States of matter Flashcards
What are the 3 states of matter?
solid, liquid and gas
state the properties of a solid
fixed vol and shape
high density
atoms vibrate in position but can’t change location
atoms packed very closely together and in a fixed position
state properties of a liquid
fixed vol but can adapt shape of a container
less dense than solids but much denser than gases
density is medium
particles move and slide past eachother= this is how they adopt the shape of a container
state properties of a gas
no fixed vol and adapt shape of a container
low density
can be compressed into a much smaller volume due to the spaces in between particles
particles are futher apart and move quickly causing collusions
they collide with eachother
How strong the forces are between particles depend on what?
the material
the temp
the pressure
What is melting?
solid changing into a liquid
requires heat energy in which transforms into KINESTIC energy so that particles are allowed to move
happens in a specific temp- melting point
what is boiling?
liquid to gas
requires heat which causes bubbles of gas found below the surface of the liquid
occurs at a specific temp- boiling point
what is freezing?
liquid to solid
reverse of melting and happens at the same temp as melting because THE MELTING AND FREEZING POINT OF A PURE SUBSTANCE IS THE SAME
required loss of thermal energy
happens in a specific temp
What is evapouration?
liquid to gas
happens in a range of temperatures
when does eveporation only occur?
in the surface of a liquid where high energy particles can escape
the larger the what in evaporation the quicklier?
the larger the surface area and the warmer the surface of the liquid surface
What is condensation?
gas into a liquid
takes place in range of temperature
explain condensation with the theory of particles
as gas is cooled, particles begin to loose more energy= when they collide with eachother they lack energy to bounce again, instead they come together and form a liquid
what is the kinetic theory of matter?
when substances are heated, particles absorb the thermal energy which is then converted into kinetic energy
what does a heating curve demonstrate?
demonstrates states and state changes aswell as time progresses
What are the effects of temperature and pressure
on the volume of a gas
as temperature increases, gas volume increases
density increases as volume increases
Give two examples to demonstrate the effects of temperature and pressure on the volume of a gas
A hot air ballon: as air inside the ballon is heated, it expands and ballon gets bigger and as density decreases, the more up it’ll go
gas syringe covered with a finger you compress it and there will be a point where yo can’t anymore bcs there’s air
Explain, in terms of kinetic particle theory, the
effects of temperature and pressure on the
volume of a gas
increase of temperature means an increase of kinetic energy of each particle, and as the heat is transformed into kinetic energy, they move faster
decrease in volume=increase of pressure
gaseous particles are..
constant and in random motion
How is the pressure that gas created inside a closed container created
by gaseous particles hitting the inside walls of the container
What happens when there is a decrease in volume in a gas container
it increases the pressure
Describe and explain diffusion in terms of kinetic
particle theory
Diffusing particles move from an area of high concentration to an area of low concentration, eventually leading to an equilibrium since concentration of particles spread evenly out to occupy available space
Does diffusion use kinetic energy/ any type of energy? Is there any input energy required too? Explain
Happens on it’s own and no energy input is required ALTHOUGH diffusion takes place in a higher rate in higher temperatures
Describe and explain the effect of relative
molecular mass on the rate of diffusion of gases
the lighter the relative mass= the faster the rate of diffusion will happen
Give an example of an experiment where diffusion is seen
Potassium Magnate (VII) and water
beaker of water and place potassium magnate (VII) at the bottom, you will remark that purple will start to spread out among particles of water.
RANDOM MOTION of particles causes the evenly spread of particles to happen.
Does diffusion occur faster in gases or liquids? Why
Gases because the particles move much quicker than liquid particles
Why do gases not diffuse at the same rate in the same temperature? Give an example
This is due to the difference in their relative atomic masses
Lighter gas particles move faster and hence further just because they have lower relative mass so they will diffuse faster
Ammonia gas in Hydrogen chloride gas inside a long glass tube
NH3 and HCL
Where the two gases meet the white ring will form, it will actually form nearest to the end with HCL because the Mr of ammonia is 17 and HCL is 36.5 meaning that NH3 is much lighter so diffusion rate is faster.
What happens when you add more water to a solution with Potassium magnate (VII) which has already diffused in the beaker evenly?
Particles of Potassium magnate will spread even further apart and solution will become less purple. =Dilute
