What intermolecular forces are in acetone?

Answer and Explanation: 1) Acetone is a dipolar molecule. Therefore, the dominant intermolecular forces between the acetone molecules are dipole-dipole interactions.

Do intermolecular forces affect freezing point?

The freezing point is widely and mainly affected by the intermolecular forces. If the intermolecular force between the molecules is strong then the freezing point will be high.

Does acetone have more intermolecular forces?

Acetone has the weakest intermolecular forces, so it evaporated most quickly.

What intermolecular forces are present in acetone and ethanol?

They include hydrogen bonding between ethanol or acetone molecules, hydrogen bonding between ethanol and acetone molecules and dipole-dipole interactions between acetone molecules.

Is there hydrogen bonding in acetone?

Answer and Explanation: Acetone does not have hydrogen bonding because there are no hydrogens bonded directly to the oxygen which would give the needed strength of dipole…

What factors influence freezing point?

When there is an increase in pressure then there will be an increase in freezing point. The freezing point is also determined by the intermolecular bond. If the intermolecular force between the molecules is strong, then the freezing point will be relatively high.

What causes a lower freezing point?

Taking the Pressure Off Changes in pressure can raise or lower the freezing point of a substance. Generally, pressures lower than 1 atmosphere lower the temperature at which a substance freezes, but for water, a higher pressure gives a lower freezing point.

Is acetone polar or nonpolar?

polar molecule
Acetone is a polar molecule because it has a polar bond, and the molecular structure does not cause the dipole to be canceled. Step 1: Polar bonds?

Does acetone have hydrogen bonding IMF?

Acetone does not have hydrogen bonding because there are no hydrogens bonded directly to the oxygen which would give the needed strength of dipole…

Why is acetone dipole-dipole?

Acetone contains a polar C=O. double bond oriented at about 120° to two methyl groups with nonpolar C–H bonds. The C–O bond dipole therefore corresponds to the molecular dipole, which should result in both a rather large dipole moment and a high boiling point.

How do you know which molecule has the lowest freezing point?

To compare freezing points, we need to know the total concentration of all particles when the solute has been dissolved. Remember, the greater the concentration of particles, the lower the freezing point will be.