Chapter 10- States Of Matter Flashcards
Particles of matter are
Always in motion
Kinetic molecular theory
Explains the behavior of atoms/ molecules in different states of matter
Particles exhibit what type of motion
Vibrational, rotational, translational
All movement stops only at
Absolute zero
K = -273 C
Kinetic energy
Measures the amount of energy contained by a moving object
Temperature
Measure of the average kinetic energy of a substance
Kinetic energy equation
KE = 1/2mv^2
At the same temperature, particles of a lower max have a
Higher velocity
STP
Standard temperature
0 degrees C
-273 degrees K
1 ATM
Solids
Typically most dense
Particles are close together
Lowest temperature
Lowest average KE of particles
Liquids
Particles still relatively close together
Temperature and average KE increase from solid state
Gasses
Particles extremely far apart
Lowest density
Highest temperature and average KE
Intramolecular forces
Chemical bonds
Intermolecular forces
Attractions between molecules, strongest in solids
Strength of intermolecular forces
- Hydrogen bonds
- Dipole - dipole attraction
- Dipole induced dipole attraction
- London dispersion forces
Cohesive
Attractive force between two like molecules
Adhesive
Attractive force between two different molecules
Gasses are
Fluids
Fluid
A non solid state of matter in which particles are free to move or flow past each other
gases have
low density and high compressibility
gases readily
diffuse
effusion
process by which gas particles pass through a tiny opening when pressure is exerted on them
the rate of effusion of a gas is directly proportional to
the gas velocity
crystalline solids
particles arranged in ordered, geometric pattern
definite melting point
ionic compounds
amorphous solids
particles arranged randomly
can flow over a wide range of temperatures
4 types of crystalline solids
ionic crystals
covalent network crystals
covalent molecular crystals
metallic crystals
liquids have
surface tension
surface tension
force that tends to pull adjacent parts of a liquids surface together, thereby decreasing surface area to the smallest possible size
capillary action
the attraction of the surface of a liquid to the surface of a solid
volatile
readily vaporizes
melting
solid to liquid
sublimation
solid to gas
freezing
liquid to solid
vaporization
liquid to gas
condensation
gas to liquid
deposition
gas to solid
phase
any part of a system with uniform composition and properties
vapor
a gas in contact with its liquid or solid phase
vapor pressure
the pressure exerted on the surface of the liquid phase by its corresponding vapor
liquid vapor equillibrium
state where the rate of evaporation is equal to the rate of condensation
boiling point
the temperature at which the equilibrium vapor pressure of the liquid equals the atmosphere pressure
normal boiling point
boiling point at 1 atm of pressure
enthalpy
a measure of the total energy of a system
molar enthalpy of vaporization
amount of heat energy needed to vaporize one mole of liquid at the liquids boiling point under constant pressure
molar enthalpy of fusion
the amount of heat energy that must be added to melt one mole of solid at the solids melting point
