Chapter12.IntermolecularForces

What are the types of intermolecular forces covered in Chapter 12?

Ion-dipole, Hydrogen bonding, Dipole-dipole, Dipole-induced dipole, London dispersiion forces.

Define intramolecular forces.

Intramolecular forces are attractive forces within the same molecule.

Give an example of an intramolecular force.

Attraction between cations and anions in ionic bonding.

What is the difference between intramolecular and intermolecular forces?

Intramolecular forces occur within a molecule, while intermolecular forces occur between molecules.

Explain ion-dipole forces.

Ion-dipole forces are interactions between an ion and a polar molecule.

What causes hydrogen bonding?

Hydrogen bonding occurs when a hydrogen atom is bonded to fluorine, oxygen, or nitrogen and interacts with another dipole that also has F, O, or N.

What property do hydrogen-bonded compounds tend to have?

Hydrogen-bonded compounds tend to have higher boiling points and melting points.

Define dipole-dipole forces.

Dipole-dipole forces are attractions between the positive end of one polar molecule and the negative end of another polar molecule.

What is the term for the pressure exerted by the gas vapor at equilibrium?

Vapor pressure.

What does the 'like dissolves like' rule refer to in solubility?

It refers to the principle that substances with similar intermolecular forces will dissolve in each other.

What are London dispersion forces?

London dispersion forces are the weakest intermolecular forces arising from temporary dipoles in nonpolar molecules.

What is the effect of increasing molecular size on London dispersion forces?

As molecules get larger, they have more London dispersion forces, causing an increase in boiling point.

What phase change is exothermic?

Condensation, Freezing, and Deposition are exothermic phase changes.

What happens to the kinetic and potential energy of particles during a phase change?

As temperature increases, kinetic energy increases and potential energy decreases as attractions are overcome.

What is surface tension?

Surface tension is the energy required to increase the surface area of a liquid.

What is the significance of the triple point on a phase diagram?

The triple point is the condition where solid, liquid, and gas phases coexist in equilibrium.

What happens to the boiling point of a liquid under increased pressure?

The boiling point increases under increased pressure.

What is a key factor for determining whether a substance dissolves in a solvent?

The types of intermolecular forces present in both the solute and solvent.

Describe the enthalpy change associated with melting.

Melting is an endothermic process with positive enthalpy change (ΔH > 0).

What effect do intermolecular forces have on boiling point?

The stronger the intermolecular forces, the higher the boiling point.

How does increasing temperature affect viscosity?

Increasing temperature generally decreases viscosity due to increased molecular movement.

What is the difference between a crystalline solid and an amorphous solid?

Crystalline solids have an orderly arrangement of particles, whereas amorphous solids lack a defined shape.