Question

review these effective/successful and ineffective/unsuccessful collisions for the same reaction. why is only the second collision effective/successful? the first collision has the incorrect orientation and may or may not also have insufficient energy. the first collision has insufficient energy. the second collision has sufficient energy but not the proper orientation. the second collision has the proper orientation but must not have sufficient energy.

Explanation:

For a collision to be effective in a chemical reaction, molecules must collide with sufficient energy (activation energy) and in the proper orientation. The first collision likely fails due to incorrect orientation and possibly insufficient energy, while the second meets the criteria for an effective collision.

Answer:

The first collision has the incorrect orientation and may or may not also have insufficient energy.