Final answer:
An activated (high energy) intermediate is a type of molecular species that is formed during a chemical reaction and has a high energy state due to the presence of excess energy within the molecule. These intermediates are often formed through the breaking and forming of chemical bonds, and can be highly reactive due to their high energy state.
Step-by-step explanation:
In a chemical reaction, reactants are transformed into products through a series of steps, each of which involves the formation and breaking of chemical bonds. During these steps, the molecular species involved in the reaction can change their energy state, with some species having a higher energy state than others. Activated intermediates are those species that have a high energy state due to the presence of excess energy within the molecule.
There are several types of activated intermediates, including carbenes, carbanions, and free radicals. Carbenes are molecules that contain a carbon atom with a double bond and one or more single bonds, while carbanions are molecules that contain a carbon atom with a triple bond and one or more single bonds. Free radicals are molecules that contain an unpaired electron, which gives them a high energy state.
Activated intermediates play a crucial role in many chemical reactions, as they can undergo a variety of reactions to form the final products. For example, enzymatic reactions often involve the formation of activated intermediates, which then undergo a series of steps to produce the final product. In addition, activated intermediates can also participate in non-enzymatic reactions, such as the oxidation of molecules or the formation of new chemical bonds.