How To Make Soap Rocks

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Phosphorus is found in Group 15 (VA) of the periodic table, the graph showing how the elements chemicals are related. Phosphorus is part of the nitrogen family along with nitrogen, arsenic, antimony and bismuth. Phosphorus was discovered in 1669 by German physician Hennig Brand, who is somewhat known in chemistry. He is sometimes called the last of the alchemists. Alchemy was a kind of pre-science existed since around 500 BC to about the late 16th century. Alchemists wanted to find a way to change the lead, iron and other metals into gold. I also wanted to find a way to have eternal life. Alchemy has too much magic and mysticism to be a real science. However, a number of techniques developed and produced many materials new later proved useful in modern chemistry.

The mark was convinced that the key to changing metals into gold is found in urine, probably because of its golden color. It therefore decided to seek "magical substance" that could change lead into gold in the urine. It was during the heating process and purification of urine which won the match. The discovery was important because it was the first time someone had discovered a substance not known to ancient peoples. In that sense, the brand was the first person who could be called the discoverer of an element. Phosphorus is a fascinating element that occurs in at least three different ways. If left exposed to air, catches fire by itself. It also glows in the dark. Today, it is more important is the use in the manufacture of phosphoric acid (H3PO4), which in turn is used to manufacture fertilizers and a number of other less important products.

Phosphorus and its compounds may have been known before the discovery of Brand. Ancient manuscripts refer to materials that glow in the dark. The word used for these materials is now fluorescent. The first Christians said the use of "perpetual lamps" that glowed in the dark. The lamps may have contained phosphorus or one of its compounds. Without But the brand was first to record the process of making pure phosphorus. Nobody knows how it was decided that the urine may contain a chemical that could be used to turn lead into gold. His experiments to find a chemical, of course, a failure. But he made the discovery an accident on the road.

Scientists were fascinated when they learned of the discovery of Brand. They tried to repeat his research. Some tried to talk to him in the sale of its discovery the kings and princes. The new element appeared to be a way to get fortune and become famous. But the brand was not interested in these ideas. Instead, he gave everyone who prepared phosphorus. Other scientists soon began experimenting with the item. One of the first discoveries made was how dangerous phosphorus is. One scientist wrote that a server left some phosphorus above his bed one day. Later that night, the bed covers burst into flames. Phosphorus had caught fire by itself!

Finally, the method of mark, making the phosphorus is widely known. The element joined iron, gold, silver, arsenic, and the handful of other elements known to early chemists. Little is known about what happened to the brand after its discovery. In fact, there record of when or where he died. Phosphorus exists in at least three allotropic forms. The three main allotropes are named for their colors: the phosphorus white (also called yellow phosphorus), red phosphorus and phosphorus black (also called violet phosphorus). These allotropes all have different properties physical and chemical properties.

White phosphorus is a waxy, transparent and robust. Its melting point is 44.1 ° C (111 ° F) and its boiling point is 280 ° C (536 ° F). Has a density of 1.88 grams per cubic centimeter. If kept in a vacuum, sublimates when exposed to light. White phosphorus is phosphorescent. It gives off a beautiful greenish-white glow. It does not dissolve well in water, but dissolves other liquids, such as benzene, chloroform and carbon disulfide. White phosphorus is sometimes slightly yellow due to traces of red phosphorus.

Red phosphorus is a red powder. It can be done by heating white phosphorus with a catalyst at 240 ° C (464 ° F). , Without a catalyst, red phosphorus is sublimated at 416 ° C (781 ° F). Its density is 2.34 grams per cubic centimeter. It does not dissolve in most liquids. Black phosphorus seems graphite powder. Black phosphorus can be done by applying pressure extreme white phosphorus. It has a density of 3.56 to 3.83 grams per cubic centimeter. One of its interesting properties is to conduct an electric current, although of being a non-metal.

White phosphorus is the form that occurs most often at room temperature. It is very reactive. It combines so readily with oxygen that ignites spontaneously (automatically). As a precaution, white phosphorus is stored under water in chemical laboratories. Phosphorus is combined readily with halogens. Phosphorus also combines with metals to form compounds known as phosphides.

The abundance of phosphorus in the cortex land is estimated at 0.12 percent, which is the most common element 11. Usually presents as a phosphate. An example is calcium phosphate, Ca3 (PO4) 2. The only important commercial source of phosphorus is phosphate rock. Phosphate rock is primarily calcium phosphate. The United States is the largest producer of phosphate rock in the world. About 86 percent of phosphate rock is from North Carolina and Florida. Smaller quantities are exploited in Idaho and Utah. Other major producers of phosphate rock are Morocco, China, Russia, Tunisia, Jordan and Israel.

Although only a natural isotope of phosphorus, phosphorus-31exists, six radioactive isotopes known phosphorus. A radioactive isotope, phosphorus-32, has applications in medicine, industry, and follow-up studies. An indicator is a radioactive isotope, whose presence in a system can be easily detected. The isotope is injected into the system that emits radiation. The radiation is followed by detectors placed throughout the system.

