Nitrogen Electrons

Valence Shell Electrons. The outer orbital of a nitrogen atom, the (p^2 ) orbital, can carry up to six electrons, just like all other (p ) orbitals. However, a nitrogen atom will only have three of these slots filled. When reacting with other chemicals, it will often try to take electrons from other atoms/ions to get a full octet.

A nitrogen atom has 5 electrons in its outer shell. Nitrogen is in group 5 of the periodic table. Two nitrogen atoms will each share three electrons to form three covalent bonds and make a nitrogen molecule (N 2). A nitrogen atom has the electronic structure represented by 1 s2 2 s2 2 p3. The five outer shell electrons screen the nuclear charge quite poorly, with the result that the effective nuclear charge felt at the covalent radius distance is relatively high. Each n, we can have at most two electrons (one with spin up and one with spin down). If we have N electrons, at T = 0, the electron occupies the lowest N’2 states. The energy of the highest filled state is known as the Fermi energy eF. The momentum of this state is known as the Fermi momentum PF. In the case of a negative ion, there are fewer protons than electrons. For example, N 3-has a -3 charge; therefore, it has gained 3 electrons compared to the neutral state. Nitrogen’s atomic number is 7, therefore this ion has 10 electrons.

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) σ_a/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

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

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 Electrons

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