1. IPS Unit 12 Chemical Equations Section 3

2. Energy Exchanges All chemical reactions release or absorb energy This energy can take many forms, such as heat, light, sound, or electricity Chemical bonds are the source of this energy When most chemical reactions take place, some chemical bonds in the reactants are broken, which requires energy In order for products to be produced, new bonds must form. Bond formation releases energy

3. Energy Exchanges – More Energy Out Chemical reactions that release energy are called exergonic reactions In these reactions less energy is required to break the original bonds than is released when new bonds form As a result, some form of energy, such as light or heat is given off by the reaction When the energy given off in a reaction is primarily in the form of heat, the reaction is called an exothermic reaction

4. Energy Exchanges – More Energy In Sometimes a chemical reaction requires more energy to break bonds than is released when new ones are formed. These reactions are called endergonic reactions The energy absorbed can be in the form of light, heat or electricity When the energy needed is in the form of heat, the reaction is called an endothermic reaction

5. Some reactions—such as the combustion of rocket fuel—proceed very rapidly. Other reactions—such as metal rusting—proceed very slowly. The reaction rate is the rate at which reactants change into products. According to the collision model, reactants must collide in order to react. Things that affect reaction rates include:  Temperature  Concentration  Volume & Pressure  Surface Area Reaction Rates

6. Reaction Rates - Temperature Increasing temperature increases the reaction rate. Temperature is a measure of the average kinetic energy of a substance’s particles. The higher the temperature, the faster the particles are moving. Faster-moving particles means more frequent collisions and collisions with greater energy.

7. Reaction Rates - Concentration Increasing the concentration of the reactants increases the reaction rate. Increased concentration means a greater number of reacting particles in a given area. Greater numbers of particles means more opportunities for collisions between reacting particles.

8. Reaction Rates – Volume and Pressure Volume and pressure are important considerations for reactions involving gases. Decreased volume leads to increased concentration. Increasing the concentration of gases increases the rate at which particles collide with each other and with the walls of their container. Increased collisions mean increased pressure. The reaction rate also increases because the reacting particles collide with each other more frequently.

9. Reaction Rates – Surface Area Sugar cubes dissolve more slowly compared to granulated sugar. The individual grains of sugar have a greater total surface area. Increased surface area leads to faster reactions. This larger area allows for more collisions between reacting particles.

10. Catalysts Some reactions proceed too slowly to be useful. To speed them up, a catalyst can be added. A catalyst is a substance that speeds up a chemical reaction without being permanently changed itself. When you add a catalyst to a reaction, the mass of the product that is formed remains the same, but it will form more rapidly. A catalyst is neither a reactant nor a product.

11. Inhibitors At times, it is worthwhile to prevent certain reactions from occurring. Substances called inhibitors are used to slow down a chemical reaction. One thing to remember when thinking about catalysts and inhibitors is that they do not change the amount of product produced. They only change the rate of production.