Chemistry 2nd Semester Exam Review Sheet
Chapters 9, 10, 11, 12, 13, 14, and 15
Chapter 9: All
1. Balance chemical equations and determine relationships between moles of reactant and moles of products and mass of reactants with mass of products.
2. How many moles of ammonium sulfate can be made from the reaction of 30.0 moles of ammonia with sulfuric acid?
3. Sodium carbonate reacts with nitric acid to produce sodium nitrate, carbon dioxide, and water. How many moles of sodium carbonate are required to produce 100.0 g of sodium nitrate?
4. Determine the limiting reagent of a chemical reaction and use it to do stoichiometric calculations.
5. According to the following reaction: 2As2O3 + 3C ®3CO2 + 4As If 8.87 g of As2O3 is used in the reaction and 5.33 g of As is produced, what is the percent yield?
Chapter 10: All. 4.3 & 4.5
6. Compare/contrast various atomic models throughout history.
7. What happens when an electron is excited and then drops to its ground state?
8. Discuss the dual nature of light.
9. Use Hund’s Rule and the Pauli Exclusion Principle to construct and interpret orbital diagrams.
10. Name the elements
a. 1s22s22p1 b. 1s22s2 c. 1s22s22p63s23p2
11. Determine it the e-config is in a ground or excited state
a. 1s22s22p6 b. 1s22s22p53s2 c. 1s22s22p63s23p64s23d3
12. Write the e-configs for
a. K+ b. O2- c. Br1- d. Be e. Mg f. Ca g. Sc
13. Show trends in the atomic properties as you move across a period or up/down a group.
Chapter 11: All
14. Compare/contrast ionic, covalent (polar and non-polar), and metallic bonds.
15. Define electronegativity. How does it relate to polar versus non-polar bonding?
16. Compare/contrast the different geometric shapes of molecules (VSEPR). Determine the shape of different compounds.
17. Determine molecular polarity based on molecular shape.
18. Write Lewis structures for molecules with single and multiple bonds.
Chapter 12: 12.1-12.5 & 12.7-12.10
19. Convert between common pressure units.
20. Describe the relationship between gas volume and temperature. What other relationships are there in regards to the gas laws?
21. Use the combined gas law to solve for pressure, temperature and volume.
22. Solve problems using PV=nRT or apply STP to solve for an unknown value.
23. Explain the behavior of gases using the kinetic molecular theory
Chapter 13: 13.1 – 13.4, 3.6 & 3.7
24. Compare/contrast the molecular structure solids, liquids, and gases.
25. Discuss the uniqueness of water due to its intramolecular and intermolecular forces.
26. Draw and completely label (using all correct terms) the heating curve of water.
27. Calculate energy change during a phase change and energy change during a temperature change.
28. Based on molecular shape, predict the type of intermolecular forces that hold liquids together.
29. Determine how a change in vapor pressure will affect the properties of a liquid.
Chapter 14: 14.1 – 14.5
30. Apply the concept of polarity to discuss why some things dissolve in water and others don’t.
31. What factors affect the solubility of a gas? Of a solid? How?
32. Compare/contrast unsaturated, saturated and supersaturated solutions.
33. Calculate the mass percent of a solution.
34. Do any molarity or dilution problem.
Chapter 15: 15.1 – 15.5
35. Define acid and base using all three theories.
36. List the properties of acids and bases.
37. Explain the relationship between acid strength and the strength of the conjugate base.
38. What happens when an acid reacts with a base?
39. Calculate the pH and pOH for various solutions.
40. Calculate the ion concentration for different acids and bases.