7.4 Collision Theory

What describes a reaction?

• Products react and become reactants.

• Reactants react and become products.

• Reactants and products react and become new reactants.

• Reactants and products react and become new products.

Collision theory states that

• particles collide at random and react

• collisions between particles often result in a reaction

• collision between molecules are sometimes needed before a reaction occurs

• reacting particles must collide with enough energy in order to reac

What criteria must be met for reactant collisions to result in a successful product?

• The reactants must collide with each other only

• The reactants must collide with enough energy and be in the right positions

• The reactants must have enough energy to form the activated complex

• The reactants must collide with enough energy only

Reactions in which the products have more energy than the reactants are_______ reactions.

• Endothermic

• Exothermic

• Redox reaction

• Elimination

Increase in temperature of the reactants can do one of the following

• Slow collision frequency

• Allow less effective collision between the particles

• Neutralise the reaction

• Increase collision between the particles thus increasing the rate.

Why does a catalyst increase the rate of reaction?

• it produces extra energy for the reactants

• it increases the speed of the reactant particles

• it increases the frequency of particle collisions

• it reduces the activation energy of the reaction 

Why don't all collisions between particles cause a reaction?

• The particles also need to collide with a catalyst

• Not all the particles collide with enough energy

• Not all the particles collide at a high enough temperature

• The particles need to collide with each other twice

Which of the following is/are the fundamental idea(s) of collision theory?

• Molecules react by colliding together

• The effective collisions must occur with certain minimum amounts of energy 

• In a large sample, the greater the number of effective collisions, and the faster the rate of reaction

• All of the above

Under the collision theory, the particles must collide with  ____ and ____ for a reaction to occur.

• sufficient rate and sufficient energy

• sufficient surface area and correct orientation

• sufficient catalyst and sufficient energy

• sufficent energy and correct orientation

What is activation energy?

• Energy barrier that does not need to be overcome before a reaction can take place.

• Maximum energy required to break the bonds and form new bonds.

• Minimum energy required to break the bonds in reactant particles

• Energy required to end a reaction