Why don't all collisions between reactant molecules lead to a chemical reaction?

Video transcript

Hello everyone in this video. Trying to explain why collisions between molecules. Directives don't always lead to a chemical reaction. So, for a chemical reaction to occur, the molecule collision should involve a collision energy equal to or greater than the activation energy. So let's go ahead and write this out again. The molecular collision has to be equal to or greater than the activation energy, and also the molecules should collide with a proper orientation for the reaction again. We'll work this out but in a different color, so molecules should collide with the proper orientation. Four. The reaction, So the answer that best explains our involves our explanations. Here is going to be statement B and this reads only a number of collisions involved collision energy equal to or greater than the activation energy and have a proper orientation for the reaction. So my final answer for this problem is going to be a statement. Be All right. Thank you all so much for watching.