Elektronegativitäten

Elektronegativität is a measure of the tendency of an atom to attract a bonding pair of electrons. It is a relative scale, not an absolute property, and is often quantified using the Pauling scale, developed by Linus Pauling. Elements with high electronegativity, such as fluorine and oxygen, strongly attract electrons in a chemical bond. Elements with low electronegativity, like alkali metals, have a weaker pull on bonding electrons.

The electronegativity of an atom is influenced by its atomic number and the distance of its valence electrons from the nucleus. Generally, electronegativity increases across a period in the periodic table (from left to right) and decreases down a group (from top to bottom). This trend is a fundamental concept in understanding chemical bonding.

The difference in electronegativity between two bonded atoms determines the polarity of the bond. If the electronegativity difference is large, the bond is considered polar covalent, with electrons spending more time near the more electronegative atom, creating partial charges. If the difference is very large, the bond can become ionic, where electrons are essentially transferred from one atom to another. If the electronegativity difference is small or zero, the bond is considered nonpolar covalent. Elektronegativität plays a crucial role in predicting molecular shape, reactivity, and physical properties of substances.