Intermolecular Forces and Properties of Liquids – Chapter 11

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Vocabulary flashcards covering key terms and definitions related to intermolecular forces, molecular interactions, and liquid properties from Chapter 11.

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38 Terms

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Intermolecular Forces (IMFs)

Attractive or repulsive forces between molecules, ions, or atoms that are not covalently bonded; collectively called van der Waals forces.

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van der Waals Forces

General term for all intermolecular forces excluding covalent and ionic bonding; includes dipole–dipole, dipole–induced dipole, and London dispersion forces.

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Coulomb’s Law

Equation (F = −k q1 q2 / d²) describing the electrostatic force between two charges; magnitude increases with larger charges and shorter distance.

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Ion–Ion Attraction

Strong electrostatic force between oppositely charged ions in ionic solids, leading to high melting and boiling points.

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Ion–Dipole Force

Attractive force between an ion and a polar molecule; strength increases with ion charge, smaller ion size, and larger dipole moment.

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Dipole–Dipole Force

Attraction between the positive end of one polar molecule and the negative end of another polar molecule.

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Hydrogen Bond

Special, strong dipole–dipole attraction where H is covalently bonded to N, O, or F and forms a bridge to another electronegative atom.

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Dipole–Induced Dipole Force (Debye Force)

Attractive force where a permanent dipole in one molecule induces a temporary dipole in a nearby non-polar molecule.

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Induced Dipole–Induced Dipole Force

Also called London dispersion force; temporary attractions arising from synchronized electron motions in neighboring non-polar molecules.

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London Dispersion Force

Weak, universal IMF caused by momentary fluctuations in electron density; strength increases with molar mass and polarizability.

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Polarizability

Ease with which an electron cloud can be distorted to form an induced dipole; larger, more diffuse clouds are more polarizable.

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Hydration Enthalpy (ΔhydrH⁰)

Heat released when an ion is solvated by water molecules; becomes more exothermic with higher ion charge and smaller ionic radius.

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Enthalpy of Vaporization (ΔvapH⁰)

Energy required to vaporize 1 mole of a liquid at its boiling point; endothermic and proportional to IMF strength.

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Enthalpy of Condensation

Heat released when 1 mole of vapor condenses to liquid; numerically equal but opposite in sign to ΔvapH⁰.

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Equilibrium Vapor Pressure

Pressure exerted by a vapor in dynamic equilibrium with its liquid at a given temperature.

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Volatility

Measure of a liquid’s tendency to evaporate; high volatility corresponds to high vapor pressure and weak IMFs.

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Normal Boiling Point

Temperature at which a liquid’s vapor pressure equals 760 mm Hg (1 atm).

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Clausius–Clapeyron Equation

ln P = −ΔvapH⁰ / (R T) + C; relates vapor pressure to temperature and allows calculation of ΔvapH⁰.

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Critical Temperature (Tc)

Highest temperature at which a substance can exist as a liquid, regardless of applied pressure.

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Critical Pressure (Pc)

Minimum pressure required to liquefy a gas at its critical temperature.

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Supercritical Fluid

State of matter above Tc and Pc where liquid and gas phases merge; combines gas-like viscosity with liquid-like density.

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Surface Tension

Energy required to increase a liquid’s surface area by one unit; caused by unequal IMF on surface molecules.

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Capillary Action

Rise or fall of a liquid in a narrow tube due to competition between adhesive and cohesive forces.

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Meniscus

Curved surface of a liquid in a container; concave for liquids that wet glass (e.g., water), convex for those that do not (e.g., mercury).

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Cohesive Forces

Intermolecular attractions between like molecules within a liquid.

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Adhesive Forces

Intermolecular attractions between unlike molecules, such as a liquid and a solid surface.

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Viscosity

Resistance of a liquid to flow; increases with stronger IMFs and decreases with higher temperature.

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States of Matter

Physical forms of matter—solid, liquid, gas—distinguished by particle spacing and IMF influence.

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Hydrogen-Bond Network in Water

Each H₂O molecule can form four H-bonds, giving water high boiling point, high specific heat, and lower-density ice.

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Dipole Moment (Debye, D)

Quantitative measure of molecular polarity; product of charge magnitude and separation distance.

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Like Dissolves Like

Rule of thumb stating polar solvents dissolve polar solutes, and non-polar solvents dissolve non-polar solutes due to compatible IMFs.

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Polar Molecule

Molecule with an uneven distribution of charge resulting in a permanent dipole moment.

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Non-Polar Molecule

Molecule with a symmetrical charge distribution and no permanent dipole moment.

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Debye (unit)

Unit (D) used to express dipole moments; 1 D ≈ 3.34 × 10⁻³⁰ C·m.

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Hydrated Salt

Ionic compound containing specific numbers of water molecules bound in its crystal lattice, often via ion–dipole interactions.

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Specific Heat Capacity of Water

4.184 J g⁻¹ K⁻¹; unusually high due to extensive hydrogen bonding, moderating Earth’s climate.

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Polarizability Trend

In homologous series, polarizability—and thus dispersion forces—increases with increasing molar mass and electron count.

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Dynamic Equilibrium (Liquid–Vapor)

Condition where rate of evaporation equals rate of condensation, resulting in constant vapor pressure.