1. HEAT
thermal energy

2. Kinetic Theory of Matter
States the following three points
1. Matter is composed of extremely small particles called atoms
2. These particles are in constant, random motion
3. The movement of the particles determines the phase of matter the substance is in

3. Matter/Energy Connection
The warmer the object, the more kinetic energy it has
The cooler, the lower the kinetic energy
As you heat or cool something it changes its phase because it changes the kinetic energy

4. Thermal Energy Is actually the average kinetic energy of a system
A system can be an object or the atmosphere in a room or... Anything

6. Temperature It is a way of telling how warm or cold something is
It is, in actuality, a measure of the kinetic energy of the system
So if we check the temperature in a room we are actually measuring the motion of the molecules and atoms in the atmosphere of the room

7. Temperature Scales Theoretically there is no upper limit to heat
Matter will keep changing phases Until it reaches the plasma phase
Stars are plasma, they have temperatures in the millions of degrees
There is a limit to low temperature though

8. Absolute zero this is the theoretical temperature at which every bit of kinetic energy from the atoms and sub-atomic particles has been removed
It cannot get any colder
Absolute zero is equal to -273 C

10. What is heat?
Heat is the thermal energy transferred from one object to another or thermal energy in transit
Thermal energy flows from warmer to cooler objects until equilibrium is reached

11. What is cold? Cold is not a thing It is not a type of energy
It is a lack of thermal energy or very low thermal energy
Something feels cold to you because you are losing heat to it

12. Ice is cold because the particles of water have very low kinetic energy and the particles of your finger have a higher kinetic energy
so, thermal energy transfers from you to the ice. You lose heat.

13. Laws of Thermodynamics
First Law
When heat is transferred it does so without a net loss or gain
This means that whatever is lost from one place is gained in another

14. Second Law
Heat never spontaneously flows from a cold substance to a hot substance
Third Law
No system can reach a temperature of absolute zero

15. Specific Heat Capacity
This is defined as the quantity of heat required to change a unit mass of a substance by 1 C.
Different substances have different capacities for storing thermal energy

16. Water has a very high capapcity for storing heat
A lot of heat is needed to change the temperature of water
Water also takes longer to cool

17. Specific heat equation
Q = mcΔT
Q = heat transferred
m = mass
c = specific heat
ΔT = change in temperature (Tfinal – Tinitial)

18. Heat Transfer There are three types of heat transfer 1. Conduction
When heat travels from the hot end of an object, through the length of the object, to the cooler end.
This happens due to particles in the object heating up, colliding with particles next to them amd transferring energy

19. 2. Convection Heat transferred by the motion of a fluid
These are called convection currents
Cooler things ae more dense, so they settle at the bottom. This forces warmer objects up, causing currents

20. 3. Radiation
This is when heat is transferred without a medium to travel through. It is neither conduction or convection.
It is a form of electromagnetic waves
This is how heat from the sun travels through the vacuum of space to get to earth
The higher the frequency of the wave, the higher the energy transfer

22. Thermal Expansion This one is easy
As objects heat up, their molecules move faster
This leads to more outward movement
The net result is an expansion of the heated object
Objects contract when they cool off