E941 NITROGEN

E941 Nitrogen is used within many industries for items that people come across every single day.
E941 Nitrogen gas is used in ordinary incandescent light bulbs as an inexpensive alternative to argon.
E941 Nitrogen is used Motor Racing Teams, Tyre inflation, Shock absorber filling.

CAS number: 7727-37-9
EC number: 231-783-9
Molecular formula: N₂
Molecular weight: 28.014 g/mol

SYNONYMS:
N, Nitrogen, Nitrogen gas, Molecular nitrogen, Dinitrogen, Nitrogen-14, nitrogen molecule, Diatomic nitrogen, Nitrogen, liquid, UNII-N762921K75, N2, CHEBI:17997, N762921K75, MOL Nitrogen, Nitrogeno, Nitrogen [NF], Nitrogen (liquified), HSDB 5060, UN1066, UN1977, Nitrogen (TN), Nitrogen, elemental, Nitrogen (n2), Nitrogen, compressed, Nitrogen (JP17/NF), Nitrogen, >=99.998%, Nitrogen, >=99.999%, CHEMBL142438, INS NO.941, DTXSID4036304, INS-941, DB09152, UN 1066, UN 1977, E941, Nitrogen, Messer(R) CANGas, 99.999%, E-941, C00697, D00083, Nitrogen, refrigerated liquid (cryogenic liquid), Nitrogen, compressed [UN1066] [Nonflammable gas], Q2370426, UNII-K21NZZ5Y0B component IJGRMHOSHXDMSA-UHFFFAOYSA-N, Nitrogen, refrigerated liquid (cryogenic liquid) [UN1977] [Nonflammable gas], N#N

E941 Nitrogen, designated E941 in the food industry, is a noble gas used as protective packaging for a wide range of food products.
As a colorless, odorless and non-toxic gas, E941 Nitrogen is ideal for preserving the freshness and extending the shelf life of food by minimizing the influence of oxygen, preventing oxidation and spoilage processes.

E941 Nitrogen's use in protective packaging technology significantly improves the quality of stored food products while maintaining their natural properties.
E941 Nitrogen has very low reactivity, which makes it an excellent choice for creating a protective atmosphere in food packaging.

E941 Nitrogen's ability to displace oxygen from the package reduces the risk of growth of bacteria and other microorganisms, and also slows down oxidation processes.
E941 Nitrogen is a colorless and odorless gas used as a food additive for packaging and preserving food products.

E941 Nitrogen is a colorless, odorless, and tasteless gas that naturally makes up the largest portion of the Earth´s atmosphere (approximately 78%).
E941 Nitrogen is a colorless, odorless, tasteless, and inert diatomic gas that naturally comprises approximately 78% of Earth's atmosphere.

When E941 Nitrogen is in direct contact with foodstuffs and serves as a food additive, it is designated with the European Union food additive code E941.
E941 Nitrogen plays a crucial role in modern food processing and packaging.

As an inert, non-reactive gas, E941 Nitrogen offers numerous benefits across the food industry—from extending shelf life to improving product consistency.
Classified as E941 when used as a food additive, food-grade E941 Nitrogen is especially valuable in applications where contact with food requires strict quality standards.

According to current food safety regulations, E941 Nitrogen used directly with food must have a minimum purity of 99.5%, with a maximum of 5000 ppm residual oxygen.
Chemically inert gas, free of any interaction with E941 Nitrogen.

E941 Nitrogen's action is basically in the mechanical removal of Oxygen.
E941 Nitrogen is a colorless, odorless, and tasteless inert gas that constitutes approximately 78% of the Earth's atmosphere.
E941 Nitrogen is a chemical element; it has symbol N and atomic number 7.

E941 Nitrogen is a nonmetal and the lightest member of group 15 of the periodic table, often called the pnictogens.
E941 Nitrogen is a common element in the universe, estimated at seventh in total abundance in the Milky Way and the Solar System.
At standard temperature and pressure, two atoms of the element bond to form E941 Nitrogen, a colourless and odourless diatomic gas.

E941 Nitrogen forms about 78% of Earth's atmosphere, making it the most abundant chemical species in the air.
Because of the volatility of E941 Nitrogen compounds, it is relatively rare in the solid parts of the Earth.
E941 Nitrogen was first discovered and isolated by Scottish physician Daniel Rutherford in 1772 and independently by Carl Wilhelm Scheele and Henry Cavendish at about the same time.

The name nitrogène was suggested by French chemist Jean-Antoine-Claude Chaptal in 1790 when it was found that E941 Nitrogen was present in nitric acid and nitrates.
Antoine Lavoisier suggested instead the name azote, from the Ancient Greek: ἀζωτικός "no life", as it is an asphyxiant gas; this name is used in a number of languages, and appears in the English names of some E941 Nitrogen compounds such as hydrazine, azides and azo compounds.

Elemental E941 Nitrogen is usually produced from air by pressure swing adsorption technology.
About 2/3 of commercially produced elemental E941 Nitrogen is used as an inert (oxygen-free) gas for commercial uses such as food packaging, and much of the rest is used as liquid E941 Nitrogen in cryogenic applications.
Many industrially important compounds, such as ammonia, nitric acid, organic nitrates (propellants and explosives), and cyanides, contain E941 Nitrogen.

The extremely strong triple bond in elemental E941 Nitrogen (N≡N), the second strongest bond in any diatomic molecule after carbon monoxide (CO), dominates E941 Nitrogen chemistry.
This causes difficulty for both organisms and industry in converting N2 into useful compounds, but at the same time it means that burning, exploding, or decomposing E941 Nitrogen compounds to form E941 Nitrogen gas releases large amounts of often useful energy.

Synthetically produced ammonia and nitrates are key industrial fertilisers, and fertiliser nitrates are key pollutants in the eutrophication of water systems.
Apart from its use in fertilisers and energy stores, E941 Nitrogen is a constituent of organic compounds as diverse as aramids used in high-strength fabric and cyanoacrylate used in superglue.

E941 Nitrogen occurs in all organisms, primarily in amino acids (and thus proteins), in the nucleic acids (DNA and RNA) and in the energy transfer molecule adenosine triphosphate.
The human body contains about 3% E941 Nitrogen by mass, the fourth most abundant element in the body after oxygen, carbon, and hydrogen.

The E941 Nitrogen cycle describes the movement of the element from the air, into the biosphere and organic compounds, then back into the atmosphere.
E941 Nitrogen is a constituent of every major pharmacological drug class, including antibiotics.
Many drugs are mimics or prodrugs of natural E941 Nitrogen-containing signal molecules: for example, the organic nitrates nitroglycerin and nitroprusside control blood pressure by metabolising into nitric oxide.

Many notable E941 Nitrogen-containing drugs, such as the natural caffeine and morphine or the synthetic amphetamines, act on receptors of animal neurotransmitters.
E941 Nitrogen is a gas that makes up about 78% of the Earth’s atmosphere.
In fact, E941 Nitrogen is an essential element for life and the nutrition of organisms.
The most E941 Nitrogen-containing foods are meat (especially beef and pork), fish, eggs, dairy products, grains and legumes.

USES and APPLICATIONS of E941 NITROGEN:
E941 Nitrogen is used within many industries for items that people come across every single day.
Lighting – E941 Nitrogen gas is used in ordinary incandescent light bulbs as an inexpensive alternative to argon.
Applications and Users of E941 Nitrogen: Motor Racing Teams, Tyre inflation, Shock absorber filling

E941 Nitrogen is commonly used in the packaging of food products such as snacks, coffees, teas, dried fruits, nuts and in oxidation-sensitive products.
E941 Nitrogen is also used in the beverage industry, including the packaging of beer and wine to prevent oxidation and preserve freshness.

In the food industry, E941 Nitrogen is used as a protective and propellant gas to shield food products from oxidation, moisture loss, and microbial spoilage.
E941 Nitrogen is used across a wide range of food categories.

Modified Atmosphere Packaging (MAP): E941 Nitrogen is used alongside other gases such as CO₂ to displace oxygen inside packaging, thereby extending shelf life (e.g., in potato chips, salads, cheese, and processed meats).
Propellant in aerosol products: E941 Nitrogen serves as a propellant in whipped cream dispensers and other food aerosols.

Cryogenic freezing: Liquid E941 Nitrogen (at approximately −196 °C) is used for rapid shock-freezing of food items, preserving quality and cellular structure.
Wine and beverage production: E941 Nitrogen protects wine and other beverages from oxidation during storage and bottling.
In the food industry, E941 Nitrogen is used as a propellant gas in spray cans, as a packaging gas for modified atmosphere packaging (MAP) to extend shelf life, and as a food-grade gas for various processing applications.

Gas Applications of E941 Nitrogen: Food and Beverage, Aquariology, Helium for Balloons, Refrigeration and Air Conditioning, Electric Arc Welding, Metal Cutting.
In the food industry, E941 Nitrogen is commonly used as a packaging gas and propellant to preserve the freshness and quality of food products.

Like dry ice, the main use of liquid E941 Nitrogen is for cooling to low temperatures.
E941 Nitrogen is used in the cryopreservation of biological materials such as blood and reproductive cells (sperm and eggs).
E941 Nitrogen is used in cryotherapy to remove cysts and warts on the skin by freezing them.

E941 Nitrogen is used in laboratory cold traps, and in cryopumps to obtain lower pressures in vacuum pumped systems.
E941 Nitrogen is used to cool heat-sensitive electronics such as infrared detectors and X-ray detectors.
Other uses of E941 Nitrogen include freeze-grinding and machining materials that are soft or rubbery at room temperature, shrink-fitting and assembling engineering components, and more generally to attain very low temperatures where necessary.

Because of its low cost, liquid E941 Nitrogen is often used for cooling even when such low temperatures are not strictly necessary, such as refrigeration of food, freeze-branding livestock, freezing pipes to halt flow when valves are not present, and consolidating unstable soil by freezing whenever excavation is going on underneath.

The applications of E941 Nitrogen compounds are naturally extremely widely varied due to the huge size of this class: hence, only applications of pure E941 Nitrogen itself will be considered here.
Two-thirds (2/3) of E941 Nitrogen produced by industry is sold as gas and the remaining one-third (1/3) as a liquid.

E941 Nitrogen in the food industry: E941 Nitrogen is a colorless, odorless, tasteless and inert gas, but more importantly it is so versatile that its use in a multitude of industries is advantageous, both in the form of E941 Nitrogen gas and in the form of liquid E941 Nitrogen.
E941 Nitrogen constitutes many biological molecules and is used in crop fertilizers.

-Gas uses of E941 Nitrogen:
E941 Nitrogen is mostly used as a low reactivity safe atmosphere wherever the oxygen in the air would pose a fire, explosion, or oxidising hazard.

Some examples include:
As a modified atmosphere, pure or mixed with carbon dioxide, to E941 Nitrogenate and preserve the freshness of packaged or bulk foods (by delaying rancidity and other forms of oxidative damage).
Pure E941 Nitrogen as food additive is labelled in the European Union with the E number E941.
In incandescent light bulbs as an inexpensive alternative to argon.
In fire suppression systems for Information technology (IT) equipment.
In the manufacture of stainless steel.
In the case-hardening of steel by nitriding.
In some aircraft fuel systems to reduce fire hazard (see inerting system).

To inflate race car and aircraft tires, reducing the problems of inconsistent expansion and contraction caused by moisture and oxygen in natural air.
E941 Nitrogen is commonly used during sample preparation in chemical analysis.

E941 Nitrogen is used to concentrate and reduce the volume of liquid samples.
Directing a pressurised stream of E941 Nitrogen gas perpendicular to the surface of the liquid causes the solvent to evaporate while leaving the solute(s) and un-evaporated solvent behind.

E941 Nitrogen can be used as a replacement, or in combination with, carbon dioxide to pressurise kegs of some beers, particularly stouts and British ales, due to the smaller bubbles it produces, which makes the dispensed beer smoother and headier.
A pressure-sensitive E941 Nitrogen capsule known commonly as a "widget" allows E941 Nitrogen-charged beers to be packaged in cans and bottles.

E941 Nitrogen tanks are also replacing carbon dioxide as the main power source for paintball guns.
E941 Nitrogen must be kept at a higher pressure than CO2, making N2 tanks heavier and more expensive.

-Equipment uses of E941 Nitrogen:
Some construction equipment uses pressurised E941 Nitrogen gas to help hydraulic system to provide extra power to devices such as hydraulic hammer.
E941 Nitrogen gas, formed from the decomposition of sodium azide, is used for the inflation of airbags.

-Execution uses of E941 Nitrogen:
As E941 Nitrogen is an asphyxiant gas in itself, some jurisdictions have considered asphyxiation by inhalation of pure E941 Nitrogen as a means of capital punishment (as a substitute for lethal injection).
In January 2024, Kenneth Eugene Smith became the first person executed by E941 Nitrogen asphyxiation.

-Liquid uses of E941 Nitrogen: 
Liquid E941 Nitrogen is a cryogenic liquid which looks like water.
When insulated in proper containers such as dewar flasks, it can be transported and stored with a low rate of evaporative loss.

-Food packaging uses of E941 Nitrogen:
E941 Nitrogen is used as a modified atmosphere, pure or mixed with carbon dioxide, to preserve the freshness of packaged or bulk foods (by delaying rancidity and other forms of oxidative damage).
Pure E941 Nitrogen as a food additive is labelled in the European Union with the E number E941.

-E941 Nitrogen for modified atmosphere packaging (MAP):
One of the best-known uses of E941 Nitrogen in the food industry is in modified atmosphere packaging.
By replacing oxygen in the packaging environment, E941 Nitrogen slows down spoilage and prevents oxidation, helping preserve the freshness, flavour, and colour of products like snacks, coffee, meat, and ready meals.

Controlled atmosphere storage for fruit and vegetables
Fresh produce such as fruits and vegetables can be stored in tanks filled with E941 Nitrogen to create a controlled atmosphere.
This technique significantly extends shelf life, sometimes by several months—while helping retain nutritional value and texture.

-Sparging and flushing uses of E941 Nitrogen: 
Removing oxygen from liquids:
E941 Nitrogen is commonly used in sparging, a process that removes dissolved oxygen from food-grade liquids like oils, juices, and wines.
Since oxygen can degrade flavour and colour, flushing it out with E941 Nitrogen helps maintain product quality and stability without introducing additives or preservatives.

-Pressure transfer of liquids and powders uses of E941 Nitrogen:
E941 Nitrogen gas can also be used to move products through pipelines under pressure, whether they’re in liquid or powdered form.
This method reduces mechanical stress and prevents oxygen exposure during transfer—ideal for sensitive products such as dairy, flour, or beverages.

-Gentle mixing of dense liquids use of E941 Nitrogen:
In processing thicker liquids such as fruit juices or sauces, E941 Nitrogen can aid in gentle mixing.
E941 Nitrogen helps separate solids like pulp, skins, or seeds without aggressive stirring, preserving the product’s natural properties and texture.

-Natural pest control in grain storage of E941 Nitrogen:
Grain silos and flour storage units can be filled with E941 Nitrogen to eliminate pests such as insects, larvae, and mites—without the use of chemical fumigants.
This E941 Nitrogen-based method also reduces the risk of combustion or explosions by removing oxygen from the storage environment.

-Processing aid for texture and dispersion uses of E941 Nitrogen:
E941 Nitrogen is widely used as a technological aid in food processing.
E941 Nitrogen helps aerate creams, foams, and mousses to create light textures.
E941 Nitrogen’s also commonly used as a propellant in aerosol food products such as whipped cream or sprayable toppings, making it a key player in convenience and ready-to-use packaging.

-Motorsports and Aircraft Tires use of E941 Nitrogen:
E941 Nitrogen gas cylinders are essential in the motorsport and aviation industries.
E941 Nitrogen Nitrogen is used for filling automotive and aircraft tires due to its inertness and lack of moisture or oxidative qualities, as opposed to air.
The difference in E941 Nitrogen content between air and pure N2 is 20%.

-Wine Preservation uses of E941 Nitrogen:
E941 Nitrogen is used as a propellant for draft wine and as an alternative to or together with carbon dioxide for other beverages.
E941 Nitrogen bottles are also replacing carbon dioxide as the primary power source for paintball guns.
E941 Nitrogen gas must be kept at a higher pressure than CO2 gas bottles, making N2 tanks heavier and more expensive.

-Air Conditioning Use of E941 Nitrogen:
Suppliers and installers use the gas within air conditioning systems throughout the UK.
E941 Nitrogen is also present in refrigeration units.

MAIN USES of E941 NITROGEN IN THE FOOD INDUSTRY:
E941 Nitrogen ensures proper storage of food liquids by reducing or eliminating the presence of air (and thus oxygen), inhibits bacterial growth, reduces the damaging effects of moisture, and protects the conduction system from external contamination.
Because of all these properties, E941 Nitrogen has extensive use in the food industry to preserve foods from losing some of their organoleptic characteristics.

Here are the main uses:
*Improving the shelf-life of packaged foods by preventing spoilage from oxidation, mould growth, moisture leakage and infestation
*Thermoregulation and cooling of food in industrial processes
*Rapid freezing (cryogenic freezing and IQF) of foods.
*For traditional transport of ingredients and the inerting of food storage tanks
*Cooling of perishable foods during transport
*Packaging in a protective atmosphere
*Cryomacination and cryocrystallization of foods
*Deodorization of edible oils
*Stripping (stripping): what it’s all about
*One particular application of E941 Nitrogen in food & beverage is stripping.

E941 Nitrogen is able to remove oxygen that may already be present in food liquids, a practice that is particularly effective in bottling wine, but also for edible oils and fats.
The operation is made possible by devices called line strippers, through which gas is dispersed into the liquid in the form of microbubbles that capture oxygen, eliminating volatile contaminants.
This technique makes E941 Nitrogen possible to counteract rancidity, preserve the aroma of products, and increase the shelf life of foods.

WHAT E941 NITROGEN IS USED FOR?
At the industrial level, E941 Nitrogen has numerous applications that result in both improved production processes and better quality products.

Here are listed the main ones:
Food industry
This is certainly the most common application, to which a paragraph a below is devoted.

Chemical industry
E941 Nitrogen in the production of ammonia efficiently moves liquids within pipelines, but more importantly it is used to inert vessels of all kinds by removing their oxygen content.

Oil industry
E941 Nitrogen removes volatile organic compounds (VOCs) from exhaust streams, cools flue gas, and also improves recovery and maintains pressure in oil and gas reservoirs.

Metal production and processing
In this area, too, E941 Nitrogen is a valuable ally that can protect steel, copper, and aluminum during annealing, carburizing, and sintering operations in high-temperature furnaces.

Iron production
E941 Nitrogen enables cooling of furnace electrodes and prevents oxidation of iron by lowering temperatures.

Medicine
E941 Nitrogen is used for cryosurgery and dermatology procedures, but also makes the transport of biological materials safer.

Construction
E941 Nitrogen retains the pouring temperature of concrete mixtures and stabilizes the soils on which it is built.

LIQUID FOOD GRADE E941 NITROGEN:
One of the most common uses of liquid E941 Nitrogen in the food industry, as an additive classified as E941, is to freeze and preserve food.
E941 Nitrogen is a liquid food gas that is also used to reduce the formation of bacteria in food and to prevent oxidation of products.
Due to its ability to inhibit the growth of microorganisms, liquid E941 Nitrogen is fundamental in preserving foods such as meat, fish and baked goods, preserving their freshness and quality.

E941 NITROGEN AND ITS FUNCTIONS IN FOOD
In the food industry, E941 Nitrogen plays a key role in protecting food from spoilage, maintaining its quality, freshness and nutritional value.
Using E941 Nitrogen as a protective gas is an effective way to extend the shelf life of food products without adding chemical preservatives.

NATURAL OCCURRENCE of E941 NITROGEN:
E941 Nitrogen is naturally present in the Earth's atmosphere, comprising about 78% of the air we breathe.
For industrial purposes, E941 Nitrogen is obtained through the fractional distillation of liquid air.

ALTERNATIVES AND SUBSTITUTES of E941 NITROGEN:
Other inert gases used for food packaging and as propellants include:

• Carbon Dioxide (E290):
Often used in combination with E941 Nitrogen to inhibit microbial growth in food products.

• Argon (E938):
Another inert gas employed to create an oxygen-free environment in food packaging.

HOW IS E941 NITROGEN PRODUCED?
E941 Nitrogen is produced by the process of air fractionation in which air is cooled and compressed to a liquid, then passed through fractional distillation columns that separate E941 Nitrogen from oxygen and other air components.

HISTORY of E941 NITROGEN:
E941 Nitrogen compounds have a very long history, ammonium chloride having been known to Herodotus. 
They were well known by the Middle Ages. 
Alchemists knew nitric acid as aqua fortis (strong water), as well as other E941 Nitrogen compounds such as ammonium salts and nitrate salts. 

The mixture of nitric and hydrochloric acids was known as aqua regia (royal water), celebrated for its ability to dissolve gold, the king of metals.
The discovery of E941 Nitrogen is attributed to the Scottish physician Daniel Rutherford in 1772, who called it noxious air. Though he did not recognise it as an entirely different chemical substance, he clearly distinguished it from Joseph Black's "fixed air", or carbon dioxide. 

The fact that there was a component of air that does not support combustion was clear to Rutherford, although he was not aware that it was an element. 
E941 Nitrogen was also studied at about the same time by Carl Wilhelm Scheele, Henry Cavendish, and Joseph Priestley, who referred to E941 Nitrogen as burnt air or phlogisticated air. 

French chemist Antoine Lavoisier referred to E941 Nitrogen gas as "mephitic air" or azote, from the Greek word άζωτικός (azotikos), "no life", due to E941 Nitrogen being asphyxiant. 
In an atmosphere of pure E941 Nitrogen, animals died and flames were extinguished. 

Though Lavoisier's name was not accepted in English since it was pointed out that all gases but oxygen are either asphyxiant or outright toxic, it is used in many languages (French, Italian, Portuguese, Polish, Russian, Albanian, Turkish, etc.; the German Stickstoff similarly refers to the same characteristic, viz. ersticken "to choke or suffocate") and still remains in English in the common names of many E941 Nitrogen compounds, such as hydrazine and compounds of the azide ion. 

Finally, it led to the name "pnictogens" for the group headed by E941 Nitrogen, from the Greek πνίγειν "to choke".
The English word E941 Nitrogen (1794) entered the language from the French nitrogène, coined in 1790 by French chemist Jean-Antoine Chaptal (1756–1832), from the French nitre (potassium nitrate, also called saltpeter) and the French suffix -gène, "producing", from the Greek -γενής (-genes, "begotten"). 

Chaptal's meaning was that E941 Nitrogen is the essential part of nitric acid, which in turn was produced from nitre. 
In earlier times, niter had been confused with Egyptian "natron" (sodium carbonate) – called νίτρον (nitron) in Greek – which, despite the name, contained no nitrate.

The earliest military, industrial, and agricultural applications of E941 Nitrogen compounds used saltpeter (sodium nitrate or potassium nitrate), most notably in gunpowder, and later as fertiliser. 

In 1910, Lord Rayleigh discovered that an electrical discharge in E941 Nitrogen gas produced "active E941 Nitrogen", a monatomic allotrope of E941 Nitrogen. 
The "whirling cloud of brilliant yellow light" produced by his apparatus reacted with mercury to produce explosive mercury nitride.

For a long time, sources of E941 Nitrogen compounds were limited. 
Natural sources originated either from biology or deposits of nitrates produced by atmospheric reactions. 

E941 Nitrogen fixation by industrial processes like the Frank–Caro process (1895–1899) and Haber–Bosch process (1908–1913) eased this shortage of E941 Nitrogen compounds, to the extent that half of global food production (see Applications) now relies on synthetic E941 Nitrogen fertilisers. 

At the same time, use of the Ostwald process (1902) to produce nitrates from industrial E941 Nitrogen fixation allowed the large-scale industrial production of nitrates as feedstock in the manufacture of explosives in the World Wars of the 20th century.
About four-fifths of Earth’s atmosphere is E941 Nitrogen, which was isolated and recognized as a specific substance during early investigations of the air. 

Carl Wilhelm Scheele, a Swedish chemist, showed in 1772 that air is a mixture of two gases, one of which he called “fire air,” because it supported combustion, and the other “foul air,” because it was left after the “fire air” had been used up. 
The “fire air” was, of course, oxygen and the “foul air” E941 Nitrogen. 

At about the same time, E941 Nitrogen also was recognized by a Scottish botanist, Daniel Rutherford (who was the first to publish his findings), by the British chemist Henry Cavendish, and by the British clergyman and scientist Joseph Priestley, who, with Scheele, is given credit for the discovery of oxygen. 

Later work showed the new gas to be a constituent of nitre, a common name for potassium nitrate (KNO3), and, accordingly, it was named E941 Nitrogen by the French chemist Jean-Antoine-Claude Chaptal in 1790. 
E941 Nitrogen first was considered a chemical element by Antoine-Laurent Lavoisier, whose explanation of the role of oxygen in combustion eventually overthrew the phlogiston theory, an erroneous view of combustion that became popular in the early 18th century. 

The inability of E941 Nitrogen to support life (Greek: zoe) led Lavoisier to name it azote, still the French equivalent of E941 Nitrogen.
E941 Nitrogen was discovered by the Scottish physician Daniel Rutherford in 1772. 

E941 Nitrogen is the fifth most abundant element in the universe and makes up about 78% of the earth's atmosphere, which contains an estimated 4,000 trillion tons of the gas. 
E941 Nitrogen is obtained from liquefied air through a process known as fractional distillation.

The largest use of E941 Nitrogen is for the production of ammonia (NH3). 
Large amounts of E941 Nitrogen are combined with hydrogen to produce ammonia in a method known as the Haber process. 

The French chemist Antoine Laurent Lavoisier named E941 Nitrogen azote, meaning "without life". 
The name became E941 Nitrogen, which derives from the Greek word nitron, which means "native soda" and genes, which means "forming". 

Credit for the discovery of the element is generally given to Daniel Rutherford, who found it could be separated from air in 1772.
E941 Nitrogen was sometimes referred to as "burnt" or "dephlogisticated" air, since air that no longer contains oxygen is almost all E941 Nitrogen. 

The other gases in air are present in much lower concentrations.
E941 Nitrogen compounds are found in foods, fertilizers, poisons, and explosives. 
Your body is 3% E941 Nitrogen by weight. 

All living organisms contain E941 Nitrogen.
E941 Nitrogen is responsible for the orange-red, blue-green, blue-violet, and deep violet colors of the aurora.
One way to prepare E941 Nitrogen gas is by liquefaction and fractional distillation from the atmosphere. 

Liquid E941 Nitrogen boils at 77 K (−196 °C, −321 °F). 
E941 Nitrogen freezes at 63 K (-210.01 °C).
Liquid E941 Nitrogen is a cryogenic fluid, capable of freezing skin on contact. 

While the Leidenfrost effect protects skin from very brief exposure (less than one second), ingesting liquid E941 Nitrogen can cause severe injury. 
When liquid E941 Nitrogen is used to make ice cream, the E941 Nitrogen vaporizes. 
E941 Nitrogen has a valence of 3 or 5. 

E941 Nitrogen forms negatively charged ions (anions) that readily react with other nonmetals to form covalent bonds.
Saturn's largest moon, Titan, is the only moon in the solar system with a dense atmosphere. 
E941 Nitrogen's atmosphere consists of over 98% E941 Nitrogen.

From the Latin word nitrum, Greek Nitron, native soda; and genes, forming. 
E941 Nitrogen was discovered by chemist and physician Daniel Rutherford in 1772. 
He removed oxygen and carbon dioxide from air and showed that the residual gas would not support combustion or living organisms. 

At the same time there were other noted scientists working on the problem of E941 Nitrogen. 
These included Scheele, Cavendish, Priestley, and others. 
They called it "burnt" or" dephlogisticated air," which meant air without oxygen.

PROPERTIES of E941 NITROGEN:
-ATOMIC:
A E941 Nitrogen atom has seven electrons. 
In the ground state, they are arranged in the electron configuration 1s2 2s2 2p1x 2p1y 2p1z. 

E941 Nitrogen, therefore, has five valence electrons in the 2s and 2p orbitals, three of which (the p-electrons) are unpaired. 
E941 Nitrogen has one of the highest electronegativities among the elements (3.04 on the Pauling scale), exceeded only by chlorine (3.16), oxygen (3.44), and fluorine (3.98). 
(The light noble gases, helium, neon, and argon, would presumably also be more electronegative, and in fact are on the Allen scale.) 

