2.2+States+of+matter

This diagram shows the nomenclature for the different phase transitions. More recently, distinctions between states have been based on differences in molecular interrelationships. Solid is the state in which intermolecular attractions keep the molecules in fixed spatial relationships. Liquid is the state in which intermolecular attractions keep molecules in proximity, but do not keep the molecules in fixed relationships. Gas is that state in which the molecules are comparatively separated and intermolecular attractions have relatively little effect on their respective motions. Plasma is a highly ionized gas that occurs at high temperatures. The intermolecular forces created by ionic attractions and repulsions give these compositions distinct properties, for which reason plasma is described as a fourth state of matter.[1][2] Forms of matter that are not composed of molecules and are organized by different forces can also be considered different states of matter. Fermionic condensate and the quark–gluon plasma are examples.
 * media type="youtube" key="ezCwUzFsoDY" width="425" height="350"media type="youtube" key="MVskAmAQpuU" width="425" height="350"​States of matter** are the distinct forms that different phases of matter take on. Historically, the distinction is made based on qualitative differences in bulk properties. Solid is the state in which matter maintains a fixed volume and shape; liquid is the state in which matter maintains a fixed volume but adapts to the shape of its container; and gas is the state in which matter expands to occupy whatever volume is available.
 * States of matter** may also be defined in terms of phase transitions. A phase transition indicates a change in structure and can be recognized by an abrupt change in properties. By this definition, a distinct state of matter is any set of states distinguished from any other set of states by a phase transition. Water can be said to have several distinct solid states.[3] The appearance of superconductivity is associated with a phase transition, so there are superconductive states. Likewise, liquid crystal states and ferromagnetic states are demarcated by phase transitions and have distinctive properties.

taken from: []  All matter is made from atoms with the configuration of the atom, the number of protons, neutrons, and electrons, determining the kind of matter present (oxygen, lead, silver, neon ...). Every substance has a unique number of protons, neutrons, and electrons. Oxygen, for example, has 8 protons, 8 neutrons, and 8 electrons. Individual atoms can combine with other atoms to form molecules. Water molecules contain two atoms of hydrogen **H** and one atom of oxygen **O** and is chemically called **H2O**. Oxygen and nitrogen, which are the major components of air, occur in nature as **diatomic** (two atom) molecules. Regardless of the type of molecule, matter normally exists as either a **solid, a liquid, or a gas**. We call this property of matter the **state** of the matter. The three normal states of matter have unique characteristics which are listed on the slide. In a **solid** the molecules are closely bound to one another by molecular forces. A solid holds its shape and the [|volume] of a solid is fixed by the shape of the solid. In a **liquid** the molecular forces are weaker than in a solid. A liquid will take the shape of its container with a free surface in a gravitational field. In microgravity, a liquid forms a ball inside a free surface. Regardless of gravity, a liquid has a fixed volume. In a **gas** the molecular forces are very weak. A gas fills its container, taking both the shape and the volume of the container || []
 * [[image:http://www.grc.nasa.gov/WWW/K-12/airplane/Images/state.gif width="709" height="533" align="center" caption="Computer graphic showing the normal states of matter; solid, liquid, and gas."]]
 * Solid**
 * Liquid**
 * Gas**





=States of Matter = There are five main states of matter. Solids, liquids, gases, plasmas, and Bose-Einstein condensates are all different states of matter. Each of these states is also known as a phase. Elements and compounds can move from one phase to another phase when special **physical forces** are present. One example of those forces is temperature. The phase or state of matter can change when the temperature changes. Generally, as the temperature rises, matter moves to a more active state.

Phase describes a physical state of matter. The key word to notice is physical. Things only move from one phase to another by physical means. If energy is added (like increasing the temperature or increasing pressure) or if energy is taken away (like freezing something or decreasing pressure) you have created a physical change.



One compound or element can move from phase to phase, but still be the same substance. You can see water **vapor** over a boiling pot of water. That vapor (or gas) can **condense** and become a drop of water. If you put that drop in the freezer, it would become a solid. No matter what phase it was in, it was always water. It always had the same chemical properties. On the other hand, a chemical change would change the way the water acted, eventually making it not water, but something completely new.

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taken from : [] ** States of Matter ** Gases, liquids and solids are all made up of microscopic particles, but the behaviors of these particles differ in the three phases. The following figure illustrates the microscopic differences.


