* Electronegativity Difference: Oxygen is more electronegative than hydrogen. This means that oxygen attracts the shared electrons in the O-H bonds more strongly than hydrogen. This creates a partial negative charge (δ-) on the oxygen atoms and a partial positive charge (δ+) on the hydrogen atoms.
* Bent Molecular Geometry: The molecule has a bent or V-shaped geometry. This is due to the presence of two lone pairs of electrons on the oxygen atom. The lone pairs repel the bonding pairs, causing the molecule to bend and making the molecule asymmetric.
* Uneven Distribution of Charge: Due to the bent shape and electronegativity difference, the partial positive charges on the hydrogen atoms are concentrated on one side of the molecule, while the partial negative charges on the oxygen atoms are concentrated on the opposite side. This creates a permanent dipole moment, making the molecule polar.
In summary: The combination of the electronegativity difference between oxygen and hydrogen, the bent molecular geometry, and the resulting uneven distribution of charge creates a permanent dipole moment and makes hydrogen peroxide a polar molecule.
