1. Lesson 1 Understanding Chemical Reactions
Chapter Introduction
Lesson 1 Understanding Chemical Reactions
Lesson 2 Types of Chemical Reactions
Lesson 3 Energy Changes and Chemical Reactions
Chapter Wrap-Up
Chapter Menu

2. What happens to atoms and energy during a chemical reaction?
Chapter Introduction

3. Lesson 1 Reading Guide - KC
Understanding Chemical Reactions
What are some signs that a chemical reaction might have occurred?
What happens to atoms during a chemical reaction?
What happens to the total mass in a chemical reaction?
Lesson 1 Reading Guide - KC

4. Lesson 1 Reading Guide - Vocab
Understanding Chemical Reactions
chemical reaction
chemical equation
reactant
product
law of conservation of mass
coefficient
Lesson 1 Reading Guide - Vocab

5. Changes in Matter A physical change does not produce new substances.
For example, water molecules are always made up of two hydrogen atoms bonded to one oxygen atom regardless of whether they are solid, liquid, or gas.
Lesson 1-1

6. Changes in Matter (cont.)
During a chemical change, one or more substances change into new substances.
A chemical reaction is a process in which *
Lesson 1-1

7. Signs of a Chemical Reaction
Changes in the physical properties of color, state of matter, and odor are all signs that *
*, it is likely that a chemical reaction has occurred.
Lesson 1-2

8. Signs of a Chemical Reaction (cont.)
The only way to know if a chemical reaction has occurred is to study the chemical properties of the substances before and after the change.
What are some signs that a chemical reaction might have occurred?
Lesson 1-2

9. What happens in a chemical reaction?
In a chemical reaction, atoms of elements or compounds rearrange and form different elements or compounds.
Atoms rearrange when *
Lesson 1-3

10. Notice that no new atoms are created in a chemical reaction
Notice that no new atoms are created in a chemical reaction. The existing atoms rearrange and form new substances.
Lesson 1-3

11. What happens in a chemical reaction? (cont.)
What happens to atoms during a chemical reaction?
Lesson 1-3

12. Chemical Equations
A chemical equation is a description of a reaction using *
In chemical equations, element symbols represent elements and chemical formulas represent compounds.
Lesson 1-4

13. Chemical Equations (cont.)
A subscript describes the number of atoms of an element in a compound.
If an element’s symbol does not have a subscript, the compound contains only one atom of that element.
Lesson 1-4

14. Lesson 1-4

15. Chemical Equations (cont.)
A chemical equation includes both the substances that react and the substances that are formed in a chemical reaction.
*are reactants.
*are products.
Lesson 1-4

16. Chemical Equations (cont.)
product
from Latin producere, means “bring forth”
Lesson 1-5

17. Chemical Equations (cont.)
The reactants are written to the left of the arrow.
The products are written to the right of the arrow.
The general structure for a chemical equation is: reactant + reactant product + product
Lesson 1-4

18. An equation is read much like a sentence
An equation is read much like a sentence. This equation is read as “carbon plus oxygen produces carbon dioxide.”
Lesson 1-4

19. Conservation of Mass
The law of conservation of mass states that the total mass of the reactants before a chemical reaction is the same as the total mass of the products after the chemical reaction.
Mass is conserved in a reaction because *.
All atoms at the start of a chemical reaction are present at the end of the reaction.
Lesson 1-5

20. Mass is conserved in the reaction between baking soda and vinegar.
Hutchings Photography/Digital Light Source
Hutchings Photography/Digital Light Source
Lesson 1-5

21. Conservation of Mass (cont.)
What happens to the total mass of the reactants in a chemical reaction?
Lesson 1-5

22. Conservation of Mass (cont.)
A chemical equation is written so that the number of atoms of each element is the same, or balanced, on each side of the arrow.
Lesson 1-5

23. Conservation of Mass (cont.)
A balanced equation often does not happen automatically when the formulas for reactants and products are written.
Lesson 1-5

24. Conservation of Mass (cont.)
A coefficient is a number placed in front of an element symbol or chemical formula in an equation.
Only coefficients can be changed when balancing an equation.
Lesson 1-5

25. Conservation of Mass (cont.)
Changing subscripts changes the identities of the substances that are in the reaction.
When no coefficient is present, only one unit of the substance takes part in the reaction.
Lesson 1-5

26. Lesson 1-6

27. Lesson 1-6

28. A chemical reaction is a process in which bonds break and atoms rearrange, forming new bonds.
Lesson 1 - VS

29. A chemical equation uses symbols to show reactants and products of a chemical reaction.
Lesson 1 - VS

30. The mass and the number of each type of atom do not change during a chemical reaction. This is the law of conservation of mass.
Lesson 1 - VS

31. Lesson 2 Reading Guide - KC
Types of Chemical Reactions
How can you recognize the type of chemical reaction by the number or type of reactants and products?
What are the different types of chemical reactions?
Lesson 2 Reading Guide - KC

32. Lesson 2 Reading Guide - Vocab
Types of Chemical Reactions
synthesis
decomposition
single replacement
double replacement
combustion
Lesson 2 Reading Guide - Vocab

33. Patterns in Reactions
The breakdown of one reactant into two or more products is one of four major types of chemical reactions.
Each type of chemical reaction follows a unique pattern in the way atoms in reactants rearrange to form products.
Lesson 2-1

34. Types of Chemical Reactions
A synthesis is a *
Lesson 2-2

35. Types of Chemical Reactions (cont.)
synthesis
from Greek syn–, means “together”; and tithenai, means “put”
Lesson 2-2

