# Why some reaction have no transition state?

All stationary point are local minimum, if any parameters changed the energy should be increase. There is no way for a stationary point that energy go straight down to reach another.

I was told that radical reaction have no transition state, but why? What kind of reaction also do not have transition state? Is there any way to confirm there is no transition state using quantum chemical calculation method?

• Radicals are very reactive. They just rapidly collide in the environment where chemical reaction are occuring they just want to one electron by forming bonds even at the price of breaking other bonds. Also they are so reactive that they can't bear a state where the bond is breaking and forming at the same state like that in transition state. – Hercules Jun 18 '18 at 10:32
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