L1. Liquids and Solids Flashcards
KINETIC MOLECULAR THEORY
- Matter is made of particles that are constantly in __________.
motion
KINETIC MOLECULAR THEORY
- The amount of kinetic energy in a substance is related to its _______________.
temperature
KINETIC MOLECULAR THEORY
- There is _________ between particles.
space
KINETIC MOLECULAR THEORY
- __________ _________ happen when the temperature of the substance changes sufficiently
Phase changes
KINETIC MOLECULAR THEORY
- There are attractive forces in between particles called _________________ _________.
intermolecular forces
PROPERTIES OF MATTER
VOLUME/SHAPE: Assumes volume and shape of container
Gas
PROPERTIES OF MATTER
VOLUME/SHAPE: Fixed volume; assumes shape of occupied part of container
Liquid
PROPERTIES OF MATTER
VOLUME/SHAPE: Fixed volume; fixed shape (regardless of size and shape of container)
Solid
PROPERTIES OF MATTER
DENSITY: Low
Gas
PROPERTIES OF MATTER
DENSITY: High (2)
Liquid and Solid
PROPERTIES OF MATTER
COMPRESSIBILITY: Easy to compress
Gas
PROPERTIES OF MATTER
COMPRESSIBILITY: Cannot be appreciably compressed (2)
Liquid and Solid
PROPERTIES OF MATTER
MOTION OF MOLECULES: Random, fast, cover large distances
Gas
PROPERTIES OF MATTER
MOTION OF MOLECULES: Random, medium speed, limited distances
Liquid
PROPERTIES OF MATTER
MOTION OF MOLECULES: Vibration in place
Solid
These are attractive forces that act between molecules or particles in the solid or liquid states.
Intermolecular Forces
TYPES OF INTERMOLECULAR FORCES
This is a special dipole-dipole interaction between the hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom.
Hydrogen Bond
TYPES OF INTERMOLECULAR FORCES
Attractive forces between an ion and a polar molecule.
Ion–Dipole Forces
TYPES OF INTERMOLECULAR FORCES
Attractive Forces between polar molecules.
Dipole–Dipole Forces
TYPES OF INTERMOLECULAR FORCES
Attractive forces that arise as a result of temporary dipoles induced in atoms or molecules
- Dispersion Forces–London forces
Dispersion forces usually increase with _______ _____.
molar mass
It is the measure of the elastic force in the surface of a liquid. It is the amount of energy required to stretch or increase the surface of a liquid by a unit area.
Surface Tension
Liquids that have strong intermolecular forces also have high _______ ________.
surface tension
This is the tendency of a liquid to rise in narrow tubes or be drawn into small openings such as those between grains of a rock.
Capillary Action
It is the intermolecular attraction between like molecules (the liquid molecules).
Cohesion
It is an attraction between unlike molecules (such as those in water and in the particles that make up the glass tube).
Adhesion
This is a measure of a fluid’s resistance to flow.
Viscosity
The greater the viscosity, the ________ the liquid flows.
slower
Viscosity ____________ as temperature increases: hot molasses flows much ________ than cold molasses.
decreases, faster
This is the pressure exerted by the gas in equilibrium with a liquid in a closed container at a given temperature.
Vapor Pressure
The __________ the number of gaseous particles, the greater the pressure exerted by the gas.
greater
This is the energy required to vaporize 1 mole of a liquid at a given temperature.
Molar Heat of Vaporization (ΔHvap)
It is the symbol for enthalpy, which means heat content at a given standard condition.
H
This is the temperature at which the vapor pressure of a liquid is equal to the external pressure.
Boiling point
What is the normal boiling point of water?
100 ° C
These can form a regular repeating three-dimensional structure called a crystal lattice, which then produces this.
Crystalline Solid
These can aggregate with no particular long range order, which then produces this. (from the Greek ámorphos, meaning “shapeless”).
Amorphous Solid
These are arranged in fixed geometric patterns or lattices. The ordered arrangement of their units maximizes the space they occupy and are essentially incompressible.
Crystalline Solid
This is a three-dimensional system of points designating the positions of the components (atoms, ions, or molecules) that make up a crystal
Lattice
It is the smallest repeating unit of a lattice
Unit Cell
They have a random orientation of particles.
Amorphous Solids
Examples of this kind of solids are glass, plastic, coal, and rubber. They are considered super-cooled liquids where molecules are arranged in a random manner similar to the liquid state.
Amorphous Solid
This is a graphical representation of the physical states of a substance under different conditions of temperature and pressure.
Phase Diagram
The lines that serve as boundaries between physical states represent the combinations of pressures and temperatures at which two phases can exist in equilibrium.
Three Lines (Curves)
It is the combination of pressure and temperature at which all three phases of matter are at equilibrium. It is the point on a phase diagram at which the three states of matter coexist.
The Triple Point
It terminates the liquid/gas phase line. It is the set of temperature and pressure on a phase diagram where the liquid and gaseous phases of a substance merge together into a single phase.
Critical point
