Chapter 7- Solids and Liquids
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64 Terms
Q: What are intermolecular forces?
A: Attractive or repulsive forces between neighboring molecules that determine physical properties like boiling point, melting point, solubility, and density.
Q: What are intramolecular forces?
A: Forces within a molecule that hold atoms together, including covalent, ionic, metallic, and hydrogen bonds.
Q: Which is stronger: intermolecular or intramolecular forces?
A: Intramolecular forces are always stronger.
Q: What are the three major intermolecular forces?
A: London Dispersion Forces (LDFs), dipole-dipole interactions, and hydrogen bonding.
Q: What are London Dispersion Forces?
A: Weak, temporary attractions caused by transient dipoles from uneven electron distribution. Present in all molecules.
Q: How does molecular size affect LDFs?
A: Larger molecules have stronger LDFs due to larger electron clouds.
Q: What are dipole-dipole forces?
A: Attractions between permanent dipoles of polar molecules.
Q: What creates a permanent dipole?
A: Atoms with different electronegativities creating an asymmetric charge distribution.
Q: How does polarity affect dipole-dipole strength?
A: More polar molecules have stronger dipole-dipole forces.
Q: What are hydrogen bonds?
A: Strong dipole-dipole interactions involving H directly bonded to N, O, or F.
Q: Relative strength of IMFs?
A: Hydrogen bonding > Dipole-dipole > London dispersion forces.
Q: How do IMFs affect boiling point?
A: Stronger IMFs lead to higher boiling points.
Q: How does molecular shape affect boiling point?
A: Branched molecules have lower boiling points due to reduced surface area.
Q: What is a polar covalent bond?
A: Unequal sharing of electrons between nonmetals with different electronegativities.
Q: What IMFs do polar covalent compounds exhibit?
A: Dipole-dipole interactions and LDFs.
Q: What is a nonpolar covalent bond?
A: Equal sharing of electrons between atoms with similar electronegativities.
Q: What IMFs exist in nonpolar covalent compounds?
A: Only LDFs.
Q: What is an ionic bond?
A: Complete electron transfer between a metal and a nonmetal.
Q: What is a metallic bond?
A: Metal cations surrounded by a sea of delocalized valence electrons.
Q: What is fusion?
A: Solid → liquid; endothermic; heat absorbed; decreased organization.
Q: What is crystallization?
A: Liquid → solid; exothermic; heat released; increased organization.
Q: What is vaporization?
A: Liquid → gas; endothermic.
Q: What is condensation?
A: Gas → liquid; exothermic.
Q: What is sublimation?
A: Solid → gas without liquid phase.
Q: What is deposition?
A: Gas → solid without liquid phase.
Q: Are phase changes physical or chemical?
A: Physical changes.
Q: What is entropy (S)?
A: A measure of disorder or randomness.
Q: What does a positive ΔS mean?
A: Increased disorder.
Q: What is enthalpy (H)?
A: Heat content of a system at constant pressure.
Q: What does ΔH > 0 indicate?
A: Endothermic process.
Q: What does ΔH < 0 indicate?
A: Exothermic process.
Q: What is a state function?
A: A property depending only on initial and final states, not the path.
Q: Which is greater: ΔH_vap or ΔH_fus?
A: ΔH_vap > ΔH_fus.
Q: Which is greatest: ΔH_sub, ΔH_vap, or ΔH_fus?
A: ΔH_sub is greatest.
Q: What is ΔH°f?
A: Enthalpy change when 1 mole of a compound forms from elements at STP.
Q: What is ΔH°f for elements in standard state?
A: 0 kJ/mol.
Q: Axes of a phase diagram?
A: Temperature (x-axis), Pressure (y-axis).
Q: What is the fusion curve?
A: Solid-liquid boundary.
Q: What is special about water’s fusion curve?
A: It has a negative slope.
Q: What is the vaporization curve?
A: Liquid-gas boundary.
Q: What is the sublimation curve?
A: Solid-gas boundary.
Q: What is the triple point?
A: All three phases coexist.
Q: What is the critical point?
A: Liquid and gas become indistinguishable.
Q: What is a supercritical fluid?
A: Substance beyond the critical point.
Q: Shape and volume of liquids?
A: Definite volume, no fixed shape.
Q: What is miscibility?
A: Ability of liquids to mix uniformly.
Q: What is surface tension?
A: Resistance of a liquid surface to external force.
Q: How does temperature affect surface tension?
A: Higher temperature lowers surface tension.
Q: What is viscosity?
A: Resistance to flow.
Q: How does temperature affect viscosity?
A: Increasing temperature decreases viscosity.
Q: What is vapor pressure?
A: Pressure exerted by vapor above a liquid in equilibrium.
Q: Shape and volume of solids?
A: Definite shape and volume.
Q: What are the four types of solids?
A: Ionic, metallic, covalent network, molecular.
Q: Properties of ionic solids?
A: Hard, brittle, high melting points, nonconductive.
Q: Properties of metallic solids?
A: Malleable, ductile, conductive, lustrous.
Q: Properties of covalent network solids?
A: Very hard, high melting points, nonconductive.
Q: Properties of molecular solids?
A: Soft, low melting points, held by IMFs.
Q: What are crystalline solids?
A: Solids with long-range ordered unit cells.
Q: What are amorphous solids?
A: Solids with no long-range order (e.g., glass).
Q: Atoms per simple cubic unit cell?
A: 1 atom.
Q: Atoms per body-centered cubic unit cell?
A: 2 atoms.
Q: Atoms per face-centered cubic unit cell?
A: 4 atoms.
Q: What happens when temperature decreases in a sealed liquid container?
A: Fewer gas molecules due to decreased vapor pressure.
Q: How do you determine formula from unit cell composition?
A: Count fractional atom contributions from corners, faces, and center.
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