Nitrogen is a chemical element with symbol “N” and atomic number 7. It was discovered by the Anglo-Irish chemist, Daniel Rutherford in 1772. Nitrogen electron configuration is 1s2 2s2 2p3
Introduction
The nitrogen atom has an atomic number of 7, which means that it has 7 protons in its nucleus. The electrons orbit the nucleus in shells. The first orbit can hold up to 2 electrons, the second orbit can hold up to 8 electrons, and the third orbit can hold up to 18 electrons. Nitrogen’s electron configuration would be written as 1s2 2s2 2p3.
Nitrogen Electron Configuration Tabular Form
| Atomic Number | 7 |
| Atomic Mass | 14.0067u |
| Symbol (Notation) | N |
| Electronic Configuration | 1s2 2s2 2p3 |
| Ground State Electronic Configuration | 1s2 2s2 2p3 or 2,5 |
| Excited State Electronic Configuration | 1s2 2s2 2p2 3s1 |
| Abbreviated Form | [He] 2s2 2p3 |
| Group | 15 |
| State | Gas |
| Allotropes | Dinitrogen |
| Color |
Blue |
| Block | P |
The element nitrogen, atomic number 7, has three isotopes with mass numbers 14, 15, and 16. The most common isotope of nitrogen is N-14, which makes up 99.6% of all naturally occurring nitrogen. N-15 is 0.4% of natural nitrogen, and N-16 is a trace amount. All three isotopes have seven electrons in their outermost energy level (shell), but the number of neutrons in the nucleus differs.
What is the Nitrogen Electron Configuration?
The Nitrogen Electron Configuration is the electronic structure of an atom of nitrogen. It consists of 7 electrons in shells 1, 2, and 3. The outermost shell (3) contains 5 of these electrons.
Molecular Orbital Diagram of Nitrogen, 3s23p3
The molecular orbital diagram of nitrogen, 3s23p3, is a visual representation of the distribution of electrons in the orbitals of the atom. The three p orbitals are shown as two lobes on either side of the nucleus, with the third lobe in the middle. The 3s orbital is shown as a single lobe on the left side of the nucleus. The diagram shows that there are two electrons in the 3s orbital and three electrons in each of the p orbitals.
What are Orbitals?
Orbitals are the three-dimensional regions around an atom’s nucleus where electrons are most likely to be found. They have specific shapes and sizes, and each orbital can hold a maximum of two electrons. The types of orbitals found in an atom depend on the number of electrons in the atom. For example, atoms with more than one electron will have multiple orbitals with different shapes and sizes.
How do Orbitals Combine?
When orbitals combine, the electron configuration of the resulting molecule is determined by a few rules. First, orbitals fill in order of energy. That is, the lowest energy orbital is filled first. Second, orbitals can only hold a certain number of electrons. The s orbitals can each hold two electrons, while p orbitals can hold six. Finally, when orbitals combine, the electrons pair up so that each orbital has one electron with spin up and one electron with spin down.
This results in some interesting patterns for combining orbitals. For example, when two p orbitals combine, they form a bonding orbital with two electrons of opposite spin. This bonding orbital is lower in energy than the original p orbitals, meaning it is more stable. On the other hand, when two s orbitals combine, they form an antibonding orbital with two electrons of the same spin. This antibonding orbital is higher in energy than the original s orbitals, meaning it is less stable.
The combination of these rules leads to some interesting consequences for molecules made of different elements. For example, carbon has four valence electrons in its outermost shell. This means that it can form bonds with four other atoms using its p orbitals (two electrons per bond). However, nitrogen has five valence electrons in its outermost shell. This means that it can only form bonds with three other atoms using its p orbitals (since each orbital can only hold two electrons).
Summary and Conclusion
The Nitrogen electron configuration is the pattern of electrons in an atom of nitrogen. The first two electrons fill the 1s orbital, the next two fill the 2s orbital, and the final three electrons go into the 2p orbital. This gives nitrogen a total of five valence electrons. The Nitrogen electron configuration can be abbreviated as [He] 2s2 2p3.