Collision Theory Mrs. Kay.

Slides:

Advertisements

Similar presentations

Factors Effecting Reaction Rate. Collision Theory In order to react molecules and atoms must touch each other. They must hit each other hard enough to.

Advertisements

Section 2.8—Speeding Up A Reaction

Unit 7 Notes Part 1 Chemical Kinetics The area of chemistry concerned with the speed at which reactions occur is called chemical kinetics. – Reaction.

RATES OF REACTION CHAPTER 17. CHEMICAL KINETICS Branch of chemistry concerned with rates and mechanisms of chemical reactions. Reaction Rate- The speed.

Day 82 Collision Theory. Agenda Learning Target I can identify and explain the effect of temperature change and concentration change on the rate of a.

Section 2.8—Speeding Up A Reaction

Collision Theory and Activation Energy Unit 3: Chemical Kinetics and Equilibrium.

  Reactant molecules MUST collide to produce a chemical reaction  The concentrations of reactants affect the # of collisions among reactants  For.

Reaction Rates. Reaction Rate Activity H 2 O 2 + Yeast  ? 1.Create a before and after table on a piece of paper to record your observations. 2.Pour about.

Chemistry of LifeSection 4 Section 4: Energy and Metabolism Preview Bellringer Key Ideas Changing Matter Chemical Reactions Biological Reactions Summary.

Section 18.1 Collision Theory, Activation Energy, & Rates of Reactions

Enzymes – the biochemical catalysts Control chemical reactions in living cells.

Chapter 6.1 Observing chemical change. Chemistry Chemistry is the study of matter and how it changes.

THE COLLISION THEORY. For the reaction A + B  C, A and B must collide For the reaction A  B + C, A must collide with itself or with the walls of the.

© 2013 Pearson Education, Inc. Chapter 9, Section 1 General, Organic, and Biological Chemistry Fourth Edition Karen Timberlake Chapter 9 © 2013 Pearson.

Kaupapa / Learning Outcomes I can explain what ‘reaction rate’ means andhow to measure the rate of reaction I can explain how reactions happen due to collisions.

General, Organic, and Biological Chemistry Copyright © 2010 Pearson Education, Inc. 1 Chapter 9 Chemical Equilibrium 9.1 Rates of Reactions.

Branch of chemistry that deals with the rates of chemical reactions TOPIC 8 Review Book.

Collision Theory Collisions needed to provide energy required for a particle to change (i.e. a bond to break) and to bring the reactants into contact.

6.3 Collision Theory and Factors Affecting Rates of Reaction

Chapter 19 Section 1 Rates of Reaction rate- measures the speed of any change that occurs within an interval of time rate = change/time -rates of chemical.

CHEMICAL CHANGE AND YOUR BODY YOUR BODY DOES A LOT OF CHEMISTRY. IT IS ESTIMATED THAT THERE ARE 6 X REACTIONS/CELL/SEC IN THE AVERAGE HUMAN. SKIN.

Section 4: Energy and Metabolism

Reactions rate and Collision Theory

States that atoms, ions, and molecules must collide in order to react.

Collision Theory and Reaction Rate

Chemical Kinetics – collision theory

Collision Theory Rates of reactions.

Chemical Kinetics – collision theory

3-4 Energy and Metabolism

Trilogy – Chemistry – CHAPTER 5 – Energy changes

Ch. 17 – Chemical Reactions

Reaction Kinetics Chapter 17.

Rates of Reactions Lesson 13.

Reaction Rates and Collision Theory

Section 2.8—Speeding Up A Reaction

Reaction Rates and Collision Theory

Reaction Rates and Collision Theory

CHEMISTRY Matter and Change

Reaction Rate A measure of the speed of any change that occurs within an interval of time Usually expressed as the amount of reactant changing per unit.

THE COLLISION THEORY.

Chapter 17A General Chemistry Mr. Mata

Chapter 18 Reaction Rates

Kinetics Branch of chemistry that deals with the rates of chemical reactions TOPIC 8 Review Book.

Chemical Kinetics.

and Chemical Equilibrium

Changing Matter Living things are made of matter, which consists of a substance with a form. Changes constantly occur in living things. A physical change.

Section 4: Energy and Metabolism

Ch. 17 – Chemical Reactions

Rates of Reactions What is Reaction Rate The Collision Theory

Kinetics Branch of chemistry that deals with the rates of chemical reactions TOPIC 8 Review Book.

Aim: How are reaction (rxn) rates affected?

Collision Theory & Reaction Rates

Factors that affect the rate of reactions

DO NOW Get out homework handout Pick up notes.

Factors that Affect the Rate of Reactions

Reaction Rates and Collision Theory

Chapter 17 General Chemistry Mr. Mata

Rate Affecting Factors

Reaction rates and equilibrium

Unit 8: Rates of Reactions

Drill # 7 (4B) 4/24/13 List 5 factors that affect reaction rate:

Unit 4: Kinetics Collision Theory.

Chapter 17 Equilibrium Reversible Reactions.

Potential Energy Diagrams

Presentation transcript:

Collision Theory Mrs. Kay

A chemical reaction… In order for a chemical reaction to occur, the particles of the reactants must come in contact and collide with each other. by calculating how many collisions are taking place per second and how quickly product is being produced, we learn that most collisions are not successful (no product formed)

to think that reactant particles collide and products are automatically produced is over simplified. There must be other requirements for a collision to be successful.

The Collision Theory is an explanation of what is necessary for a chemical reaction to occur. This theory states when a chemical reaction takes place, the reactant particles must meet two conditions (or requirements) during collision for the collisions to be successful

Conditions… Particles must collide with a certain minimum amount of energy, called activation energy. This energy is required to break chemical bonds in the reactants. The energy of each particle is not important, it is the energy of the collision.

Particles must collide with the proper geometry or orientation for atoms to come in direct contact and form the chemical bonds of the products.

If both of these conditions are not met, particles will merely collide and bounce off one another without forming products.

Although, the percentage of successful collisions is extremely small, chemical reactions still take place at a reasonable rate because there are so many collisions per second between reactant particles.

Practice: 1. State the collision theory for chemical reactions. 2. Why is not enough for reactant particles just to collide in order to produce products? 3. In spite of the extremely small percentage of successful collisions, why is it that chemical reactions are still observed to take place at a reasonable rate? 4. Why is the energy requirement needed for a successful collision? 5. Why is the geometry or orientation requirement needed for a successful collision?

More Practice: Pg 478 # 5-7 Read Pg 470-473