States of matter

Solid

-Particles are touching each other

-Regular arrangement

-Cannot change positions and can only vibrate

Liquid

-Particles are close to each other

-Fairly random arrangement

-Have limited movement and can slide past each other

Gas

-Particles are far apart from each other

-Random arrangement

-Can move freely in all directions

Kinetic theory of gas

The idea that molecules in gases are in constant movement.

Assumptions:

-The gas molecules move rapidly and randomly

-The distance between the gas molecules is much greater than the diameter of the molecules so the volume is negligible

-There are no forces of attraction or repulsion between the molecules

-All collisions are elastic

-The temperature of the gas is related to the average kinetic energy of the molecules

Ideal gas vs Real gas

Most likely in:

-Low pressures, distance between particles is large therefore volume and intermolecular forces are negligible.

-High temperature, negligible intermolecular forces due to having sufficient kinetic energy that can overcome intermolecular forces

Most likely in:

-High pressures, particles are closely packed together thus volume is relevant

-Low temperature, particles are closely packed together and have insufficient kinetic energy thus intermolecular forces are relevant

However, an ideal gas does not exist because intermolecular forces are present and volume occupied is not zero

General equation

P=pressure, pa

V=volume, m^3

n=no of moles of gas

R=constant( 8.31JK^-1mol^-1)

T=temperature, K

Here are a list of videos for better understanding

Ideal gas vs Real gas

Equations and Graphs

Kinetic Theory

Structures

Giant metallic lattice and alloy

Giant ionic lattice

The liquid state

Melting

Melting is the change of state of solid to liquid at a specific temperature called the melting point. Particles vibrate more vigorously

Freezing

Freezing is the change of liquid to solid, the particles lose energy until they do not have enough energy to move freely

Boiling

Boiling is the change of state from liquid to gas at a specific temperature called boiling point. Upon heating, the vapour pressure will increase and eventually becomes equal to the vapour atmospheric pressure, bubbles of vapour then form and rise to the surface bursting open and escaping into the atmosphere as a gas.

Condensation

Condensation is the change of state from gas to liquid. The reverse happens in the process of boiling

Evaporation

Evaporation is a type of vaporization that occurs on the surface of a liquid as it changes into the gas phase. The surrounding gas must not be saturated with the evaporating substance. When the molecules of the liquid collide, they transfer energy to each other based on how they collide with each other.

Vapour pressure

Vapour pressure is a pressure that is exerted by collisions of the wall with particles that have higher energy. As more particles escape, the vapour particles become close together and particles with lower energy will not be able to overcome the attractive forces causing them to condense and return to liquid.