Question

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1. in general, does the orientation of colliding molecules affect whether a reaction occurs?
2. what name is given to the minimum amount of energy required for a chemical reaction to occur?
3. what is the unstable, high - energy arrangement of atoms that is thought to form during a chemical reaction?

Explanation:

• Question 5: According to the collision theory in chemistry, for a reaction to occur, molecules must collide with proper orientation (along with sufficient energy). So, the orientation of colliding molecules affects whether a reaction occurs.
• Question 6: The minimum amount of energy required for a chemical reaction to occur is called the activation energy. It is the energy barrier that reactant molecules must overcome to form products.
• Question 7: The unstable, high - energy arrangement of atoms that is thought to form during a chemical reaction is called the activated complex (or transition state).

Answer:

1. Yes, the orientation of colliding molecules affects whether a reaction occurs.
2. Activation energy.
3. Activated complex (or transition state).