Ohh so can I explain it like this: when the reactants collide with greater or equal to activation energy, a transition state will have a higher probability of forming. With the modification I made in bold, yes. Not every collision having the requisite energy will yield a reaction. Consider A-B-C + D A + B-C-D.
If D comes "from the right" to form the transition state A----B-C----D, and they have enough energy, then the reaction will proceed. If D comes "from the left", the transition state A----B-C-----D can't form even if the reactants have enough energy, because the geometries aren't right.
But now that what actually occurs is that when the reactants collide with activation energy the a bond is partially broken just as it is partially formed so I'm a bit lost now..
Well that's exactly what would happen. In A + B-C A-B + C, as A approaches B-C, there is an attraction between A and B that grows gradually as the distance between them shrinks. Simultaneously, the bond between B and C gradually weakens because electron density is shifted away from it. The transition state is the halfway point.
While "billiard ball" collisions is a helpful way to visualize things, and indeed it's a way reactions are often modelled, that's just an approximation. It doesn't quite happen like that in reality.
Hi thanks for the great reply
and sorry for the late reply (just started my tertiary education on applied chemistry wish me luck
Ohh that clarifies a lot of doubts. So when we draw that spike to activation energy, that only shows that the energy level increases as its temperature increases? The once it reaches as specific temperature and bumps in the right orientation then a the transition state is formed? I have a few more questions regarding the aftermath of that collision.
After which would it be correct to say that as the new bond is formed the old bond starts weaken and break off? Because at the transition state a bond is partially formed as another bond is partially broken? If so wouldn't more energy be required to break that old bond?
But what about other reactions that only involve one reactant such as decomposition? Because I'm not sure about how the reaction would take place now that there aren't any collision..
Also what about ionization, electron affinity and melting/boiling reactions?
For instance in ionization Li
+e so in this case again I don't really know if there should be an activation energy or not..
Similarly for Li+
Li I'm not sure if the ion and electron would have to collide with an activation energy.
Lastly, for stuff like NaCl(s)
(g) I'm not sure if there is an activation energy spike and vice versa.
Thanks so much for the help and I'm so sorry for the late reply. Was quite busy integrating into the polytechnic.