6. Carbon

Carbon has two electrons in its p-orbital. These are not sphere-shaped harmonics and, like boron, carbon’s p-electrons cannot achieve symmetry around a sphere on their own because they lie in orthogonal directions.

Each p-orbital lobe holds 1 electron. An electron pair occupies two opposite lobes.

Carbon therefore cannot simply add its two p-electrons on top of the same (2s2) configuration that beryllium has, as shown above, because it would not be a stable configuration. The asymmetry therefore causes the two electrons in the 2s orbital to uncouple from their di-electron state and hybridize with the two p-electrons in order to achieve 4-directional, tetrahedral symmetry. This yields four electrons with equivalent (degenerate) energy. Carbon is therefore the first atom that can achieve tetrahedral electron geometry on its own, which is why carbon typically makes 4 bonds. (The wireframe indicates the boundary of the n=2 shell.)

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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.)

Carbon’s four 2sp3-orbitals (left), and an exploded view (right)

Carbons small size, being only the 6th element, as well as the fact that it can bond in up to four directions, makes it one of the most versatile elements, structurally, on the periodic table. It can facilitate linear, trigonal, or tetrahedral electron geometry and it can make single, double, triple, or resonance bonds in linear, bent, or ring configurations.

Carbon can form structures as hard and beautiful as diamond, as strong as carbon fiber, as fine and versatile as graphene and nanotubes, as well as being the spindle around which the chemistry of life itself turns. It is almost single-handedly responsible for organic chemistry, which makes genetic information storage and biochemistry possible.

Methane (CH4)

When carbon bonds covalently with 4 hydrogen atoms, the symmetrical and non-polar methane (natural gas) molecule is formed.

The formation of methane (CH4) gas
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Methane (CH4) can be “oxidized” in air if it is ignited. A little instigating energy will cause molecular bonds to be destabilized just enough to allow the oxygen in the air to attack both the hydrogen and the carbon in the methane molecule. Since carbon and hydrogen both have lower electronegativities than oxygen, they provide an easier source of electrons for oxygen atoms than oxygen atoms provide for each other. The result is that oxygen atoms from dioxygen (O2) in the air let go of one another and instead bond to all of the carbon and hydrogen atoms in the methane. Water vapor (H2O) and carbon dioxide (CO2) are formed as a result. This is an example of a combustion (burning) reaction:

CH4 + 2O2 —> 2H2O + CO2

Interestingly, it is then these two substances (H2O & CO2) that plants take in and convert into sugar (C6H12O6) and oxygen (O2) through photosynthesis. As such, the more trees and green plants on the planet, the more carbon dioxide (CO2) is removed from the atmosphere. The more phytoplankton and kelp forests in the ocean, the more carbon dioxide (CO2) is removed from the water, and thereby indirectly from the atmosphere.

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