 * Microscopic view of a gas. || Microscopic view of a liquid. || Microscopic view of a solid. ||
 * Microscopic view of a gas. || Microscopic view of a liquid. || Microscopic view of a solid. ||

Note that:

solid vibrate (jiggle) but generally do not move from place to place taken from :http://www.chem.purdue.edu/gchelp/atoms/states.html
 * Particles in a:
 * gas are well separated with no regular arrangement.
 * liquid are close together with no regular arrangement.
 * solid are tightly packed, usually in a regular pattern.
 * Particles in a:
 * gas vibrate and move freely at high speeds.
 * liquid vibrate, move about, and slide past each other.

PHYSICAL STATES OF MATTER
**Refractory** Refractory materials viewed on an atomic scale will have small domains of various crystal, liquid and amorphous states. Although this may sound like a very unstable material, refractory materials can be very stable. Refractory bricks are used for lining high temperature blast furnaces. Very little is known about the atomic structure of refractories and why they are so stable.
 * Gas **A gas is a substance which takes the shape of its container and expands to completely fill it's container. There are several types of gases with slightly different behaviors. These are ideal gasses, real gasses, super critical fluids, plasmas and critical opalescent materials.
 * Ideal Gas **Ideal gasses (sometimes called perfect gases) refer to the behavior which gasses approach as the pressure nears zero. This behavior is described mathematically by the ideal gas law. Although no gas behaves exactly as an ideal gas, many substances come very close to ideal behavior at atmospheric pressure and most behave ideally at very low pressures.
 * Real Gas **<span style="font-family: Arial,Helvetica,sans-serif;">Most molecules attract one another until they come very close together, when they become repulsive. This attraction is due to the electrostatic interactions between the two molecules. These interactions are often categorized into dispersion forces, van der Waals forces, hydrogen bonding and dipole-dipole interactions. The repulsion between molecules at very close distances is due to the repulsion between the nuclei of the two molecules. These forces give rise to relationships between the pressure, temperature, volume and quantity of a substance which do not exactly obey the ideal gas law. Gasses under physical conditions which give non-ideal behavior are called real gasses.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Supercritical Fluids **<span style="font-family: Arial,Helvetica,sans-serif;">At a given temperature, a gas can be compressed until it starts to condense into a liquid displaying a clear boundary between the liquid at the bottom of the container and the gas. Above a certain temperature, called the critical temperature, a gas can be compressed without ever observing a clear liquid - gas boundary. Gasses in this state are called super-critical fluids.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Critical Opalescence **<span style="font-family: Arial,Helvetica,sans-serif;">The critical point is the temperature and pressure where the boundary between liquids and gasses ceases to exist and the substance becomes a supercritical fluid. Under this one set of physical conditions, the substance is neither gas or liquid. The substance will have liquid like regions of every size from the size of the container down to single molecules. As such there are regions of the size of every wave length of visible light and all wave lengths of light are refracted. This results in a milky, silvery appearing state called critical opalescence.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Plasma **<span style="font-family: Arial,Helvetica,sans-serif;">A plasma is a material which has been heated to a temperature where molecules are not stable. In a plasma state, a substance is a mixture of neutral molecules, ions, atoms, clusters of atoms and free electrons. A spark is an example of a plasma.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Liquid **<span style="font-family: Arial,Helvetica,sans-serif;">A liquid is a substance which takes the shape of it's container and has a fixed volume at a given temperature and pressure. A superfluid is a special type of liquid. Suspensions, colloids, liquid crystals and visceoelastic materials have properties intermediate between those of a liquid and a solid.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Superfluid **<span style="font-family: Arial,Helvetica,sans-serif;">At very low temperatures certain compounds such as 3He will show a superfluid state. In this state quantum mechanical effects will be visible on a macroscopic scale. For example, spinning a sample of superfluid will give two or four counter rotating vortices in order to conserve angular momentum in the fluid as a whole rather than just at the atomic level.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Suspension **<span style="font-family: Arial,Helvetica,sans-serif;">A material in which small solid particles are mixed uniformly with a liquid. A suspension behaves as a liquid.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Colloid **<span style="font-family: Arial,Helvetica,sans-serif;">A colloid is a material which appears to be liquid but actually is a suspension of particles too small to observe with a microscope but bigger than normal molecules.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Liquid Crystal **<span style="font-family: Arial,Helvetica,sans-serif;">In crystals the atoms are arranged in an ordered repeating pattern. In liquids there is no ordered pattern. In liquid crystals there is order in one or two directions while there is no order in the other directions. This gives a number of unique properties such as optical properties which can be turned off and on to make liquid crystal displays for watches and computers. There will also be changes in the viscosity of a substance when it reaches a liquid crystal phase.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Visceoelastic **<span style="font-family: Arial,Helvetica,sans-serif;">Some compounds such as natural rubber appear to be solid when they are stretched, bent or set on a table top. However, over a period of time these materials will slowly deform to take the shape of the container. Substances which act as solid on short time scales and act as liquids on long time scales are called visceoelastic materials.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Solid **<span style="font-family: Arial,Helvetica,sans-serif;">Solid state materials are characterized by having a fixed volume and shape. Crystals, glasses and elastomers are all types of solids.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Crystal **<span style="font-family: Arial,Helvetica,sans-serif;">Crystals are solid state materials in which the atoms are arranged in an ordered repeating pattern. Many molecules will form crystals in which the original molecules are still distinguishable only stacked neatly. Organic compounds often form these molecular crystals. In other crystals, such as metal alloys, there is a repeating pattern but no distinguishable molecular units.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Glass **<span style="font-family: Arial,Helvetica,sans-serif;">Glasses are amorphous solids, meaning that the atoms are not arranged in any repeating pattern. When a liquid is cooled very slowly it tends to form a crystal, while cooling quickly usually results in amorphous phases. Glasses are distinguished from elastomers by being brittle.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Elastomer **<span style="font-family: Arial,Helvetica,sans-serif;">An elastomer is an amorphous solid which can be deformed with out breaking. A rubber band is an elastomer.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Superplastic **<span style="font-family: Arial,Helvetica,sans-serif;">Many metals and alloys can be stretched by about 100% before breaking. Some alloys can be stretched by a few thousand percent before breaking. This is referred to as superplasticity.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Bose-Einstein Condensate **<span style="font-family: Arial,Helvetica,sans-serif;">Atoms which are bosons behave according to Bose-Einstein statistics. Unlike fermions, many bosons can occupy the same quantum state. A laser beam is a collection of photons, which are bosons, all in the same quantum state, thus giving perfectly coherent light. At very low temperatures, atoms can all occupy the ground state of the system thus giving a coherent matter analogous to the laser. This process is called Bose-Einstein condensation.