Following periodic trends, E941 Nitrogen's single-bond covalent radius of 71 pm is smaller than those of boron (84 pm) and carbon (76 pm), while E941 Nitrogen is larger than those of oxygen (66 pm) and fluorine (57 pm). 
The nitride anion, N3−, is much larger at 146 pm, similar to that of the oxide (O2−: 140 pm) and fluoride (F−: 133 pm) anions. 

The first three ionisation energies of E941 Nitrogen are 1.402, 2.856, and 4.577 MJ•mol−1, and the sum of the fourth and fifth is 16.920 MJ•mol−1. 
Due to these very high figures, E941 Nitrogen has no simple cationic chemistry. 

The lack of radial nodes in the 2p subshell is directly responsible for many of the anomalous properties of the first row of the p-block, especially in E941 Nitrogen, oxygen, and fluorine. 
The 2p subshell is very small and has a very similar radius to the 2s shell, facilitating orbital hybridisation. 

E941 Nitrogen also results in very large electrostatic forces of attraction between the nucleus and the valence electrons in the 2s and 2p shells, resulting in very high electronegativities. 

Hypervalency is almost unknown in the 2p elements for the same reason, because the high electronegativity makes it difficult for a small E941 Nitrogen atom to be a central atom in an electron-rich three-center four-electron bond since it would tend to attract the electrons strongly to itself. 

Thus, despite E941 Nitrogen's position at the head of group 15 in the periodic table, E941 Nitrogen's chemistry shows huge differences from that of its heavier congeners phosphorus, arsenic, antimony, and bismuth.
E941 Nitrogen may be usefully compared to its horizontal neighbours carbon and oxygen as well as its vertical neighbours in the pnictogen column, phosphorus, arsenic, antimony, and bismuth. 

Although each period 2 element from lithium to oxygen shows some similarities to the period 3 element in the next group (from magnesium to chlorine; these are known as diagonal relationships), their degree drops off abruptly past the boron–silicon pair. 

The similarities of E941 Nitrogen to sulfur are mostly limited to sulfur nitride ring compounds when both elements are the only ones present.
E941 Nitrogen does not share the proclivity of carbon for catenation. 

Like carbon, E941 Nitrogen tends to form ionic or metallic compounds with metals. 
E941 Nitrogen forms an extensive series of nitrides with carbon, including those with chain-, graphitic-, and fullerenic-like structures.

E941 Nitrogen resembles oxygen with E941 Nitrogen's high electronegativity and concomitant capability for hydrogen bonding and the ability to form coordination complexes by donating its lone pairs of electrons. 
There are some parallels between the chemistry of ammonia NH3 and water H2O. 

For example, the capacity of both compounds to be protonated to give NH4+ and H3O+ or deprotonated to give NH2− and OH−, with all of these able to be isolated in solid compounds.
E941 Nitrogen shares with both its horizontal neighbours a preference for forming multiple bonds, typically with carbon, oxygen, or other E941 Nitrogen atoms, through pπ–pπ interactions. 

Thus, for example, E941 Nitrogen occurs as diatomic molecules and therefore has very much lower melting (−210 °C) and boiling points (−196 °C) than the rest of its group, as the N2 molecules are only held together by weak van der Waals interactions and there are very few electrons available to create significant instantaneous dipoles. 

This is not possible for its vertical neighbours; thus, the E941 Nitrogen oxides, nitrites, nitrates, nitro-, nitroso-, azo-, and diazo-compounds, azides, cyanates, thiocyanates, and imino-derivatives find no echo with phosphorus, arsenic, antimony, or bismuth. 

By the same token, however, the complexity of the phosphorus oxoacids finds no echo with E941 Nitrogen. 
Setting aside their differences, E941 Nitrogen and phosphorus form an extensive series of compounds with one another; these have chain, ring, and cage structures.

ISOTOPES of E941 NITROGEN:
E941 Nitrogen has two stable isotopes: 14N and 15N. 
The first is much more common, making up 99.634% of natural E941 Nitrogen, and the second (which is slightly heavier) makes up the remaining 0.366%. 

This leads to an atomic weight of around 14.007 u. 
Both of these stable isotopes are produced in the CNO cycle in stars, but 14N is more common as E941 Nitrogen's neutron capture is the rate-limiting step. 

14N is one of the five stable odd–odd nuclides (a nuclide having an odd number of protons and neutrons); the other four are 2H, 6Li, 10B, and 180mTa.
The relative abundance of 14N and 15N is practically constant in the atmosphere but can vary elsewhere, due to natural isotopic fractionation from biological redox reactions and the evaporation of natural ammonia or nitric acid. 

Biologically mediated reactions (e.g., assimilation, nitrification, and denitrification) strongly control E941 Nitrogen dynamics in the soil. 
These reactions typically result in 15N enrichment of the substrate and depletion of the product.

The heavy isotope 15N was first discovered by S. M. Naudé in 1929, and soon after heavy isotopes of the neighbouring elements oxygen and carbon were discovered. 
E941 Nitrogen presents one of the lowest thermal neutron capture cross-sections of all isotopes. 

E941 Nitrogen is frequently used in nuclear magnetic resonance (NMR) spectroscopy to determine the structures of E941 Nitrogen-containing molecules, due to E941 Nitrogen's fractional nuclear spin of one-half, which offers advantages for NMR such as narrower line width. 

14N, though also theoretically usable, has an integer nuclear spin of one and thus has a quadrupole moment that leads to wider and less useful spectra. 
15N NMR nevertheless has complications not encountered in the more common 1H and 13C NMR spectroscopy. 
The low natural abundance of 15N (0.36%) significantly reduces sensitivity, a problem which is only exacerbated by its low gyromagnetic ratio, (only 10.14% that of 1H). 

As a result, the signal-to-noise ratio for 1H is about 300 times as much as that for 15N at the same magnetic field strength. 
This may be somewhat alleviated by isotopic enrichment of 15N by chemical exchange or fractional distillation. 
15N-enriched compounds have the advantage that under standard conditions, they do not undergo chemical exchange of their E941 Nitrogen atoms with atmospheric E941 Nitrogen, unlike compounds with labelled hydrogen, carbon, and oxygen isotopes that must be kept away from the atmosphere. 

The 15N:14N ratio is commonly used in stable isotope analysis in the fields of geochemistry, hydrology, paleoclimatology and paleoceanography, where it is called δ15N.
Of the ten other isotopes produced synthetically, ranging from 12N to 23N, 13N has a half-life of ten minutes and the remaining isotopes have half-lives on the order of seconds (16N and 17N) or milliseconds. 
No other E941 Nitrogen isotopes are possible as they would fall outside the nuclear drip lines, leaking out a proton or neutron. 

Given the half-life difference, 13N is the most important E941 Nitrogen radioisotope, being relatively long-lived enough to use in positron emission tomography (PET), although its half-life is still short and thus E941 Nitrogen must be produced at the venue of the PET, for example in a cyclotron via proton bombardment of 16O producing 13N and an alpha particle.

The radioisotope 16N is the dominant radionuclide in the coolant of pressurised water reactors or boiling water reactors during normal operation. 
E941 Nitrogen is produced from 16O (in water) via an (n,p) reaction, in which the 16O atom captures a neutron and expels a proton. 
E941 Nitrogen has a short half-life of about 7.1 s, but during E941 Nitrogen's decay back to 16O produces high-energy gamma radiation (5 to 7 MeV). 

Because of this, access to the primary coolant piping in a pressurised water reactor must be restricted during reactor power operation. 
E941 Nitrogen is a sensitive and immediate indicator of leaks from the primary coolant system to the secondary steam cycle, and is the primary means of detection for such leaks.

ALLOTROPES of E941 NITROGEN:
Atomic E941 Nitrogen, also known as active E941 Nitrogen, is highly reactive, being a triradical with three unpaired electrons. 

Free E941 Nitrogen atoms easily react with most elements to form nitrides, and even when two free E941 Nitrogen atoms collide to produce an excited N2 molecule, they may release so much energy on collision with even such stable molecules as carbon dioxide and water to cause homolytic fission into radicals such as CO and O or OH and H. 

Atomic E941 Nitrogen is prepared by passing an electric discharge through E941 Nitrogen gas at 0.1–2 mmHg, which produces atomic E941 Nitrogen along with a peach-yellow emission that fades slowly as an afterglow for several minutes even after the discharge terminates.

Given the great reactivity of atomic E941 Nitrogen, elemental E941 Nitrogen usually occurs as molecular N2, diE941 Nitrogen. 
E941 Nitrogen is a colourless, odourless, and tasteless diamagnetic gas at standard conditions: E941 Nitrogen melts at −210 °C and boils at −196 °C. 

DiE941 Nitrogen is mostly unreactive at room temperature, but E941 Nitrogen will nevertheless react with lithium metal and some transition metal complexes. 
This is due to its bonding, which is unique among the diatomic elements at standard conditions in that it has an N≡N triple bond. 

Triple bonds have short bond lengths (in this case, 109.76 pm) and high dissociation energies (in this case, 945.41 kJ/mol), and are thus very strong, explaining diE941 Nitrogen's low level of chemical reactivity.

Other E941 Nitrogen oligomers and polymers may be possible. 
If they could be synthesised, they may have potential applications as materials with a very high energy density, that could be used as powerful propellants or explosives. 

Under extremely high pressures (1.1 million atm) and high temperatures (2000 K), as produced in a diamond anvil cell, E941 Nitrogen polymerises into the single-bonded cubic gauche crystal structure. 

This structure is similar to that of diamond, and both have extremely strong covalent bonds, resulting in its nickname "E941 Nitrogen diamond".

At atmospheric pressure, molecular E941 Nitrogen condenses (liquefies) at 77 K (−195.79 °C) and freezes at 63 K (−210.01 °C) into the beta hexagonal close-packed crystal allotropic form. 
Below 35.4 K (−237.6 °C) E941 Nitrogen assumes the cubic crystal allotropic form (called the alpha phase). 

Liquid E941 Nitrogen, a colourless fluid resembling water in appearance, but with 80.8% of the density (the density of liquid E941 Nitrogen at its boiling point is 0.808 g/mL), is a common cryogen. 

Solid E941 Nitrogen has many crystalline modifications. 
E941 Nitrogen forms a significant dynamic surface coverage on Pluto and outer moons of the Solar System such as Triton. 

Even at the low temperatures of solid E941 Nitrogen it is fairly volatile and can sublime to form an atmosphere, or condense back into E941 Nitrogen frost. 
E941 Nitrogen is very weak and flows in the form of glaciers and on Triton geysers of E941 Nitrogen gas come from the polar ice cap region.

CHEMISTRY and COMPOUNDS of E941 NITROGEN:
DINITROGEN COMPLEXES:
The first example of a diE941 Nitrogen complex to be discovered was [Ru(NH3)5(N2)]2+ (see figure at right), and soon many other such complexes were discovered. 

These complexes, in which a E941 Nitrogen molecule donates at least one lone pair of electrons to a central metal cation, illustrate how N2 might bind to the metal(s) in E941 Nitrogenase and the catalyst for the Haber process: these processes involving diE941 Nitrogen activation are vitally important in biology and in the production of fertilisers.

DiNitrogen is able to coordinate to metals in five different ways. 
The more well-characterised ways are the end-on M←N≡N (η1) and M←N≡N→M (μ, bis-η1), in which the lone pairs on the E941 Nitrogen atoms are donated to the metal cation. 

The less well-characterised ways involve diE941 Nitrogen donating electron pairs from the triple bond, either as a bridging ligand to two metal cations (μ, bis-η2) or to just one (η2). 

The fifth and unique method involves triple-coordination as a bridging ligand, donating all three electron pairs from the triple bond (μ3-N2). 
A few complexes feature multiple N2 ligands and some feature N2 bonded in multiple ways. 

Since N2 is isoelectronic with carbon monoxide (CO) and acetylene (C2H2), the bonding in diE941 Nitrogen complexes is closely allied to that in carbonyl compounds, although N2 is a weaker σ-donor and π-acceptor than CO. 

Theoretical studies show that σ donation is a more important factor allowing the formation of the M–N bond than π back-donation, which mostly only weakens the N–N bond, and end-on (η1) donation is more readily accomplished than side-on (η2) donation.

Today, diE941 Nitrogen complexes are known for almost all the transition metals, accounting for several hundred compounds. 
They are normally prepared by three methods:

Replacing labile ligands such as H2O, H−, or CO directly by E941 Nitrogen: these are often reversible reactions that proceed at mild conditions.

Reducing metal complexes in the presence of a suitable coligand in excess under E941 Nitrogen gas. 
A common choice include replacing chloride ligands by dimethylphenylphosphine (PMe2Ph) to make up for the smaller number of E941 Nitrogen ligands attached than the original chlorine ligands.

Converting a ligand with N–N bonds, such as hydrazine or azide, directly into a diE941 Nitrogen ligand.
Occasionally the N≡N bond may be formed directly within a metal complex, for example by directly reacting coordinated ammonia (NH3) with nitrous acid (HNO2), but this is not generally applicable. 

Most diE941 Nitrogen complexes have colours within the range white-yellow-orange-red-brown; a few exceptions are known, such as the blue [{Ti(η5-C5H5)2}2-(N2)].

NITRIDES, AZIDES, and NITRIDO COMPLEXES of E941 NITROGEN:
E941 Nitrogen bonds to almost all the elements in the periodic table except the first three noble gases, helium, neon, and argon, and some of the very short-lived elements after bismuth, creating an immense variety of binary compounds with varying properties and applications. 

Many binary compounds are known: with the exception of the E941 Nitrogen hydrides, oxides, and fluorides, these are typically called nitrides. 
Many stoichiometric phases are usually present for most elements (e.g. MnN, Mn6N5, Mn3N2, Mn2N, Mn4N, and MnxN for 
9.2 < x < 25.3). 

They may be classified as "salt-like" (mostly ionic), covalent, "diamond-like", and metallic (or interstitial), although this classification has limitations generally stemming from the continuity of bonding types instead of the discrete and separate types that it implies. 

They are normally prepared by directly reacting a metal with E941 Nitrogen or ammonia (sometimes after heating), or by thermal decomposition of metal amides:

3 Ca + N2 → Ca3N2
3 Mg + 2 NH3 → Mg3N2 + 3 H2 (at 900 °C)
3 Zn(NH2)2 → Zn3N2 + 4 NH3

Many variants on these processes are possible. 
The most ionic of these nitrides are those of the alkali metals and alkaline earth metals, Li3N (Na, K, Rb, and Cs do not form stable nitrides for steric reasons) and M3N2 (M = Be, Mg, Ca, Sr, Ba). 

These can formally be thought of as salts of the N3− anion, although charge separation is not actually complete even for these highly electropositive elements.
However, the alkali metal azides NaN3 and KN3, featuring the linear N−3 anion, are well-known, as are Sr(N3)2 and Ba(N3)2. 

Azides of the B-subgroup metals (those in groups 11 through 16) are much less ionic, have more complicated structures, and detonate readily when shocked.

Many covalent binary nitrides are known. 
Examples include cyanogen ((CN)2), triphosphorus pentanitride (P3N5), disulfur dinitride (S2N2), and tetrasulfur tetranitride (S4N4). 

The essentially covalent silicon nitride (Si3N4) and germanium nitride (Ge3N4) are also known: silicon nitride in particular would make a promising ceramic if not for the difficulty of working with and sintering it. 

In particular, the group 13 nitrides, most of which are promising semiconductors, are isoelectronic with graphite, diamond, and silicon carbide and have similar structures: their bonding changes from covalent to partially ionic to metallic as the group is descended. 

In particular, since the B–N unit is isoelectronic to C–C, and carbon is essentially intermediate in size between boron and E941 Nitrogen, much of organic chemistry finds an echo in boron–E941 Nitrogen chemistry, such as in borazine ("inorganic benzene"). 

Nevertheless, the analogy is not exact due to the ease of nucleophilic attack at boron due to its deficiency in electrons, which is not possible in a wholly carbon-containing ring.

The largest category of nitrides are the interstitial nitrides of formulae MN, M2N, and M4N (although variable composition is perfectly possible), where the small E941 Nitrogen atoms are positioned in the gaps in a metallic cubic or hexagonal close-packed lattice. 

They are opaque, very hard, and chemically inert, melting only at very high temperatures (generally over 2500 °C). 
They have a metallic lustre and conduct electricity as do metals. 
They hydrolyse only very slowly to give ammonia or E941 Nitrogen.

The nitride anion (N3−) is the strongest π donor known amongst ligands (the second-strongest is O2−). 
Nitrido complexes are generally made by thermal decomposition of azides or by deprotonating ammonia, and they usually involve a terminal {≡N}3− group. 

The linear azide anion (N−3), being isoelectronic with nitrous oxide, carbon dioxide, and cyanate, forms many coordination complexes. Further catenation is rare, although N4−4 (isoelectronic with carbonate and nitrate) is known.

HYDRIDES of E941 NITROGEN:
Industrially, ammonia (NH3) is the most important compound of E941 Nitrogen and is prepared in larger amounts than any other compound, because it contributes significantly to the nutritional needs of terrestrial organisms by serving as a precursor to food and fertilisers. 

It is a colourless alkaline gas with a characteristic pungent smell. 
The presence of hydrogen bonding has very significant effects on ammonia, conferring on it its high melting (−78 °C) and boiling (−33 °C) points. 

As a liquid, it is a very good solvent with a high heat of vaporisation (enabling it to be used in vacuum flasks), that also has a low viscosity and electrical conductivity and high dielectric constant, and is less dense than water. 

However, the hydrogen bonding in NH3 is weaker than that in H2O due to the lower electronegativity of E941 Nitrogen compared to oxygen and the presence of only one lone pair in NH3 rather than two in H2O. 
It is a weak base in aqueous solution (pKb 4.74); its conjugate acid is ammonium, NH+4. 
It can also act as an extremely weak acid, losing a proton to produce the amide anion, NH−2. 

It thus undergoes self-dissociation, similar to water, to produce ammonium and amide. 
Ammonia burns in air or oxygen, though not readily, to produce E941 Nitrogen gas; it burns in fluorine with a greenish-yellow flame to give E941 Nitrogen trifluoride. 

Reactions with the other nonmetals are very complex and tend to lead to a mixture of products. 
Ammonia reacts on heating with metals to give nitrides.

Many other binary E941 Nitrogen hydrides are known, but the most important are hydrazine (N2H4) and hydrogen azide (HN3). 
Although it is not a E941 Nitrogen hydride, hydroxylamine (NH2OH) is similar in properties and structure to ammonia and hydrazine as well. 

Hydrazine is a fuming, colourless liquid that smells similarly to ammonia. 
Its physical properties are very similar to those of water (melting point 2.0 °C, boiling point 113.5 °C, density 1.00 g/cm3). 

Despite it being an endothermic compound, it is kinetically stable. 
It burns quickly and completely in air very exothermically to give E941 Nitrogen and water vapour. 
It is a very useful and versatile reducing agent and is a weaker base than ammonia. 

