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Jetzt kostenlos anmeldenIce, water, steam - three different forms of the same molecule, H2O. Despite having the same chemical formula and being made of the exact same elements, these three species have very different structures, Intermolecular Forces and characteristics. They're great examples of states of matter.
States of matter are one of the distinct physical forms in which matter can exist.
In 1742, the Swedish astronomer Anders Celsius invented a way of measuring temperature. He noticed that the melting point of water was almost entirely independent of its pressure, and labelled this point as 100 on his new scale. On the other hand, he showed that the boiling point of water did depend on its pressure, and labelled its boiling temperature at sea level as 0. In the following years, various scientists reversed his system until we ended up with the familiar scale we know today: the Celsius scale. Now, 0 indicates the melting point of water whilst 100 indicates its boiling point at sea level, and the units are named degrees Celsius, °C. Unlike other temperature scales, such as the Fahrenheit scale, it is based on defined and measurable states of matter.
There are three main states of matter. They're characterised by their structure, arrangement of particles, Intermolecular Forces and relative energy, and can be represented by the particle model, in which particles are shown as spheres. These three states are:
We'll look at them all in turn, starting from solids.
You might also hear the term 'phase' being used when talking about states of matter. Although these terms are similar, they have slightly different meanings. A phase is defined as a chemically distinct, physically uniform region of a species. This means that each distinct phase has the same structure, density, index of refraction and magnetisation. States of matter are all examples of phases, but you can get different phases within states of matter. For example, solid ice has many different phases, differentiated by their unique crystal structures.
The first state of matter we'll explore today is solid. In solids, the particles are held together very closely in a regular pattern. There are very strong intermolecular forces between particles, and because of this, the particles can't move freely but instead vibrate around a fixed spot. This means that solids maintain a certain shape and volume, no matter their container. The particles also have a low energy.
Fig. 1 - The arrangement of particles in a solid
You'll look at different types of solids in the article "Lattice Structures". There, you'll be able to compare molecular, covalent, ionic and metallic lattice structures and their properties.
If you heat up a solid, it eventually turns into a liquid. In liquids, the particles are randomly arranged. They're still held together closely by intermolecular forces, but these forces are partially overcome and so the particles are able to move around more freely. This means that liquids flow to take the shape of their container. However, they still have a definite volume. Because we've heated the particles, they have more energy than those in a solid.
Fig. 2 - The arrangement of particles in a liquid
The third main state of matter is gas. This is produced when you heat a liquid to an even higher temperature. In gases, the particles are randomly arranged and are spaced very far apart. There are (almost) no intermolecular forces between particles, and this means that they move freely in all directions at high speeds and have a lot of energy. Gases always fill their containers and don't have a fixed volume - instead, they can be compressed or expand.
Fig. 3 - The arrangement of particles in a gas
An ideal gas is a theoretical gas that doesn't have any intermolecular forces or interactions between molecules. Molecules are assumed to be particles with no volume, and no kinetic energy is lost when they collide.
Ideal gases are useful because they obey a certain law relating pressure (P), temperature (T) and volume (V), where PV = nRT. Here, n represents the number of moles of the gas, and R represents the universal gas constant, a value equalling 8.134 J mol-1 K-1. This is known as the ideal gas law, and it means that one mole of any ideal gas occupies the same volume at the same temperature and pressure. Although no gas is perfectly ideal, many gases are close enough for this law to be used in chemical calculations.
Gases that don't behave quite like ideal gases are known as real gases. We have an article all about ideal and real gases which should help you compare the two. Check out "Ideal and Real Gases" for more. And if you want to try your hand at calculations involving the ideal gas law, then head over to "Ideal Gas Law" for plenty of worked examples.
There is actually a fourth state of matter that is more common than you think. In fact, it plays a role in many everyday objects and phenomena. This state is called plasma.
