If you mean what takes place in each transformation between different states of matter then you must first understand the components of each state.
A solid: •The particles cannot move, only vibrate
• The bonds that hold particles close together will be very tight
• The solid will not be able to be deformed due to the fact, that the particles cannot get any closer, and the object will denser than a gas or liquid.
A liquid: • The particles can move past one another but are still held so that they have a fixed volume
• The particles are held together by loose bonds and they can move.
• The liquid can be moulded to a shape and be deformed, it is not as dense as a solid but denser than a gas.
A gas: • The particles can go anywhere and are not held by any bonds and can take on any form.
• They can be moulded into any shape.
•The gas is not as dense as liquid or solid.
Plasma: •The particles are separate and the nuclei are apart from the electrons (ionization).
A picture is below of the states of matter:
There is a graph to show changing states of matter below:
The graphs shows that when there is a mixture of states of matter the particles cannot heat up anymore due to the fact, certain states of matter cannot be above or below certain temperatures.
When freezing water specifically, (at a particle level), the bonds strengthen and the particles become locked into place, this results in ice which is solid and cannot be deformed. At an atomic level though, water is different to all other liquids, as it expands. This happens when water particles join together they must have a certain formation. This is because water is made up of 2 positive particles and one negative. The positive must pair with a negative, resulting in a gap between particles, this is shown in the picture below:
Hope that helps.
The premise is wrong. Not all materials exist in exactly three different states; this is just the simplest schema and is applicable for some simple molecular or ionic substances.
Let's picture what happens to a substance if you start at low temperature, and add ever more heat.
Solid
At very low temperatures, there is virtually no thermal motion that prevents the molecules sticking together. And they stick together because of various forces (the simplest: opposite-charged ions attract each other electrostatically). If you picture this with something like lots of small magnets, it's evident enough that you get a solid phase, i.e. a rigid structure where nothing moves.
Actually though:
- Helium won't freeze at any temperature: its ground state in the low-temperature limit at atmospheric pressure is a superfluid. The reason is that microscopically, matter does not behave like discrete magnets or something, but according to quantum mechanics.
- There is generally not just one solid state. In the magnet analogy, you can build completely different structures from the same components. Likewise, what we just call “ice” is actually just one possible crystal structure for solid water, more precisely called Ice Ih. There are quite a lot of other solid phases.
Liquid
Now, if you increase temperature, that's like thoroughly vibrating your magnet sculpture. Because these bonds aren't infinitely strong, some of them will release every once in a while, allowing the whole to deform without actually falling apart. This is something like a liquid state.
Actually though:
- Not all materials have a liquid phase (at least not at all pressures). For instance, solid CO2 (dry ice) sublimates at atmospheric pressure if you increase the temperature, i.e. it goes immediately into the gas state.
- Many materials have huge molecules, i.e. the size of the chemical structure approaches the size of the physical structure. Now, that chemical structure can also be shaken loose by heat, but this isn't called melting but decomposition then. For instance, plastics decompose at some point between 200°C and 350°C. Some melt before i.e. they have two states; some stay solid all the way, they basically just have one state (solid).
A decomposed material hasn't entered a new state of matter, it simply has ceased to be the original material.
- Furthermore, materials that aren't purely composed of one kind of molecule also generally don't have a simple fix melting point. There's a certain range in which two phases may coexist. (More generally, you can have all sorts of emulsions, dispersions, gels etc.)
Gaseous
Small and sturdy molecules or single atoms aren't so bothered by high temperatures though. They also don't have so strong forces between molecules. So, if you shake strongly enough, they simply start fizzing all around independently. That's a gas then.
Actually though:
- Even the most sturdy molecules won't survive if you make the temperature high enough. Even single atoms will at some point lose their hold on the electrons. This results in a further phase, a plasma.
- At high enough pressure – above a critical point, the gas phase won't really be distinguishable from the liquid one: you only have a supercritical fluid. (IMO this could still be labelled a gas, but it does have some properties which are more like a liquid.)
Now, the question why a particular material is in some particular state at some given temperature and pressure isn't easy to answer. You need statistical physics to predict the behaviour. The crucial quantities are energy and entropy. Basically, the random thermal motion tends to cause disorder (which is quantified by rising entropy). At any given temperature there's a corresponding amount of energy available to overcome the attractive force, and within that energy budget the system approaches the state with the highest entropy. A solid has little entropy, but if there's not much energy available this is the only feasible state. A liquid has higher entropy but requires some energy to temporarily unstick the molecules. A gas requires enough energy to keep the particles apart all the time, but is completely disordered and therefore has a lot of entropy.
But how much energy and entropy a given state has exactly varies a lot between materials, therefore you can't simply say solid-liquid-gas.
Best Answer
Yep, you're right, we can only talk about the phase of matter if we have a collection of molecules. It wouldn't make any sense to talk about a single molecule as being a solid, liquid, or gas because what matters is how the kinetic energy of the molecules (related to temperature) compares to the intermolecular bonding energy.
Solid: KE << BE
Liquid: KE < BE
Gas: KE >> BE
I think the context that this sentence appeared in adds further clarity, so I've included it below.
Here's the full paragraph along with Fig. 3: