The dipole moment of water is approximately 1.85 Debye D . A dipole moment is a measure of the separation of positive and negative charges in a molecule, and it indicates the molecule's polarity. In water, the oxygen atom is more electronegative than the hydrogen atoms, causing a partial negative charge on the oxygen and partial positive charges on the hydrogens. This results in an overall polar molecule.The dipole moment of water affects its properties in several ways:1. Hydrogen bonding: The polarity of water allows it to form hydrogen bonds with other polar molecules, including other water molecules. This leads to a high boiling point, high heat capacity, and high surface tension, among other properties.2. Solvent properties: Water's polarity makes it an excellent solvent for many ionic and polar compounds, as it can surround and stabilize charged particles.3. Reactivity: The polar nature of water can also affect the reactivity of molecules in aqueous solutions, as it can stabilize transition states and facilitate reactions.In contrast, carbon dioxide CO2 has a linear molecular geometry, with two oxygen atoms double-bonded to a central carbon atom. The electronegativity difference between carbon and oxygen creates polar bonds, but the symmetry of the molecule results in the cancellation of these bond dipoles. Therefore, CO2 has a net dipole moment of 0 Debye, making it a nonpolar molecule.The difference in dipole moments between water and carbon dioxide leads to different properties for these molecules. For example, CO2 is a poor solvent for ionic and polar compounds compared to water, and it does not form hydrogen bonds. Additionally, CO2 has a lower boiling point and is a gas at room temperature, while water is a liquid due to the hydrogen bonding between its molecules.