Phosphorus-32 is especially useful in medical studies, because phosphorus is produced in many parts of the body. Of radioactive phosphorus can be used as a marker to study body parts and chemical changes inside the body. Radioactive phosphorus can also determine the amount of blood in the body of a person. It can also help locate the presence of tumors in the brain, eyes, sinuses and skin. Finally, it is sometimes used to treat certain forms of cancer. Radiation emitted by phosphorus-32 can kill cancer cells and help slow or stop the disease. Phosphorus-32 is important in a variety scientific studies. For example, in addition to the tires when they are made. Then, the radiation emitted can be studied as the tires are used. This information indicates that the tire is worn and how long it takes to perform.

It is possible to make pure phosphorus from phosphate rock. The rock is mixed with sand and coke (pure carbon). The mixture is heated in an electric furnace. An oven is a device for producing very high temperatures. Of pure phosphorus is produced in this reaction. Escape the mixture as a vapor (gas). The vapor cooled solidifies into white phosphorus. This reaction is not very important because pure phosphorus has some applications. The most important compounds of phosphorus are all made of rock phosphate or calcium phosphate. Therefore, the most important step in the production of "match" is simply to separate the pure calcium phosphate from phosphate rock. This can be done quite easily. Two compounds phosphorus are used for the coating at the tip of safety matches.

In 1996, 91 percent of all phosphate rock mined in the U.S. was used to make fertilizer. Modern farmers use huge amounts of synthetic (artificial) fertilizers on their crops. This synthesis fertilizers containing nitrogen, phosphorus and potassium, the three critical elements for growing plants. These elements are presented on the floor, but can not be present in large enough quantities. Adding them through synthetic fertilizer helps plants grow better. Most farmers add some synthetic fertilizer to their fields each year. This demand for synthetic fertilizers accounts for the increased use of phosphorus compounds.

Phosphorus and its compounds have other uses too. These uses account for about 10 percent of all phosphorus produced. For example, compounds known as pentasulphide phosphorus (P2S5) and sesquisulfide phosphorus (P4 S3) are used to make ordinary wood and paper safety matches. These compounds coat the tip of the match. When the party is scratched on a surface, the phosphorus pentasulfide phosphorus sesquisulfide bursts into flames. Lights other chemicals in the head of the party. Another compound phosphorus with a number of uses is phosphorus oxychloride (POCl3). This compound is used in the manufacture of gasoline additives in the production of certain types of plastics as a fire retardant agent, and in the manufacture of transistors for electronic devices.

Phosphorus is essential for health of plants and animals. Many essential chemicals in living cells containing phosphorus. One of the most important of these chemicals is tris adenosine (ATP). ATP provides the energy the cells need to survive and carry out all tasks to be performed. Phosphorus is essential for the development bones and teeth. Nucleic acids also contain phosphorus. Nucleic acids are chemicals that carry out many functions in living organisms. By example, carry the genetic information in a cell. They tell the cell what chemicals should be done. It also serves as director of the "" in the formation of these chemicals.

The recommended daily amount of phosphorus in humans is a gram. It's pretty easy to get the phosphorus much every day through meat, milk, beans and grains. Two phosphorus compounds are used to cover the end of a game. Moreover, elemental phosphorus is extremely dangerous. Ingesting even a hint of white phosphorus causes severe diarrhea and blood loss, liver damage, stomach, intestines and blood (system of blood flow), and coma. Eating a piece of white phosphorus no greater than 50 to 100 milligrams (0.0035 ounce) can even cause death. Phosphorus Management White is dangerous. Causes severe burns. Interestingly, red phosphorus does not have the same effects. It is considered relatively safe. It is dangerous if it contains white phosphorus mixed with him.

The second most important use of phosphate compounds in the manufacture of detergents. The compound used in detergents, is called sodium tripolyphosphate, or STPP (Na5P3O10), which adds a number of benefits to a detergent. For example, can kill some bacteria and prevent them from becoming corroded washers (oxidized) and capped. The most important function in detergents, however, is like a water softening agent. Natural water often contains chemicals that keep the foam soaps and detergents. Reduce the ability of soaps and detergents for washing clothes. STPP has the ability to capture these chemicals. It greatly improves the ability of soaps and detergents to lather and clean clothes. The first use of STPP detergent Tide was in 1947. The Tide's introduction brought about a revolution in clothes cleaning.

But STPP can create problems for the environment. After detergents were used, often end up in rivers and streams and eventually in lakes from waste water. And that is fine for the algae that live in lakes. Algae are small green plants that use of phosphorus as they grow. As most detergents get into lakes, increases the amount of STPP. That means there is more phosphorus in a lake and, in turn, means that the algae begin to grow much faster.

In some cases, it is both STPP and phosphorus in a lake algae grow out of control, clogging the lake with green plants, algae and others. The lake gradually becomes a swamp, and finally into a meadow. The lake is gone. Many people are concerned about this problem in the 1960s. They demanded that less STPP be used in detergents. A number of cities and states have banned the sale of detergents STPP. STPP production increased rapidly from 1.10 million pounds in 1955 to 2.44 billion pounds in 1970. But then the production began to fall. In the mid 1990s, production had fallen well below billion pounds a year.

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