Unit 2: Physical Properties of Matter Flashcards
what are the 3 phases?
- gas
- liquid
- solid
what are physical properties?
characteristics of a substance that can be determined without altering the substance
what are characteristic properties?
properties that remain the same regardless of the amount of the substance
list examples of physical properties
- length
- mass
- temperature
- color
- shape
- texture
- phase
list examples of characteristic properties
- density
- melting point
- boiling point
what are the 3 types of motion?
translational, rotational, vibrational
describe the motion of gas particles
mainly translational
some rotational and vibrational
describe the motion of liquid particles
vibrational and rotational
some translational
describe the motion of solid particles
mainly vibrational
some rotational
no translational
what is kinetic energy and what is the formula for it
the energy based on the motion of the particle(s) involved
KE = 1/2 mv^2
what is potential energy?
- energy based on the position of state of matter
- depends on the forces (IMF) acting on it
KE is related to __________
PE is related to __________
KE is related to temperature
PE is related to phase
describe the correlation between KE and temperature
- it is a direct correlation
- an increase in temperature leads to an increase in motion which leads to an increase in KE
considering a change in phase from solid to gas, is it an endothermic or exothermic process?
it is endothermic
from solid to gas, does the negative potential energy increase or decrease?
the negative potential energy decreases
what is an exothermic change?
when energy is removed from matter
what is an endothermic change?
when energy is added to the matter
what is heat of fusion?
how much energy needs to be added in order to change the state between solid and liquid
what is heat of vaporization?
the amount of energy required to turn the liquid substance into a gaseous substance
which is greater? heat of vaporization or heat of fusion and why?
heat of vaporization > heat of fusion
this is because more heat energy is required to break the individual IMF to turn a liquid into a gas
the _____ the slope, the ____ the SHC
the steeper the slope, the lower the SHC
state 3 characteristic of high SHC materials
- heat up and cool down at a slower rate
- requires more heat to raise its temperature by a specific amount
- can absorb a great amount of heat
during a phase change, what happens to the KE and PE?
KE doesn’t change
PE increases
during heating, what happens to the KE and PE?
KE increases
PE doesn’t change
what are the 5 points of KMT?
- the gas consists of objects with a defined mass and zero volume
- the gas particles travel randomly in straight-line motion where their movement can be described by the fundamental laws of mechanics
- all collisions involving gas particles are elastic; the KE among the particles is redistributed
- the gas particles don’t interact with each other or with the walls of any container
- the gas phase system will have an average KE that is proportional to temperature; the KE will be distributed among the particles according to a Boltzman type of distribution
read how a galileo thermometer works
what cab you use to illustrate the effect of heat on a solid in regards to volume
the ball and ring apparatus
what is boiling point
the KE needed to make the particles break their bonds
read how a drinking bird works
what is a vapour?
the gas that escapes from a liquid
what is vapour pressure?
the pressure the gas that escapes from a liquid exerts
what type of correlation does vapour pressure have with temperature?
a direct correlation
when does boiling point occur on a vapour pressure curve?
when there is a match between the vapour pressure of the liquid and the atmospheric pressure
what 2 factors hold back a particle that is trying to escape into the gas phase?
- the IMF between the particles
- the atmospheric pressure (usually more important)
