Nitrogen facts for kids

	carbon ← nitrogen → oxygen
Appearance
	a gas, liquid or solid without color; ; Liquid nitrogen; ; Spectral lines of nitrogen
General properties
Name, symbol, number	nitrogen, N, 7
Pronunciation	/ˈnaɪtrədʒən/ NY-trə-jən
Element category	nonmetal
Group, period, block	15, 2, p
Standard atomic weight	14.007(1) g/mol
Electron configuration	[He] 2s2 2p3
Electrons per shell	2, 5 (Image)
Physical properties
Phase	gas
Density	(0 °C, 101.325 kPa); 1.251 g/L
Liquid density at b.p.	0.808 g/cm3
Melting point	63.15 K, -210.00 °C, -346.00 °F
Boiling point	77.36 K, -195.79 °C, -320.33 °F
Triple point	63.1526 K (-210°C), 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
Specific heat capacity	(25 °C) (N2); 29.124 J/(mol·K)
Vapor pressure
Atomic properties
Oxidation states	5, 4, 3, 2, 1, -1, -2, -3; (strongly acidic oxide)
Electronegativity	3.04 (Pauling scale)
Ionization 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
Miscellanea
Crystal structure	hexagonal
Magnetic ordering	diamagnetic
Thermal conductivity	(300 K) 25.83 × 10−3 W/(m·K)
Speed of sound	(gas, 27 °C) 353 m/s
CAS registry number	7727-37-9
Most stable isotopes
	Main article: Isotopes of nitrogen

Nitrogen is a nonmetal chemical element. The atmosphere contains more than 78 percent of nitrogen. It has the chemical symbol N and atomic number 7. Its stable inside typically contains 14 nucleons (7 protons and 7 neutrons). It has 5 electrons in its outer shell.

Properties

Cup of liquid nitrogen

Nitrogen is a colorless odorless gas at normal temperature. It is normally attached to another nitrogen atom, making a nitrogen molecule (N₂). The bond is very strong. That is why many explosives contain nitrogen. The bond is broken when the explosive is made. When it explodes the bond forms, releasing a lot of energy.

It turns into a liquid at -195.8°C and turns into a solid at -210°C. If it is compressed, it can be turned into a liquid without making it cold.

It usually does not combine with other atoms because of its strong bond. The bond prevents it from reacting. Lithium is one of the only chemical elements that react with nitrogen without being heated. Magnesium can burn in nitrogen. Nitrogen also makes blue electric sparks. The blue color is caused by the atoms being excited. When they get normal again, they release light. When nitrogen is excited, it reacts with many things that it does not normally react with.

A nice electric spark through a tube filled with nitrogen

Compounds

See also: Category:Nitrogen compounds

Many chemical compounds that are important for industrial purposes contain nitrogen ions. These include ammonia, nitric acid, nitrates and cyanides. Nitrogen comes in several oxidation states; -3, -2, -¹/₃, +1, +3, +4, and +5. Each of those oxidation states has its set of compounds.

Compounds in the -3 oxidation state are weak reducing agents. These include ammonia, ammonium, amide and nitrides. Amino acids and proteins contain nitrogen in this oxidation state. Hydrazine, a compound in the -2 oxidation state, is a strong reducing agent. Azides contain nitrogen in the -¹/₃ oxidation state. They are extremely powerful reducing agents, and most are very toxic.

Nitrous oxide contains nitrogen in the +1 oxidation state. It is used as an anesthetic. Compounds containing nitrogen in the +2 oxidation state, such as nitric oxide, are reducing agents. +3 oxidation state compounds are strong oxidizing agents and weak reducing agents. Nitrites are the most common +3 compounds. Compounds in the +4 oxidation state are strong oxidizing agents. They include nitrogen dioxide and dinitrogen tetroxide.

Compounds containing nitrogen in the +5 oxidation state are strong oxidizing agents. They are one of the more common groups of nitrogen compounds. They include nitric acid and dinitrogen pentoxide. They also include nitrates, which are used in explosives such as dynamite, nitroglycerin and trinitrotoluene.

Occurrence and preparation

Air is made up of about 78% nitrogen and about 20.95% oxygen, < 1% argon, and traces of other gasses such as carbon dioxide, and water vapor, among others. It is also in a few nitrates in the ground. Ammonium minerals are rare. Nitrogen is in proteins.

Pure liquid nitrogen can be made by cooling air. The nitrogen turns into a liquid at a different temperature than the oxygen. It can also be made by heating certain chemical compounds, such as sodium azide.

Uses

Liquid nitrogen used to freeze a balloon

Nitrogen is an element is used to prevent things from reacting with the oxygen in the air. It can be used to fill crisp bags and incandescent bulbs. It is also used to fill some tires. It can be used to make electric components like transistors. Liquid nitrogen can be used to freeze things.

Nitrogen compounds have many uses, such as anesthetics (nitrous oxide), explosives (dynamite), cleaners (ammonia), and meat (protein), and planes (fuel).

History

Nitrogen was discovered by Daniel Rutherford in 1772, who called it noxious gas or fixed gas. They discovered that part of air did not burn. It was found that animals died in it. It was known as "azote". Many nitrogen compounds also contain the "azide" or "azine" letters, such as hydrazine.

In 1910, Lord Rayleigh found out that when a spark was passed through nitrogen, it made a reactive form of nitrogen. This nitrogen reacted with many metals and compounds.

Safety

Nitrogen is not poisonous. We can safely breathe it when it is a part of air, but we cannot breathe pure nitrogen by itself, because it does not have the oxygen that we need to live. Anyone that inhales pure nitrogen will just pass out.

Related pages

List of common elements

Images for kids

Daniel Rutherford, discoverer of nitrogen
The shapes of the five orbitals occupied in nitrogen. The two colours show the phase or sign of the wave function in each region. From left to right: 1s, 2s (cutaway to show internal structure), 2px, 2py, 2pz.
Table of nuclides (Segrè chart) from carbon to fluorine (including nitrogen). Orange indicates proton emission (nuclides outside the proton drip line); pink for positron emission (inverse beta decay); black for stable nuclides; blue for electron emission (beta decay); and violet for neutron emission (nuclides outside the neutron drip line). Proton number increases going up the vertical axis and neutron number going to the right on the horizontal axis.
Nitrogen trichloride
Fuming nitric acid contaminated with yellow nitrogen dioxide