It is also commonly used as a rocket fuel.
Hydrazine is generally made by reaction of ammonia with alkaline sodium hypochlorite in the presence of gelatin or glue:

NH3 + OCl− → NH2Cl + OH−
NH2Cl + NH3 → N2H+5 + Cl− (slow)
N2H+5 + OH− → N2H4 + H2O (fast)

(The attacks by hydroxide and ammonia may be reversed, thus passing through the intermediate NHCl− instead.) 
The reason for adding gelatin is that it removes metal ions such as Cu2+ that catalyses the destruction of hydrazine by reaction with monochloramine (NH2Cl) to produce ammonium chloride and E941 Nitrogen.

Hydrogen azide (HN3) was first produced in 1890 by the oxidation of aqueous hydrazine by nitrous acid. 
It may be considered the conjugate acid of the azide anion, and is similarly analogous to the hydrohalic acids.

HALIDES and OXOHALIDES of E941 NITROGEN:
All four simple E941 Nitrogen trihalides are known. 
A few mixed halides and hydrohalides are known, but are mostly unstable; examples include NClF2, NCl2F, NBrF2, NF2H, NFH2, NCl2H, and NClH2.

Five E941 Nitrogen fluorides are known. 
E941 Nitrogen trifluoride (NF3, first prepared in 1928) is a colourless and odourless gas that is thermodynamically stable, and most readily produced by the electrolysis of molten ammonium fluoride dissolved in anhydrous hydrogen fluoride. 

Like carbon tetrafluoride, it is not at all reactive and is stable in water or dilute aqueous acids or alkalis. 
Only when heated does it act as a fluorinating agent, and it reacts with copper, arsenic, antimony, and bismuth on contact at high temperatures to give tetrafluorohydrazine (N2F4). 

The cations NF+4 and N2F+3 are also known (the latter from reacting tetrafluorohydrazine with strong fluoride-acceptors such as arsenic pentafluoride), as is ONF3, which has aroused interest due to the short N–O distance implying partial double bonding and the highly polar and long N–F bond. 

Tetrafluorohydrazine, unlike hydrazine itself, can dissociate at room temperature and above to give the radical NF2•. 
Fluorine azide (FN3) is very explosive and thermally unstable. 

DiE941 Nitrogen difluoride (N2F2) exists as thermally interconvertible cis and trans isomers, and was first found as a product of the thermal decomposition of FN3.

E941 Nitrogen trichloride (NCl3) is a dense, volatile, and explosive liquid whose physical properties are similar to those of carbon tetrachloride, although one difference is that NCl3 is easily hydrolysed by water while CCl4 is not. 

It was first synthesised in 1811 by Pierre Louis Dulong, who lost three fingers and an eye to its explosive tendencies. 
As a dilute gas it is less dangerous and is thus used industrially to bleach and sterilise flour. 
E941 Nitrogen tribromide (NBr3), first prepared in 1975, is a deep red, temperature-sensitive, volatile solid that is explosive even at −100 °C. 

E941 Nitrogen triiodide (NI3) is still more unstable and was only prepared in 1990. 
Its adduct with ammonia, which was known earlier, is very shock-sensitive: it can be set off by the touch of a feather, shifting air currents, or even alpha particles. 

For this reason, small amounts of E941 Nitrogen triiodide are sometimes synthesised as a demonstration to high school chemistry students or as an act of "chemical magic". 
Chlorine azide (ClN3) and bromine azide (BrN3) are extremely sensitive and explosive.

Two series of E941 Nitrogen oxohalides are known: the nitrosyl halides (XNO) and the nitryl halides (XNO2). 
The first are very reactive gases that can be made by directly halogenating nitrous oxide. 
Nitrosyl fluoride (NOF) is colourless and a vigorous fluorinating agent. 

Nitrosyl chloride (NOCl) behaves in much the same way and has often been used as an ionising solvent. 
Nitrosyl bromide (NOBr) is red. The reactions of the nitryl halides are mostly similar: nitryl fluoride (FNO2) and nitryl chloride (ClNO2) are likewise reactive gases and vigorous halogenating agents.

OXIDES of E941 NITROGEN:
E941 Nitrogen forms nine molecular oxides, some of which were the first gases to be identified: N2O (nitrous oxide), NO (nitric oxide), N2O3 (diE941 Nitrogen trioxide), NO2 (E941 Nitrogen dioxide), N2O4 (diE941 Nitrogen tetroxide), N2O5 (diE941 Nitrogen pentoxide), N4O (nitrosylazide), and N(NO2)3 (trinitramide). 

All are thermally unstable towards decomposition to their elements. 
One other possible oxide that has not yet been synthesised is oxatetrazole (N4O), an aromatic ring.

Nitrous oxide (N2O), better known as laughing gas, is made by thermal decomposition of molten ammonium nitrate at 250 °C. This is a redox reaction and thus nitric oxide and E941 Nitrogen are also produced as byproducts. 

It is mostly used as a propellant and aerating agent for sprayed canned whipped cream, and was formerly commonly used as an anaesthetic. 
Despite appearances, it cannot be considered to be the anhydride of hyponitrous acid (H2N2O2) because that acid is not produced by the dissolution of nitrous oxide in water. 

It is rather unreactive (not reacting with the halogens, the alkali metals, or ozone at room temperature, although reactivity increases upon heating) and has the unsymmetrical structure N–N–O (N≡N+O−↔−N=N+=O): above 600 °C it dissociates by breaking the weaker N–O bond. 

Nitric oxide (NO) is the simplest stable molecule with an odd number of electrons. 
In mammals, including humans, it is an important cellular signaling molecule involved in many physiological and pathological processes. 

It is formed by catalytic oxidation of ammonia. 
It is a colourless paramagnetic gas that, being thermodynamically unstable, decomposes to E941 Nitrogen and oxygen gas at 1100–1200 °C. 

Its bonding is similar to that in E941 Nitrogen, but one extra electron is added to a π* antibonding orbital and thus the bond order has been reduced to approximately 2.5; hence dimerisation to O=N–N=O is unfavourable except below the boiling point (where the cis isomer is more stable) because it does not actually increase the total bond order and because the unpaired electron is delocalised across the NO molecule, granting it stability. 

There is also evidence for the asymmetric red dimer O=N–O=N when nitric oxide is condensed with polar molecules. 
It reacts with oxygen to give brown E941 Nitrogen dioxide and with halogens to give nitrosyl halides. 
It also reacts with transition metal compounds to give nitrosyl complexes, most of which are deeply coloured.

Blue diE941 Nitrogen trioxide (N2O3) is only available as a solid because it rapidly dissociates above its melting point to give nitric oxide, E941 Nitrogen dioxide (NO2), and diE941 Nitrogen tetroxide (N2O4). 

The latter two compounds are somewhat difficult to study individually because of the equilibrium between them, although sometimes diE941 Nitrogen tetroxide can react by heterolytic fission to nitrosonium and nitrate in a medium with high dielectric constant. 

E941 Nitrogen dioxide is an acrid, corrosive brown gas. 
Both compounds may be easily prepared by decomposing a dry metal nitrate. 
Both react with water to form nitric acid. 

DiE941 Nitrogen tetroxide is very useful for the preparation of anhydrous metal nitrates and nitrato complexes, and it became the storable oxidiser of choice for many rockets in both the United States and USSR by the late 1950s. 

This is because it is a hypergolic propellant in combination with a hydrazine-based rocket fuel and can be easily stored since it is liquid at room temperature.

The thermally unstable and very reactive diE941 Nitrogen pentoxide (N2O5) is the anhydride of nitric acid, and can be made from it by dehydration with phosphorus pentoxide. 
It is of interest for the preparation of explosives. 

It is a deliquescent, colourless crystalline solid that is sensitive to light. 
In the solid state it is ionic with structure [NO2]+[NO3]−; as a gas and in solution it is molecular O2N–O–NO2. 

Hydration to nitric acid comes readily, as does analogous reaction with hydrogen peroxide giving peroxonitric acid (HOONO2). 
It is a violent oxidising agent. 
Gaseous diE941 Nitrogen pentoxide decomposes as follows:

N2O5 ⇌ NO2 + NO3 → NO2 + O2 + NO
N2O5 + NO ⇌ 3 NO2

OXOACIDS, OXOANIONS, and OXOACID SALTS of E941 NITROGEN:
Many E941 Nitrogen oxoacids are known, though most of them are unstable as pure compounds and are known only as aqueous solution or as salts. 

Hyponitrous acid (H2N2O2) is a weak diprotic acid with the structure HON=NOH (pKa1 6.9, pKa2 11.6). 
Acidic solutions are quite stable but above pH 4 base-catalysed decomposition occurs via [HONNO]− to nitrous oxide and the hydroxide anion. 

Hyponitrites (involving the N2O2−2 anion) are stable to reducing agents and more commonly act as reducing agents themselves. 
They are an intermediate step in the oxidation of ammonia to nitrite, which occurs in the E941 Nitrogen cycle. 
Hyponitrite can act as a bridging or chelating bidentate ligand.

Nitrous acid (HNO2) is not known as a pure compound, but is a common component in gaseous equilibria and is an important aqueous reagent: its aqueous solutions may be made from acidifying cool aqueous nitrite (NO−2, bent) solutions, although already at room temperature disproportionation to nitrate and nitric oxide is significant. 
It is a weak acid with pKa 3.35 at 18 °C. 

They may be titrimetrically analysed by their oxidation to nitrate by permanganate. 
They are readily reduced to nitrous oxide and nitric oxide by sulfur dioxide, to hyponitrous acid with tin(II), and to ammonia with hydrogen sulfide. 
Salts of hydrazinium N2H+5 react with nitrous acid to produce azides which further react to give nitrous oxide and E941 Nitrogen. 

