# Chemistry - Insight into covalent bonds from electrostatic perspective

## Solution 1:

I assume you mean from the classical electrodynamics side only, not from quantum electrodynamics side. By the former, even H atom cannot exist, as the electron would fall along a spiral curve on the nucleus, continually emitting radiation being radially accelerated.

For a hydrogen molecule, both electrons move around both protons, they are not dedicated to the one they came with.

Consider a similar case of charged macro objects, where applying the pre-relativistic classical electrostatics is justified. Imagine 4 respectively charged balls in gravityless vacuum.

The scenario in the bottom picture is one of the less preferred positions, having rather higher energy due short distance of negative charges. But there is plenty of different positions where the whole system would have lower energy than if they were 2 and 2 separately.

Note that even classical system have no general analytic solution for the motion equations for more than 2 objects.

## Solution 2:

Such questions troubled physicists in the early 20th century. Their inability to add more than one electron to the planetary Bohr-model was one of the reasons that quantum mechanics was developed. Nevertheless, continuing to ask this type of questions may help us sharpen our thinking and develop our intuition, as far as it goes (you might also take a look at the simpler Gedanken-experiment about Helium explored here).

In the case at hand, we will not be able to find an analytical solution because this is a four-body problem. However, if you did want to portray the molecule with point charges in a plane then it might be more fruitful to draw an ellipse with —for argument's sake— two electrons in opposite positions ‘chasing each other’. The time-varying force balance will depend on the specific configuration as illustrated with two sketches below.

The intuitively most favourable position would be figure A. In this case, the sum of the attractive forces from the electrons on each proton is higher than the repulsive force between the protons: i.e. there is a net attraction. The least favourable case would seem to be figure B where the electrons pull the protons away from each other in addition to their natural repulsion. One might imagine that the actual force balance is some sort of convoluted average between these extremes — but calculating any such point charge model with multiple electrons has so far proven to be a dead end.

Surprisingly, the parameters of the $$\ce{H2}$$ molecule can be calculated using classical electrodynamics provided we approach the electron not as a point charge but as a membrane of distributed charge, as proposed by Mills. The shape of the molecule in his theory turns out to be the 3D version of the ellipse pictured above, with the (large) electrons physically encompassing the (small) nuclei. The internuclear distance is calculated at $$\sqrt2$$ times the Bohr radius and the binding energy, i.e. the difference between 2 separate $$\ce{H}$$ atoms and an $$\ce{H2}$$ molecule, works out to 4.5 eV — in line with the experimental value. It is this more advantageous energy level that makes $$\ce{H2}$$ a stable molecule.

• Randell L. Mills, "Classical Quantum Mechanics" Physics Essays, Volume 16: Pages 433-498, 2003 [equation 156 gives the binding energy of $$\ce{H2}$$]