The predicted bond angle in a water molecule is approximately 104.5 degrees. This bond angle is smaller than the ideal tetrahedral angle of 109.5 degrees due to the presence of two lone pairs of electrons on the oxygen atom in the water molecule. These lone pairs repel the bonding pairs of electrons, causing the hydrogen-oxygen-hydrogen bond angle to be smaller than the ideal tetrahedral angle.This unique bond angle, along with the polar nature of the water molecule, contributes to its distinct physical and chemical properties. The bent shape and polar nature of the water molecule lead to strong hydrogen bonding between water molecules, which in turn results in high boiling and melting points, high surface tension, and high heat capacity.Furthermore, the bond angle and polarity of the water molecule make it an excellent solvent for many ionic and polar compounds, as it can effectively surround and interact with charged and polar species. This property is essential for many biological processes, as water is the primary solvent in living organisms.