chem 2. chapter 11 liquids & intermolecular forces
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49 Terms
What are intermolecular forces (IMFs)?
Forces of attraction between molecules that determine physical properties like boiling point, melting point, and vapor pressure.
What are the three main types of intermolecular forces?
London dispersion forces, dipole-dipole forces, and hydrogen bonding.
What causes London dispersion forces?
Temporary fluctuations in electron distribution that create temporary dipoles.
Which molecules experience London dispersion forces?
All molecules (polar and nonpolar).
What increases the strength of London dispersion forces?
Larger molar mass and more electrons.
What is a dipole-dipole interaction?
Attraction between polar molecules with permanent dipoles.
What is hydrogen bonding?
A strong dipole-dipole force involving H bonded to N, O, or F.
Why is hydrogen bonding stronger than dipole-dipole?
N, O, and F are highly electronegative and create strong polarity with H.
What is vapor pressure?
Pressure exerted by vapor in equilibrium with its liquid phase in a closed system.
What does high vapor pressure indicate?
Weak intermolecular forces and high volatility.
What does low vapor pressure indicate?
Strong intermolecular forces and low volatility.
What is boiling point?
Temperature at which vapor pressure equals external pressure.
How do intermolecular forces affect boiling point?
Stronger IMFs → higher boiling point.
What is evaporation?
Surface molecules escaping from liquid to gas below boiling point.
What is condensation?
Gas changing into liquid as molecules lose energy.
What is melting?
Solid changing into liquid as intermolecular forces weaken.
What is freezing?
Liquid changing into solid as energy decreases and structure forms.
What is sublimation?
Solid changing directly into gas without becoming liquid.
What is deposition?
Gas changing directly into solid.
What is dynamic equilibrium in phase changes?
Rate of evaporation equals rate of condensation.
What is a phase diagram?
A graph showing phase (solid, liquid, gas) under different temperature and pressure conditions.
What do phase boundaries represent?
Conditions where two phases coexist in equilibrium.
What is the triple point?
The temperature and pressure where solid, liquid, and gas coexist.
What is the critical point?
Point where liquid and gas phases become indistinguishable.
What is a supercritical fluid?
State beyond critical point with properties of both liquid and gas.
How does pressure affect phase changes?
Higher pressure favors the more condensed phase (solid or liquid).
How does temperature affect phase changes?
Higher temperature favors gas phase.
Which has the highest kinetic energy: solid, liquid, or gas?
Gas particles have the highest kinetic energy.
Which has the lowest kinetic energy?
Solid particles.
How are particles arranged in solids?
Tightly packed in fixed positions.
How are particles arranged in liquids?
Close together but able to flow past each other.
How are particles arranged in gases?
Far apart and move freely.
Which state is most compressible?
Gases.
Which state is least compressible? Solids.
Why are gases compressible?
Particles are far apart with lots of empty space.
Why are liquids not easily compressible?
Particles are already close together.
What property defines a liquid’s resistance to flow?
Viscosity.
What increases viscosity?
Stronger intermolecular forces and larger molecules.
What is surface tension?
Resistance of a liquid surface to being stretched or broken.
What causes surface tension?
Strong intermolecular forces at the surface of a liquid.
How does IMF strength affect surface tension?
Stronger IMFs → higher surface tension.
Which has stronger IMFs: gases, liquids, or solids?
Solids generally have the strongest IMFs.
Why do solids have fixed shapes?
Strong intermolecular forces lock particles in place.
Why do liquids take shape of container?
Particles can move but stay close together.
Why do gases fill containers?
Particles move freely and expand.
How does IMF strength affect vapor pressure?
Stronger IMFs → lower vapor pressure.
What is volatility?
How easily a substance evaporates (inverse of IMF strength).
What is the relationship between boiling point and vapor pressure?
Higher boiling point means lower vapor pressure at a given temperature.
What happens at phase equilibrium?
Two phases change at equal rates, no net change occurs.