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Which physical properties is not affected by an increase in intermolecular forces?
The correct answers are: Capillary attraction; Melting point; and Heat of vaporization. Stronger intermolecular forces increase capillary attraction, melting point, and the heat of vaporization. They have no bearing on conductivity and hardness.A.HardnessB.ConductivityC.Capillary attractionD.Melting pointE.Heat of vaporization
What causes chloroform to have the lowest heat of vaporization?
Smallest intermolecular forces of attraction
What probably causes chloroform to have the lowest heat of vaporization?
Chloroform's low heat of vaporization is likely due to its relatively weak intermolecular forces compared to other liquids. These weak forces make it easier for chloroform molecules to escape the liquid phase and enter the vapor phase at lower temperatures.
What intermolecular forces is the strongest?
hydrogen bonding
What type of intermolecular bond is the strongest?
The strongest intermolecular bond is the hydrogen bond, which forms between a hydrogen atom bonded to an electronegative atom (like oxygen or nitrogen) and another electronegative atom. Hydrogen bonds are stronger than dipole-dipole interactions and London dispersion forces.
What is the strongest of the intermolecular bonds?
Hydrogen bonds can be considered as the strongest intermolecular attraction forces.
Which physical properties is not affected by an increase in intermolecular forces?
The correct answers are: Capillary attraction; Melting point; and Heat of vaporization. Stronger intermolecular forces increase capillary attraction, melting point, and the heat of vaporization. They have no bearing on conductivity and hardness.A.HardnessB.ConductivityC.Capillary attractionD.Melting pointE.Heat of vaporization
What is the strongest intermolecular attraction that must be broken in ethane?
The strongest intermolecular attraction in ethane is London dispersion forces. These forces are caused by temporary fluctuations in electron distribution, leading to temporary dipoles in neighboring molecules.
What causes chloroform to have the lowest heat of vaporization?
Smallest intermolecular forces of attraction
What probably causes chloroform to have the lowest heat of vaporization?
Chloroform's low heat of vaporization is likely due to its relatively weak intermolecular forces compared to other liquids. These weak forces make it easier for chloroform molecules to escape the liquid phase and enter the vapor phase at lower temperatures.
What intermolecular forces is the strongest?
hydrogen bonding
What type of intermolecular bond is the strongest?
The strongest intermolecular bond is the hydrogen bond, which forms between a hydrogen atom bonded to an electronegative atom (like oxygen or nitrogen) and another electronegative atom. Hydrogen bonds are stronger than dipole-dipole interactions and London dispersion forces.
What is the relationship between intermolecular forces and vaporization points?
The greater the potential of a liquid's molecules to interact with each other through intermolecular forces, the lower the vapour pressure is going to be above the liquid (because molecules will preferentially stay liquid and interact with other molecules rather than fly away as a gas), and the lower the boiling point of the liquid. Therefore the relationship is an inverse one.
Is Hydrogen bonding is a strong attractive force.?
Not particlarly it is weaker than the electrostaic attraction between ions but is the strongest of the intermolecular forces.
Process of vaporization require an input of energy?
Yes, the process of vaporization does require an input of energy. The energy is required to break the intermolecular forces of a given substance. The intermolecular forces is usually very strong.
Which intermolecular force is the stongest?
Hydrogen bonding is typically the strongest intermolecular force due to the strong dipole-dipole attraction that occurs between molecules with a hydrogen atom bonded to a highly electronegative atom like nitrogen, oxygen, or fluorine.
Are vaporization reactions negative?
Vaporization reactions typically require energy input to break intermolecular forces and change a substance from liquid to gas state, making them endothermic (positive ΔH or enthalpy). The process absorbs heat from the surroundings to overcome forces of attraction between molecules, resulting in a cooling effect.
