1. Chapter 8 Notes Recognizing Chemical Reactions
When a substance undergoes a chemical change, it takes part in a chemical reaction.
After it reacts, it no longer has the same chemical identity.

2. Recognizing Chemical Reactions
While it may seem amazing that a substance can undergo a change and become part of a different substance, chemical reactions occur around you all the time.
Many important clues indicate when chemical reactions occur.
None of them alone proves that such a change occurs because some physical changes involve one or more of these signs.

3. Writing Chemical Equations
In order to completely understand a chemical reaction, you must be able to describe any changes that take place.
Part of that description involves recognizing what substances react and what substances form.

4. Writing Chemical Equations
A substance that undergoes a reaction is called a reactant.
When reactants undergo a chemical change, each new substance formed is called a product.

5. Writing Chemical Equations
For example, a familiar chemical reaction involves the reaction between iron and oxygen (the reactants) that produces rust, which is iron(III) oxide (the product).
The simplest reactions involve a single reactant or a single product, but some reactions involve many reactants and many products.

6. Word Equations
The simplest way to represent a reaction is by using words to describe all the reactants and products, with an arrow placed between them to represent change.
Reactants are placed to the left of the arrow, and products are placed to the right.
Plus signs are used to separate reactants and also to separate products.

7. Word Equations
Vinegar and baking soda are common names.
The compound in vinegar that is involved in the reaction is acetic acid, and baking soda is sodium hydrogen carbonate.
These scientific names can also be used in a word equation.

8. Chemical Equations
Word equations describe reactants and products, but they are long and awkward and do not adequately identify the substances involved.
Word equations can be converted into chemical equations by substituting chemical formulas for the names of compounds and elements.

9. Chemical Equations
The equation for the reaction of vinegar and baking soda can be written using the chemical formulas of the reactants and products.
By examining a chemical equation, you can determine exactly what elements make up the substances that react and form.

10. Chemical Equations
It may also be important to know the physical state of each reactant and product.
How can we indicate the bubbles we see during this reaction are CO2?
Symbols in the parentheses are put after formulas to indicate the state of the substance.
Solids, liquids, gases, and water (aqueous) solutions are indicated by the symbols (s), (l), (g), and (aq).

11. Chemical Equations
The following equation shows these symbols added to the equation for the reaction of vinegar and baking soda.

12. Chemical Equations
Now the equation tells us that mixing an aqueous solution of acetic acid (vinegar) with solid sodium hydrogen carbonate (baking soda) results in the formation of an aqueous solution of sodium acetate, liquid water, and carbon dioxide gas.

13. Energy and Chemical Equations
Noticeable amounts of energy are often released or absorbed during a chemical reaction.
Some reactions absorb energy. If energy is absorbed, the reaction is known as an endothermic reaction.
For a reaction that absorbs energy, the word energy is sometimes written along with the reactants in the chemical equation.

14. Energy and Chemical Equations
For example, the equation for the reaction in which water breaks down into hydrogen and oxygen shows that energy must be added to the reaction.
Reactions that release heat energy are called exothermic reactions.

15. Energy and Chemical Equations
When writing a chemical equation for a reaction that produces energy, the word energy is sometimes written along with the products.
Some of this energy is in the form of light.

16. Energy and Chemical Equations
You may have also noticed that the word energy is not always written in the equation.
It is used only if it is important to know whether energy is released or absorbed.

17. Balancing Chemical Equations
The mass of the products is always the same as the mass of the reactants that react to form them.
The law of conservation of mass summarizes these findings.
Matter is neither created nor destroyed during a chemical reaction.

18. Balancing Chemical Equations
Remember that atoms don’t change in a chemical reaction; they just rearrange.
The number and kinds of atoms present in the reactants of a chemical reaction are the same as those present in the products.
When stated this way, it becomes the law of conservation of atoms.

19. Balancing Chemical Equations
For a chemical equation to accurately represent a reaction, the same number of each kind of atom must be on the left side of the arrow as are on the right side.
If an equation follows the law of conservation of atoms, it is said to be balanced.

20. Balancing Chemical Equations
The easiest way to count atoms is to practice—first with a simple reaction and then with some that are more complex.
For example, consider the equation that represents breaking down carbonic acid into water and carbon dioxide.

