Question

Define Effective collision.

Hint:

Only a small fraction of total collisions are effective. Increasing temperature increases the number of effective collisions by raising molecular energy.

Answer 1

Concept: According to collision theory, chemical reactions occur due to collisions between reactant molecules. However, only a fraction of these collisions actually lead to product formation.
Step 1: Define effective collision. An effective collision is a collision between reactant molecules that results in the formation of products.
Step 2: Conditions for an effective collision. For a collision to be effective, two requirements must be satisfied simultaneously:

• 
  Energy factor: Molecules must possess minimum energy called threshold energy (equal to or greater than activation energy) to break existing bonds.
• 
  Orientation factor: Molecules must collide with proper spatial orientation so that bond breaking and bond formation can occur.

Step 3: Final conclusion. An effective collision is one in which reactant molecules collide with sufficient kinetic energy and correct orientation to form products.