This is a draft cheat sheet. It is a work in progress and is not finished yet.
Kinetic Theory
Lighter particles move faster than heavier particles (depends on Mr). |
Gas particles can spread/expand to fill any volume, due to weak intermolecular attraction forces between the molecules. |
Increasing the temperature causes the particles to gain kinetic energy and move faster. |
Increasing the temperature causes the particles to move further apart while decreasing the temperature causes the particles to get closer together. |
For gases, the pressure is due to the collisions of gas particles with the walls of the container. |
For gases, when temperature is increased and the particles move faster, the number of collisions increases, causing the pressure to increase. |
Diffusion
It is the movement of particles from area of high concentration to area of low concentration, until they are evenly spread. |
The rate of diffusion depends on the molecular mass...The smaller the Mr, the faster the rate of diffusion. |
Increasing the temperature increases the speed of molecules and thus, the rate of diffusion increases (particles diffuse in a shorter time). |
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Conversion of Physical States
Checking the state of a substance
Solids |
Melting & Boiling points > room temperature (25°C) |
Gases |
Melting & Boiling points < room temperature (25°C) |
Liquids |
Melting point < room temperature (25°C) < Boiling point |
$ Melting and Boiling points are specific for each substance.
$ Impurities increase the boiling points and decrease the melting points of substances.
$ Impurities have a range/less sharp melting and boiling points.
Heating & Cooling Curves
Temperature does not change during melting and boiling as the energy supplied is used to overcome the attraction forces between molecules.
Comparison between Evaporation & Boiling
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