36. Types of Chemical Reactions (cont.)
In a decomposition reaction, *.
Lesson 2-2

37. Types of Chemical Reactions (cont.)
How can you tell the difference between synthesis and decomposition reactions?
Lesson 2-2

38. Types of Chemical Reactions (cont.)
In a single-replacement reaction, *
Lesson 2-2

39. Types of Chemical Reactions (cont.)
In a double-replacement reaction, the *.
Lesson 2-2

40. Types of Chemical Reactions (cont.)
Combustion is a *
Lesson 2-2

41. Types of Chemical Reactions (cont.)
What are the different types of chemical reactions?
Lesson 2-2

42. Chemical reactions are classified according to patterns seen in their reactants and products.
Lesson 2 - VS

43. In a synthesis reaction, there are two or more reactants and one product. A decomposition reaction is the opposite of a synthesis reaction.
Lesson 2 - VS

44. In replacement reactions, an element, or elements, in a compound is replaced with another element or elements.
Lesson 2 - VS

45. 4. Water can be broken down into simpler substances.
Do you agree or disagree?
3. Reactions always start with two or more substances that react with each other.
4. Water can be broken down into simpler substances.
Lesson 2 - Now

46. Lesson 3 Reading Guide - KC
Energy Changes and Chemical Reactions
Why do chemical reactions always involve a change in energy?
What is the difference between an endothermic reaction and an exothermic reaction?
What factors can affect the rate of a chemical reaction?
Lesson 3 Reading Guide - KC

47. Lesson 3 Reading Guide - Vocab
Energy Changes and Chemical Reactions
endothermic
exothermic
activation energy
catalyst
enzyme
inhibitor
Lesson 3 Reading Guide - Vocab

48. Energy Changes
Chemical bonds contain a form of energy called chemical energy.
Breaking a bond absorbs energy from the surroundings.
The formation of a chemical bond releases energy to the surroundings.
Lesson 3-1

49. Energy Changes (cont.)
Some chemical reactions release more energy than they absorb.
Some chemical reactions absorb more energy than they release.
Energy is conserved in all chemical reactions.
Lesson 3-1

50. Energy Changes (cont.)
Why do chemical reactions involve a change in energy?
Lesson 3-1

51. * are endothermic reactions.
In an endothermic reaction, more energy is required to break the bonds of the reactants than is released when the products form.
Lesson 3-1

52. An exothermic reaction is a *.
In an exothermic reaction, more energy is released when the products form than is required to break the bonds in the reactants.
Lesson 3-1

53. Energy Changes (cont.) exothermic
from Greek exo–, means “outside”; and therm, means “heat”
Lesson 3-1

54. Energy Changes (cont.)
What is the difference between an endothermic reaction and an exothermic reaction?
Lesson 3-1

55. Activation energy is the minimum amount of *.
Lesson 3-1

56. Reaction Rates The rate of a reaction is the speed at which it occurs.
Chemical reactions occur faster if particles collide more often or move faster when they collide.
Lesson 3-2

57. Reaction Rates (cont.)
Increased surface area increases reaction rate because more particles on the surface of a solid come into contact with the particles of another substance.
At higher temperatures, the average speed of particles is greater, particles collide more often, and collisions with more energy are more likely to break chemical bonds.
Lesson 3-2

58. Reaction Rates (cont.)
Increasing the concentration of one or more reactants increases collisions between particles, resulting in a fast reaction rate.
In gases, an increase in pressure pushes gas particles closer together, resulting in more collisions.
Lesson 3-2

59. A catalyst is a substance that * An enzyme is a *
Lesson 3-2

60. Reaction Rates (cont.) An inhibitor is a *
What factors can affect the rate of a chemical reaction?
Lesson 3-2

61. Chemical reactions that release energy are exothermic, and those that absorb energy are endothermic.
Lesson 3 - VS

62. Activation energy must be added to a chemical reaction for it to proceed.
Lesson 3 - VS

63. Catalysts, including enzymes, speed up chemical reactions
Catalysts, including enzymes, speed up chemical reactions. Inhibitors slow them down.
Lesson 3 - VS

64. Interactive Concept Map Chapter Review Standardized Test Practice
Key Concept Summary
Interactive Concept Map
Chapter Review
Standardized Test Practice
Chapter Review Menu

65. Atoms are neither created nor destroyed in chemical reactions
Atoms are neither created nor destroyed in chemical reactions. Energy can be released when chemical bonds form or absorbed when chemical bonds are broken.
The BIG Idea

66. Lesson 1: Understanding Chemical Reactions
There are several signs that a chemical reaction might have occurred, including a change in temperature, a release of light, a release of gas, a change in color or odor, and the formation of a solid from two liquids.
In a chemical reaction, atoms of reactants rearrange and form products.
The total mass of all the reactants is equal to the total mass of all the products in a reaction.
Key Concepts 1

67. Lesson 2: Types of Chemical Reactions
Most chemical reactions fit into one of a few main categories—synthesis, decomposition, combustion, and single- or double-replacement.
Synthesis reactions create one product. Decomposition reactions start with one reactant. Single- and double-replacement reaction involve replacing one element or group of atoms with another element or group of atoms. Combustion reactions involve a reaction between one reactant and oxygen, and they release thermal energy.
Key Concepts 2

68. Lesson 3: Energy Changes and Chemical Reactions
Chemical reactions always involve breaking bonds, which requires energy, and forming bonds, which releases energy.
In an endothermic reaction, the reactants contain less energy than the products. In an exothermic reaction, the reactants contain more energy than the products.
The rate of a chemical reaction can be increased by increasing the surface area, the temperature, or the concentration of the reactants or by adding a catalyst.
Key Concepts 3