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Name ______________________________ Date: __ _______ Chemistry Semester I Final Exam Review Guide Topics Covered Unit 1: Metric system, Temperature Conversions, Unit Conversions, Significant Figures, Percent Error, Scientific Notation, Density, Dimensional Analysis with conversions, reading a graduated cylinder, recording significant figures in the lab Unit 2: Elements, Compounds, Pure Substances, Mixtures, Physical and Chemical Changes and Properties, heat, specific heat Unit 3: Groups on the Periodic table, Atomic Structure, Atoms, Ions, Isotopes, Atomic Mass, characteristics of metals, and nonmetals, balancing nuclear reactions, half-life problems, Identifying a pure substance, homogenous mixture, heterogenous mixture, element, and compound through molecular diagrams. Unit 4: Naming and writing formulas for ionic compounds, molecules, and acids, cations, anions, polyatomic ions. Unit 5: Percent composition, molar mass, mole conversions, empirical formulas, and molecular formulas UNIT 1: Scientific Measurement (Chapter 2) 1. How many sig figs are in the following numbers? 2.04 ______ 0.002804 ______ 1,230 ______ 0.00989 ______ 2. When adding and subtracting, the rule for sig figs is to look at the number of ___________ __________. Calculate the following using correct sig figs: 18.345 + 4.12 = _________ 21.672 – 0.5 = _________ 3. When multiplying and dividing, the rule for sig figs is to look at the number of _________ _________. Calculate the following using correct sig figs: 5.678 x 2.3 = _________ 18.1 x 3 = _________ 4. Put the following numbers in scientific notation: 8,923,000,000 = _________________ 0.00000345 = _________________ 0.00045 = ________________ 5. Do the following unit conversions: 6.7dm = _______________ mm 6. How many kilometers are in 7650 milimeters? ________________ 7. How many centigrams are in 8.56 decigrams? ________________ 325 cL = ____________ L 8. The formula for density is: ____________ Density is the ratio of ____________ to ____________. 9. Calculate the density of an object if it has a mass of 13.2 grams and a volume of 3.4 liters. Density = _____________ 10. Calculate the mass of a piece of plastic that has a density of 3.14 g/mL and a volume of 7.2 mL. Mass = _______________ 11. Calculate the volume of an unknown substance that weighs 23.1 grams and has a density of 5.6 g/mL. Volume = ______________ 12. Perform the following temperature conversions: 967ºC = ________ K 13. Calculate the percent error: Experimental Length = 14.1 cm 435 K = ________ ºC Accepted Length = 14.9 cm 14. Use dimensional analysis to solve the following density problem: How many liters are 45.7 kg of bromine? The density of bromine is 3.10g/mL. UNIT 2: Matter and Change (Chapter 3) 15. What is a chemical change? _______________________________________________________________ Which of the following is a chemical change: ripping a piece of paper, melting ice, burning wood? 16. Give 2 examples of physical changes: _______________________________________________________ 17. What is the difference between physical and chemical properties? _________________________________ ______________________________________________________________________________________ Which of the following is NOT a physical property? color, boiling point, texture, density, reactivity 18. Name 2 chemical properties: _______________________ __________________________ 19. What is the difference between heterogeneous and homogeneous mixtures? _________________________ _____________________________________________________________________________________ Which of the following is an example of a homogeneous mixture? copper, salsa, salt, Gatorade 20. Determine if each is a pure substance or a mixture: sodium (Na) ______________ Kool-Aid ______________ water _______________ 21. Name the 4 indicators of chemical change: _____________________, _____________________, _____________________, ______________________ 22. Define heat: 23. Define specific heat: 24. Convert the following: 38.65 cal = J 934 J = kcal 25. How much energy (in joules) is required to heat a piece of iron weighing 1.30g from 25.0oC to 46.0oC? 26. A 55.0g sample of a metal requires 675 J of energy to hear it from 25.0oC to 118.0oC. Calculate the specific heat of the metal. UNIT 3: Atomic Structure (Chapter 4) 27. Calculate the atomic mass of iron based on the following information: Fe-56 (94.5 %) Fe-57 (2.3 %) Fe-59 (3.2 %) 28. The mass number is found by adding _______________ plus _________________. 