Transition states have partially formed bonds whereas intermediates have fully formed bonds. Transition states occur at minima on reaction coordinate diagrams. An intermediate is always produced after the rate-determining step of a reaction mechanism. Both transition states and intermediates occur at maxima on reaction coordinate diagrams. none of the above

Transition states have partially formed bonds whereas intermediates have fully formed bonds.

Explanation:

According to Wikipedia, a transition state "is defined as the state corresponding to the highest potential energy along a reaction coordinate. It is easily seen as an energy maxima.

A reaction intermediate  is defined as any unstable molecular entity formed as a result of interaction between reactants. This entity undergoes further chemical changes to yield the products of the chemical reaction. Intermediates occur at an energy minima in the reaction coordinate.

The bonds in a transition state are partially formed because a transition state often involves a simultaneous breaking and making of bonds while an intermediate contains fully formed chemical bonds

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