Final answer:
A chemical reaction following a molecule collision requires sufficient minimum energy, equal to or greater than the activation energy, and a favorable orientation, not an exchange of electrons or catalyst interaction.
Step-by-step explanation:
For a chemical reaction to occur following a collision between molecules, it is imperative that they possess not only the necessary minimum energy which must be equal to or greater than the activation energy (Ea) but also a proper orientation upon impact. The orientation is crucial as it allows the molecules to come into contact with each other in a manner that will enable the formation of new bonds. Therefore, the correct response to the student's question is that for a collision between molecules to result in reaction, the molecules must possess a certain minimum energy and c. have a favorable orientation relative to each other when they collide.
It is not necessary for molecules to exchange electrons or to interact with a catalyst for at least one second for a reaction to occur, as the reaction can proceed solely with enough energy and the correct molecular alignment. These factors, which influence the rate and success of chemical reactions, are explained by the collision theory of chemical reactions.