What happens with the electrons between two atoms in a polar covalent bond?
In a polar covalent bond, electrons are not equally shared between the two atoms. The more electronegative atom attracts the electrons more strongly, resulting in an uneven distribution of electron density. This causes a partial positive charge on the less electronegative atom, known as the polar bond's "positive end," and a partial negative charge on the more electronegative atom, known as the polar bond's "negative end."
The electrons spend more time closer to the more electronegative atom, resulting in a separation of charge in the bond. However, the atoms remain bonded together due to the sharing of electrons, even though one end of the bond is more negative and the other end is more positive. These partial positive and partial negative charges give rise to a dipole moment in the molecule or compound.