
Wikipedia's article - Electronegativity

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Electronegativity