<span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">MAGNETIC STATES OF MATTER

 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Diamagnetic **<span style="font-family: Arial,Helvetica,sans-serif;">A diamagnetic compound has all of it's electron spins paired giving a net spin of zero. Diamagnetic compounds are weakly repelled by a magnet.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Paramagnet **<span style="font-family: Arial,Helvetica,sans-serif;">A paramagnetic compound will have some electrons with unpaired spins. Paramagnetic compounds are weakly attracted by a magnet.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Ferromagnet **<span style="font-family: Arial,Helvetica,sans-serif;">In a ferromagnetic substance there are unpaired electron spins, which are held in alignment by a process known as ferromagnetic coupling. Ferromagnetic compounds, such as iron, are strongly attracted to magnets.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Ferrimagnet **<span style="font-family: Arial,Helvetica,sans-serif;">Ferrimagnetic compounds have unpaired electron spins, which are held in an pattern with some up and some down. This is known as ferrimagnetic coupling. In a ferrimagnetic compound, there are more spins held in one direction, so the compound is attracted to a magnet.
 * <span style="color: #ff0000; font-family: Arial,Helvetica,sans-serif;">Antiferromagnetic **<span style="font-family: Arial,Helvetica,sans-serif;">When unpaired electrons are held in an alignment with an equal number of spins in each direction, the substance is strongly repelled by a magnet. This is referred to as an antiferromagnet.

Materials which will be repelled by magnetic fields because the magnetic field is excluded from passing through them. This property of superconductors is used to test for the presence of a superconducting state. taken from: [] ​

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particles can move past one another || <span style="color: #000000; font-family: Arial,Helvetica,sans-serif;">assumes the shape of the part of the container which it occupies particles can move/slide past one another || <span style="color: #000000; font-family: Arial,Helvetica,sans-serif;">retains a fixed volume and shape rigid - particles locked into place || lots of free space between particles || <span style="color: #000000; font-family: Arial,Helvetica,sans-serif;">not easily compressible little free space between particles || <span style="color: #000000; font-family: Arial,Helvetica,sans-serif;">not easily compressible little free space between particles || particles can move past one another || <span style="color: #000000; font-family: Arial,Helvetica,sans-serif;">flows easily particles can move/slide past one another || <span style="color: #cc0000; font-family: Arial,Helvetica,sans-serif;">does not flow easily <span style="color: #cc0000; font-family: Arial,Helvetica,sans-serif;">rigid - particles cannot move/slide past one another
 * ~ **<span style="color: #ff0000; font-family: Tahoma,Geneva,sans-serif; font-size: 130%;">Some Characteristics of Gases, Liquids and Solids and the Microscopic Explanation for the Behavior ** ||
 * **<span style="color: #000000; font-family: Tahoma,Geneva,sans-serif; font-size: 130%;">gas ** || **<span style="color: #000000; font-family: Tahoma,Geneva,sans-serif; font-size: 130%;">liquid ** || **<span style="color: #000000; font-family: Tahoma,Geneva,sans-serif; font-size: 130%;">solid ** ||
 * <span style="color: #000000; font-family: Arial,Helvetica,sans-serif;">assumes the shape and volume of its container
 * <span style="color: #000000; font-family: Arial,Helvetica,sans-serif;">compressible
 * <span style="color: #000000; font-family: Arial,Helvetica,sans-serif;">flows easily

