phases of matter (10) Flashcards
solids (macroscopic)
- have a high density
- have a fixed shape
- have low kinetic energy
- have a fixed volume
- cannot be pressed together
liquids (macroscopic)
- do not have a fixed form ; take the shape of the container
- not hard
- have a high density
- have a fixed volume
- can flow
gas (macroscopic)
- has no fixed form ; spreads to take the form of the container
- not hard
- low density
- can easily be compressed
- can flow
- does not have a fixed volume
describe the relationship of energy and temperature
they are directly proportional, when you increase temperature you increase kinetic energy
explain the melting process
when a solid is heated, it’s particles absorb the heat energy - that heat energy turns into kinetic energy which makes the particles move faster. at the melting point the particles are able to overcome the inter molecular forces ; the particles now slide over one another becoming a liquid
explain the freezing process
- the temperature is decreased therefor heat is released, because the temperature is decreasing so does the kinetic energy which in turn makes the particles move slower and closer together - forces of attraction set up between these particles and they take up a solid form
boiling
- the temperature increases (as well as the heat) hence the kinetic energy increases and the particles move faster therefor the intermolecular forces are overcome turning the liquid to a gas
evaporation
- takes place at temperatures lower than boiling point
- only takes place on the surface if the liquid
- takes place slower
- causes cooling because heat is absorbed out of the environment
boiling (in terms of evaporation vs boiling)
- occurs at boiling point
- occurs throughout the liquid
- quicker then evaporation
- once it boils, temperature stays constant
condensation
- heat energy is released so both temperature and kinetic energy decreases, therefor the particles move slower and closer together - in turn the inter molecular forces become stronger
sublimation
- straight from solid to gas
- particles have enough energy to escape into the gaseous phase
deposition
straight from gas to solid, elements that can sublimate can do this too
A - B (heating curve)
as the temperature increases so does the kinetic energy
B - C (heating curve)
temperature is constant
molecules overcome intermolecular forces and move further apart
C - D (heating curve)
temperature and kinetic energy increase
D - E (heating curve)
temperature and kinetic energy are constant
energy is taken up by molecules and the molecules overcome intermolecular forces and move further apart
E - F (heating curve)
Steam
temperature and kinetic energy increases, molecules move further apart
A - B (cooling curve)
temperature and kinetic energy decrease, molecules move slower and closer together
B - C (cooling curve)
intermolecular become stronger, energy’s is released
temperature and kinetic energy stay constant
C - D (cooling curve)
temperature and kinetic energy decrease, molecules move slower and closer together
D - E (cooling curve)
intermolecular forces are stronger, energy is released
temperature and kinetic energy are constant
E - F (cooling curve)
temperature and kinetic energy decrease
molecules move much slower and it becomes a solid
kinetic molecular theory
- all matter is made up if small particles
- the particles move constantly
- there are spaces between particles
- particles are constantly colliding with each other and the wall
- forces of attraction exist between the particles
solids (microscopic)
space - have small spaces between the particles
energy - low
movement - particles move little and only vibrate in their position
forces of attraction - very strong intermolecular forces
liquid (microscopic)
space - bigger then solids
energy - more then solids less then gas
movement - particles rotate and vibrate simultaneously
forces of attraction - weaker then solids but stronger then gases
gas (microscopic)
space - very big spaces between particles
energy - high
movement - particles can move around freely
forces of attraction - weak to no intermolecular forces