21. Balancing Chemical Equations
Because a subscript after the symbol for an element represents how many atoms of that element are found in a compound, you can see that there are two hydrogen, one carbon, and three oxygen.
All of the atoms in the reactants are the same as those found in the products.

22. Balancing Chemical Equations
Examine the equation for the formation of sodium carbonate and water from the reaction between sodium hydroxide and carbon dioxide.

23. Balancing Chemical Equations
One carbon atom is on each side of the arrow, but the sodium, oxygen, and hydrogen atoms are not balanced.
The equation, as written, does not truly represent the reaction because it does not show conservation of atoms.

24. Balancing an Equation
To indicate more than one unit taking part or being formed in a reaction, a number called a coefficient is placed in front of it to indicate how many units are involved.
Look at the previous equation with a coefficient of 2 in front of the sodium hydroxide formula.

25. Balancing an Equation
Is the equation balanced now?
Two sodium atoms are on each side. How many oxygen atoms are on each side?
You should be able to find four on each side. How about hydrogen atoms?
Now two are on each side.
Because one carbon atom is still on each side, the entire equation is balanced; it now represents what happens when sodium hydroxide and carbon dioxide react.

26. Balancing an Equation
The balanced equation tells us that when sodium hydroxide and carbon dioxide react, two units of sodium hydroxide react with each molecule of carbon dioxide to form one unit of sodium carbonate and one molecule of water.

27. Major Classes of Reactions
If you can classify a reaction into one of five major categories by recognizing patterns that occur, you already know a lot about the reaction.
In one type of reaction, two substances—either elements or compounds—combine to form a compound.
Whenever two or more substances combine to form a single product, the reaction is called a synthesis reaction.

28. A Synthesis Reaction
When iron rusts, iron metal and oxygen gas combine to form one new substance, iron(III) oxide.
The balanced equation for this synthesis reaction shows that there is more than one reactant but only one product.

29. A Synthesis Reaction

30. Major Classes of Reactions
In a decomposition reaction, a compound breaks down into two or more simpler substances.
The compound may break down into individual elements, such as when mercury(II) oxide decomposes into mercury and oxygen.

31. Major Classes of Reactions
The products may be an element and a compound, such as when hydrogen peroxide decomposes into water and oxygen.
The compound may break down into simpler compounds.

32. A Decomposition Reaction
When ammonium nitrate is heated to a high temperature, it explosively breaks down into dinitrogen monoxide and water.
The decomposition reaction taking place is represented by a balanced equation that shows one reactant and more than one product.

33. A Decomposition Reaction

34. Major Classes of Reactions
In a single-displacement reaction, one element takes the place of another in a compound.
The element can replace the first part of a compound, or it can replace the last part of a compound.

35. Single Displacement
If an iron nail is placed into an aqueous solution of copper(II) sulfate, the iron displaces the copper ions in solution, and copper metal forms on the nail.

36. Single Displacement

37. Major Classes of Reactions
In double-displacement reactions, the positive portions of two ionic compounds are interchanged.
For a double-displacement reaction to take place, at least one of the products must be a precipitate or water.

38. Double Displacement
When clear aqueous solutions of lead(II) nitrate and potassium iodine are mixed, a double-displacement reaction takes place and a yellow solid appears in the mixture.
This solid is lead(II) iodine, and it precipitates out because it is insoluble in water, unlike the two reactants and the other product.

39. Double Displacement

40. Major Classes of Reactions
A combustion reaction is one in which a substance rapidly combines with oxygen to form one or more oxides.

41. Combustion
When welding is done with an acetylene torch, acetylene combines with oxygen to form carbon dioxide and water.
This combustion reaction is exothermic, and enough energy is released to melt metal.

42. Combustion

43. Basic Assessment Questions
Write a word equation and a skeleton equation for each of the following descriptions of chemical reactions.

44. Basic Assessment Questions
Question 1a
Solid lithium reacts with chlorine gas to produce solid lithium chloride.
Answer 1a

45. Basic Assessment Questions
Question 1b
Nitrogen gas reacts with oxygen gas to produce nitrogen dioxide gas.
Answer 1b

46. Basic Assessment Questions
Write a balanced chemical equation for the following reactions, making sure coefficients are in their lowest possible ratio.