29. What is the difference between a cation and an anion? (Which is positive/negative? Gained or lost e-?) Cation: _____________________________________________________________________________ Anion: _____________________________________________________________________________ 30. Nickel: Protons = _______ Neutrons = _______ Electrons = _______ Chlorine: Protons = _______ Neutrons = _______ Electrons = _______ 31. How many neutrons are in the following isotopes? Co-60 ________ U-235 _________ 32. Name 2 noble gases: ___________, ____________ W-185 ________ Name 2 halogens: ___________, ____________ 33. Give 3 examples of transition metals: ___________, ___________, ___________ 34. What do the numbers represent in the following symbol? 190Os 76 190 = _______________________ 35. The rows on the periodic table are called ________________. 76 = _______________________ The columns on the periodic table are called ________________. 36. Write the correct charge and name for the following ions. Example: Calcium = Ca2+ Calcium ion Sulfur = S2- Sulfide Lithium = ___________________ Fluorine = _____________________ Magnesium = ___________________ Nitrogen = _____________________ 37. As Potassium becomes as ion, it likes to __________ (gain/lose) electrons. How many? ________ As Oxygen becomes an ion, it likes to __________ (gain/lose) electrons. How many? ________ 38. Sn-120: Protons = ________ Neutrons = ________ Electrons = ________ 39. Atoms of the same element always have the same number of _____________ (protons, neutrons, electrons) 40. An isotope has 12 protons, 12 electrons, and 14 neutrons. Name the isotope using hyphen notation: _______ 41. Metals are located on the form side of the periodic table, and tend to . List two characteristics of metals: 42. Nonmetals are located on the electrons to form side of the periodic table, and tend to . List two characteristics of nonmetals: 43. List the metalloids: 44. What are the four nuclear particles? __________ __________ __________ __________ 45. Balance the following nuclear reactions: 198 86 22 11 Rn 24 He 194 84 Po 22 Na 10 e10 Ne U 10 e 237 93 Np 237 92 26 14 26 Si 13 Al 10 e 46. Write a balanced reaction for each nuclear reaction. Decay of polonium-218 by alpha emission. Decay of chlorine-32 by positron emission. electrons to Decay of promethium-142 by electron capture. Decay of oxygen 18 by emission of two neutrons 47. What is half-life? 48. The half-life of phosphorous-30 is 2.5 min. If you start with 35 g of phosphorus-30, how many grams would remain after 20.0 min? 49. The half-life of polonium-210 is 138.4 days. How many milligrams of polonium-210 remain after 415.2 days if you start with 2.0 mg of the isotope? 50. 20.0 g of a radioactive isotope are present at 1:00 p.m., and 5.0 g remain at 2:00 p.m. a. How many half-lives have gone by? _________________________ b. How long is the half-life of the isotope? _________________________ c. Predict how many grams will be left at 2:30 p.m. _________________________ 51. Know the safety rules 52. Be able to identify the various lab equipment and know their uses and know what units each measures. Unit 4: Naming (Chapter 5) 53. What do all ionic compounds begin with? 54. Why do you have to use a roman numeral to identify some cations? 55. What do all acids begin with? 56. What do all molecules begin with? 57. Name the following compounds/molecules. Zn3(PO3)2 __________________________________________ Co3N2 __________________________________________ S4Br7 __________________________________________ H2CO3 __________________________________________ 58. Write the formula for the following compounds/molecules. Hydrofluoric acid _______________________ Nickel (II) chlorate _______________________ Dicarbon pentaiodide _______________________ Aluminum nitrate _______________________ Unit 6 The Mole (Chapter 8) 59. What is Avogadro’s number? 60. How many things are in one mole? 61. What is the molar mass of MgCl2? 62. How many moles of SO3 are in 2.4 x 1024 molecules of SO3? 63. How many atoms of aluminum are present in a 0.275 mole sample of Al 2(CO3)3? 64. How many grams of Ba(IO3)2 are there in a 1.25 x 1022 formula unit sample of Ba(IO3)2? 65. Determine the percentage composition of sulfur in SCl2 66. Given the following percent composition data. Determine the empirical formula of the following compound. 56.8 % C 6.50 % H 28.4 % O 8.30 % N 67. The empirical formula was found to be C2H4O. What is the molecular formula if the molar mass of this molecule is 132.16?