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Chapter 6: Chemical Reactions

Chapter 6: Chemical Reactions. The Nature of Chemical Reactions Reaction Types Balancing Chemical Equations Rates of Change. Overview. What are some signs of a chemical reaction? What do they do to substances?. The Nature of Chemical Reactions.

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Chapter 6: Chemical Reactions

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  1. Chapter 6: Chemical Reactions

  2. The Nature of Chemical Reactions • Reaction Types • Balancing Chemical Equations • Rates of Change Overview

  3. What are some signs of a chemical reaction? • What do they do to substances? The Nature of Chemical Reactions

  4. Finish the first sheet. Those are important to know. • Attempt the final sheets and ask questions if the graph statement is unclear. Worksheet

  5. Energy must be added to break bonds(Endothermic). • Forming bonds releases energy(Exothermic). • Ex. C + O > CO Energy is released • Ex. CO > C + O Energy needs to be added Energy Involved With Reactions

  6. Energy is conserved in chemical reactions. • Example on Board Chemical Reactions Continued

  7. Reaction Arrow • Products • Reactants Parts of a Chemical Reaction

  8. Fill out front of sheet. • We will go over when you finish. Worksheet

  9. Synthesis • Decomposition • Combustion • Single-displacement • Double-displacement Types of Reactions

  10. Two reactants combine to become a reactant. A new molecule is synthesized or made. • Example: Synthesis

  11. A reactant breaks apart into its parts to become a product that is less than the reactants. • Example: Decomposition

  12. Every combustion reaction has oxygen as a reactant. Basis of combustion. How engines work. • Example: Combustion Reactions

  13. There is an exchange. One element in the reactants will trade places with one other element in the reactants for the product. • Example: Single-Displacement Reaction

  14. Usually when you have two compounds and an element from each switch places. • Examples: Double-Displacement Reactions

  15. Pg 197 Problem 1 Classwork

  16. Chemical equations summarize reactions. • Mass and energy are conserved in equations. • Must balance so that they are conserved. Balancing Chemical Equations

  17. Coefficients in front of chemical compounds increase the number of that compound in a chemical equation. Balance By Coefficients

  18. H2 + O2 > H20 • Fe + Cl2 > FeCl3 • Zn + HCl > ZnCl2 + H2 • Hw: Pg. 204 Problem 2 a-d Other Examples

  19. Each reaction has a certain rate or time that it will take to complete the reaction. • Example-It takes you a certain amount of time to get ready in the morning. Rates Of Change

  20. What are some factors that affect you time getting ready in the morning? Factors Affecting Rates of Change

  21. Temperature • Surface area • Concentrated solutions • Pressure • Size of molecules • Catalysts- What is this? Enzymes? Factors affecting Chemical Reactions

  22. List the ways in which I can get a block of Iron to react faster with hydrochloric acid. Sample Problems

  23. Some equations have a constant back and forth in the reaction. Reaction arrows go both ways. • Equilibrium is when they are balanced. Equilibrium Systems

  24. Predicts changes in equilibrium. Three factors that change this: • Temperature • Pressure • Concentration Le Chatelier’s Principle

  25. Reactants > Products + Heat • 2x Reactants > Products • Reactants liquid > Products gas Predict which way the reaction will go.

  26. Pg. 212 1-8 Class Work

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