chapter 10, section 2 liquids. liquids & kinetic-molecular theory 1. liquid particles are...
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Chapter 10, Section 2
LIQUIDS
Liquids & Kinetic-Molecular Theory
1. Liquid particles are closer together than gas particles.
Liquids & Kinetic-Molecular Theory
2. More ordered arrangement than gases.
Liquids & Kinetic-Molecular Theory
3. Attractive forces exist between liquid particles. (Remember: this is not true of ideal gases.) These forces hold liquids
together.
FLUID Liquids, like gases,
can flow and therefore take the shape of their container.
Properties of Liquids
1. Relatively high density.
Properties of Liquids
2. Relative incompressibility
Properties of Liquids
3. Ability to diffuse due to constant random motion. Diffusion is slower
than in gases.
Properties of Liquids 4. Surface Tension: a force
that pulls adjacent parts of a liquid’s surface together, thereby decreasing surface area to the smallest possible size.
Capillary ActionThe attraction of the surface of a liquid to the surface of a solid.
GAS vs VAPOR Vapor refers to the
gaseous state of a substance that is normally a liquid or solid at ROOM TEMPERATURE.
VISCOSITYA measure of a liquid’s resistance to flow.
VAPORIZATION
The conversion of a liquid or solid to a gas or vapor
EVAPORATION Process by which
particles escape from the surface of a NONBOILING liquid and enter the gas state.
Only molecules with KE above a certain minimum amount can escape.
COOLING EFFECTS Molecules with highest
KE escape first. Those left behind have
lower KE; temperature of the liquid decreases.
FREEZING: The physical change of a
liquid to a solid by removal of energy as heat.
As a liquid cools, the KE decreases & particles are pulled together in a more orderly arrangement – a solid.
BOILING:Vaporization (appearance of bubbles) throughout a liquid.
VAPOR PRESSURE
The force exerted by the gas above a liquid in a closed container.
Increasing temperature increases vapor pressure
DYNAMIC EQUILIBRIUM
The point when the rate of evaporation equals the rate of condensation.
BOILING POINT The temperature at
which the vapor pressure of the liquid is just equal to the external pressure.
NORMAL BOILING POINT
The boiling point at 101.3 kPa of pressure
INTERMOLECULAR FORCES
Attraction between molecules.
Generally weaker than bonds in a molecule
3 types of IM forces 1. Dipole-Dipole
Forces 2. Hydrogen bonding 3. London Dispersion
Forces
Dipole-Dipole Forces Strongest IM force Occurs between polar
molecules Equal but opposite charges
separated by a short distance creates a dipole.
Hydrogen Bonding A Hydrogen atom that is
bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule.
Hydrogen bonding (cont.)
H is small; can get very close to the unpaired electrons
Strong intermolecular force Unusually high boiling
points for molecular compounds
London Dispersion Forces
Electrons are constantly moving – can be distributed unequally.
Creates a temporary dipole
Weak forces
London Dispersion Forces
The IM attractions resulting from the constant motion of electrons and the creation of instantaneous temporary dipoles.
London Dispersion Forces
LDF are present between ALL atoms and molecules.
For NOBLE GASES and NONPOLAR MOLECULES, London Dispersion Forces are the ONLY IM force