The diagram below shows the proper orientation of two reactants in order for a successful collision to occur. Use this model to explain why some collisions are not successful by describing the other ways these two reactants can collide. Draw additional images to illustrate.
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I understand the molecular collision theory, but I'm not fond of this image. It's really throwing me for a loop and making it hard to answer the question.
In this diagram though the collision take place the contact between the reactant is too low as result it may not be the successful collision to result a new product similarly u can draw other images in what other way both can A and B collide
@chmvijay Okay, that definitely helps. Thank you! Like I said, I understand that molecules must collide with proper orientation and with sufficient energy, but that diagram was really odd in my opinion.