November 23rd, 2011 Final Exam ReviewThis is the review for the final exam. It by no means intends to depictthe exam’s format, and it is NOT everything you need to know for thefinal exam. This review is intended to help you have more chemistrypractice. Below I have written the topics we have covered thissemester (I may have missed some, but you SHOULD have all ofthem in your notes!The old reviews should help you study as well.Make sure you go over your notes and homework. Do not wait untilthe day before the exam to study, begin now!70 percent of the exam will be based on the material covered afterthird partial.10 percent will come from first partial.10 percent will come from second partial.10 percent will come from third partial.For a total of 100 percent 1. Introduction to chemistry: definition of chemistry 2. Matter 3. Substance 4. Mass vs. Weight 5. Conversions (SI Units and English Units) 6. Properties and changes of matter (physical and chemical… include states of matter) 7. Elements name and symbol of common elements 8. Methods of separating mixtures 9. Types of mixtures 10. The atom and the atomic model 11. Atomic structure (composition, atomic mass, atomic number, average atomic mass) 12. Ions 13. Isotopes 14. Atomic models 15. Ground vs. Excited State 16. Quantum numbers 17. Electron configurations 18. Periodic Table and periodic trends 19. Types of bonds 20. Types of inorganic compounds
November 23rd, 2011 Final Exam Review 21. Types of reactions 22. Nomenclature 23. Oxidation Numbers 24. Balancing (This will include Redox) 25. Stoichiometry 26. Ideal Gas Law 27. Solutions 28. Concentrations 29. pHSolve the following problems:1. Draw the orbital diagram, the electron configuration, electron dot notation, andthe noble notation of the following elements. Then find the four quantum numbersfor the given electron. a. Re (hint this element goes through the f-orbitals): 30th electron b. Cd: 14th electron c. Ra: 83rd electron d. In: 36th electron2. Differentiate between chemical and physical property and change, giveexamples of each.3.Give the names of the following compounds and find the oxidation numbers. a. Ca(C2H3O2)2 b. NO2 c. SiF4 d. VCl54. Complete the following reactions, state the type of reaction and balance wherenecessary, identify the type of inorganic compound: a. K(s) + Cl2(g) b. H2CO3 c. MCO3 d. Fe(s) + CuSO4(aq) e. AgNO3(aq) + KCl(aq) f. HCl (aq) + NaOH (aq) g. HBr (aq) + Ba(OH)2 (aq)
November 23rd, 2011 Final Exam Review5. Stoichiometry a. Ethanol, also known as grain, can be made from thefermentation of sugar (C6H12O6). The unbalanced chemical equation for thereaction is shown below. C6H12O6 C2H5OH + CO2Balance the chemical equation and determine the mass of C2H5OH producedfrom 750 g of C6H12O6. b. Hydrofluoric acid solutions cannot be stored in glass containersbecause HF reacts readily with silica dioxide in glass to produce hexafluorosilicicacid (H2SiF6). 40.0g SiO2 and 40.0g HF react to yield 45.8 g H2SiF6. SiO2 (s) + 6HF (aq) H2SiF6 (aq) + 2H2O (l)I. What is the limiting reactant?II. What is the mass of the excess reactant?III. What is the theoretical yield of H2SiF6?IV. What is the percent yield? c. This problem is a challenge problem, harder than the ones wehave done before… but not so hard as to where you cannot answer it. Read theproblem carefully!Phosphorus (P4) is commercially prepared by heating a mixture of calciumphosphate (Ca3(PO4)2), sand (SiO2), and coke (C) in an electric furnace. Theprocess involves two reactions. 2Ca3(PO4)2 (s) + 6SiO2 (s) 6CaSiO3 (l) + P4O10 (g) P4O10 (g) + 10C (s) P4 + 10CO (g)The P4O10 produced in the first reaction reacts with an excess of coke (C) in thesecond reaction. Determine the theoretical yield P4if 250.0 g of Ca3(PO4)2and400.0 g of SiO2are heated. If the actual yield of P4 is 45.0g, determine thepercent yield of P4.
November 23rd, 2011 Final Exam Review6. Concentrations a. What mass of NaOH is in 250 mL of a 3.OM NaOH solution? b. How many milliliters of a 5.0 M H2SO4 stock solution would you need to prepare 100.0mL of 0.15M H2SO4? c. What is the molality of a solution that contains 75.3 g of KCl dissolved in 95.0 g of water? d. How many grams of Na2CO3 must be dissolved into 155 g of water to create a solution with a molality of 8.20 mol/kg? e. This is also a challenge problem. Hint fin the moles and then use stoichiometry to solve for the rest of it… What volume of ethanol (C2H3OH) is in a 100.0 mL of 0.15 M solution? The density of ethanol is 0.7893 g/mL.7. Balance the following equations using redox a. Identify each of the following as either oxidation or reduction. 1. I2 + e- 2I- 2. Fe2+Fe3+ + e- 3. K K+ + e- 4. Ag+ +e- Ag b. Identify what is being oxidized and what is being reduced i. 2Br- + Cl2 Br2 + Cl- ii. 2Zn + O2 2ZnO iii. 2Na + 2H+ 2Na+ + H2 c. Balance the following reactions using Redox: i. Fe + CuSO4 FeSO4 + Cu ii. Fe + HBr H2 + FeBr3