1. Chemical Reactions
Chapter 9

2. Chemical Reactions
chemical reaction- The process by which one or more substances are rearranged to form different substances
Evidence that a chemical reaction may have occurred:
Change in temperature
Change in color
Odor
Gas bubbles
Appearance of a solid

3. Activity In your notebook complete the thinking map by
Identifing three examples of chemical reactions you have seen, heard, or smelled in the last 24 hours. Think about activities at home, at school, or outside.
Depict each example
Include any evidence you have that a chemical reaction was occurring.

4. Representing Chemical Reactions
Chemists use statements called equations to represent chemical reactions.
Reactants are the starting substances.
Products are the substances formed in the reaction.

5. Activity (l) __________________________________________________
Label the chemical state each symbol below identifies in a chemical equation.
(s) _________________________________________________________
(g) _________________________________________________________
(aq) _________________________________________________________
(l) __________________________________________________

6. Representing Chemical Reactions
Word equations
aluminum(s) + bromine(l) → aluminum bromide(s)
reads as “aluminum and bromine react to produce aluminum bromide”
Skeleton equations
use symbols and formulas to represent the reactants and products)
Al(s) + Br(l) → AlBr3(s)
Both word and skeleton equations lack information about how many atoms are involved in the reaction.

7. Representing Chemical Reactions
Chemical equation- a statement that uses chemical formulas to show the identities and relative amounts of the substances involved in a chemical reaction.

8. Activity In your notebook on the next page
Recreate the following table
Organize types of equations that can express a chemical reaction.
In the second column, list the elements (words, coefficients, etc.) that are used to create each equation.
In the third column, rank each equation from 1 to 3, giving a 3 to the equation that provides the most information, and a 1 to the equation that provides the least information.

9. Balancing Chemical Equations
This figure shows the balanced equation for the reaction between aluminum and bromine.

10. Balancing Chemical Equations
Coefficient
in a chemical equation is the number written in front of a reactant or product,
describing the lowest whole-number ratio of the amounts of all the reactants and products

11. Balancing Chemical Equations
The most fundamental law in chemistry is the law of conservation of mass.
Balanced equations show this law.

12. Classifying Chemical Reactions
Classify chemical reactions.
metal: an element that is a solid at room temperature, a good conductor of heat and electricity, and is generally shiny
Identify the characteristics of different classes of chemical reactions.

13. Classifying Chemical Reactions
synthesis reaction
combustion reaction
decomposition reaction
single-replacement reaction
double-replacement reaction
precipitate
There are four types of chemical reactions: synthesis, combustion, decomposition, and replacement reactions.

14. Classifying Chemical Reactions
Types of Chemical Reactions
Chemists classify reactions in order to organize the many types.
A synthesis reaction is a reaction in which two or more substances react to produce a single product.
A + B → AB

15. Classifying Chemical Reactions
Types of Chemical Reactions (cont.)
When two elements react, the reaction is always a synthesis reaction.

16. Classifying Chemical Reactions
Types of Chemical Reactions (cont.)
In a combustion reaction, oxygen combines with a substance and releases energy in the form of heat and light.
Heated hydrogen reacts with oxygen to produce heat and water in a combustion reaction. This is also a synthesis reaction.

17. Classifying Chemical Reactions
Decomposition Reactions
A decomposition reaction is one in which a single compound breaks down into two or more elements or new compounds.
Decomposition reactions often require an energy source, such as heat, light, or electricity, to occur.
AB → A + B

18. Classifying Chemical Reactions
Replacement Reactions
A reaction in which the atoms of one element replace the atoms of another element in a compound is called a single replacement reaction.
A + BX → AX + B

19. Classifying Chemical Reactions
Replacement Reactions (cont.)
A metal will not always replace a metal in a compound dissolved in water because of differing reactivities.
An activity series can be used to predict if reactions will occur.

20. Classifying Chemical Reactions
Replacement Reactions (cont.)
Halogens frequently replace other halogens in replacement reactions.
Halogens also have different reactivities and do not always replace each other.

21. Classifying Chemical Reactions
Replacement Reactions (cont.)
Double replacement reactions occur when ions exchange between two compounds.
This figure shows a generic double replacement equation.

22. Classifying Chemical Reactions
Replacement Reactions (cont.)
The solid product produced during a chemical reaction in a solution is called a precipitate.
ANIMATION
All double replacement reactions produce either water, a precipitate, or a gas.

23. Classifying Chemical Reactions
Replacement Reactions (cont.)
This table shows the steps to write double replacement reactions.

