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GEN CHEMISTRY FALL FINAL SEMESTER REVIEW: CHAPTER #1, 2, 3, 4, 5, 7, 8, 9 NAME______________________________ DATE________________ Per________ These are sample questions that cover the material tested on the Final Exam. You should understand the process and not memorize the answers here since Final will have different elements, etc. Consult your notes and the textbook. Watch the tutorials on MCHS website. Unit #0: LAB SAFETY 1. How to neutralize a spilled acid: ________________________________________________ And a base: ___________________________________________________________________ 2. Define volatile: _________________________________ Corrosive: _______________________ Unit #1: DATA ANALYSIS& SCIENTIFIC METHOD 3. Define the study of Chemistry: the study of _____________________ and ________________ 4. Distinguish between mass and weight __________________________________________________ qualitative and quantitative data __________________________________________________ a control and the constants: _____________________________________________________ 5. Be able to convert between units 35.0 meters to micrometers = ____________________ 0.0549 kg to cg = __________________ and 300.0 millimoles to micromoles = ________________ 6. Define density: _________________________________ What are the units of measurement for density? _________________ Solve density problems: 7. Convert to scientific notation: 0.000 853 = _______________ 67, 839, 000 = ________________ 8. How do we add and subtract using scientific notation? 9.0387 g + 2.08 = _____________ 9. How do we multiply and divide using scientific notation? 38.7g / 2.1987 mL = _____________ 10. Convert temperatures between 0C and K. 45.8 °C = ____________ K 1286 K = __________ °C 11. Use conversion factors and solve problems by Factor label: Show work by factor label. Convert 37.9 miles to km Convert 1.45 gal/min to liters/hour 12. Distinguish between accuracy and precision ____________________________________________ 13. Determine the correct number of significant digits. 0.000 0560 = ______ 23, 860, 000 = _______ 14. Round numbers. 78.6539g rounded to 3 sig figs = ________ 0.000 064 210 to 2 = ____________ UNIT #2: MATTER-PROPERTIES AND CHANGES 15. Diagram the breakdown of matter. Matter = ________________ & _______________________ substances = ______________________ & ________________________ mixtures = ___________________________ & ________________________ 16. Give an example of an element: _____________________, a compound: ____________________, a homogeneous mixture: ____________________ and heterogeneous mixture: __________________ 17. What are the 4 states of matter? Describe the properties of each and tell their particle movement. ___________________________________________________________________________ ____________________________________________________________________________ ____________________________________________________________________________ ____________________________________________________________________________ 18. Recognize physical (give 3 examples: _____________________________________________ ______________________________) and chemical changes (give 3 examples: ___________________________________________________________________________) 19. Intensive (give 2 examples: _____________________________________________ ______________________________) versus extensive physical properties (give 2 examples: __________________________________________________________________________) 20. Define the Law of Conservation of Mass.: _________________________________________ _________________________________________________________________________ 21. Homogeneous and heterogeneous mixtures ________________________________________ 22. What are is the difference between filtration, distillation, chromatography, and crystallization? ____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ _____________________________________________________________________________ UNIT #3: THE STRUCTURE OF THE ATOM and ELECTRON STRUCTURE 23. Describe the work of major contributors to modern atomic theory, be able to describe their atomic models and which subatomic particles they knew of: Democritus: Dalton: J.J. Thompson and his expt with the Cathode Ray Tube: Rutherford and his gold foil expt: 24. List and describe the location, mass and charge of the three major subatomic particles: ______________________________________________________________________________ 25. Distinguish between and define: atomic number, mass number, isotope: __________________ ____________________________________________________________________________ write the isotope symbol for carbon-14 __________ and for iodine-131 __________ 26. Know how to find numbers of protons, electrons and neutrons Ex for gold = ________ p ________ e _______n 23 Na1+ 11 _____p _____e ____ n copper = ________ p ________ e _______n 27. Define valence electron __________________________________ How many v e does O have? _________ and Mg ________ and Te ______ All halogens have ______ valence electrons ____ 28. Types of radiation: alpha, beta, and gamma _________________________________________ ____________________________________________________________________________ 29. What happens when an electron moves from a higher energy level to a lower one? 30. What happens when an electron moves from a lower energy level to a higher one? 31. What is wrong with this isotope symbol? 32. What is wrong with this isotope symbol? 81 36 30 Br _________________________________ 65 Zn ______________________________________ Atom Protons Neutrons Electrons A 3 4 2 B 9 10 10 C 12 12 12 D 17 18 17 E 17 20 15 F 18 22 18 33. From above table: Which atom(s) represents: a metal? ___________ a non-metal? ________ a metalloid? ____________ a halogen? _________ a noble gas? __________ an alkali metal? _________ an ion w/1+ charge? _______ an ion w/2+ charge? _______ an ion w/1- charge? _______ a neutral element? ___________ a cation? ___________ an anion? _____________ the mass number of “A” is __________________ the mass number of “E” is ___________________ the atomic number for “B” is ______________ 34. Tell what each number and letter means in 4s2 the atomic number for “D” is ______________ 4 = _____________________________, s = ________________________ and the 2 = _____________________________________ 35. The element with electron configuration 1s² 2s² 2p⁶ 3s² is _________________________ 36. What element is this? 1s² 2s² 2p³ _________________________________________ 37. What element is this? 1s² 2s³ 2p6 3s2 3p² ___________________________________________ 38. Tell what is wrong: 1s² 2s³ 2p¹ __________________________________________________ 39. Tell what is wrong: 1s² 2s² 2p² 3p¹ ___________________________________________________ 40. An element has the electron configuration [Kr]5s2. What group does it belong to and what element is it? __________________________________________________ 41. An element has the electron configuration [Ar]4s2 3d6. What group does it belong to and what element is it? _____________________________________________________ 42. Write the long form electron configuration of Se ( 1s22s22p4 ________________________________ ) How many more electrons does it need to satisfy the octet rule?______________________ 43. Write the long form electron configuration of Sr ( 1s22s22p4 ________________________________ ) How many more electrons does it need to satisfy the octet rule?_________________________ 44. The energy levels of atoms can be divided into ____________ with designations of s, p, ____ and ____. The number of electrons each can hold are: s = ____ p = ____ d = ___ f = ___ 45. A specific shaped “cloud” or region (that has specific orientations in space (x, y, z) where only 2 electrons are found is called a (an) ___________________ 46. The set of orbitals that are figure-eight-shaped and directed along the x, y, and z axes are called _________ sublevel. A spherical (ball shaped) electron cloud surrounding an atomic nucleus would best represent a ________ sublevel. The orbitals that are shaped like a four-leaf clover OR like a dumbbell with a doughnut are __________ sublevel. UNIT #4: IONIC COMPOUNDS 47. Define ionic chemical bond: ________________________________________________________ 48. Difference in properties of an element (Al) and its ion (Al3+). _______________________________ _______________________________________________________________________________ 49. The electrons involved in the formation of a chemical bond are called _________________ 50. Explain the formation of an ionic bond._____________________________________________ ____________________________________________________________________________ 51. Given an ion table be able to write correct formulas and name ionic compounds (also w/ Roman #) HCN = ______________________________ Fe (CN)2 = ___________________________ copper (I) oxide = ______________________ aluminum nitrate = ________________________ UNIT #5: COVALENT BONDING 52. Explain the formation of a covalent bond.______________________________________________ 53. What type of elements are usually involved in covalent bonding? ___________________________ 54. Define: electronegativity: _______________________________________________________ octet rule:___________________________________________________________________: 55. Given an electronegativity table, be able to classify the bonds within a compound as ionic, pure covalent, or polar covalent [0.0-0,39 : pure covalent, 0.40-1.69: polar covalent, 1.70-3.2: ionic] What type? C-Si ______________ Al-O _____________ N-F ________________ 56. Be able to write formulas & name molecules using Greek prefixes N3 O7 H3 = _________________________________________ 57. VSEPR Models: Linear, Bent, Trigonal planar, trigonal pyramidal, tetrahedral pyramidal: know the differences in shape and paired and lone pairs of electrons. Be able to determine what shape from the Lewis structure. Do C Br4 Si S2 MORE REVIEW PROBLEMS FOR SEMESTER EXAM FALL 1. How many significant figures are in 0.034? 10? 10.0? 2. How many significant figures are in the product of 8.31 x 7.5 x 9.34? 3. What is the density of a material that has a mass of 3.5 g and a volume of 5 L? 4. Convert 3.50 m to cm Convert 65 g to kg 5. Draw a Lewis Dot Diagram of sodium, chlorine and then sodium chloride. 6. Find the number of protons, neutrons, and electrons for the following: a) 2512Mg b) c) hydrogen-3 d) 137 Ba 56 35 Cl17 7. Write the formula for calcium nitrate: cobalt(II) carbonate: aluminum sulfate: carbon tetrachloride: sulfur trioxide 8. Write the name for BaCl2: Li2SO4: FePO4: H3PO4: HBr: MgSO2: Na CN 9. What is the percent error if the correct value is 55.6 g and you measured 57.5 g? 10. Write 546, 700 in scientific notation. 11. Write 0.00765 in scientific notation. 12. Write 6.789 x 10-6 in numbers. Write 7.89 x 105 in numbers. 13. Calculate the following problems in scientific notation: a) 4.35 x 103 + 6.12 X 102 = b) 7.32 x 102 - 9.68 x 103 = c) 3.12 x 10-2 x 6.23 x 10-5 = d) 9.33 x 103 3.11 x 102 = 14. Write the electron configuration for gold and tell how many valence electrons 15. What is the molecular shape of H2Se? How many shared pairs? 16. What is the molecular shape of SiO2? How many unshared pairs? 17. Hint: Make flash cards for vocab you need to remember.