What is the basic premise of the collision theory?

What is the basic premise of the collision theory?

• A. Reactions occur when particles collide with correct orientation and energy above activation energy
• B. Reactions occur spontaneously
• C. Reactions require catalysts always
• D. Reactions occur only at high pressure

Answer: (A)

Collision theory says that for a reaction to happen, particles must collide with the right orientation and with enough energy to overcome the energy barrier, the activation energy. If the energy is below that barrier, collisions don’t lead to products. Only collisions with sufficient energy and correct alignment can break old bonds and form new ones. Temperature matters because it increases the average kinetic energy of particles, so more collisions have enough energy to get over the barrier, and collisions happen more often. Even when energy is enough, the orientation must be suitable for bonds to break and new ones to form. Catalysts aren’t required for every reaction; they provide an alternative pathway with a lower activation energy, making reactions faster, but reactions can occur without them if the collisions are energetic enough. High pressure isn’t a universal requirement either; it affects gas reactions by changing how often particles collide, but many reactions occur across a range of pressures or in liquids and solids.

Collision theory says that for a reaction to happen, particles must collide with the right orientation and with enough energy to overcome the energy barrier, the activation energy. If the energy is below that barrier, collisions don’t lead to products. Only collisions with sufficient energy and correct alignment can break old bonds and form new ones.

Temperature matters because it increases the average kinetic energy of particles, so more collisions have enough energy to get over the barrier, and collisions happen more often. Even when energy is enough, the orientation must be suitable for bonds to break and new ones to form.

Catalysts aren’t required for every reaction; they provide an alternative pathway with a lower activation energy, making reactions faster, but reactions can occur without them if the collisions are energetic enough. High pressure isn’t a universal requirement either; it affects gas reactions by changing how often particles collide, but many reactions occur across a range of pressures or in liquids and solids.