Question

Define Effective collision.

Hint:

Effective Collision = Sufficient Energy + Proper Orientation.

Answer 1

Step 1: Concept
Collision theory of chemical kinetics.

Step 2: Meaning
Not all collisions between reactant molecules lead to the formation of products. Only a specific fraction of collisions are successful.

Step 3: Analysis
For a collision to be considered "effective," two strict conditions must be met simultaneously.
First, the colliding molecules must possess kinetic energy equal to or greater than the activation energy (threshold energy).
Second, the molecules must have the proper spatial orientation at the moment of impact so that the correct bonds can break and form.

Step 4: Conclusion
Collisions fulfilling both energetic and spatial criteria result in chemical reactions.

Final Answer: Effective collisions are those collisions between reactant molecules that result in a chemical reaction, which only occur when the molecules possess sufficient kinetic energy (activation energy) and collide with the proper spatial orientation.