In collision theory, which statement describes the conditions for a collision to lead to a reaction?

In collision theory, which statement describes the conditions for a collision to lead to a reaction?

• A. Any collision regardless of energy
• B. Collisions must occur in gas phase only
• C. The collision must involve sufficient energy to overcome activation energy and proper orientation
• D. Only one molecule must collide

Answer: (C)

Collision theory says that a reaction only happens when reacting particles meet under two key conditions: they collide with enough energy to overcome the activation energy barrier, and they hit in a suitable orientation so that bonds can break and new bonds form. If the energy is too low, the collision doesn’t lead to reaction and the particles just bounce apart. Even with sufficient energy, an improper alignment can prevent reaction because the atoms wouldn’t be positioned to make the necessary new bonds. Temperature influences how many collisions have enough energy, increasing the reaction rate by boosting kinetic energy. Reactions aren’t limited to gas phase either; they can occur in liquids and on surfaces. And a single molecule colliding by itself isn’t enough—typically two reacting species must come together, sometimes with the help of catalysts or surfaces, to proceed.

Collision theory says that a reaction only happens when reacting particles meet under two key conditions: they collide with enough energy to overcome the activation energy barrier, and they hit in a suitable orientation so that bonds can break and new bonds form. If the energy is too low, the collision doesn’t lead to reaction and the particles just bounce apart. Even with sufficient energy, an improper alignment can prevent reaction because the atoms wouldn’t be positioned to make the necessary new bonds. Temperature influences how many collisions have enough energy, increasing the reaction rate by boosting kinetic energy. Reactions aren’t limited to gas phase either; they can occur in liquids and on surfaces. And a single molecule colliding by itself isn’t enough—typically two reacting species must come together, sometimes with the help of catalysts or surfaces, to proceed.