Натрий химические свойства, назначение, производство
Описание
In its ionic form, sodium is one of the most important biological
nutrients and is found nearly everywhere on Earth.
Although it was isolated as a free metal in 1807 by Sir
Humphry Davy and makes up 2.83% of Earth’s lithosphere, it
is not found in its metallic form in nature. Pure sodium is
extremely reactive, particularly with water to form explosive
hydrogen gas and lye (NaOH); it can also react with water
vapor in air or biological tissues.
Mined and refined salts from terrestrial and aquatic sources
contain sodium in the form of sodium chloride, sodium
iodide, and other compounds. Natron, a naturally occurring
mixture of sodium compounds, has been used since the time of
the ancient Egyptians, and sodium compounds are essential to
numerous industries, including those involving glass, paper,
and soap production. Since it does not occur in its metallic
form in nature, pure sodium metal must be produced industrially,
which is accomplished via electrolysis of molten sodium
chloride.
Химические свойства
Sodium is a soft silvery white metallic element. Pyrophoric solid or molten liquid. Odorless, oxidizing rapidly in air; waxlike at room temperature, brittle at low temperatures. Store in airtight containers or in naphtha or similar liquid that does not contain water or free oxygen. Decomposes water on contact, with evolution of hydrogen to form sodium hydroxide; insoluble in benzene, kerosene, and naphtha. Has excellent elec- trical conductivity and high heat-absorbing capacity.
Физические свойства
Sodium is a soft, wax-like silver metal that oxidizes in air. Its density is 0.9674 g/cm3, andtherefore it floats on water as it reacts with the water releasing hydrogen. It has a rather lowmelting point (97.6°C) and a boiling point of 883°C. Sodium is an excellent conductor ofheat and electricity. It looks much like aluminum but is much softer and can be cut with aknife like butter. Its oxidation state is +1.
Изотопы
Sodium has 14 isotopes. The only stable isotope of sodium has an averageatomic weight of 23 (23Na) and makes up about 100% of all the isotopes of the element sodium found on Earth. All the other 13 isotopes (from 19Na to 31Na) are radioactive with relatively short half-lives and thus are unstable.
Происхождение имени
The Latin name for the symbol for “sodium” (Na) is natrium, and the
name “sodium” in Latin is sodanum, which was known as an ancient headache remedy
and was called “soda” in English.
Вхождение
Sodium is the sixth most abundant of the Earth’s elements. Since it is a highly electropositive metal and so reactive with nonmetals, it is not found in its pure elemental form on Earth.Rather, it is found in numerous compounds in relatively abundant quantities. About 2.83%of the Earth’s crust consists of sodium in compounds.Sodium is produced by an electrolytic process, similar to the other alkali earth metals. (Seefigure 4.1). The difference is the electrolyte, which is molten sodium chloride (NaCl, common table salt). A high temperature is required to melt the salt, allowing the sodium cationsto collect at the cathode as liquid metallic sodium, while the chlorine anions are liberated aschlorine gas at the anode: 2NaCl (salt) + electrolysis → Cl2↑ (gas) + 2Na (sodium metal). Thecommercial electrolytic process is referred to as a Downs cell, and at temperatures over 800°C,the liquid sodium metal is drained off as it is produced at the cathode. After chlorine, sodiumis the most abundant element found in solution in seawater.
Характеристики
On the periodic table sodium is located between lithium and potassium. A fresh cut intosodium looks silvery but turns gray as sodium oxidizes rapidly in air, forming sodium oxideon its surface.Sodium is extremely reactive. It reacts explosively in water as it releases hydrogen fromthe water with enough heat to ignite the hydrogen. The resulting compound of this reactionis sodium hydroxide (2Na + 2H2O → 2NaOH + H2↑). Due to its extremely electropositivereactivity, there are few uses for the pure metallic form of sodium. Because of its reactivity,hundreds of sodium compounds are found on the Earth’s surface.Guide to the Elements | 51An unusual characteristic of several alkali metals is that a mixture of two or more has alower melting point than the melting point of the separate metals. This is referred to as aeutectic system of metallic alloys. For instance, sodium has a melting point of 97.6°C, andpotassium’s melting point is 63.25°C, but when the two are mixed, the eutectic melting point(turning into a liquid phase) of the combined Na-K system is below zero degrees Celsius(–10°C). If cesium metal (melting point of 38.89°C) is added to the Na and K mixture, themelting point of this eutectic alloy (Na-K-Cs) is the lowest of any eutectic alloy at –78°C.
