Potential Energy Curve of H₂: The Dance of Attraction and Repulsion

The video explains the formation of a hydrogen molecule using a potential energy vs. inter-nuclear distance graph. Initially, hydrogen atoms have nearly zero potential energy when far apart. As they approach, 1S orbitals overlap, leading to attractive forces and decreased potential energy. The minimum potential energy occurs at a bond length of 0.74 angstroms, where the molecule is stable. If the distance decreases further, nuclear repulsions increase, causing instability. Sigma bonds form through head-to-head or end-on overlap of orbitals.

How do nuclear attractions and inter electronic repulsions affect the stability of a hydrogen molecule?

What type of bond is formed by the overlap of 1 S orbitals, and how does it contribute to molecular stability?