Sodium nitrite is mildly toxic in concentrations above 100 mg/kg, but small amounts are often used to cure meat and as a preservative to avoid bacterial spoilage. 
It is also used to synthesise hydroxylamine and to diazotise primary aromatic amines as follows:

ArNH2 + HNO2 → [ArNN]Cl + 2 H2O
Nitrite is also a common ligand that can coordinate in five ways. 
The most common are nitro (bonded from the E941 Nitrogen) and nitrito (bonded from an oxygen). 
Nitro-nitrito isomerism is common, where the nitrito form is usually less stable.

Nitric acid (HNO3) is by far the most important and the most stable of the E941 Nitrogen oxoacids. 
It is one of the three most used acids (the other two being sulfuric acid and hydrochloric acid) and was first discovered by the alchemists in the 13th century. 

It is made by catalytic oxidation of ammonia to nitric oxide, which is oxidised to E941 Nitrogen dioxide, and then dissolved in water to give concentrated nitric acid. 
In the United States of America, over seven million tonnes of nitric acid are produced every year, most of which is used for nitrate production for fertilisers and explosives, among other uses. 

Anhydrous nitric acid may be made by distilling concentrated nitric acid with phosphorus pentoxide at low pressure in glass apparatus in the dark. 

It can only be made in the solid state, because upon melting it spontaneously decomposes to E941 Nitrogen dioxide, and liquid nitric acid undergoes self-ionisation to a larger extent than any other covalent liquid as follows:
2 HNO3 ⇌ H2NO+3 + NO−3 ⇌ H2O + [NO2]+ + [NO3]−

Two hydrates, HNO3•H2O and HNO3•3H2O, are known that can be crystallised. 
It is a strong acid and concentrated solutions are strong oxidising agents, though gold, platinum, rhodium, and iridium are immune to attack. 

A 3:1 mixture of concentrated hydrochloric acid and nitric acid, called aqua regia, is still stronger and successfully dissolves gold and platinum, because free chlorine and nitrosyl chloride are formed and chloride anions can form strong complexes. 
In concentrated sulfuric acid, nitric acid is protonated to form nitronium, which can act as an electrophile for aromatic nitration:
HNO3 + 2 H2SO4 ⇌ NO+2 + H3O+ + 2 HSO−4

The thermal stabilities of nitrates (involving the trigonal planar NO−3 anion) depends on the basicity of the metal, and so do the products of decomposition (thermolysis), which can vary between the nitrite (for example, sodium), the oxide (potassium and lead), or even the metal itself (silver) depending on their relative stabilities. 

Nitrate is also a common ligand with many modes of coordination.
Finally, although orthonitric acid (H3NO4), which would be analogous to orthophosphoric acid, does not exist, the tetrahedral orthonitrate anion NO3−4 is known in its sodium and potassium salts:

These white crystalline salts are very sensitive to water vapour and carbon dioxide in the air:
Na3NO4 + H2O + CO2 → NaNO3 + NaOH + NaHCO3
Despite its limited chemistry, the orthonitrate anion is interesting from a structural point of view due to its regular tetrahedral shape and the short N–O bond lengths, implying significant polar character to the bonding.

ORGANIC E941 NITROGEN COMPOUNDS:
E941 Nitrogen is one of the most important elements in organic chemistry. 
Many organic functional groups involve a carbon–E941 Nitrogen bond, such as amides (RCONR2), amines (R3N), imines (RC(=NR)R), imides (RCO)2NR, azides (RN3), azo compounds (RN2R), cyanates and isocyanates (ROCN or RCNO), nitrates (RONO2), nitriles and isonitriles (RCN or RNC), nitrites (RONO), nitro compounds (RNO2), nitroso compounds (RNO), oximes (RCR=NOH), and pyridine derivatives. 

C–N bonds are strongly polarised towards E941 Nitrogen. 
In these compounds, E941 Nitrogen is usually trivalent (though it can be tetravalent in quaternary ammonium salts, R4N+), with a lone pair that can confer basicity on the compound by being coordinated to a proton. 

This may be offset by other factors: for example, amides are not basic because the lone pair is delocalised into a double bond (though they may act as acids at very low pH, being protonated at the oxygen), and pyrrole is not acidic because the lone pair is delocalised as part of an aromatic ring. 

The amount of E941 Nitrogen in a chemical substance can be determined by the Kjeldahl method. 
In particular, E941 Nitrogen is an essential component of nucleic acids, amino acids and thus proteins, and the energy-carrying molecule adenosine triphosphate and is thus vital to all life on Earth.

Although the other applications are important, by far the greatest bulk of elemental E941 Nitrogen is consumed in the manufacture of E941 Nitrogen compounds. 
The triple bond between atoms in the E941 Nitrogen molecules is so strong (226 kilocalories per mole, more than twice that of molecular hydrogen) that it is difficult to cause molecular E941 Nitrogen to enter into other combinations.

The chief commercial method of fixing E941 Nitrogen (incorporating elemental E941 Nitrogen into compounds) is the Haber-Bosch process for synthesizing ammonia. 
This process was developed during World War I to lessen the dependence of Germany on Chilean nitrate. 
E941 Nitrogen involves the direct synthesis of ammonia from its elements.

With oxygen, E941 Nitrogen forms several oxides, including nitrous oxide, N2O, in which E941 Nitrogen is in the +1 oxidation state; nitric oxide, NO, in which it is in the +2 state; and E941 Nitrogen dioxide, NO2, in which it is in the +4 state. 
Sodium nitrate (NaNO3) and potassium nitrate (KNO3) are formed by the decomposition of organic matter with compounds of these metals present. 

In certain dry areas of the world these saltpeters are found in quantity and are used as fertilizers. 
Other inorganic E941 Nitrogen compounds are nitric acid (HNO3), ammonia (NH3), the oxides (NO, NO2, N2O4, N2O), cyanides (CN-), etc.

The E941 Nitrogen cycle is one of the most important processes in nature for living organisms. 
Although E941 Nitrogen gas is relatively inert, bacteria in the soil are capable of “fixing” the E941 Nitrogen into a usable form (as a fertilizer) for plants. 
In other words, Nature has provided a method to produce E941 Nitrogen for plants to grow. 

Animals eat the plant material where the E941 Nitrogen has been incorporated into their system, primarily as protein. 
The cycle is completed when other bacteria convert the waste E941 Nitrogen compounds back to E941 Nitrogen gas. 
E941 Nitrogen is crucial to life, as it is a component of all proteins.

PRODUCTION of E941 NITROGEN:
E941 Nitrogen gas is an industrial gas produced by the fractional distillation of liquid air, or by mechanical means using gaseous air (pressurised reverse osmosis membrane or pressure swing adsorption). 

E941 Nitrogen gas generators using membranes or pressure swing adsorption (PSA) are typically more cost and energy efficient than bulk delivered E941 Nitrogen. 
Commercial E941 Nitrogen is often a byproduct of air-processing for industrial concentration of oxygen for steelmaking and other purposes. 

When supplied compressed in cylinders it is often called OFN (oxygen-free E941 Nitrogen). 
Commercial-grade E941 Nitrogen already contains at most 20 ppm oxygen, and specially purified grades containing at most 2 ppm oxygen and 10 ppm argon are also available.

In a chemical laboratory, E941 Nitrogen is prepared by treating an aqueous solution of ammonium chloride with sodium nitrite.
NH4Cl + NaNO2 → N2 + NaCl + 2 H2O

Small amounts of the impurities NO and HNO3 are also formed in this reaction. 
The impurities can be removed by passing the gas through aqueous sulfuric acid containing potassium dichromate. 
Very pure E941 Nitrogen can be prepared by the thermal decomposition of barium azide or sodium azide.
2 NaN3 → 2 Na + 3 N2

Commercial production of E941 Nitrogen is largely by fractional distillation of liquefied air. 
The boiling temperature of E941 Nitrogen is −195.8 °C (−320.4 °F), about 13 °C (−23 °F) below that of oxygen, which is therefore left behind. 

E941 Nitrogen can also be produced on a large scale by burning carbon or hydrocarbons in air and separating the resulting carbon dioxide and water from the residual E941 Nitrogen. 

On a small scale, pure E941 Nitrogen is made by heating barium azide, Ba(N3)2. 
Various laboratory reactions that yield E941 Nitrogen include heating ammonium nitrite (NH4NO2) solutions, oxidation of ammonia by bromine water, and oxidation of ammonia by hot cupric oxide.

OCCURRENCE of E941 NITROGEN:
E941 Nitrogen is the most common pure element in the earth, making up 78.1% of the volume of the atmosphere (75.5% by mass), around 3.89 million gigatonnes. 

Despite this, E941 Nitrogen is not very abundant in Earth's crust, making up somewhere around 19 parts per million of this, on par with niobium, gallium, and lithium. 
(This represents 300,000 to a million gigatonnes of E941 Nitrogen, depending on the mass of the crust.) 

The only important E941 Nitrogen minerals are nitre (potassium nitrate, saltpetre) and soda nitre (sodium nitrate, Chilean saltpetre). 
However, these have not been an important source of nitrates since the 1920s, when the industrial synthesis of ammonia and nitric acid became common.

E941 Nitrogen compounds constantly interchange between the atmosphere and living organisms. 
E941 Nitrogen must first be processed, or "fixed", into a plant-usable form, usually ammonia. 

Some E941 Nitrogen fixation is done by lightning strikes producing the E941 Nitrogen oxides, but most is done by diazotrophic bacteria through enzymes known as E941 Nitrogenases (although today industrial E941 Nitrogen fixation to ammonia is also significant). 

