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Nitrogen, 7N
Liquidnitrogen.jpg
Nitrogen
Allotropes see Allotropes of nitrogen
Appearance a gas, liquid or solid without color
Standard atomic weight Ar, std(N) [14.0064314.00728] conventional: 14.007
Nitrogen in the periodic table
Hydrogen Helium
Lithium Beryllium Boron Carbon Nitrogen Oxygen Fluorine Neon
Sodium Magnesium Aluminium Silicon Phosphorus Sulfur Chlorine Argon
Potassium Calcium Scandium Titanium Vanadium Chromium Manganese Iron Cobalt Nickel Copper Zinc Gallium Germanium Arsenic Selenium Bromine Krypton
Rubidium Strontium Yttrium Zirconium Niobium Molybdenum Technetium Ruthenium Rhodium Palladium Silver Cadmium Indium Tin Antimony Tellurium Iodine Xenon
Caesium Barium Lanthanum Cerium Praseodymium Neodymium Promethium Samarium Europium Gadolinium Terbium Dysprosium Holmium Erbium Thulium Ytterbium Lutetium Hafnium Tantalum Tungsten Rhenium Osmium Iridium Platinum Gold Mercury (element) Thallium Lead Bismuth Polonium Astatine Radon
Francium Radium Actinium Thorium Protactinium Uranium Neptunium Plutonium Americium Curium Berkelium Californium Einsteinium Fermium Mendelevium Nobelium Lawrencium Rutherfordium Dubnium Seaborgium Bohrium Hassium Meitnerium Darmstadtium Roentgenium Copernicium Nihonium Flerovium Moscovium Livermorium Tennessine Oganesson
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N

P
carbonnitrogenoxygen
Atomic number (Z) 7
Group group 15 (pnictogens)
Period period 2
Block   p
Electron configuration [He] 2s2 2p3
Electrons per shell 2, 5
Physical properties
Phase at STP gas
Melting point 63.15 K ​(-210.00 °C, ​-346.00 °F)
Boiling point 77.36 K ​(-195.79 °C, ​-320.33 °F)
Density (at STP) 1.251 g/L
when liquid (at b.p.) 0.808 g/cm3
Triple point 63.1526 K, ​12.53 kPa
Critical point 126.19 K, 3.3978 MPa
Heat of fusion (N2) 0.72 kJ/mol
Heat of vaporization (N2) 5.56 kJ/mol
Molar heat capacity (N2)
29.124 J/(mol·K)
Vapor pressure
P (Pa) 1 10 100 1 k 10 k 100 k
at T (K) 37 41 46 53 62 77
Atomic properties
Oxidation states −3, −2, −1, +1, +2, +3, +4, +5 (a strongly acidic oxide)
Electronegativity Pauling scale: 3.04
Ionization energies
  • (more)
Covalent radius 71±1 pm
Van der Waals radius 155 pm
Color lines in a spectral range
Spectral lines of nitrogen
Other properties
Natural occurrence primordial
Crystal structure ​hexagonal
Hexagonal crystal structure for nitrogen
Speed of sound (gas, 27 °C) 353 m/s
Thermal conductivity 25.83 × 10−3 W/(m⋅K)
Magnetic ordering diamagnetic
CAS Number 7727-37-9
History
Discovery Daniel Rutherford (1772)
Named by Jean-Antoine Chaptal (1790)
Main isotopes of nitrogen
Iso­tope Abun­dance Half-life (t1/2) Decay mode Pro­duct
13N syn 9.965 min ε 2.220 13C
14N 99.634% 14N is stable with 7 neutrons
15N 0.366% 15N is stable with 8 neutrons

Nitrogen is a nonmetal chemical element. It has the chemical symbol N and atomic number 7. More than 78 percent of the air we breathe is made of nitrogen.

A typical nitrogen atom has 7 protons and 7 neutrons. It also has 5 electrons in its outer shell.

What is Nitrogen Like?

Liquid nitrogen dsc04496
A cup of liquid nitrogen

Nitrogen is a gas that has no color or smell at normal temperatures. It usually joins with another nitrogen atom to form a nitrogen molecule (N2). The bond between these two atoms is very strong.

This strong bond is why nitrogen is found in many explosives. When an explosive is made, this bond is broken. When it explodes, the bond forms again, releasing a lot of energy.

Nitrogen turns into a liquid at -195.8°C. It becomes a solid at -210°C. If you squeeze nitrogen gas very hard, it can turn into a liquid without getting cold.

Because of its strong bond, nitrogen usually does not easily combine with other atoms. Lithium is one of the few elements that reacts with nitrogen without needing heat. Magnesium can also burn in nitrogen.

Nitrogen can make blue electric sparks. This blue color happens when nitrogen atoms get "excited." When they return to normal, they release light. Excited nitrogen can react with many things it normally wouldn't.

Nitrogen-glow
A bright electric spark in a tube filled with nitrogen

Nitrogen Compounds

Many important chemical compounds used in industry contain nitrogen. These include ammonia, nitric acid, nitrates, and cyanides. Nitrogen can exist in different forms, called oxidation states. Each form has its own set of compounds.

Where is Nitrogen Found and How is it Made?

Air is mostly nitrogen, making up about 78% of it. The rest is about 20.95% oxygen, a small amount of argon, and tiny bits of other gases like carbon dioxide and water vapor. Nitrogen is also found in some nitrates in the ground. You can also find nitrogen in proteins, which are in all living things.

To make pure liquid nitrogen, air is cooled down. Nitrogen turns into a liquid at a different temperature than oxygen, allowing them to be separated. It can also be made by heating certain chemical compounds, such as sodium azide.

Uses of Nitrogen

Nitrogen is used to stop things from reacting with oxygen in the air. For example, it fills crisp bags to keep snacks fresh. It's also used in some light bulbs and tires. Nitrogen helps make electronic parts like transistors. Liquid nitrogen is very cold and can be used to freeze things quickly.

Nitrogen compounds have many uses too:

History of Nitrogen

Nitrogen was discovered by Daniel Rutherford in 1772. He called it "noxious gas" or "fixed gas." Scientists noticed that this part of the air did not burn and that animals could not live in it. For a while, it was known as "azote." Many nitrogen compounds still use parts of this old name, like "azide" or "azine" (for example, hydrazine).

In 1910, Lord Rayleigh found that if an electric spark was passed through nitrogen, it created a very reactive form of nitrogen. This special nitrogen could then react with many metals and other compounds.

Safety with Nitrogen

Nitrogen itself is not poisonous. We breathe it safely every day as part of the air. However, we cannot breathe pure nitrogen by itself. This is because pure nitrogen does not have the oxygen our bodies need to live. If someone breathes pure nitrogen, they will simply pass out due to lack of oxygen.

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