Which of the following is a correct statement about collision theory?

• A. Increasing the temperature always decreases the rate of collisions between reactant particles.
• B. All collisions between reactant particles result in the formation of products.
• C. Collision theory states that reactions occur without the need for particle collisions.
• D. For a reaction to occur, reactant particles must collide with sufficient energy and proper orientation.

Answer: (D)

Verified step by step guidance

1. Understand that collision theory explains how chemical reactions occur at the molecular level by focusing on the collisions between reactant particles.
2. Recall that for a reaction to happen, particles must collide with enough energy to overcome the activation energy barrier; this is called the minimum energy requirement.
3. Recognize that not all collisions lead to a reaction because particles must also have the correct orientation during the collision to form products.
4. Note that increasing temperature generally increases the rate of collisions because particles move faster, so the statement that temperature always decreases collision rate is incorrect.
5. Conclude that the correct statement about collision theory is: reactant particles must collide with sufficient energy and proper orientation for a reaction to occur.