LESSON 3 CHEM - PROP OF LIQUIDS Flashcards
- resist penetration
- can act like skin
- directly correlated to intermolecular attraction
- result to an inward pull among the molecules
- strong attractions between water that pulled slightly toward
- tightness across the surface
- polar molecules repelling each other
- causes raindrops to form beads
- insects “skate”
SURFACE TENSION
HIGH SURFACE TENSION
stronger IMFA
LOW SURFACE TENSION
weaker IMFA
the ability of liquids to flow
FLUIDITY
thickness or resistance to flow of a liquid
VISCOSITY
VISCOUS
HIGH VISCOSITY, SLOW FLOW
FLUID
LOW VISCOSITY, FAST FLOW
MEASURES THE TIME OF A LIQUID TO FLOW
VISCOMETER
Tendency polar of liquids to rise against gravity into small fine tubes (a capillary)
CAPILLARITY
IMF within the liquid molecules
COHESIVE FORCES
Forces between the liquid molecules and the walls of the tube
ADHESIVE FORCES
The upper surface of a liquid in a tube is called the
meniscus
WATER - Meniscus is concave
(Curved upward/inward) because adhesive forces are greater than cohesive forces.
MERCURY - Meniscus is convex
(curved downward/outward) because cohesive forces are greater than adhesive forces.
It explains how water moves against the force of gravity.
* It is due to the attraction among molecules of water and surrounding materials.
* It prevents water from moving through materials with pores.
* It causes clothing to stay dry.
Capillarity
- Liquids can dissolve solids and other liquids and gases.
- Dissolve: when a solid, liquid, or gas becomes integrated into a host liquid (solvent)
- Particles become evenly dispersed among liquid particles
Miscibility
- MISCIBLE LIQUIDS
- Dissolve in each other
- IMMISCIBLE LIQUIDS
- Cannot dissolve in each other
- Particles remain separate
- The equilibrium pressure of a vapor above its liquid (or solid)
- The pressure of the vapor resulting from evaporation of a liquid (or solid) above a sample of the liquid (or solid) in a closed container
- Depends on the magnitude of the intermolecular forces present and on the temperature
Vapor pressure
HIGH VAPOR PRESSURE
volatile (easily evaporated) because of WEAK IMF
* Examples: acetone and alcohol
LOW VAPOR PRESSURE
non-volatile (not easily evaporated) because of STRONG IMF
* Examples: honey and molasses
- The ____________ of a liquid at a given temperature is determined by it intermolecular forces of attraction
VOLATILITY
When liquid particles gain enough KE to overcome IMF, the liquid becomes gas.
When liquid particles lose energy so that the IMF become strong enough to hold the particles in fixed positions, the liquid becomes a solid.
- Freezing: KE < IMF
- Melting: KE > IMF
- Condensation: KE < IMF
- Boiling: KE > IMF
is the rapid phase change of a liquid becoming a gas.
BOILING
VAPOR PRESSURE=ATMOSPHERIC PRESSURE
BOILING POINT
The higher the boiling point,
the stronger the IMFA.
a change of state from liquid to gas.
VAPORIZATION
is the energy required to vaporize 1 mole of a liquid at its boiling point.
Molar heat of vaporization
- The amount of heat needed to vaporize a given amount of liquid at its boiling point is called .
heat of vaporization
The stronger the IMF,
the higher the heat of vaporization is.
