Difference between intermediates and transition states Can someone please explain what exactly the difference between an intermediate and a transition state is?

I understand that they are formed as part of the process in converting the reactants to products in a chemical reaction. Other than that, all I know is that usually a transition state exists very briefly (if at all) whereas an intermediate can be isolated. But why?
An intermediate is a short-lived unstable molecule in a reaction which is formed inbetween the reaction when reactants change into products.

Whereas, transition state is just the state before formation of new molecule(involves breaking of bonds of reactants and formation of new ones) 

An intermediate differs from a transition state in that the intermediate has a discrete lifetime (be it a few nanoseconds or many days), whereas a transition state lasts for just one bond vibration cycle. Intermediates may be unstable molecules (in which case they are called reactive intermediates) or highly stable molecules.
The difference between them can be better described through the energy profile diagram.

Transition states are local energy maximums and have partial bonds. This might be one of the reasons why they cant be isolated as intermediates.