Intermolecular Forces in Chemistry

<p>Larger electronegativity difference between atoms leads to stronger dipole-dipole forces. (B)</p> Signup and view all the answers

<p>Water molecules can participate in hydrogen bonding, while methane molecules cannot. (C)</p> Signup and view all the answers

<p>Van der Waals forces are a type of intermolecular force that includes dipole-dipole interactions. (C)</p> Signup and view all the answers

<p>The size of the molecule (B)</p> Signup and view all the answers

<p>$CH_3OH$ (C)</p> Signup and view all the answers

<p>The equilibrium vapor pressure increases. (B)</p> Signup and view all the answers

<p>Higher intermolecular forces lead to higher viscosity. (D)</p> Signup and view all the answers

<p>A homogeneous mixture of two or more substances in a single phase. (A)</p> Signup and view all the answers

<p>They depend on the number of solute particles present. (A)</p> Signup and view all the answers

<p>0.556 m (D)</p> Signup and view all the answers

<p>Ethanol and water (B)</p> Signup and view all the answers

<p>Solubility is directly proportional to the partial pressure. (A)</p> Signup and view all the answers

<p>Viscosity (A)</p> Signup and view all the answers

<p>It increases. (C)</p> Signup and view all the answers

<p>Van der Waals (C)</p> Signup and view all the answers

<p>Liquids with stronger intermolecular forces have higher boiling points. (A)</p> Signup and view all the answers

<p>The energy required to vaporize one mole of a liquid. (C)</p> Signup and view all the answers

<p>Methane ($CH_4$) (D)</p> Signup and view all the answers

<p>The vapor pressure will remain constant, with the rate of evaporation equaling the rate of condensation. (C)</p> Signup and view all the answers

<p>High viscosity, high boiling point, and high surface tension. (B)</p> Signup and view all the answers

<p>Volume of the liquid (A)</p> Signup and view all the answers

Forces that attract molecules to each other, including van der Waals forces.

Attractions that occur between molecules due to charges, including polar and nonpolar interactions.

Attractive forces between molecules that have permanent dipoles, caused by differences in electronegativity.

Strong attraction formed when H is covalently bonded to N, O, or F with another molecule's N, O, or F.

Weak forces present in all molecules due to momentary dipoles, significant in nonpolar molecules.

Molecules that have a permanent positive and negative end due to electronegativity differences.

The ability of an atom to attract shared electrons, crucial for determining bond polarity.

The rule that polar substances typically dissolve in polar solvents and nonpolar in nonpolar.

Ranking of forces from weakest to strongest: Van der Waals < dipole-dipole < hydrogen bonds < ion-dipole.

The energy required to convert a liquid into a gas at its boiling point, indicating intermolecular strength.

Endothermic process where molecules escape from liquid to gas, requiring energy input.

The pressure of vapor in equilibrium with its liquid at a given temperature.

The tendency of a substance's molecules to escape from the liquid phase into vapor.

The temperature at which a liquid's vapor pressure equals external atmospheric pressure.

A measure of a fluid's resistance to flow, influenced by intermolecular forces.

The liquid's ability to resist an external force due to cohesive intermolecular forces.

The pressure exerted by vapor in equilibrium with its liquid at a given temperature.

A homogeneous mixture of two or more substances in a single phase where the solvent is the largest component.

Properties that depend only on solute particle number, not their identity.

The amount of solute (in moles) per kilogram of solvent; m = moles of solute/kg of solvent.

Liquids that can mix completely to form a homogeneous solution.

Describes the direct relationship between gas solubility and the gas pressure above the solution.