Solids, liquids, and gases are the three main, or fundamental phases of matter. Each one has a different density and a different level of stability. What determines the stability of each phase is the bond between it's atoms. The tighter the bond between it's atoms the more stable that phase of matter is. Solids are the most stable form of matter, followed by liquids, and then gases. Solids have a definite shape and do not take the shape of their container. Liquids do not have any definite shape and do take the shape of their container, the same is true with gases. Once again it is the bond between the atoms of liquids, and gases that make it have no definite shape. The first phase of matter is solids.
Solids are the most stable form of matter. Solids are more stable than liquids and gases. One type of solid is a Crystalline solid. The particles in a crystalline solid have a regular repeating pattern.
The types of crystalline solids are metals, alloys, salts, valence crystals, molecular crystals, polymers, and plastics. Most elementscrystalize as metals. Some solids can also be frozen liquids.
The atoms in a solid are tightly bonded which means it has a definiteshape. The second phase of matter is liquids. Liquids have no definite shape.
Liquids are less orderly than solids but more orderly than gases. Liquids can flow very easily.
Liquids also take the shape of their container.
Most liquids are very good conductors. Most liquids are also good solvents. Some solids float in liquids depending on their density. If the solid is less dense than the liquid then it floats on the liquids surface. If the solid is more dense than the liquid then it sinks in the liquids. For example an egg normally sinks in water because it's density is higher than water's density. When you add salt to the water the density of the water becomes higher than the egg's density so the egg floats. The third and final fundamental phase of matter is gas.
Gases are the least orderly of the three phases of matter. Gases take the shape of their container because of the very weak bond between their atoms. Gases are also very low in density. The average gas is 1000 times less than that of the average liquid. The volume of gas varies with many things including temperature and pressure.
These are explained in Charles's and Boyle's laws.
Boyle's law states that the volume of gas varies indefinitely with the pressure applied to it.
Matter exists in three basic states: solid, liquid, or gas. A substance experiences a phase change when the physical characteristics of that substance change from one state to another state. Perhaps the most recognizable examples of phase changes are those changes from a solid to a liquid or a liquid to a gas. When a substance goes through a phase change, there is a change in the internal energy of the substance but not the temperature of the substance (Serway, et al. 611).
Matter is assumed to be composed of an enormous number of very tiny particles which are indestructible. Gas is a state of matter. These tiny particles are separated by relatively large distances, which interact elastically. This large space between the particles make it easy to compress a gas. Which gives low mass to volume ratio. Particles must be in continual motion. These particles are very fast (usually about 500 meters per second). The molecules in a gaseous state have enough kinetic energy to be essentially independent of each other.
On earth, substances tend to exist in one of three phases; either a solid, liquid, or gas. While solids and liquids have defining factors such as volume, and for solids only, a shape, gases exhibit neither of these. Gases naturally take the shape of and expand into the volume of the container, and change when placed in different surroundings. As gases are constantly moving around and colliding with the walls, they exert a force, or pressure, on the walls of its container. Pressure is one of the characteristic behaviors that gases exhibit, but due to their nature, various factor effect the pressures that a gas can exert. Towards the end of the eighteenth century, scientist began to stumble upon these various factors that affect gases, especially
In this inquiry the relationship between force and mass was studied. This inquiry presents a question: when mass is increased is the force required to move it at a constant velocity increased, and how large will the increase be? It is obvious that more massive objects takes more force to move but the increase will be either linear or exponential. To hypothesize this point drawing from empirical data is necessary. When pulling an object on the ground it is discovered that to drag a four-kilogram object is not four times harder than dragging a two-kilogram object. I hypothesize that increasing the mass will increase the force needed to move the mass at a constant rate, these increases will have a liner relationship.
The Equation Of State These three gas laws that were proposed by Boyle, Amontons and Charles can be summarised as follows: For a fixed mass of gas pV = constant if T = constant (i) p/T = constant if V = constant (ii) V/T = constant if p = constant (iii)
In 1803 this theory was finalised and stated that (1) all matter is made up of the smallest possible particles termed atoms, (2) atoms of a given element have unique characteristics and weight, and (3) three types of atoms exist: simple (elements), compound (simple molecules), and complex (complex molecules).