Similar to how heating a liquid turns it into a gas, heating a gas turns it into plasma. Plasma can also be created using a laser, microwaves or any magnetic field. Much like gases, the particles in plasma are randomly arranged and spread far apart. They don't have a fixed shape or volume and expand to fill their container. However, unlike gases, plasma is made from charged particles. When you heat a gas to a high enough temperatures (or carry out one of the other methods of creating plasma), you separate some of the particles into negatively charged electrons and positively charged ions. These electrons are called free electrons. These charged particles mean that plasma can conduct electricity. If only some of the particles in plasma are ionised, the plasma is said to be partially ionised. But if all of the particles are ionised, the plasma is said to be fully ionised.
Fig. 4 - The arrangement of particles in plasma
You'll find plasma in stars, neon lights, plasma televisions and lightning.
To help consolidate your learning, we've created a handy table comparing the three main states of matter:
Fig. 5 - A table comparing the three main states of matter
Now that we know what the different states of matter are, let's look at changes in states of matter. As the name suggests, this involves switching from one state of matter to another.
If you heat a solid, its temperature increases. However, at some point, its temperature stops increasing. Instead, the solid starts to melt. The thermal energy supplied is used to increase the kinetic energy of the particles and overcome the intermolecular forces holding them tightly together. This point is known as the substance's melting point.
Once all of the substance has melted, its temperature increases again. But as before, it reaches a plateau at a certain point. The substance starts to boil. Once again, the thermal energy supplied is used to increase the kinetic energy of the particles even further and overcome the remaining intermolecular forces between them. This is known as the substance's boiling point. Its temperature remains the same until all of the substance has turned into a gas; only then does it increase again.
The opposite is also true. If you take a gas and cool it down, it eventually condenses into a liquid. Cool it even further, and it freezes into a solid. Some solids can go straight from a solid to a gas, skipping the liquid state altogether. This is known as sublimation. The reverse process, turning from a gas to a solid, is known as deposition.
Here's a handy diagram showing you the names of the changes from one state of matter to another:
Fig. 6 - Changes in states of matter
We can expand on this to talk about changes of state when it comes to plasma. Turning from a gas to plasma is known as ionisation, whilst turning from plasma back to a gas is known as deionisation or recombination.
To finish, let's explore some common examples of states of matter:
States of matter are one the distinct physical forms in which matter can exist. There are three main states of matter: solid, liquid and gas. However, plasma is another common state of matter.
The most common example you'll come across for describing states of matter is water. At temperatures below 0°C, it forms a solid we call ice. At temperatures above 100°C, it boils to form a gas we call steam. At temperatures in between, it is found in its liquid state.
Solid and liquid are two distinct states of matter. The particles in a solid are arranged very closely together and vibrate on the spot with a low energy. Solids also have a fixed volume and shape. The particles in a liquid, on the other hand, are packed less closely together and move about randomly with more energy. Although liquids still have a definite volume, they change shape to fill their container.
Gas is a type of state of matter, in which the particles are spaced far apart and move about quickly and randomly, with a lot of energy. Gases don't have a fixed volume or shape. Instead, they expand to fill their container.
Heating or cooling a substance causes it to change its state of matter. The thermal energy is used to increase the kinetic energy of the particles and overcome some of the intermolecular forces between them, causing a change of state.
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SIGNUP SIGNUPFlashcards in States of Matter38
Start learningWhat Law explains the behaviour of Ideal Gas?
Ideal Gas Law
Where can you find Ideal Gas in the environment?
Nowhere. Ideal gas is a hypothetical gas. It does not exist in the environment.
Which real gas behaves the most like an ideal gas?
Helium.
What is Standard Temperature and Pressure (STP) defined as and who defines it?
STP is defined as T = 273.15K (0oC) and P = 105 Pa (1bar).
It is defined by the IUPAC (International Union of Pure and Applied Chemistry)
What kind of collision do molecules/atoms of a real gas have?
Elastic
Under what conditions do real gases deviate from ideal gas behaviour?
High pressure and low temperature.
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