-
Density
- the mass of matter divided by its volume
- greater mass greater density- directly proportional
- density and volume are inversly proportional
- D=m/v
-
Shape
is it fixed or does it take the shape of the container
-
Compressiblity
if we apply pressure, does the volume decrease?
-
Thermal expansion
- how much does the volume change when heated?
- Review table 6:1 on pg 168
-
Kinetic Molecular Theory
- Matter is composed of small particles
- each particle is in constant motion (kinetic energy)
- particles contain potential energy due to attractions and repulsions between them
- particles move faster as the temp. increases
- particles transfer energy during a collision with no net energy change
- Kinetic energy (KE)= 1/2mv2(m=mass, v=valucity)
-
Interatomic forces
- dipole- dipole
- Van der Waal's Forces
- Hydrogen Bonding
-
solids at room temp:
- 1. are not compressible
- 2.have regular repeating units
-
Two types of solids observed
- 1.crystalline solids- crystal latus structure
- 2.amorphous solid- no specific shape
-
Types of Solids
- 1.ionic solids
- 2.covalent solids
- 3.metallic solids
- 4.molecular solids
-
The liquid state
- As a result of the forces that hold a liquid together, several properties are observed
- 1.viscosity- doesn't want to flow
- 2.surface tension
- 3.vapor pressure
- 4.boiling points
-
The Gas Laws
- Sinces gases are highly compressible and will expand when heated interesting relationships exist
- these relationships between volume (V), pressure (P), temp (T) and moles (N), are referred to as the gas law; (R)= gas law constant
-
Gas Pressure
- pressure is defined as force per unit area
- P=F/A; pressure= force/ area
-
Units of Pressure
- 1.Atmosphere
- 2.Torr or mmHg
- 3.Inches of Hg
- 4.lbs/ square inch
- 5.kilopascals
-
STP
standard temp and pressure
-
Standard Pressure: mm of Hg and torr
760
-
Standard Pressure: lbs/in2
14.7
-
Standard Pressure: kilopascals
101.325
-
Standard Pressure: atmosphere
1
-
conversion of standard pressure
new pressure= old p (new SP/ old SP)
-
Boyle's Law
- the volume of a dry gas is inversely proportional to the pressure exerted upon the gass if the temp remains the same
- P1V2=P2V1
-
Charle's Law
- the volume of a dry gas is directly proportional to the Kelvin temp. if the pressure exerted upon the gas remains constant
- K1V2=K2V1
-
Combined Gas law
P1V1T2=P2V2T1
-
Avogadro's Law
- equal volumes of gases at the same temp. and pressure contain an equal number of molecules
- V=Kn
-
The Ideal Gas Equation
- the ideal gas is a hypothetical gas whose pressure, volume, and temperature behavior is completely described by the ideal gas equation
- PV=nRT
-
Dalton's Law
- the total pressure exerted by a mixture of different gases kept at a constant volume and temp. is equal to the sum of the partial pressures of the gases in the mixture
- the partial pressure is the pressure each gas would exert if it were confined done under the same temp and volume condition as the mixture
- *Pt=P1+P2+P3...etc.
-
Graham's Law
- the rate of effusion of 2 gases is inversely proportional to the square root of their masses
- rate a/rate b= square root mass a/ mass b
-
specific heat
the amount of heat energy required to raise the temp of 1 gram of a substance 1 celsius
-
unit used in specific heat
calories or joules per gram celcius
-
Specific heat of ice
0.51 cal/gram degree celcius or 2.1 J/g
-
Specific heat of water
1.00 cal/g degree celcius or 4.18 J/g degree celcius
-
Specific heat of steam
0.48 cal/g degree celcius or 2.00 J/g degree
-
Heat fusion
- the amount of energy required to melt 1 gram of a substance (contstant temperature)
- for water 80 cal/g
-
Heat Vaporization
- the amount of energy required to vaporize 1 gram of a substance at a constant temperature
- for water 80 cal/g
|
|
