Which statement correctly applies to the collision theory of chemical reactions?

• A. Chemical reactions occur only when reactant particles are in the solid state.
• B. Reactant particles must collide with sufficient energy and proper orientation to result in a reaction.
• C. The rate of a chemical reaction is independent of the frequency of collisions between reactant particles.
• D. All collisions between reactant particles will always lead to the formation of products.

Answer: (B)

Verified step by step guidance

1. Understand that the collision theory explains how chemical reactions occur at the particle level, focusing on 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 having 'sufficient energy'.
3. Recognize that not only energy but also the correct spatial arrangement or 'proper orientation' during collisions is necessary for the reaction to proceed.
4. Note that the state of reactants (solid, liquid, gas) is not a strict requirement for reactions; reactions can occur in various states as long as effective collisions happen.
5. Remember that not all collisions lead to a reaction; only those with sufficient energy and proper orientation result in product formation, and the reaction rate depends on the frequency of such effective collisions.