Использование
manufacture of sodium Compounds, such as the cyanide, azide, peroxide, etc.; manufacture of tetraethyllead; manufacture of refractory metals; in org syntheses; for photoelectric cells; in sodium lamps; as catalyst for many polymerization reactions. Alloyed with potassium in heat transfer media.
Методы производства
Sodium is an essential element needed for all organic life.
Sodium is produced commercially through the electrolysis of
liquid sodium chloride mixed with calcium chloride in a
Downs Cell. Very pure sodium can be isolated by the thermal
decomposition of sodium azide (NaN3).
Sodium, in its metallic form, can be used to refine some
reactive metals, such as zirconium and potassium, from
their compounds and is very important in making esters.
Определение
sodium: Symbol Na. A soft silveryreactive element belonging to group1 (formerly IA) of the periodic table(see alkali metals); a.n. 11; r.a.m.22.9898; r.d. 0.97; m.p. 97.8°C; b.p.882–889°C. Sodium occurs as thechloride in sea water and in the mineralhalite. It is extracted by electrolysisin a Downs cell. The metal isused as a reducing agent in certainreactions and liquid sodium is also acoolant in nuclear reactors. Chemically,it is highly reactive, oxidizingin air and reacting violently withwater (it is kept under oil). It dissolvesin liquid ammonia to formblue solutions containing solvatedelectrons. Sodium is a major essentialelement required by living organisms.The element was first isolatedby Humphry Davy in 1807.
Общее описание
Sodium,Na, melts at 97.8°C and boils at 892°C. It is silver-white in color, is soft and malleable, and oxidizes in air. When exposed to air, a silvery soft metal that becomes grayish white upon. It occurs naturally only in the forms of its salts. Shipped as a solid or molten liquid. Burns violently with explosions that may spatter the material. Sodium is used as a chemical intermediate. and in pharmaceuticals, petroleum refining and metallurgy, electric power cable, Sodium lamps, other chemicals.
Реакции воздуха и воды
May ignite spontaneously in air. Reacts violently with water to give Sodium hydroxide and hydrogen, which ignites spontaneously [Merck, 11th ed. 1989)]. The ignition temperature of Sodium in air depends on the area of surface exposed: vapor ignites at room temperature; droplets at about 250°F; an agitated pool at 400°F. In the absence of moisture and hydrogen, the reaction is insignificant [Mellor 2 Supp. 2:440 1961].
Опасность
Sodium as the elemental metal is very dangerous because of its extreme electropositivenature, particularly when it comes in contact with moist air, water, snow, or ice or otheroxidizing agents. It readily gives up electrons to electronegative atoms (nonmetals). In thesereactions, it releases hydrogen gas with enough heat to explosively ignite the hydrogen.
Numerous sodium compounds are hazardous as carcinogens (cancer-causing) and astoxins (poisons) in plants and animals. On the other hand, we benefit greatly from the manycompounds containing the element sodium. We could not live without it.
Угроза здоровью
Sodium reacts with the moisture on skin and other tissues to form highly corrosive
sodium hydroxide. Contact of metallic sodium with the skin, eyes, or mucous
membranes causes severe burns; thermal burns may also occur due to ignition of the
metal and liberated hydrogen.
Пожароопасность
Sodium spontaneously ignites when heated above 115 °C in air that has even
modest moisture content, and any sodium vapor generated is even more flammable.
Sodium reacts violently on contact with water and often ignites or explodes the
hydrogen formed. Sodium fires must be extinguished with a class D dry chemical
extinguisher or by the use of sand, ground limestone, dry clay or graphite, or ''Met-
L-X ? " type solids. Water or CO 2 extinguishers must never be used on sodium fires.
Воспламеняемость и взрывоопасность
Sodium spontaneously ignites when heated above 115 °C in air that has even
modest moisture content, and any sodium vapor generated is even more flammable.
Sodium reacts violently on contact with water and often ignites or explodes the
hydrogen formed. Sodium fires must be extinguished with a class D dry chemical
extinguisher or by the use of sand, ground limestone, dry clay or graphite, or "Met-
L-X ?" type solids. Water or CO2 extinguishers must never be used on sodium fires.
