Fall Final Exam Review of Problem Solving: These problems come from a previous year’s final exam. Work each problem on a separate sheet of paper. You may work on these in a small group. For each calculation show the intermediate steps use to reach the final value. Record numbers with the appropriate number of significant figures. 1. Write a balanced chemical equation for the combustion of butane, C4H10. 2. Write a balanced chemical equation for a double replacement reaction in which silver nitrate reacts with iron(III) chloride. 3. How many grams of silver will be produced when 105 grams of magnesium metal react with excess silver nitrate in the reaction below? Mg (s) + 2 AgNO3 (aq) Mg(NO3)2 (aq) + 2 Ag (s) 4. An astronaut must measure the mass of a solid cube of iron in outer space. Given that the density of iron is 7.14 g/cm3 and that the cube’s side measures is 2.5 cm, find the mass of the cube. 5. Heating a mixture of iron filings and powdered sulfur produces a compound of 63.7% Fe and 36.3% S. Determine whether the correct name of the compound is iron(III) sulfide or iron(III) sulfide. 6. Calculate the number of moles of sodium contained in a 5.55 grams sample of sodium nitrate. 7. Calculate the number of oxygen atoms in 19.5 grams of lead(IV) oxide. 8. Draw Lewis dot structures for the following:
a. H4N2O
b. CO32-
c. CSF2
10. In a synthesis reaction which makes iron(III) oxide, calculate the number of moles of product formed if 5.59 grams of iron an 4.58 grams of oxygen gas are allowed to react? 11. If a 111 grams of manganese react with excess chlorine gas to make manganese(II) chloride, what is the total number of electrons that the manganese atoms give to the chlorine atoms? 12. Edward is determining the density of 25 pure copper pennies by volume displacement. The volume of the 25 pennies is found to be 10.5 mL. Assuming these pennies have a density of 8.94 g/mL, calculate the number copper atoms in a single penny. Try to do a couple of these each weekend or on a light homework evening.
Chapter Inventory for Final Exam Chapter 1
Section 1: Defining matter and its three states and Evidence of Physical vs Chemical Changes Key Vocabulary
Section 2: Describing Matter and Working with SI units, prefixes and Recording data Key Vocabulary
Section 3: Classifying Matter Key Vocabulary
Chapter Review pg 31-35: 2, 3, 10, 16, 19, 23, 26, 29, 37, 48, 49 & Standardized Test Prep Chapter 2 Section 1: Conservation of energy Key Vocabulary
Section 3: Measurements and Calculations Key Vocabulary
Chapter Review pg 66-71: 10, 11, 18, 20, 24, 30, 37, 39, 55, and Standardized Test Prep Chapter 3 Section 1: Dalton’s Theory of the Atom Key Vocabulary
Section 2: Structure of the atom discoveries and Deducing the arrangement of an atom given information from the atomic symbol Key Vocabulary
Section 3: Electron Arrangement Key Vocabulary Chapter Review pg 107-113: 13-15, 18, 22, 25, 45, 62, 82, and Standardized Test Prep
Chapter 4 Section 1: Periodic Law and Families of the periodic table Key Vocabulary
Section 2: Periodic table trends are generally predictable Key Vocabulary
Chapter Review pg 150-155: 1-3, 7-9, 17, 20-22, 31c, 32, Chapter 5 Section 1 & 2: Stability is gained by moving electrons to reach NG-configuration Key Vocabulary
Section 3: Naming simple salts, transition metals salts and polyatomic ion salts Key Vocabulary
Chapter Review pg 183-187: 2-4, 8, 11, 16, 17, 22, 23, 25, 27, 42 and Standardized Test Prep Chapter 6 Section 1: Comparing types of bonds and Predicting them Key Vocabulary
Section 2: Lewis dots to diagrams and Prefix naming system Key Vocabulary
Section 3: Drawing structural formulas given Lewis dots and Describing Shapes Key Vocabulary
Chapter Review pg 216-221: 2, 5, 6, 8, 9, 11, 14, 15, 17, 27, 28, 31, 32abe, 33a, 41 and Standardized Test Prep Chapter 3 Section 4: Counting Atoms Key Vocabulary
Chapter Review pg 107-113: 34-38, 55, 63, 92 Chapter 7 Section 1: Avagadro’s work with gases gives first relative mass scale and Mole concept Key Vocabulary
Section 2: Relative atomic masses and formula masses Key Vocabulary Section 3: Empirical formulas and Percent Composition Key Vocabulary
Chapter Review pg 251-255: 1, 2, 6, 22, 23, 29, 35, 37, 48, 84 and Standardized Test Prep
Section 1: Describing Chemical Reactions Key Vocabulary
Section 2: Balancing Chemical Equations Key Vocabulary
Section 3: Identifying the 5 Types of Reactions and Predicting Equations Key Vocabulary
Chapter Review pg 292-299: 8, 9, 11, 16, 18-21, 51,52, 53, 57, and Standardized Test Prep
Chapter 9 Section 1: The Mole Ratio is at the Heart of Stoichiometry Problems (mole-mole, mass-mass, massmolecules etc…) Key Vocabulary
Section 2: Limiting and Excess in Predicting Theoretical Yields Key Vocabulary
Chapter Review pg 329-335: 5-10, 17, 20, 27, 29, 31, 37, 39, 55 and Standardized Test Prep Larger Topics for Essays: How are accuracy and precision demonstrated in laboratory practice? How is our current model of the atom based on the work of Thompson, Rutherford and Bohr? Why is knowledge of the periodic table the most important tool for doing chemistry? Chemists use stoichiometry the way that a cook uses a recipe for menu planning. Explain this statement