Saferstein lists the three forms that fall under: solid, liquid, and gas. “A solid is rigid and therefore has a definite shape and volume. A liquid also occupies a specific volume, but its fluidity causes it to take the shape of the container in which it is residing. A gas has neither a definite shape nor volume, and it will completely fill any container into which it is place” (2011, Pg. 120). Chromatography, spectrophotometry, and mass spectrometry are used to identify or compare organic materials.
Thermodynamics is defined as “the study of heat transfer and its relationship to doing work.” Specifically, it is a field of physics that has to do with “the transfer of energy from one place to another or from one form to another” (Drake P.1). Heat acts as a form of energy that equates to a total amount of work. Heat was recognized as a form of energy around the year 1798. Count Rumford (Sir Benjamin Thompson), a British military engineer, observed that “numerous amounts of heat could be generated in the boring of cannon barrels” (Drake P.1), which is where a cannon’s firing port is enlarged using a drill and immense amounts of heat to make the metal malleable. He also observed that “the work done in turning a blunt boring tool was proportional
the bulk to ordinary matter; the volume of an atom is nearly all occupied by the
Thermodynamics is the branch of science concerned with the nature of heat and its conversion to any form of energy. In thermodynamics, both the thermodynamic system and its environment are considered. A thermodynamic system, in general, is defined by its volume, pressure, temperature, and chemical make-up. In general, the environment will contain heat sources with unlimited heat capacity allowing it to give and receive heat without changing its temperature. Whenever the conditions change, the thermodynamic system will respond by changing its state; the temperature, volume, pressure, or chemical make-up will adjust accordingly in order to reach its original state of equilibrium. There are three laws of thermodynamics in which the changing system can follow in order to return to equilibrium.
These phases can go from one to another when affected by certain things, which is known as phase changes. To switch from a solid to a liquid, the solid must melt. On the other hand, to switch from a liquid to a solid, freezing must occur. Furthermore, to switch from a liquid to a gas, a process known as evaporation must take place. In contrast, to go from a gas to a liquid, condensation must take place. Furthermore, sublimation must take place for a solid to turn to a gas. Inversely, deposition must occur for a gas to change to a solid.
The first law of thermodynamics is that heat is work and work is heat. Energy can’t be created or destroyed but it can be converted from one form to another form. First law of thermodynamics would be eating food. Humans turn food into chemical energy and humans need that energy to keep functioning. The second law of thermodynamics is heat can only transfer to colder objects not hotter objects. An example would be ice melting in a cooler. The coldness from the ice doesn’t leave the cooler, instead the heat transfers into the cooler to melt the ice. The third law is that the work or energy put in is equal to the work out plus heat. Some heat energy will always be wasted, such as a computer giving off heat. Using the first law, when the energy is transferred from one form to another, there will always be wasted heat because of the second law. This is because the energy is converted from a useful form to a less useful form. The less useful form is heat.
its state (Solid, liquid, gas); thus water has a higher melting point and a higher boiling
Since the days of Aristotle, all substances have been classified into one of three physical states. A substance having a fixed volume and shape is a solid. A substance, which has a fixed volume but not a fixed shape, is a liquid; liquids assume the shape of their container but do not necessarily fill it. A substance having neither a fixed shape nor a fixed volume is a gas; gases assume both the shape and the volume of their container. The structures of gases, and their behavior, are simpler than the structures and behavior of the two condensed phases, the solids and the liquids
Chemical reactions involve the making and breaking of bonds. It is essential that we know what bonds are before we can understand any chemical reaction. To understand bonds, we will first describe several of their properties. The bond strength tells us how hard it is to break a bond. Bond lengths give us valuable structural information about the positions of the atomic nuclei. Bond dipoles inform us about the electron distribution around the two bonded atoms. From bond dipoles we may derive electronegativity data useful for predicting the bond dipoles of bonds that may have never been made before.