Nitrogen Atomic Number

| Posted on by



Atomic

Nitrogen (atomic number 7, symbol N) is a tasteless, odorless, and colorless chemical element, which, by volume, constitutes 78.09 percent of the earth's atmosphere. According to estimates, this element is 7th in abundance in the solar system and our galaxy. 2020-11-21 by Nick Connor Atomic Mass of Nitrogen Atomic mass of Nitrogen is 14.0067 u.

Element Nitrogen - N

Comprehensive data on the chemical element Nitrogen is provided on this page; including scores of properties, element names in many languages, most known nuclides of Nitrogen. Common chemical compounds are also provided for many elements. In addition technical terms are linked to their definitions and the menu contains links to related articles that are a great aid in one's studies.

Nitrogen Menu

  • Nitrogen Page One
  • Nitrogen Page Two
  • Nitrogen Page Three

Overview of Nitrogen

  • Atomic Number: 7
  • Group: 15
  • Period: 2
  • Series: Nonmetals

Nitrogen's Name in Other Languages

  • Latin: Nitrogenium
  • Czech: Dusík
  • Croatian: Dušik
  • French: Azote
  • German: Stickstoff - r
  • Italian: Azoto
  • Norwegian: Nitrogen
  • Portuguese: Nitrogênio
  • Russian: Азот
  • Spanish: Nitrógeno
  • Swedish: Kväve

Atomic Structure of Nitrogen

  • Atomic Radius: 0.75Å
  • Atomic Volume: 17.3cm3/mol
  • Covalent Radius: 0.75Å
  • Cross Section (Thermal Neutron Capture) σa/barns: 1.91
  • Crystal Structure: Hexagonal
  • Electron Configuration:
    1s2 2s2p3
  • Electrons per Energy Level: 2,5
    Shell Model
  • Ionic Radius: 0.13Å
  • Filling Orbital: 2p3
  • Number of Electrons (with no charge): 7
  • Number of Neutrons (most common/stable nuclide): 7
  • Number of Protons: 7
  • Oxidation States:±3,5,4,2
  • Valence Electrons: 2s2p3
    Electron Dot Model

Chemical Properties of Nitrogen

  • Electrochemical Equivalent: 0.10452g/amp-hr
  • Electron Work Function:
  • Electronegativity: 3.04 (Pauling); 3.07 (Allrod Rochow)
  • Heat of Fusion: 0.3604kJ/mol
  • Incompatibilities:
  • Ionization Potential
    • First: 14.534
    • Second: 29.601
    • Third: 47.448
  • Valence Electron Potential (-eV): 550

Physical Properties of Nitrogen

Nitrogen
  • Atomic Mass Average: 14.00674
  • Boiling Point: 77.5K -195.65°C -320.17°F
  • Coefficient of lineal thermal expansion/K-1: N/A
  • Conductivity
    Electrical:
    Thermal: 0.0002598 W/cmK
  • Density: 1.2506g/L @ 273K & 1atm
  • Description:
    Colorless, odorless, tasteless gas
  • Enthalpy of Atomization: 472.8 kJ/mole @ 25°C
  • Enthalpy of Fusion: 0.36 kJ/mole
  • Enthalpy of Vaporization: 2.79 kJ/mole
  • Flammablity Class:
  • Freezing Point:see melting point
  • Heat of Vaporization: 2.7928kJ/mol
  • Melting Point: 63.29K -209.86°C -345.75°F
  • Molar Volume: 17.3 cm3/mole
  • Optical Refractive Index: 1.000298 (gas) 1.197 (liquid)
  • Physical State (at 20°C & 1atm): Gas
  • Specific Heat: 1.04J/gK

Regulatory / Health

Nitrogen Atomic Number
  • CAS Number
    • 7727-37-9
  • OSHAPermissible Exposure Limit (PEL)
    • No limits set by OSHA
  • OSHA PEL Vacated 1989
    • No limits set by OSHA
  • NIOSHRecommended Exposure Limit (REL)
    • No limits set by NIOSH
  • Levels In Humans:
    Note: this data represents naturally occuring levels of elements in the typical human, it DOES NOT represent recommended daily allowances.
    • Blood/mg dm-3: 34300
    • Bone/p.p.m: 43000
    • Liver/p.p.m: 72000
    • Muscle/p.p.m: 72000
    • Daily Dietary Intake: n/a
    • Total Mass In Avg. 70kg human: 1.8 kg
  • Discovery Year: 1772
  • Name Origin:
    Greek: zôê (vie).
  • Abundance of Nitrogen:
    • Earth's Crust/p.p.m.: 25
    • Seawater/p.p.m.:
      • Atlantic Suface: 0.00008
      • Atlantic Deep: 0.27
      • Pacific Surface: 0.00008
      • Pacific Deep: 0.54
    • Atmosphere/p.p.m.: 780900
    • Sun (Relative to H=1E12): 8.71E+07
  • Sources of Nitrogen:
    Nitrogen can be made by liquification and then fractional distillation of the air. It is very easily done commercially. It can also be made by heating NaN3 to 300 degrees C. Annual world wide production is around 44,000,000 tons.
  • Uses of Nitrogen:
    Nitrogen has many industrial uses in the gaseous forms, but probably the most interesting is liquid nitrogen, which is extremely cold. Items that must be frozen to extremely low temperatures for preservation are frequently stored in liquid nitrogen. Fertility clinics store sperm, eggs and embryos used to help infertile couples become pregnant in ampoules in liquid nitrogen.Since nitrogen gas is very stable, at standard temperature and pressure, it is used as the air in inert welding atmospheres. Documents, foods and chemicals are sometimes stored in nitrogen to keep them from oxidizing or reacting with air or water.
  • Additional Notes:

