Intermolecular Forces & Properties of Liquids – Chapter 11 Review

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Vocabulary flashcards summarizing key terms and definitions from Chapter 11 sections on states of matter, intermolecular forces, and liquid properties.

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39 Terms

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Intermolecular Forces (IMFs)

Attractive forces between separate particles (atoms, ions, or molecules) that influence physical properties of liquids and solids.

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van der Waals Forces

Collective term for all intermolecular attractions other than covalent or ionic bonding: dipole-dipole, dipole-induced dipole (Debye), and London dispersion forces.

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Coulomb’s Law

Electrostatic force between two charges is proportional to the product of the charges and inversely proportional to the square of the distance between them (F = –k q₁q₂ / d²).

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Ion–Ion Attraction

Strong electrostatic force between oppositely charged ions; dominates in ionic solids and gives high melting/boiling points.

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Ion–Dipole Force

Attraction between an ion and a polar molecule’s permanent dipole; strength increases with ion charge, dipole magnitude, and proximity.

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Enthalpy of Hydration (ΔₕydrH°)

Heat released when gaseous ions dissolve in water; becomes more exothermic with higher ion charge and smaller ion radius.

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Dipole–Dipole Force

Attractive interaction 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 in which H bonded to N, O, or F is electrostatically attracted to a lone pair on N, O, or F of a neighboring molecule (5–30 kJ mol⁻¹).

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Debye Force

Dipole-induced dipole attraction created when a polar molecule induces a dipole in a non-polar molecule.

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London Dispersion Force

Induced dipole–induced dipole attraction arising from instantaneous electron cloud distortions; present in all particles and increase with molar mass and polarizability.

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Polarizability

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

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Volatility

Tendency of a liquid to evaporate; liquids with weak intermolecular forces and high vapor pressures are more volatile.

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Enthalpy of Vaporization (ΔvapH°)

Energy required to convert 1 mol of liquid to vapor at its boiling point; always positive (endothermic).

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Enthalpy of Condensation

Energy released when 1 mol of vapor becomes liquid; equal in magnitude and opposite in sign to ΔvapH°.

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Vaporization (Evaporation)

Process by which molecules escape the liquid surface to enter the gas phase; requires energy input to overcome IMFs.

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Condensation

Process by which gas molecules lose energy and return to the liquid phase; exothermic.

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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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Boiling Point

Temperature at which a liquid’s vapor pressure equals the external pressure.

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Normal Boiling Point

Boiling temperature of a liquid when the external pressure is 760 mm Hg (1 atm).

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Clausius–Clapeyron Equation

ln P = –ΔvapH°/RT + C ; relates vapor pressure to temperature and enables calculation of ΔvapH° from P–T data.

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Critical Temperature (Tc)

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

Single homogeneous phase above Tc and Pc with density like a liquid and viscosity like a gas.

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Surface Tension

Energy required to increase a liquid’s surface area by one unit; results from net inward cohesive forces on surface molecules.

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Capillary Action

Rise or depression of a liquid in a narrow tube resulting from competing adhesive and cohesive forces.

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Meniscus

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

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Viscosity

Resistance of a liquid to flow; increases with stronger intermolecular forces or molecular entanglement and decreases with temperature.

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Like Dissolves Like

Rule of thumb stating that solubility is favored when solute and solvent have similar polarity and intermolecular forces.

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Dipole Moment (Debye)

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

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Induced Dipole

Temporary dipole created when an external electric field or neighboring dipole distorts an electron cloud.

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Hydration Shell

Arrangement of solvent (commonly water) molecules surrounding and stabilizing an ion via ion–dipole forces.

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Hydrogen Bond Donor

Molecule or group containing H bonded to N, O, or F capable of forming a hydrogen bond.

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Hydrogen Bond Acceptor

Electronegative atom (N, O, or F) with a lone pair that can attract the H of a neighboring molecule in hydrogen bonding.

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Tetrahedral Ice Lattice

Open, hexagonal arrangement in solid water where each H₂O forms four hydrogen bonds, giving ice lower density than liquid water.

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Specific Heat Capacity of Water

4.184 J g⁻¹ K⁻¹; unusually high because energy must disrupt extensive hydrogen-bond network to raise temperature.

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Polar Molecule

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

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Non-Polar Molecule

Molecule with symmetrically distributed charge and no permanent dipole; interactions are dominated by London forces.

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Dynamic Equilibrium

Condition in which two opposing processes occur at equal rates, leading to constant macroscopic properties (e.g., liquid ↔ vapor).

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Critical Point

Specific combination of critical temperature and critical pressure where liquid and gas phases become indistinguishable.