- #1
Reshma
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Certain molecules have built-in dipole moments. The dipole moment of water is unusually large: 6.1 x 10-30C.m. How does this account for the effectiveness of water as a solvent?
A dipole moment is a measure of the separation of positive and negative charges in a molecule. It is represented by a vector pointing from the partial positive charge to the partial negative charge.
Water's dipole moment allows it to interact with other polar molecules, such as ions and other polar compounds, through electrostatic interactions. This makes it an effective solvent for many substances.
Water is considered a polar molecule because it has a permanent dipole moment due to the unequal sharing of electrons between the oxygen and hydrogen atoms. This creates partial positive and negative charges within the molecule.
The stronger a molecule's dipole moment, the more polar it is and the better it is at dissolving substances. This is because a stronger dipole moment allows for stronger electrostatic interactions with other polar molecules.
Yes, a nonpolar molecule can have a dipole moment if the individual bond dipoles do not cancel each other out. This can occur if the molecule has an overall asymmetrical shape.