24. Classifying Chemical Reactions
Replacement Reactions (cont.)
This table summarizes different ways to predict the products of a chemical reaction.

25. LAB
Looking at some examples of chemical reactions

26. QUIZ TOMORROW

27. Which of the following is NOT one of the four types of reactions?
Section Check
Which of the following is NOT one of the four types of reactions?
A. deconstructive
B. synthesis
C. single replacement
D. double replacement

28. The following equation is what type of reaction?
Section Check
The following equation is what type of reaction?
KCN(aq) + HBr(aq) → KBr(aq) + HCN(g)
A. deconstructive
B. synthesis
C. single replacement
D. double replacement

29. Reactions in Aqueous Solutions
Describe aqueous solutions.
Write complete ionic and net ionic equations for chemical reactions in aqueous solutions.
Predict whether reactions in aqueous solutions will produce a precipitate, water, or a gas.
solution: a uniform mixture that might contain solids, liquids, or gases

30. Reactions in Aqueous Solutions
solute
solvent
complete ionic equation
spectator ion
net ionic equation
Double-replacement reactions occur between substances in aqueous solutions and produce precipitates, water, or gases.

31. Reactions in Aqueous Solutions
An aqueous solution contains one or more dissolved substances (called solutes) in water.
The solvent is the most plentiful substance in a solution.

32. Reactions in Aqueous Solutions
Aqueous Solutions (cont.)
Water is always the solvent in an aqueous solution.
There are many possible solutes—sugar and alcohol are molecular compounds that exist as molecules in aqueous solutions.
Compounds that produce hydrogen ions in aqueous solutions are acids.

33. Reactions in Aqueous Solutions
Aqueous Solutions (cont.)
Ionic compounds can also be solutes in aqueous solutions.
When ionic compounds dissolve in water, their ions separate in a process called dissociation.

34. Reactions in Aqueous Solutions
Types of Reactions in Aqueous Solutions
When two solutions that contain ions as solutes are combined, the ions might react.
If they react, it is always a double replacement reaction.
Three products can form: precipitates, water, or gases.

35. Reactions in Aqueous Solutions
Types of Reactions in Aqueous Solutions (cont.)
Aqueous solutions of sodium hydroxide and copper(II) chloride react to form the precipitate copper(II) hydroxide.
2NaOH(aq) + CuCl2(aq) → 2NaCl(aq) + Cu(OH)2(s)
Ionic equations that show all of the particles in a solution as they actually exist are called complete ionic equations.
2Na+(aq) + 2OH–(aq) + Cu2+ (aq)+ 2Cl–(aq) → 2Na+(aq) + 2Cl–(aq) + Cu(OH)2(s)

36. Reactions in Aqueous Solutions
Types of Reactions in Aqueous Solutions (cont.)
Ions that do not participate in a reaction are called spectator ions and are not usually written in ionic equations.
Formulas that include only the particles that participate in reactions are called net ionic equations.
2OH–(aq) + Cu2+(aq) → Cu(OH)2(s)

37. Reactions in Aqueous Solutions
Types of Reactions in Aqueous Solutions (cont.)
Some reactions produce more water molecules.
No evidence of a chemical reaction is observable.
HBr(aq) + NaOH(aq) → H2O(l) + NaBr(aq)
Without spectator ions H+(aq) + OH–(aq) → H2O(l).

38. Reactions in Aqueous Solutions
Types of Reactions in Aqueous Solutions (cont.)
Gases that are commonly produced are carbon dioxide, hydrogen cyanide, and hydrogen sulfide.
2HI(aq) + Li2S(aq) → H2S(g) + 2LiI(aq)

39. Reactions in Aqueous Solutions
Types of Reactions in Aqueous Solutions (cont.)
Another example is mixing vinegar and baking soda, which produces carbon dioxide gas.
HCl(aq) + NaHCO3(aq) → H2CO3(aq) + NaCl(aq)
H2CO3(aq) decomposes immediately.
H2CO3(aq) → H2O(l) + CO2(g)

40. Reactions in Aqueous Solutions
SECTION9.3
Reactions in Aqueous Solutions
Types of Reactions in Aqueous Solutions (cont.)
Two reactions can be combined and represented by a single chemical reaction.

