what is the difference between effective collisions and regular collisions?

Question

i have notes down about factors that affect the rate of chemical reaction.. and its things like
change in concentration (for collisions)
increase temp (for effective collisions)

whats the difference

Answer 1

Collisions occur when two potentially reactive molecules come into contact with each other. However, they may not have sufficient entergy to cause them to react, in which case, the collision is not effective.

Increasing the concentration of two chemicals increases the number of molecules available to collide (and therefore, the rate of reaction); but if there's no extra energy,.the *percentage* of collisions that are effective will not change.

Increasing the temperature gets whatever molecules that are available for reaction zipping around much faster and more excitedly, so that if a collision occurs, it's more likely to be successful (effective).

Answer 2

For a reaction to take place there must be an effective collision between the reactants to form the activated complex. For the collsion to be effective, the reactant molecules must have enough energy and they must be facing the right way, so that the collision sticks together successfully. Otherwise the molecules will collide and just bounce off like billiard balls. This would be the regular collision.

Higher concentration = more colllisions

Higher temperature = higher energy and more likely to have effective collsions.