Возможный контакт
A potential danger to those involved in tetra-alkyl lead manufacture using lead-sodium alloy as a reactant; those using sodium as a liquid metal coolant, as a catalyst, or in the manufacture of sodium hydride, borohydride, or peroxide.
Экологическая судьба
Elemental sodium that is released into the environment reacts
almost immediately with water to form sodium hydroxide and
hydrogen gas. Even small quantities of metallic sodium can be
explosive when brought into contact with sources of water; the
formation sodium hydroxide raises the local pH and is
extremely caustic. Sodium cations formed from this reaction
are rapidly absorbed into the surrounding environment to
form a large variety of salts.
хранилище
Safety glasses,
impermeable gloves, and a fire-retardant laboratory coat should be worn at all times
when working with sodium, and the metal should be handled under the surface of an
inert liquid such as mineral oil, xylene, or toluene. Sodium should be used only in
areas free of ignition sources and should be stored under mineral oil in tightly
sealed metal containers under an inert gas such as argon.
Перевозки
UN1428 Sodium, Hazard Class: 4.3; Labels: 4.3-Dangerous when wet material. Note: Finely divided sodium is pyrophoric.
Методы очистки
The metal is placed on a coarse grade of sintered-glass filter, melted under vacuum and forced through the filter using argon. The Pyrex apparatus is then re-evacuated and sealed off below the filter, so that the sodium could be distilled at 460o through a side arm and condenser into a receiver bulb which is then sealed off [Gunn & Green J Am Chem Soc 80 4782 1958]. EXPLODES and IGNITES in water.
Несовместимости
A strong reducing agent. A dangerous fire hazard when exposed to heat and moisture. Violent reaction with water, forming NaOH. Violent reaction with oxidizers (chlorates, nitrates, peroxides, permanganates, perchlorates, chlorine, bromine, fluorine, etc.); contact may cause fires or explosions. Keep away from alkaline materials, strong bases, strong acids, oxoacids, epoxides. halogenated hydrocarbons; phosphorus and phosphorus compounds; sulfur and sulfur compounds; and many other chemicals.
Утилизация отходов
Incineration with absorption of oxide fumes.
Натрий препаратная продукция и сырье
сырьё
препарат
SODIUM PHENOLATE TRIHYDRATE
Этиловый альфа-формиловый эфир бензоуксусной кислоты
10-(МЕТИЛСУЛЬФОНИЛ)КАПРАМИД
3,3-дифенилпропанол
Этил пиколиноилацета
6-AMINO-2-METHYLTHIO-3-METHYLURACIL
2-Amino-4-methoxypyridine
4-Methylbenzene-1-carboximidamide hydrochloride
2,4-диметилхинолин
2-гептанол
2-метоксифурана
4-AMINO-2-METHYLPYRIMIDINE-5-CARBONITRILE
4-AMINO-2-MERCAPTOPYRIMIDINE-5-CARBONITRILE
2-Amino-6-hydroxypyrimidin-4(3H)-one ,97%
Tiotropium bromide
ETHYL 3-AMINOTHIOPHENE-2-CARBOXYLATE
4-METHOXY-BENZAMIDINE
2-AMINO-4-METHOXYPYRIMIDINE
4,4,4-Трифтор-1-фенил-1,3-бутандион
4-AMINO-2-(TRIFLUOROMETHYL)PYRIMIDINE-5-CARBOXYLIC ACID
4,6-DIAMINO-2-MERCAPTOPYRIMIDINE
4-AMINO-2-METHYL-PYRIMIDINE-5-CARBOXYLIC ACID
бис (2-этилгексил) фенилфосфит
Трифенилолова хлорид
5-BROMO-2-CHLORO-4-METHOXYPYRIMIDINE
2-amino-6-chloropyrimidin-4(3H)-one
Глицидилизопропиловый эфир
4-хлорбензамидин гидрохлорид
4-METHYL-BENZAMIDINE
4-Chlorobenzamidine гидройодид
Перекись натрия
4-аминопиримидин-5-карбонитрил
6-AMINO-1-METHYL-5-NITROSOURACIL
3-октанол
2,2'-DIPYRIDYLAMINE
4-METHOXYBENZAMIDINE, HYDROCHLORIDE
2,4-DIOXO-4-THIOPHEN-2-YL-BUTYRIC ACID METHYL ESTER
2-ETHOXYPYRIMIDIN-4-YLAMINE
4-Methyl-2-thiophenecarboxylic acid
2-Метил-1-бутантиола