<span style="display: block; font-family: Arial,Helvetica,sans-serif; font-size: 80%; text-align: right;">taken from:__http://www.chem.purdue.edu/gchelp/atoms/states.html__ || media type="youtube" key="s-KvoVzukHo" height="385" width="480" Matter is everything around you. **Matter** is anything made of [|atoms] and molecules. Matter is anything that has a **mass**. Matter is also related to light and electromagnetic radiation. Even though matter can be found all over the universe, you usually find it in just a few forms. As of 1995, scientists have identified five **states of matter**. They may discover one more by the time you get old.
 * || =Matter is the Stuff Around You=

You should know about solids, liquids, gases, plasmas, and a new one called Bose-Einstein condensates. The first four have been around a long time. The scientists who worked with the [|Bose-Einstein condensate] received a Nobel Prize for their work in 1995. But what makes a state of matter? It's about the physical state of molecules and atoms.

=Changing States of Matter= [|Elements] and compounds can move from one [|physical state] to another and not change. Oxygen (O2) as a gas still has the same properties as liquid oxygen. The [|liquid] state is colder and denser but the molecules are still the same. Water is another example. The **compound** water is made up of two hydrogen (H) atoms and one oxygen (O) atom. It has the same molecular structure whether it is a [|gas], liquid, or [|solid]. Although its physical state may change, its chemical state remains the same.

So you ask, "What is a chemical state?" If the formula of water were to change, that would be a **chemical change**. If you added another oxygen atom, you would make hydrogen peroxide (H2O2). Its molecules would not be water anymore. Changing states of matter is about changing densities, pressures, temperatures, and other physical properties. The basic chemical structure does not change

taken from [|www.chem4kidscom]

**CLASSICAL STATES**

**SOLID**

The particles (ions, atoms or molecules) are packed closely together. The forces between particles are strong enough so that the particles cannot move freely but can only vibrate. As a result, a solid has a stable, definite shape, and a definite volume. Solids can only change their shape by force, as when broken or cut. In crystalline solids, the particles (atoms, molecules, or ions) are arranged in an ordered three-dimensional structure. There are many different crystal structueres, and the same substance can have more than one structure (or solid phase). For example, iron has a body-centred cubic structure at temperatures below 912 °C, and a face-centred cubic structure between 912 and 1394 °C. Ice has fifteen known crystal structures, or fifteen solid phases which exist at various temperatures and pressures. Solids can be transformed into liquids by melting, and liquids can be transformed into solids by freezing. Solids can also change directly into gases through the process of sublimation.




 * ​LIQUI D **

The volume is definite if the temperature and constant. When a solid is heated aboves its melting point, it becomes liquid. Intermolecular (or interatomic or interionic) forces are still important, but the molecules have enough energy to move relative to each other and the structure is mobile. This means that the shape of a liquid is not definite but is determined by its container. The volume is usually greater than that of the corresponding solid, the most well known exception being water, H2O. The highest temperature at which a given liquid can exist is its critical temperature.


 * GAS **

In a gas, the molecules have enough kinetic energy, so that the effect of intermolecular forces is small (or zero for an ideal gas), and the typical distance between neighboring molecules is much greater than the molecular size. A gas has no definite shape or volume, but occupies the entire container in which it is confined. A liquid may be converted to a gas by heating at constant pressure to the boiling point, or else by reducing the pressure at constant temperature. At temperatures below its critical temperature, a gas is also called a vapor, and can be liquefied by compression alone without cooling. A vapor can exist in equilibrium with a liquid (or solid), in which case the gas pressure equals the vapor pressure of the liquid (or solid). A supercritical fluid (SCF) is a gas whose temperature and pressure are above the critical temperature and critical pressure respectively. It has the physical properties of a gas, but its high density confers solvent properties in some cases which lead to useful applications. For example, supercritical carbon dioxide is used to extract caffeine in the manufacture of decaffeinated coffee.

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