| 4 no 3-2-1 yes
There are over 100 chemical elements (artificial or natural) discovered so far. Most compounds are bonded by sharing electron pairs called covalence bonding. One of the unsolved mysteries of chemistry is why quadruple bonds do not occur naturally or even artificially. Is it because it violates the octet rule of electron numbers in the outermost shells of chemical elements? The element carbon has 4 valence electrons. By the octet rule it needed four more to complete its outer orbitals. However, two carbon atoms could never share 4 pairs of valence electron even though they can share 3 or 2 or 1 valence electrons called respectively as the triple bond, double bond, and the single bond.
On the other hand, if bond lengths are analyzed with a principle of proximity. It can be shown that the 4-bond structure would need the overlap of nuclear wavefunctions of both carbon atoms. This implies that even wavefunctions cannot possibly violate the proximity theorem of all natural structure. The atomic radius of the neutral carbon atom is 77 picometers while the ionic radius of carbon ion is only 15 picometers. There is a difference of 62 picometers for which the overlapping wavefunctions can take place where the electromagnetic force must overcome the strong nuclear force. This is even worst if the neutral atomic radius of hydrogen (37 picometers) is taken into consideration. Alternatively, a quadruple covalent bond would also break the perfect symmetry of volume determinant from its relation to the scalar triple product: A´B×C where A, B, and C are 3 dimensional vectors.
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Time independence: [∂E(g)]²=[∂F(a)×∂r(a)]·[∂F(b)×∂r(b)] and Mass independence: ¶a(t)·¶r(t)=c²
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