Energy in all forms

Thermodynamics is the study of energy transformations. In physics, energy is defined as the ability to do work(work=force/distance). Although we are unable to see or directly measure energy, we know that energy has the ability to make things happen. Two common forms of energy in chemistry are kenetic energy, the energy of motion, and potential energy, or stored energy.

Kinetic energy- energy of motion KE=1/2mv^2
Radiant energy- energy from the sun or solar energy
Thermal energy-energy associated with random motion of atoms and molecules
Chemical energy-energy stored within the structural units of chemical substances
Potential energy-energy stored or energy of position

Cooling and heating

Change of state is a physical change where intermolecular bonds are broken. Melting and boiling points are determined by vapor pressures of the solid and liquid states. At 0 degrees Celsius, ice and liquid water have the same vapor pressure. At 100 degrees Celsius, water vapor and atmospheric pressure are equal.

Super cooling is cooling of liquid below freezing point and it occurs when the particles lack the internal arrangement to solidify at freezing point.

Super heating is heating of a liquid is raised above its boiling point and it occurs when vapor bubbles fail to form and it may suddenly boil violently when vapor bubbles do form.
http://hyperphysics.phy-astr.gsu.edu/hbase/thermo/phase.html
http://hyperphysics.phy-astr.gsu.edu/hbase/thermo/watice.html
https://www.chem.wisc.edu/deptfiles/genchem/netorial/rottosen/tutorial/modules/intermolecular_forces/02imf/imf2.htm
http://zonalandeducation.com/mstm/physics/mechanics/energy/heatAndTemperature/changesOfPhase/changeOfState.html
http://zonalandeducation.com/mstm/physics/mechanics/energy/heatAndTemperature/changesOfPhase/changeOfState.html
http://www.shmoop.com/matter-properties/phase-change.html