When the ammonia is taken up by plants, E941 Nitrogen is used to synthesise proteins. 
These plants are then digested by animals who use the E941 Nitrogen compounds to synthesise their proteins and excrete E941 Nitrogen-bearing waste. 

Finally, these organisms die and decompose, undergoing bacterial and environmental oxidation and denitrification, returning free diE941 Nitrogen to the atmosphere. 

Industrial E941 Nitrogen fixation by the Haber process is mostly used as fertiliser, although excess E941 Nitrogen–bearing waste, when leached, leads to eutrophication of freshwater and the creation of marine dead zones, as E941 Nitrogen-driven bacterial growth depletes water oxygen to the point that all higher organisms die. 
Furthermore, nitrous oxide, which is produced during denitrification, attacks the atmospheric ozone layer.

Many saltwater fish manufacture large amounts of trimethylamine oxide to protect them from the high osmotic effects of their environment; conversion of this compound to dimethylamine is responsible for the early odour in unfresh saltwater fish. 

In animals, free radical nitric oxide (derived from an amino acid), serves as an important regulatory molecule for circulation.
Nitric oxide's rapid reaction with water in animals results in the production of its metabolite nitrite. 
Animal metabolism of E941 Nitrogen in proteins, in general, results in the excretion of urea, while animal metabolism of nucleic acids results in the excretion of urea and uric acid. 

The characteristic odour of animal flesh decay is caused by the creation of long-chain, E941 Nitrogen-containing amines, such as putrescine and cadaverine, which are breakdown products of the amino acids ornithine and lysine, respectively, in decaying proteins.

SOURCE of E941 NITROGEN:
E941 Nitrogen is synthetically produced through industrial processes, primarily by fractional distillation of liquid air.
The production method involves cooling atmospheric air to extremely low temperatures, causing the different components to liquefy at different points, allowing E941 Nitrogen to be separated from oxygen and other atmospheric gases.

E941 Nitrogen can also be produced through the Haber Process for commercial applications involving ammonia synthesis.
While the source material (atmospheric air) is natural and abundant, the production method involves industrial synthetic processes, classifying E941 Nitrogen as synthetically produced for food-grade applications.
E941 Nitrogen is not derived from animal, plant, microbial, or mineral sources.

PURPOSE of E941 NITROGEN IN PRODUCTS:
• Packaging Gas: 
E941 Nitrogen is employed to displace oxygen in food packaging, creating an inert atmosphere that inhibits oxidation and the growth of aerobic microorganisms.
This process extends the shelf life of perishable items without altering their taste or nutritional value.

• Propellant: 
In aerosol products, E941 Nitrogen serves as a propellant to expel contents without reacting with the product, ensuring safety and maintaining product integrity.

HEALTH CONSIDERATIONS of E941 NITROGEN:
E941 Nitrogen is chemically inert and does not react with food components, making it safe for use in food packaging and as a propellant.
There are no known adverse health effects associated with E941 Nitrogen's application as a food additive.

PHYSICAL and CHEMICAL PROPERTIES of E941 NITROGEN:
Appearance: colorless gas, liquid or solid
Standard atomic weight Ar°(N): [14.00643, 14.00728] 14.007±0.001 (abridged)
Atomic number (Z): 7
Group group: 15 (pnictogens)
Period period: 2
Block: p-block
Electron configuration: [He] 2s2 2p3
Electrons per shell: 2, 5
Phase at STP: gas

Melting point: (N2) 63.23[2] K ​(−209.86[2] °C, ​−345.75[2] °F)
Boiling point: (N2) 77.355 K ​(−195.795 °C, ​−320.431 °F)
Density (at STP): 1.2506 g/L[3] at 0 °C, 1013 mbar
when liquid (at b.p.): 0.808 g/cm3
Triple point: 63.151 K, ​12.52 kPa
Critical point: 126.21 K, 3.39 MPa
Heat of fusion: (N2) 0.72 kJ/mol
Heat of vaporisation: (N2) 5.57 kJ/mol
Molar heat capacity: (N2) 29.124 J/(mol·K)

Oxidation states: −3, −2, −1, 0,[4] +1, +2, +3, +4, +5 (a strongly acidic oxide)
Electronegativity: Pauling scale: 3.04
Ionisation energies:
1st: 1402.3 kJ/mol
2nd: 2856 kJ/mol
3rd: 4578.1 kJ/mol
Covalent radius: 71±1 pm
Van der Waals radius: 155 pm
Natural occurrence: primordial

Crystal structure: ​hexagonalHexagonal crystal structure for nitrogen
Speed of sound: 353 m/s (gas, at 27 °C)
Thermal conductivity: 25.83×10−3 W/(m⋅K)
Magnetic ordering: diamagnetic
Molecular Weight: 28.014    
XLogP3-AA: 0.1    
Hydrogen Bond Donor Count: 0    
Hydrogen Bond Acceptor Count: 2    
Rotatable Bond Count: 0    

Exact Mass: 28.006148008    
Monoisotopic Mass: 28.006148008    
Topological Polar Surface Area: 47.6 Ų    
Heavy Atom Count: 2    
Formal Charge: 0    
Complexity: 8    
Isotope Atom Count: 0    
Defined Atom Stereocenter Count: 0    
Undefined Atom Stereocenter Count: 0    

Defined Bond Stereocenter Count: 0    
Undefined Bond Stereocenter Count: 0    
Covalently-Bonded Unit Count: 1    
Compound Is Canonicalized: Yes
Atomic number: 7
Atomic mass: 14.0067 g.mol -1
Electronegativity according to Pauling: 3.0
Density: 1.25*10-3 g.cm-3 at 20°C
Melting point: -210 °C

Boiling point: -195.8 °C
Vanderwaals radius: 0.092 nm
Ionic radius: 0.171 nm (-3) ; 0.011 (+5) ; 0.016 (+3)
Isotopes: 4
Electronic shell: [ He ] 2s22p3
Energy of first ionisation: 1402 kJ.mol -1
Energy of second ionisation: 2856 kJ.mol -1
Energy of third ionisation: 4578 kJ.mol -1
Discovered by: Rutherford in 1772

Chemical formula : N 2
Purity level : ≥ 99.9%
Relative density (air = 1) : 0.97
Aspect : colorless gas
Odor : odorless gas
Limit of flammability in air : not flammable
Appearance Form: Compressed gas
Color: colorless
Odo:r odorless
Odor Threshold: No data available

pH: No data available
Melting point/freezing point: -209,99 °C
Initial boiling point and boiling range: -195,79 °C
Flash point: Not applicable
Evaporation rate: No data available
Flammability (solid, gas): No data available
Upper/lower flammability or explosive limits: No data available
Vapor pressure: No data available
Vapor density: No data available

Relative density: 0,97 g/cm3
Water solubility: No data available
Partition coefficient: n-octanol/water: No data available
Autoignition temperature: No data available
Decomposition temperature: No data available
Viscosity: No data available
Explosive properties: No data available
Oxidizing properties: No data available
Other safety information: No data available

Atomic number (number of protons in the nucleus): 7
Atomic symbol (on the Periodic Table of Elements): N
Atomic weight (average mass of the atom): 14.0067
Density: 0.0012506 grams per cubic centimeter
Phase at room temperature: Gas
Melting point: minus 321 degrees Fahrenheit (minus 210 degrees Celsius)

Boiling point: minus 320.42 F (minus 195.79 C)
Number of isotopes (atoms of the same element with a different number of neutrons): 16 including 2 stable ones
Most common isotopes: Nitrogen-14 (Abundance: 99.63 percent)
Molecular formula: n₂
Molecular weight: 28.014 g/mol
Atomic number: 7
CAS number: 7727-37-9
EC number: 231-783-9

FIRST AID MEASURES of E941 NITROGEN:
-Description of first-aid measures:
*General advice:
Consult a physician. 
*If inhaled:
If breathed in, move person into fresh air. 
Consult a physician.
*In case of skin contact:
Wash off with soap and plenty of water. 
Consult a physician.
*In case of eye contact:
Flush eyes with water as a precaution.
*If swallowed:
Rinse mouth with water. 
Consult a physician.
-Indication of any immediate medical attention and special treatment needed:
No data available

ACCIDENTAL RELEASE MEASURES of E941 NITROGEN:
-Environmental precautions:
Do not let product enter drains.
-Methods and materials for containment and cleaning up:
Clean up promptly by sweeping or vacuum.

FIRE FIGHTING MEASURES of E941 NITROGEN:
-Extinguishing media:
*Suitable extinguishing media:
Use water spray, alcohol-resistant foam, dry chemical or carbon dioxide.
-Further information:
Use water spray to cool unopened containers.

EXPOSURE CONTROLS/PERSONAL PROTECTION of E941 NITROGEN:
-Control parameters:
--Ingredients with workplace control parameters:
-Exposure controls:
--Appropriate engineering controls:
Handle in accordance with good industrial hygiene and safety practice. 
Wash hands before breaks and at the end of workday.
--Personal protective equipment:
*Eye/face protection:
Use equipment for eye protection.
*Skin protection:
Handle with gloves. 
Wash and dry hands.
-Control of environmental exposure:
Do not let product enter drains.

HANDLING and STORAGE of E941 NITROGEN:
-Conditions for safe storage, including any incompatibilities:
Store in cool place. 
Keep container tightly closed in a dry and well-ventilated place.
Contents under pressure.

STABILITY and REACTIVITY of E941 NITROGEN:
-Reactivity:
No data available
-Chemical stability:
Stable under recommended storage conditions.
-Possibility of hazardous reactions:
No data available
-Conditions to avoid:
No data available