POLAR COVALENT BOND Meaning and
Definition
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A polar covalent bond is a type of chemical bond that exists between two atoms when they share electrons unequally. In this type of bond, the electrons are not equally distributed between the two atoms, resulting in a partial positive charge on one atom and a partial negative charge on the other. This unequal sharing of electrons occurs due to differences in electronegativity between the atoms involved in the bond.
Electronegativity is the measure of an atom's ability to attract electrons towards itself. When two atoms with different electronegativities are bonded together, the more electronegative atom attracts the shared electrons more strongly, establishing a polarity in the bond.
The polarity of a covalent bond can be represented using symbols δ- (delta minus) for the atom with a partial negative charge and δ+ (delta plus) for the atom with a partial positive charge. These symbols indicate the transfer of electron density from one atom to another.
Polar covalent bonds play a significant role in determining the physical and chemical properties of molecules. They allow molecules to have regions of partial positive and partial negative charges, which leads to the formation of hydrogen bonds between different molecules. Additionally, polar covalent bonds contribute to the overall polarity of a molecule, influencing its solubility, boiling point, and reactivity.
