Collison Theory
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Collisions between reactants are necessary for chemical reactions to occur. The reactants must collide with the proper orientation and with sufficient kinetic energy to overcome the activation energy barrier. Adding a catalyst can also increase the reaction rate by lowering the activation energy needed for collisions between reactants to be productive.
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Collison Theory
- 1. How do reactions occur?Collision TheoryCollision TheoryCollision TheoryIn order for a chemical reaction to take place, the reactants must collide.The collision transfers kinetic energy needed to break the necessary bonds so that new bonds can be formed.
- 2. Collision requirementsRequirement 1Must have the proper orientation.2HCl + Mg MgCl2 + H2H---ClMgH-ClMgH Cl-MgWrong OrientationCorrect Orientation
- 3. Collision requirementsRequirement 2Must have enough kinetic energy to reach a threshold of energy called activation energyMgH---ClH---ClMgH Cl--Mg
- 6. Increasing the Rate of ReactionsWhat needs to happen in order for the rate of the chemical reaction to increase (go faster)?More collisions= Faster reaction rate
- 7. 5th way in increase Rxn RateAdd a Catalyst= Speeds up a reaction but is not used in the reactionLowers the activation energy