41. Reactions in Aqueous Solutions
Types of Reactions in Aqueous Solutions (cont.)
Reaction 1
HCl(aq) + NaHCO3(aq) → H2CO3(aq) + NaCl(aq)
Reaction 2
H2CO3(aq) → H2O(l) + CO2(g)
Combined equation
HCl(aq) + NaHCO3(aq) + H2CO3(aq) → H2CO3(aq) + NaCl(aq) + H2O(l) + CO2(g)
Overall equation
HCl(aq) + NaHCO3(aq) → H2O(l) + CO2(g) + NaCl(aq)

42. What is the solvent in an aqueous solution?
Section Check
What is the solvent in an aqueous solution?
A. hydrogen
B. sodium ions
C. water
D. alcohol

43. Section Check
An equation that includes only the particles that participate in a reaction is called:
A. net ionic equation
B. spectator ions
C. complete ionic equation
D. reduced ionic equation

44. Reactions and Equations
SECTION9.1
Reactions and Equations
Study Guide
Key Concepts
Some physical changes are evidence that indicate a chemical reaction has occurred.
Word equations and skeleton equations provide important information about a chemical reaction.
A chemical equation gives the identities and relative amounts of the reactants and products that are involved in a chemical reaction.
Balancing an equation involves adjusting the coefficients until the number of atoms of each element is equal on both sides of the equation.

45. Classifying Chemical Reactions
SECTION9.2
Classifying Chemical Reactions
Study Guide
Key Concepts
Classifying chemical reactions makes them easier to understand, remember, and recognize.
Activity series of metals and halogens can be used to predict if single-replacement reactions will occur.

46. Reactions in Aqueous Solutions
SECTION9.3
Reactions in Aqueous Solutions
Study Guide
Key Concepts
In aqueous solutions, the solvent is always water. There are many possible solutes.
Many molecular compounds form ions when they dissolve in water. When some ionic compounds dissolve in water, their ions separate.
When two aqueous solutions that contain ions as solutes are combined, the ions might react with one another. The solvent molecules do not usually react.
Reactions that occur in aqueous solutions are double-replacement reactions.

47. CHAPTER9
Chemical Reactions
Chapter Assessment
The law of conservation of mass requires what in a chemical reaction equation?
A. both sides of the equation to contain the same substances
B. the reactants to have the same amount of molecules as the products
C. both sides to have the same amount of atoms of each element
D. the products to have fewer molecules than the reactants

48. A reaction that gives off heat is what type of reaction?
CHAPTER9
Chemical Reactions
Chapter Assessment
A reaction that gives off heat is what type of reaction?
A. single replacement reaction
B. double replacement reaction
C. synthesis reaction
D. combustion reaction

49. CHAPTER9
Chemical Reactions
Chapter Assessment
Ions that are present in a solution and do not participate in a chemical reaction when another substance is added are called ____.
A. spectator ions
B. reactants
C. products
D. net ions

50. CHAPTER9
Chemical Reactions
Chapter Assessment
A double replacement reaction produces all of the following except ____.
A. gases
B. solids
C. light
D. water

51. What type of reaction is the following?
CHAPTER9
Chemical Reactions
Chapter Assessment
What type of reaction is the following?
2H2O(l) + energy → H2(g) + O2(g)
A. synthesis reaction
B. decomposition reaction
C. combustion reaction
D. replacement reaction

52. What type of reaction is the following? 2H2(g) + O2(g) → 2H2O(l)
CHAPTER9
Chemical Reactions
Standardized Test Practice
What type of reaction is the following?
2H2(g) + O2(g) → 2H2O(l)
A. replacement reaction
B. synthesis
C. decomposition reaction
D. double replacement reaction

53. A precipitate forms in a double replacement reaction only if:
CHAPTER9
Chemical Reactions
Standardized Test Practice
A precipitate forms in a double replacement reaction only if:
A. the reactivities of the compounds differ
B. the new compound is denser than water
C. the new compound is soluble in water
D. the new compound is not soluble in water

54. CHAPTER9
Chemical Reactions
Standardized Test Practice
A ____ is a statement that uses chemical formulas to show the identities and relative amounts of the substances involved in a chemical reaction.
A. word equation
B. skeleton equation
C. chemical equation
D. balanced equation

55. Predict the type of reaction. LiBr2 (aq) + 2NaOH (aq) → ____
CHAPTER9
Chemical Reactions
Standardized Test Practice
Predict the type of reaction.
LiBr2 (aq) + 2NaOH (aq) → ____
A. synthesis reaction
B. combustion reaction
C. single replacement reaction
D. double replacement reaction

56. Which reactions are essentially the opposite of synthesis reactions?
CHAPTER9
Chemical Reactions
Standardized Test Practice
Which reactions are essentially the opposite of synthesis reactions?
A. single-replacement
B. decomposition
C. combustion
D. double-replacement