Chemistry Final Exam Study Guide, Lecture notes of Chemistry

Download Chemistry Final Exam Study Guide and more Lecture notes Chemistry in PDF only on Docsity! Chemistry Final Exam Study Guide STRATEGY: Start by reading through your notes to refresh your memory on these topics. Then, use this review sheet as a starting point to identify the areas on which you need to spend more study time. For those areas, go back to homework assignments, quizzes, and reviews to practice more problems. Don’t just answer the questions you know! If you don’t know an answer, look it up in your notes, book or online. Also, these are not the questions that will be on the test, you need to be able to understand WHY an answer is correct, and not just WHAT the answer is…copying won’t help you on the Final Exam! Introduction Unit (Ch. 1-4) 1. In a lab, the average measured density for Pre-1982 pennies was 7.98 g/cm3. Given that the literature value for the density is 8.92 g/cm3, calculate the percent error. 2. Convert the following numbers into or out of scientific notation. a. 548,000 b. 0.0000770 c. 1.200 × 10-3 d. 9.25 × 107 3. Osmium is the densest element with a density of 22.57 g/cm3. Find the mass of a 56.2 cm3 sample of osmium. 4. Perform the following SI prefix conversions. a. 65.2 mm = ? cm b. 2.3 kg = ?g c. 65,000 ml = ? L d. 0.502 km = ? cm 5. How many milliliters are in a 2.0 quart jug of milk? (1L = 1.06qts) 6. Ms. Townsend spent last weekend grading tests. If she spent 4 min on each test, how many hours did it take her to grade all 74 tests? 7. Calculate the density from the slope of a "Mass vs. Volume" graph. 8. Write the isotope symbol, including atomic number & mass number, for the following isotopes. a. carbon-14 b. chromium-53 c. nickel-63 d. zirconium-92 9. Complete the table for the following isotopes. Symbol Atomic # Mass# Protons Neutrons electrons Zn 65 20 21 74 34 40 18 10. Calculate the average atomic mass of copper if 69.17% of the copper atoms occurring in nature are 63Cu and 30.83% are 65Cu. Atoms/Electrons (Ch. 5) 11. Draw an orbital diagram, complete electron configuration and noble gas notation for: a. Na b. C c. Mo d. Se 12. How does an electron become excited? What does it do when it returns to the ground state? 13. What is a photon? Quantum? 14. Describe the relationship between wavelength and frequency. 15. What type of electromagnetic radiation is emitted when an electron moves from n=4 to n=1? 16. Where are the s,p,d,f blocks located on the periodic table? How many orbitals are associated with each? How many electrons can be in each orbital? Periodic Table (Ch. 6) 17. DEFINE each of the following trends, describe WHAT the trend is (increases up, etc), explain WHY each trend occurs a. Atomic Radius b. Ionic Radius c. Ionization Energy d. Electronegativity 18. Circle the atom with the LARGER radius. a. Be N b. Ne Xe 19. Circle the particle with the LARGER radius. a. Cl Cl – b. Mg Mg2+ 20. Circle the atom with the HIGHER first ionization energy. a. Li Cs b. Ca As 21. Circle the atom with the HIGHER electronegativity. a. Cl Si b. O Po Bonds/Names (Ch. 8&9) 22. Based on their electronegativities (p. 169), are the bonds in the following substances IONIC, POLAR, or NONPOLAR? a. MgO b. LiCl c. H2O d. Br2 23. Are the following properties characteristics of ionic, covalent, or metallic bonding? a. These bonds are formed by delocalized electrons in an “electron sea.” b. These bonds involve a transfer of electrons. c. Substances containing these bonds are malleable and have very high melting points. d. Substances containing these bonds do not conduct electricity and have low melting points. e. Compounds containing these bonds have a crystal lattice structure. f. These bonds are formed by sharing electrons. 24. Use Lewis Diagrams to show the formation of MgO. 25. Use Lewis Diagrams to show the formation of H2O. 26. Explain the relationship between potential energy and stability. 27. Write formulas for the following compounds (HINT: First determine ionic/acid/covalent). a. calcium bromide d. silicon dioxide b. iron(III) sulfate e. dinitrogen tetroxide c. lithium phosphate f. ammonium carbonate 28. Write names for the following compounds (HINT: First determine ionic/acid/covalent). a. CrCl3 d. MgSO4 b. Cu2CO3 e. P4O6 c. AsCl5 f. NaClO3 29. Explain the difference between nonpolar covalent, polar covalent, and ionic bonds in terms of sharing of electrons and electric charge. Molecular Geometry (Ch. 9&13.2) 30. Explain the main idea of the VSEPR Theory 31. For each of the following molecules, draw the Lewis structure, name the number of lone and bond pairs, and give the name of the shape. a. BeCl2 b. AlCl3 c. CF4 d. H2O e. NH3 32. For each of the molecules in the previous question, draw the dipole moments, state whether the molecule is polar or nonpolar, then list any intermolecular forces that each molecule will have. 33. What type of IMF is indicated by each statement? Hint: IMF’s are: hydrogen bonding, dipole-dipole and London dispersion a. Attraction between any two polar molecules b. Very weak force that increases with molar mass c. Attraction between two momentary (or temporary) dipoles d. Very strong attractive force between molecules with N-H, O-H or F-H bonds. Moles (Ch. 11) 34. How many magnesium sulfate molecules are in 25g? 35. Find the percent composition of each element in copper (II) chloride 36. The percent composition of a compound is 40%C, 6.7% H and 53.7%O. The molecular mass of the compound is 180.0g/mol. Find its empirical and molecular formulas. 37. How many moles are in 5g of H2SO4? 38. How many grams of H2 is in 34L of H2? 39. 2.3 moles of Ca(OH)2 is equal to how many grams? 40. How many liters will 3.4 mol of O2 occupy? Reactions (Ch. 10) 41. Rewrite and balance the following word equation using chemical formulas, states, and energy. When solid sodium chlorate absorbs energy, it produces solid sodium chloride and oxygen gas. 42. Predict the products of the following single replacement reactions using the Activity Series in your Reference Tables. If no reaction occurs, write NR. If a reaction occurs be sure to write the correct formulas and balance. a. K + ZnCl2 b. Cl2 + HF c. Fe + Na3PO4