    Nitrogen in the elemental form was considered to be inert and was even named ozote which refers to the fact that it is not reactive. Of course nitrogen does form compounds, but the gaseous form consists of diamers (2 nitrogens bonded together). The diamer is very stable.

    Nitrogen is a major element in organic compounds, especially proteins. Some nitrogen compounds are highly reactive. Trinitrotoluene is TNT or dynamite. Ammonium Nitrate is a fertilizer, but was used as the major explosive ingredient in the Oklahoma City bombing. Anfo, or Ammonium Nitrate and fuel oil mixture is the primary explosive used in the mining industry because it is inexpensive, easy to manufacture and can be easily manufactured near the mine site thus reducing the risks and expenses related to the transportation of explosives. Nitrates, Nitrites and Azides (all nitrogen compounds are either oxidizers or reactives and will react violently under the right conditions.

Nitrogen Menu

  • Nitrogen Page One
  • Nitrogen Page Two
  • Nitrogen Page Three

References

A list of reference sources used to compile the data provided on our periodic table of elements can be found on the main periodic table page.

Related Resources

  • Anatomy of the Atom
    Answers many questions regarding the structure of atoms.
  • Molarity, Molality and Normality
    Introduces stoichiometry and explains the differences between molarity, molality and normality.
  • Molar Mass Calculations and Javascript Calculator
    Molar mass calculations are explained and there is a JavaScript calculator to aid calculations.
  • Chemical Database
    This database focuses on the most common chemical compounds used in the home and industry.

Citing this page

If you need to cite this page, you can copy this text:

Kenneth Barbalace. Periodic Table of Elements - Nitrogen - N. EnvironmentalChemistry.com. 1995 - 2021. Accessed on-line: 4/24/2021
https://EnvironmentalChemistry.com/yogi/periodic/N.html/
.

Linking to this page

If you would like to link to this page from your website, blog, etc., copy and paste this link code (in red) and modify it to suit your needs:

<a href='https://EnvironmentalChemistry.com/yogi/periodic/N.html/'>echo Periodic Table of Elements: Nitrogen - N (EnvironmentalChemistry.com)</a>- Comprehensive information for the element Nitrogen - N is provided by this page including scores of properties, element names in many languages, most known nuclides and technical terms are linked to their definitions.
.

NOTICE: While linking to articles is encouraged, OUR ARTICLES MAY NOT BE COPIED TO OR REPUBLISHED ON ANOTHER WEBSITE UNDER ANY CIRCUMSTANCES.

Nitrogen Atomic Number And Mass Number

Symbol

PLEASE, if you like an article we published simply link to it on our website do not republish it.

How To Find The Atomic Number Of Nitrogen

This is an ammonia molecule with the formula, NH3. Scientists use the name 'ammonia', the same way they call H2O 'water'. In this compound, three hydrogen (H) atoms share their electrons with the nitrogen (N) atom. This way the nitrogen has a filled outer shell and the hydrogens have two electrons to fill their shells.
Nitrogen can combine with three chlorine (Cl) atoms, forming nitrogen trichloride, or NCl3. Nitrogen shares its electrons with the chlorine atoms, so all of the atoms have their shells filled.
Take a look at the dots around the atoms. All of them now have eight electrons, and a filled outer shell!

Here's something new! We have three different elements here, carbon, nitrogen, and chlorine. That's not special, but the way they combine is! Look at the carbon and the nitrogen, they are sharing six electrons!
When two atom share two electrons, that's a single bond. If they share four it's a double bond. Well these two are sharing six, that's a triple bond. It's extremely strong and powerful. It would take a lot of work to separate the C and the N!
One more thing! Because the bond between carbon and nitrogen is so strong, scientists call them 'cyanogen' instead of carbon-nitrogen. Scientists know that cyanogen is always CN.