Collison Theory

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Collison Theory

  1. 1. How do reactions occur?<br />Collision Theory<br />Collision Theory<br />Collision Theory<br />In order for a chemical reaction to take place, the reactants must collide.<br />The collision transfers kinetic energy needed to break the necessary bonds so that new bonds can be formed.<br />
  2. 2. Collision requirements<br />Requirement 1<br />Must have the proper orientation.<br />2HCl + Mg  MgCl2 + H2<br /><br />H---Cl<br />Mg<br />H-Cl<br />Mg<br />H Cl-Mg<br />Wrong Orientation<br />Correct Orientation<br />
  3. 3. Collision requirements<br />Requirement 2<br />Must have enough kinetic energy to reach a threshold of energy called activation energy<br />Mg<br />H---Cl<br />H---Cl<br />Mg<br />H Cl--Mg<br />
  4. 4. Energy of Activation <br />
  5. 5. Energy of Activation<br />
  6. 6. Increasing the Rate of Reactions<br />What needs to happen in order for the rate of the chemical reaction to increase (go faster)?<br />More collisions<br />= Faster reaction rate<br />
  7. 7. 5th way in increase Rxn Rate<br />Add a Catalyst<br />= Speeds up a reaction but is not used in the reaction<br /><ul><li>Lowers the activation energy</li>

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