Nitrogen has three electrons in its p-orbital. This is not a sphere-shaped harmonic, and so three p-electrons cannot achieve a stable electron symmetry around a spherical core. Nitrogen therefore cannot simply add its three p-electrons on top the same (2s2) configuration that beryllium has, as shown here, because it would not be a stable configuration:
The asymmetry therefore causes the three p-orbital electrons to combine (hybridize) with the two s-orbital electrons in order to achieve 4-directional, symmetry. Nitrogen’s tetrahedral (sp3) symmetry features one di-electron (lone pair) and 3 unpaired, degenerate electrons. This is why nitrogen typically makes 3 bonds. The quantum states of the three degenerate electrons become linked, which stabilizes them and thereby increases nitrogen’s ionization energy. (The wireframe indicates the boundary of the n=2 shell.)
The outer spheres above simply indicate the directions of maximum electron density. The orbitals themselves will be more like spherical tetrahedra that can only occupy volume within their shell. The entire shell will be filled with electron density. It will be highest at the center of the face of each orbital and will decrease toward the nodal regions that divide the orbitals, where electron density will be lowest. (This includes the inner and outer faces, as well as the sides of each orbital.) In the case of nitrogen, the orbital containing the lone pair (dark blue) will occupy slightly more volume than the three containing an unpaired electron.
Nitrogen is keen to obtain three extra electrons to fill its second shell, which it can do so by making three covalent bonds. It can also gain three electrons in ionic interaction in order to reach the stability of a full 2nd shell. This is the same electron configuration as the 2s22p6 noble gas configuration of neon — a multi-di-electron state with two concentric full shells. That is why nitrogen forms a 3– ionic state. The negative ion is much larger than the neutral atom because electrons now outnumber protons by three. This results in a much lower effective nuclear charge — a lower average attraction by the nucleus on each electron, which expands the size of the electron shell as it is attracted inward with less force.
When nitrogen bonds covalently with three hydrogen atoms, the biologically important ammonia (NH3) molecule is formed. Like the water molecule, its asymmetrical structure gives it important properties. The most significant is that it creates an electron imbalance which makes the side of the molecule where the hydrogen atoms attach slightly positive (𝛿+) and the opposite (nitrogen) side slightly negative (𝛿–). The presence of the di-electron (lone pair) on the nitrogen atom also makes this molecule alkaline (basic) in solution.
The ammonia molecule is vitally important in the manufacture of fertilizer. The invention of a process to make it efficiently (by Fritz Haber) revolutionized humanity’s ability to provide enough agricultural produce to feed our growing global population.
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