Which statement correctly defines steric repulsion in the context of Gibbs energy?

Steric repulsion refers to the increased energy that arises from the physical presence of atoms or groups of atoms that are in close proximity to one another, preventing them from occupying the same space. This spatial crowding creates unfavorable interactions, which can increase the Gibbs energy of a system.

In the case of complex formation, steric repulsion can significantly hinder the ability of reactants to come together and form a stable complex. When bulky groups are present, they can occupy space around a central atom or molecule, making it more difficult for other particles to approach closely enough to interact effectively. This repulsion increases the Gibbs energy, making the formation of the complex less favorable.

The other statements do not accurately describe the nature of steric repulsion in relation to Gibbs energy. For instance, saying that it enhances stability of complexes overlooks how increased steric hindrance typically makes complex formation less stable. Similarly, the idea that it decreases the energy of interactions contradicts the core principle that steric effects usually lead to less favorable energetic interactions. Lastly, to claim it has no effect on chemistries disregards the significant impact of molecular geometry and crowding on the reaction pathways and equilibria of chemical systems. Therefore, stating that steric repulsion can hinder