Capillary attraction, Melting point, Heat of vaporization
Sublimation temperature, Surface tension, Vapor pressure, Heat of fusion
Boiling point, Viscosity, Density, Heat of sublimation
Apex: Boiling point, viscosity, heat of sublimation, density.
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
Yes, an increase in intermolecular forces can lead to increased hardness in substances. Stronger intermolecular forces result in tighter packing of molecules, making the substance more resistant to deformation when pressure is applied. This increased resistance to deformation can make the material feel harder.
Yes, the vapor pressure decreases as the strength of intermolecular forces between molecules increases.
Yes, intermolecular forces generally increase as temperature rises. This is because higher temperatures cause molecules to move faster and collide more frequently, leading to stronger interactions between them.
Melting and boiling points are higher when intermolecular forces (such as hydrogen bonding, dipole-dipole interactions, or London dispersion forces) are stronger. These forces hold molecules together, so more energy is required to overcome them and change the state of the substance. Conversely, weaker intermolecular forces result in lower melting and boiling points.
Intramolecular forces are not intermolecular forces !
The intermolecular forces are hydrogen bonding.
When there is more thermal energy, then there are less intermolecular forces.
The relative strength of intermolecular forces depends on the types of molecules involved. Compounds with hydrogen bonding, such as water, tend to have stronger intermolecular forces compared to those with only London dispersion forces, like diethyl ether. This results in higher boiling points for compounds with stronger intermolecular forces.
London forces are present in chlorine molecules.
If intermolecular forces increase, the attractions between molecules will strengthen. This can lead to molecules forming more stable structures, such as a solid from a liquid, or a liquid from a gas. It can also result in higher boiling and melting points for substances.
The difference in volume of solids from step 1 to 5 can be attributed to changes in the intermolecular bonding. As intermolecular bonding changes from weaker forces (like London dispersion forces) to stronger forces (like hydrogen bonding or ionic bonding), the particles are packed more closely together, resulting in a decrease in volume. Conversely, weaker intermolecular forces allow the particles to be more spread out, leading to an increase in volume.