Chapter 10 Chemical Reactions
Section #1: Simple Balancing
Steps for balancing:
1. Since these are written in symbol form, DO NOT mess with the subscripts.
2. Place Co-efficients IN FRONT of elements and/or compounds. NEVER in between compounds. Example: 2H2O is correct. H22O is not correct.)
3. Balance both sides so that you have the same number of elements on the reactants side as on the products side
1.HgO Hg + O2
2.H2 O H2 + O2
3.Al + Pb (NO3) 2 Al(NO3) 3 + Pb
4.Cu + AgNO3 Cu(NO3) 2 + Ag
5.K + H2O KOH + H2
6.Cl2 + LiI LiCl + I2
7.F2 + H2O HF + O2
8.AgNO3 + K2SO4 Ag2SO4 +KNO3
9.Na + Cl2 NaCl
10. CaO + H2O Ca(OH) 2
11. Mg + O2 MgO
12.Fe + O2 Fe2O3
13.H2O + N2O3 HNO2
14. Na2O + H2O NaOH
15.Fe + H2O Fe3O4 + H2
Section #2: Names into Symbols, then balance
Write and Balance equations for the following chemical reactions
Steps for balancing:
1. Change the names into symbols.
2. Remember, names ending in –ide are monoatomic ions. (Except for hydroxide and cyanide). Names ending in –ate or –ite are polyatomic ions.
3. Don’t forget your seven diatomic atoms (H2, N2, O2, F2, Cl2, Br2, I2)
4. Write the oxidation numbers for each element ABOVE the element so that you can balance the charges within the compound. Remember, if an element stands “alone”, its oxidation number plays no role until it is combined with another element (for example, Al is +3, but when it is alone, the +3 doesn’t do anything. But, when you put Al together with Cl, it becomes AlCl3).
5. Remember that the roman numerals tell you the POSITIVE oxidation number of the first element in the compound. Example: Copper (II) Nitrate means that copper has a +2 oxidation state. ALSO, if there is a Roman numeral but you expect the oxidation state to be different, go with the Roman numeral. Example: Nitrogen (II) Oxide. I know that you think nitrogen should be –3 from the chart, but the (II) makes it +2.
6. Once you have all of your subscripts in place, balance with co-efficients.
1.Magnesium Bromide + Chlorine Magnesium chloride + Bromine
2.Chlorine + Sodium Iodide Sodium Chloride + iodine
3.Aluminum Nitrate + Sodium Hydroxide Aluminum hydroxide + sodium nitrate
4. Sulfur trioxide sulfur dioxide + oxygen
(Sulfur trioxide is: SO3 , sulfur dioxide is: SO2)
5. Aluminum hydroxide + Iron Iron (II) hydroxide + Aluminum
6.Ammonium nitrite nitrogen + water
(Ammonium is: NH4+and ammonia is: NH3)
7. Silver(I)Chloride + Aluminum Sulfate Aluminum Chloride + Silver Sulfate
8.Barium Chloride + sodium sulfate sodium chloride + barium sulfate
9. Iron (III) oxide + carbon monoxide iron + carbon dioxide
10.Aluminum + Copper (II) chloride aluminum chloride + copper
11.Iron + silver (I) acetate iron (II) acetate + silver
Textbook Helpful Sections
P. 290 Table 10-2 has guidelines for Double-Replacement Reactions
Section #3: Combustion Reactions (p. 285)
Steps for Balancing Combustion Reactions:
1. Balance the C’s and the H’s First.
2. Write a fraction in front of the O2 on the reactant’s side such that the numerator of the fraction is equal to the number of oxygen’s you need divided by 2. Example: For question #1, you will write 7/2O2.
3. Multiply the entire equation through by 2
1. C2H6 + O2 ------ CO2 + H2O
2. C4H10 + O2 ------ CO2 + H2O
3. C6H14 + O2 ------ CO2 + H2O
4. C8H18 + O2 ------ CO2 + H2O
5. C10H22 + O2 ------ CO2 + H2O
6. CH3OH + O2 ------ CO2 + H2O
7. C2H5OH + O2 ------ CO2 + H2O
8. C3H7OH + O2 ------ CO2 + H2O
9. C4H9OH + O2 ------ CO2 + H2O
10. C5H11OH + O2 ------ CO2 + H2O
Section #4: Predict the Products (p. 291)
Balance and predict the products
Textbook Helpful Sections
P. 291 Table 10-3 has How to Predict Products of a Chemical Reaction
1.Aluminum + hydrochloric acid
2.Iron + copper (II) sulfate (iron II compound is formed).
3. Chlorine + magnesium iodide
4.Magnesium + hydrochloric acid
5. Magnesium + oxygen
6.Iron metal + oxygen (an Iron (III) compound is formed)
7.Iron (II) sulfide + hydrochloric acid
8.Ammonium sulfide + iron (II) nitrate (ammonium is NH4+)
9.Aluminum sulfate + calcium phosphate
10.Barium carbonate + hydrochloric acid
11.Silver (I) acetate + potassium chromate
12.Ammonium phosphate + barium hydroxide
Section #5: Reactions in Aqueous Solutions
(Section 10.3, p. 292-299)
Read Section 10.3 and answer the following questions:
1. What is an aqueous solution?
2. In salt water, which is the solvent? Salt or Water?
3. In salt water, which is the solute? Salt or Water?
4. T or F: A precipitate is when a metal and a non-metal ion come together to form an insoluble (not soluble in water) product.
5. What is a spectator ion?
6. Which of the following is included in a Complete Ionic Equation:
a. Precipitate ions b. Spectator Ions c. Both
7. Which of the following is included in a NET Ionic Equation:
a. Precipitate ions b. Spectator Ions c. Both
8. Why are spectator ions NOT included in the net ionic equation (oops, did I just give away the answer to #7?) Write your response here:
Turn to Page 920 (yes, 920, go ahead, I'll wait here while you turn to that page…).
9. Which letter on Table C-10 Solubility Guidelines indicates a precipitate
a. S b. I
10. Which letter on Table C-10 Solubility Guidelines indicates a set of spectator ions?
a. S b. I
12. Look at the rules on p. 920 and circle the Precipitates in the list of a-h below. Some are precipitates, and some remain as spectator ions.
a. Sodium Chloride
b. Aluminum Acetate
c. Sodium Fluoride
d. Sodium Bromide
e. Mercury (I) Chloride
f. Strontium Sulfate
g. Sodium Carbonate
h. Magnesium Carbonate
ON THE TEST, I WILL GIVE YOU ONLY THE RULES #1-5, not the large grid below the rules. Be sure you know how to apply the rules!
Now turn back to p. 292
13. There are three types of double replacement reactions listed in section 10.3. The first one is Reactions that Form Precipitates. What do the other two form?
PRACTICE PROBLEMS p. 294-299SHOW ONLY THE SKELETAL and NET IONIC EQUATIONS for each one
Do practice problems 33, 36, 38, 39, 44