Question

which of the following correctly describes intermediates and/or transition states? an intermediate is always produced after the rate-determining step of a reaction mechanism. transition states have partially formed bonds whereas intermediates have fully formed bonds. both transition states and intermediates occur at maxima on reaction coordinate diagrams. transition states occur at minima on reaction coordinate diagrams. none of the above

Answer 1

Intermediates are formed in early steps and consumed in later steps of a reaction, while transition states occur at the top of the energy hill. Both intermediates and transition states occur at maxima on reaction coordinate diagrams.

Step-by-step explanation:

Intermediates are species that appear in the mechanism of a reaction but not in the overall balanced equation. They are formed in an early step and consumed in a later step of the reaction. On the other hand, transition states are high-energy, unstable states that occur at the top of the energy hill in a reaction coordinate diagram. They correspond to the processes of bond-making and bond-breaking.

The statement that correctly describes intermediates and transition states is:

• Both transition states and intermediates occur at maxima on reaction coordinate diagrams.

This means that both intermediates and transition states are associated with energy maxima in reaction pathways.