1. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Reactions Table of Contents Section 1 Forming New Substances Section 2 Chemical Formulas and Equations Section 3 Types of Chemical Reactions Section 4 Energy and Rates of Chemical Reactions Chapter 7 Balancing Chemical Equations The Nature of Reactions Reaction Types Rates of Reaction Change

2. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives Describe how chemical reactions produce new substances that have different chemical and physical properties. Identify four signs that indicate that a chemical reaction might be taking place. Explain what energy has to do with chemical reactions Chapter 7 Section 1 Forming New Substances

3. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Reactions A chemical reaction is a process in which one or more substances change to make one or more new substances. The chemical and physical properties of the new substances differ from those of the original substances. Chapter 7 Section 1 Forming New Substances

4. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Reactions, continued Signs of Chemical Reactions include color changes, gas formation, the formation of a precipitate (a solid substance formed in a solution), energy given off as light, thermal energy, or electrical energy. A Change of Properties The most important sign of a chemical reaction is the formation of new substances that have different properties. Chapter 7 Section 1 Forming New Substances

5. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Bonds: Holding Molecules Together A chemical bond is an attraction that holds atoms together in a molecule. Breaking and Making Bonds If molecules bump into each other with enough energy, the chemical bonds in the molecules break. The atoms then rearrange, and new bonds form to make new substances. Chapter 7 Section 1 Forming New Substances

6. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 7 Section 1 Forming New Substances

7. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives Compare exothermic and endothermic reactions. Explain activation energy. Describe how energy is transferred during chemical reactions. Interpret an energy diagram. Describe five factors that affect the rate of a reaction. Chapter 7 Section 1 Energy & Chemical Reactions

8. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Reactions and Energy Exothermic Reactions are reactions in which energy is released. Energy can be released as light, electrical energy, or thermal energy. Endothermic Reactions are reactions in which energy is taken in. The Law of Conservation of Energy states that energy cannot be created or destroyed. The energy released in exothermic reactions was first stored in the chemical bonds of the reactants. The energy taken in during endothermic reactions is stored in the products. Chapter 7 Section 1 Energy & Chemical Reactions

9. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Rates of Reactions The speed at which new particles form is called the rate of a reaction. Activation Energy is the smallest amount of energy that molecules need to react. Some chemical reactions need a boost of energy greater than or equal to the activation energy before the reaction can start. Chapter 7 Section 1 Energy & Chemical Reactions

10. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Rates of Reactions, continued Sources of Activation Energy Friction is one source of activation energy. In a match, friction provides the energy needed to break the bonds in the reactants and allow new bonds to form. An electric spark in a car’s engine is another source of activation energy. This spark begins the burning of gasoline. Light can also be a source of activation energy for a reaction. Also Heat, Fire and Radio Waves can be used Chapter 7 Section 1 Energy & Chemical Reactions

11. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Activation Energy and Chemical Reactions Chapter 7 Section 1 Energy & Chemical Reactions

12. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu

13. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu

14. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Bond Chapter 7 Section 1 Forming New Substances

15. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives Interpret and write simple chemical formulas. Write and balance simple chemical equations. Explain how a balanced equation shows the law of conservation of mass. Chapter 7 Section 2 Chemical Formulas and Equations

16. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Formulas A chemical formula is a combination of chemical symbols and numbers to represent a substance. A chemical formula shows how many atoms of each kind are present in a molecule. Chapter 7 Section 2 Chemical Formulas and Equations

17. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Formula Chapter 7 Section 2 Chemical Formulas and Equations

18. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Formulas, continued Writing Formulas for Ionic Compounds To write the formula for an ionic compound, make sure the compound’s charge is 0. The Metal is named first, followed by the Non- Metal with an –ide suffix Example: NaCl (Na (+1) Cl (-1) – Sodium Chloride MgF 2 (Mg (+2) F (-1) = Magnesium Fluoride The formula must have subscripts that cause the charges of the ions to cancel out. Chapter 7 Section 2 Chemical Formulas and Equations

19. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Formulas, continued Writing Formulas for Covalent Compounds The name of a covalent compound frequently indicates its chemical formula. The names of covalent compounds use prefixes. Each prefix represents a number, as shown below. Chapter 7 Section 2 Chemical Formulas and Equationsmono-1hexa-6di-2hepta-7 tri-3octa-8 tetra-4nona-9 penta-5deca-10

20. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 7 Section 2 Chemical Formulas and Equations

21. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Equations Describing Reactions by Using Equations A chemical equation uses chemical symbols and formulas to describe a chemical reaction. From Reactants to Products The starting materials in a reaction are reactants. The substances formed from a reaction are products. Chapter 7 Section 2 Chemical Formulas and Equations

22. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 7 Section 2 Chemical Formulas and Equations

23. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Equations, continued The Importance of Accuracy The symbol or formula for each substance in a chemical equation must be written correctly or it will not correctly describe the reaction. Some formulas and symbols can be confused. Chapter 7 Section 2 Chemical Formulas and Equations

24. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Equations, continued The Reason Equations Must Be Balanced Atoms are never lost or gained in a chemical reaction, they are just rearranged. Every atom in the reactants becomes part of the products. make sure the number of atoms of each element in the reactants equals the number of atoms of those same elements in the products. This is called balancing the equation. Chapter 7 Section 2 Chemical Formulas and Equations

25. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Equations, continued In the 1700s, French chemist Antoine Lavoisier found that the total mass of the reactants was always the same as the total mass of the products. Lavoisier’s work led to the law of conservation of mass, which states that mass is neither created nor destroyed in ordinary chemical and physical changes. Chapter 7 Section 2 Chemical Formulas and Equations

26. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chemical Equations, continued How to Balance an Equation To balance an equation, you must use coefficients. A coefficient is a number that is placed in front of a chemical symbol or formula. For an equation to be balanced, all atoms must be counted. You multiply the subscript of each element in a formula by the formula’s coefficient. Chapter 7 Section 2 Chemical Formulas and Equations

27. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 7 Section 2 Chemical Formulas and Equations

28. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Objectives Describe four types of chemical reactions. Classify a chemical equation as one of four types of chemical reactions. Chapter 7 Section 3 Types of Chemical Reactions

29. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Synthesis Reactions A synthesis reaction is a reaction in which two or more substances combine to form one new compound. For example, a synthesis reaction takes place when sodium reacts with chlorine to produce sodium chloride, which you know as table salt. Chapter 7 Section 3 Types of Chemical Reactions

30. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Decomposition Reactions A decomposition reaction is a reaction in which a single compound breaks down to form two or more simpler substances. Decomposition is the reverse of synthesis. Chapter 7 Section 3 Types of Chemical Reactions

31. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Single-Displacement Reactions A single-displacement reaction is a reaction in which an element replaces another element that is part of a compound. The products of single- displacement reactions are a new compound and a different element. Reactivity of Elements In a single-displacement reaction, a more reactive element can displace a less reactive element in a compound. Chapter 7 Section 3 Types of Chemical Reactions

32. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Double-Displacement Reactions A double-displacement reaction is a reaction in which ions from two compounds exchange places. One of the products of this type of reaction is often a gas or a precipitate. The next slide shows models of each of the four types of chemical reactions. Chapter 7 Section 3 Types of Chemical Reactions

33. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 7 Section 3 Types of Chemical Reactions

34. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Factors Affecting Rates of Reactions Temperature A higher temperature causes a faster rate of reaction. At high temperatures, particles of reactants move quickly and collide hard and often. At low temperatures, particles move slowly and collide less often. Chapter 7 Section 4 Energy and Rates of Chemical Reactions

35. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Factors Affecting Rates of Reactions, continued Concentration In general, a high concentration of reactants causes a fast rate of reaction. Concentration is a measure of the amount of one substance when it is dissolved in another substance. High concentration has many reactant particles in a given volume. there is little distance between particles and the particles collide more often and react faster. Chapter 7 Section 4 Energy and Rates of Chemical Reactions

36. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Factors Affecting Rates of Reactions, continued Surface Area is the amount of exposed surface of a substance. Increasing the surface area of solid reactants increases the rate of a reaction. Inhibitors are substances that slow down or stop a chemical reaction. The rate of a reaction decreases in the presence of an inhibitor. Chapter 7 Section 4 Energy and Rates of Chemical Reactions

37. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Factors Affecting Rates of Reactions, continued Catalysts are substances that speed up a reaction without being permanently changed. Because it is not changed, a catalyst is not a reactant. A catalyst lowers the activation energy of a reaction, which allows the reaction to happen more quickly. Catalysts called enzymes speed up most reactions in your body. Chapter 7 Section 4 Energy and Rates of Chemical Reactions

38. Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Factors Influencing Reaction Speed: Factors Influencing Reaction Speed: Higher Temperature = Faster Higher Temperature = Faster Higher Concentration = Faster Higher Concentration = Faster Stirring = Faster Stirring = Faster More Surface Area (smaller particle sizes) = Faster More Surface Area (smaller particle sizes) = Faster Catalysts = Faster (by reducing activation energy) Catalysts = Faster (by reducing activation energy) Enzymes are biological catalysts Enzymes are biological catalysts Section 4 Energy and Rates of Chemical Reactions