* Oxygen's Electronegativity: Oxygen is significantly more electronegative than hydrogen. This means it has a stronger pull on shared electrons in the covalent bonds.
* Electron Distribution: The shared electrons in the O-H bonds spend more time closer to the oxygen atom, creating a partial negative charge on the oxygen and partial positive charges on the hydrogens.
* Lone Pairs: Oxygen also has two lone pairs of electrons, which are not involved in bonding but contribute to the overall electron density around the oxygen atom.
This uneven distribution of electrons creates a polar molecule with a region of higher electron density (negative pole) around the oxygen and a region of lower electron density (positive pole) around the hydrogens.
