How does a covalent bond affect the stability of atoms?

Question

Skylar Alexander · Accepted Answer

It increases their stability; otherwise the bond is not favorable.

You should have seen a diagram similar to this one before:

This depicts a general bond-forming process.

The bond-dissociation limit; this is where the two nuclei are so far apart that either making a bond is not going to happen, or a bond is going to break.
The nuclei are moving closer together, but aren't quite close enough yet. An attraction is happening between the electrons of atom A and the nucleus of atom B, and vice versa.
Now the nuclei are at the optimal internuclear distance (separation between two nuclei) for a bond to form.
This would be when the nuclei are getting closer than they should be; they start repelling each other due to each of their positive charges (remember? Protons can be found in nuclei).
This is too close; past this point, the repulsion energy is infinitely high, and basically, the nuclei want to move apart because this state is too unstable.
Thus, 3 is the most stable configuration, i.e. it is the location at which the equilibrium geometry can be established and at which there is the greatest possible amount of stability.

Isabella Acosta · Answer

undefined A covalent bond forms when two atoms share electrons, creating a stable arrangement for both atoms. This sharing of electrons allows each atom to achieve a full outer shell of electrons, typically resulting in greater stability for the atoms involved. By sharing electrons, atoms can satisfy the octet rule, which states that atoms tend to gain, lose, or share electrons to achieve a full outer shell of eight electrons. This stable configuration reduces the likelihood of the atoms undergoing chemical reactions and increases their overall stability.