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Molecularity

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Molecularity

One piece at a time

Many people enjoy putting jigsaw puzzles together. Often these puzzles come in a box, so you have to spread all the pieces out before you start. Nowadays you can also find internet sites that have jigsaw puzzles. You can choose the level of difficulty, the shape of the pieces – and you can time yourself to see how well you did compare to others that tried the puzzle. The puzzle looks complicated with the final product often numbering hundreds of pieces. However, in assembling the puzzle, you have a series of elementary steps and the puzzle goes together one piece at a time.

Molecularity of a Reaction

The molecularity of a reaction is the number of molecules reacting in an elementary step. A unimolecular reaction is one in which only one reacting molecule participates in the reaction. Two reactant molecules collide with one another in a bimolecular reaction. A termolecular reaction involves three reacting molecules in one elementary step.  Termolecular reactions are relatively rare because they involve the simultaneous collision of three molecules in the correct orientation, a rare event. When termolecular reactions do occur, they tend to be very slow.

If we have the reaction:

2 \text{NO}(g) + \text{O}_2(g) \rightarrow 2 \text{NO}_2(g)

We might guess that the reaction was termolecular since it appears that three molecules of reactants are involved.  However, our definition of molecularity states that we need to look at an elementary step and not the overall reaction. Data on the reaction mechanism shows us that the reaction occurs in two steps:

Step 1: 2 \text{NO}(g) \rightarrow \text{N}_2 \text{O}_2(g)

Step 2: \text{N}_2 \text{O}_2(g)+ \text{O}_2(g) \rightarrow 2 \text{NO}_2(g)

So we see that each elementary step is bimolecular and not termolecular. Notice that the colliding molecules may be the same (as in step 1 above) or different (as in step 2 above).

Another reaction involves the conversion of ozone (O 3 ) to oxygen (O 2 ) with ultraviolet light. The two elementary steps are as follows:

& \text{O}_3 + \text{ultraviolet light} \rightarrow \text{O}_2+ {\text{O} \cdot} (\text{free radical}) \ \text{slow reaction} \\& {\text{O} \cdot} + \text{O}_3 \rightarrow 2 \text{O}_2  \ \text{fast reaction}

The first step is unimolecular (one molecule of ozone reacts) and the second step is bimolecular (one ozone free radical and one ozone molecule react together).

Summary

  • Molecularity is defined and examples are given.

Practice

Do the molecularity parts of problems 4 and 5 at the link below:

http://faculty.scottsdalecc.edu/borick/files/2011/05/8-30HW.pdf

Review

  1. What is a unimolecular reaction?
  2. What is a bimolecular reaction?
  3. Why are termolecular reactions rare?

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