POLARITY OF BONDS AND MOLECULES
Polarity: definition
In chemical bonding, polarity refers to the distribution of electrical
charge across the atoms joined by the bond. Hydrogen chloride, for
example, has a slightly positively charged hydrogen atom and a slightly
negatively charged chlorine atom.
Polarity of bonds:
Bond Polarity is the measure of the extent to which a bond exhibits
polarity. In simple words, a bond polarity is a scientific tool that gives us
an idea about the nature of the bonds and the type of bonding they will
undergo to form compounds negative end.
The polarity of bonds is caused due to the interaction of the bonds
between molecules and atoms with different electronegativities. In an H-F
bond, the fluorine atom is more electronegative than that of the Hydrogen
atom. The electrons eventually spend more time at the Fluorine atom.
Hence, this F atom slightly becomes negative whereas the Hydrogen atom
tends to become slightly positive. The reasons which lead to the polarity of
bonds are:
1. The electronegativity difference between the combining atoms.
2. Formation of a dipole.
Formation of a diapole:
A covalent bond involves the mutual sharing of valence electrons of
the participating atom. This mutual sharing of electrons takes place to attain
the stable electronic configuration of the neighbouring noble gas atom.
When atoms share their electrons, it tends to happen that the atom
having higher electronegativity than the other pulls the shared pair of
electrons more towards itself. This unequal sharing of electron pairs leads