47. Basic Assessment Questions
Question 2a
Solid potassium reacts with liquid water to produce hydrogen gas and a water solution of potassium hydroxide.
Answer 2a

48. Basic Assessment Questions
Question 2b
Calcium chloride and sodium carbonate in water solution produce solid calcium carbonate and a water solution of sodium chloride.
Answer 2b

49. Basic Assessment Questions
Identify each of the following skeleton equations as representing a synthesis reaction, a combustion reaction, both synthesis and combustion, or decomposition reaction. Balance each equation if necessary.

50. Basic Assessment Questions
Question 3a
Answer 3a
synthesis;

51. Question 3b Answer 3b decomposition; already balanced
Basic Assessment Questions
Question 3b
Answer 3b
decomposition; already balanced

52. Reactions in Aqueous Solutions
When aqueous solutions that contain ions are mixed, the ions may react in a double-replacement reaction.
The product is typically a solid precipitate, water, or a gas.

53. Reactions in Aqueous Solutions
An example of a double-replacement reaction that produces a precipitate occurs when aqueous solutions of sodium chloride and silver nitrate are mixed to form a precipitate of solid silver chloride.

54. Reactions in Aqueous Solutions
To show all of the particles in solution as they really exist, a complete ionic equation can be written.
The sodium and nitrate ions are on both sides of the equation.
Such ions that do not participate in a reaction are called spectator ions.

55. Reactions in Aqueous Solutions
An ionic equation that does not show spectator ions but only the particles that participate in a reaction is called a net ionic equation.
In the case of the reaction above, the net ionic equation from which the sodium and nitrate ions have been removed is as follows.

56. Writing Ionic Equations
Write the balanced chemical equation for the reaction between aqueous solutions of strontium nitrate and potassium sulfate, which forms the precipitate strontium sulfate.
Then write the complete ionic and net ionic equations.

57. Writing Ionic Equations
Write the correct skeleton equation.
Use coefficients to produce the balanced chemical equation.

58. Writing Ionic Equations
Write the complete ionic equation.

59. Writing Ionic Equations
Cross out the spectator ions, which are those that are on both sides of the equation.
That leaves the net ionic equation.

60. Reactions that form water or a gas
Some double-replacement reactions in aqueous solution produce water or a gas (or both) rather than a precipitate.
In such cases, the water or gas is shown as a product in the net ionic equation, as are the ions that produced it.
The remaining ions are eliminated as spectator ions.
The following example problem illustrates this concept.

61. Reactions that form water or a gas
When hydrochloric acid and potassium hydroxide solutions are mixed, water results, together with an aqueous solution of potassium chloride.
Write the balanced chemical equation, a complete ionic equation, and a net ionic equation for this reaction.

62. Reactions that form water or a gas
The balanced chemical equation is the same as the skeleton equation.

63. Reactions that form water or a gas
Write the complete ionic equation, which includes all of the ions.
Remove the spectator ions to produce the net ionic equation.

64. Additional Assessment Questions
Write a balanced chemical, complete ionic, and net ionic equations for the following reaction:
Aqueous solutions of lead(II) nitrate and ammonium chloride are mixed, forming a precipitate of lead(II) chloride.

65. Answer Chemical: Complete Ionic: Net ionic:
Additional Assessment Questions
Answer
Chemical:
Complete Ionic:
Net ionic:

66. Additional Assessment Questions
Write a balanced chemical, complete ionic, and net ionic equations for the reaction between the following substances, which produce water:
nitric acid (HNO3) and aqueous barium hydroxide

67. Answer Chemical: Complete ionic: Net ionic:
Additional Assessment Questions
Answer
Chemical:
Complete ionic:
Net ionic:
or, with coefficients reduced to lowest terms,

68. Additional Assessment Questions
Write a balanced chemical, complete ionic, and net ionic equations for the reaction between the following substances, which produce a gas:
hydrochloric acid and aqueous sodium cyanide, with production of hydrogen cyanide gas (HCN)

69. Answer Chemical: Complete ionic: Net ionic:
Additional Assessment Questions
Answer
Chemical:
Complete ionic:
Net ionic: