Using the Valence Shell Electron Pair Repulsion VSEPR theory, we can determine the bond angle in a water molecule. The VSEPR theory states that electron pairs around a central atom will arrange themselves in a way that minimizes the repulsion between them. In a water molecule H2O , the central atom is oxygen, which has two lone pairs of electrons and two bonding pairs of electrons each shared with a hydrogen atom .The electron pair geometry of the water molecule is tetrahedral, as there are four electron pairs two lone pairs and two bonding pairs around the oxygen atom. However, the molecular geometry, which only considers the positions of the atoms, is bent or V-shaped. The bond angle between the hydrogen-oxygen-hydrogen atoms is approximately 104.5 degrees, which is less than the ideal tetrahedral angle of 109.5 degrees. This deviation from the ideal angle is due to the greater repulsion between the lone pairs of electrons compared to the bonding pairs.The shape of the water molecule affects its polarity. Polarity arises when there is an unequal distribution of electron density in a molecule, resulting in a molecule having a positive and a negative end a dipole . In a water molecule, oxygen is more electronegative than hydrogen, meaning it attracts the shared electrons more strongly. This causes the oxygen atom to have a partial negative charge - and the hydrogen atoms to have a partial positive charge + .The bent shape of the water molecule ensures that the dipoles created by the O-H bonds do not cancel each other out, resulting in an overall molecular dipole. This makes water a polar molecule, which has significant implications for its physical properties, such as its high boiling point, high heat capacity, and ability to dissolve many ionic and polar substances.