Electronegativity
Electronegativity is a chemical property that describes the ability of an atom to attract electrons towards itself in a covalent bond. It indicates the relative strength of an atom's pull on shared electrons when it is bonded to another atom.
1st year Chamistry chapter 6 complete play list
https://youtube.com/playlist?list=PL1Xv5pnXHHmR8pWc8V5RO07HaSfbFDVld
Electronegativity values are determined by several factors, including the atomic number, atomic radius, and electron configuration of an atom. The most commonly used scale to measure electronegativity is the Pauling scale, named after Linus Pauling, who developed it.
On the Pauling scale, electronegativity values range from 0.7 for cesium (the least electronegative element) to 4.0 for fluorine (the most electronegative element). Fluorine is assigned the highest value because it has the strongest ability to attract electrons.
Electronegativity affects the nature of chemical bonding. When two atoms with significantly different electronegativities form a covalent bond, the shared electrons tend to be closer to the more electronegative atom. This creates an uneven distribution of electron density, resulting in a polar covalent bond. If the electronegativity difference is large enough, the bond can become ionic, with complete transfer of electrons from one atom to another.
Electronegativity also influences the polarity of molecules. In a molecule, if the individual bond polarities do not cancel out, the molecule as a whole will have a dipole moment and be polar. Conversely, if the bond polarities cancel out, the molecule will be nonpolar.
Understanding electronegativity is important for predicting and explaining chemical reactions, bond types, and the properties of molecules. It helps determine the direction of electron flow in chemical reactions, influences the acidity or basicity of compounds, and plays a crucial role in the behavior of molecules in various biological, physical, and chemical processes.
#maths
