- Created: 14-01-22
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VRFd185rty
With the rapid development of industry, a larger and larger range
of Chemicals are invented and widely used in the production like
Fluorine
Chemicals.
Fluorine is an univalent poisonous gaseous halogen, it is pale
yellow-green and it is the most chemically reactive and
electronegative of all the elements. Fluorine readily forms compounds
with most other elements, even with the noble gases krypton, xenon
and radon. It is so reactive that glass, metals, and even water, as
well as other substances, burn with a bright flame in a jet of
fluorine gas.
In aqueous solution, fluorine commonly occurs as the fluoride ion
F-. Fluorides are compounds that combine fluoride with some
positively charged counterpart.
Atomic fluorine and molecular fluorine are used for plasma etching in
semiconductor manufacturing, flat panel display production and MEMs
fabrication. Fluorine is indirectly used in the production of low
friction plastics such as teflon and in halons such as freon, in the
production of uranium. Fluorochlorohydrocarbons are used extensively
in air conditioning and in refrigeration. Fluorides are often added
to toothpaste and, somewhat controversially, to municipal water
supplies to prevent dental cavities. Fore more information visit our
page on mineral water.
Small amounts of fluorine are naturally present in water, air, plants
and animals. As a result humans are exposed to fluorine through food
and drinking water and by breathing air. Fluorine can be found in any
kind of food in relatively small quantities. Large quantities of
fluorine can be found in tea and shellfish. Fluorine is essential for
the maintenance of solidity of our bones. Fluorine can also protect
us from dental decay, if it is applied through toothpaste twice a
day. If fluorine is absorbed too frequently, it can cause teeth
decay, osteoporosis and harm to kidneys, bones, nerves and muscles.
Fluorine gas is released in the industries. This gas is very
dangerous, as it can cause death at very high concentrations. At low
concentrations it causes eye and nose irritations.
When fluorine from the air ends up in water it will settle into the
sediment. When it ends up in soils, fluorine will become strongly
attached to soil particles. In the environment fluorine cannot be
destroyed; it can only change form. Fluorine that is located in soils
may accumulate in plants. The amount of uptake by plants depends upon
the type of plant and the type of soil and the amount and type of
fluorine found in the soil. With plants that are sensitive for
fluorine exposure even low concentrations of fluorine can cause leave
damage and a decline in growth. Too much fluoride, wheater taken in
form the soil by roots, or asdorbed from the atmosphere by the
leaves, retards the growth of plants and reduces crop yields. Those
more affected are corns and apricots.
Animals that eat fluorine-containing plants may accumulate large
amounts of fluorine in their bodies. Fluorine primarily accumulates
in bones. Consequently, animals that are exposed to high
concentrations of fluorine suffer from dental decay and bone
degradation. Too much fluorine can also cause the uptake of food from
the paunch to decline and it can disturb the development of claws.
Finally, it can cause low birth-weights.
Just like Fluorine Chemicals
Lithium
Chemicals are also commonly used. Lithium is the first of the
alkalis in the periodic table. In nature it’s found like a mixture
of the isotopes Li6 and Li7. It's the lightest solid metal, and
is soft, silvery-white, with a low melting point and reactive. Many
of its physical and chemical properties are more similar to those of
the alkaline earth metals than to those of its own group. Between the
most significant properties of lithium we find its high specific heat
(calorific capacity), the huge temperature interval in the liquid
state, high termic conductivity, low viscosity and very low density.
Metallic lithium is soluble in short chain aliphatic amines, like
etilamine. It's insoluble in hydrocarbons.
Lithium takes part in a huge number of reactions, with organic
reactants as well as with inorganic reactants. It reacts with oxygen
to form monoxide and peroxide. It’s the only alkaline metal that
reacts with nitrogen at ambient temperature to produce a black
nitrure. It reacts easily with hydrogen at almost 500oC (930oF) to
form lithium hydride. Metallic lithium’s reaction with water is
extremely vigorous. Lithium reacts directly with the carbon to
produce the carbure. It binds easily with halogens and forms
halogenures with light emission. Although it doesn’t react with
parafinic hydrocarbons, it experiments addition reactions with
alquenes substituted by arile and diene groups. It also reacts with
acetylenic compounds, forming lithium acetylures, which are important
in vitamin A synthesis.
The main lithium compound is the lithium hydroxide. It's a white
powder; the manufactured material is monohydrate lithium hydroxide.
The carbonate can be used in the pottery industry and in medicine as
an antidepressant. The bromine and the lithium chloride both form
concentrated brine, which have the property of absorbing the humidity
in a wide interval of temperature; these brines are used in the
manufactured air conditioning systems.
The main industrial use of lithium is in lithium stearatum form, as
lubricant grease's thickener. Other important applications of
lithium compounds are in pottery, specifically in porcelain glaze; as
an additive to extend the life and performance of alkaline storage
batteries and in autogenous welding and brass welding.
Except for the kinds metioned above, there are
other
chemicals especially for
Electronic Grade Chemicals like
Alumina Chemicals.