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Transcript
First Semester Final Exam 2013 Chemist: __________________________ Unit 1: Metric System and Density 1. Define “quantitative data” __Data that includes numerical measurements (numbers)______________ 2. Define “qualitative data” _Data that does not include numbers but qualities such as color, odor etc.____________________________________________ 3. Define “matter” __Anything that has mass and volume_____________________________ 4. Define “mass” (include unit) __measures the amount of matter in an object__in grams.__________________________________________________________ 5. Define “volume” (include unit) _ measures the amount of space an object occupies in an object__in mL or cm3 ___________________________________________________________ For every 1 mL of volume there is ___1___ cm3 of volume. 6. Define “density” (include units) _the amount of mtter in a given amount of space, measured in g/mL or g/cm3 ___ 7. When are you required to wear googles? _when using glassware, heat or chemicals_______ 8. When lighting a Bunsen burner do you turn gas on first or light the match first? _light the match___ Skills/ Practice Problems: K H D (base) d c m 9. Convert the following: Kilo Hecto Deca (base) deci centi milli 0.01 g = ______10_______mg 100 cm = _____1000_________mm 1.2 Km = __1,200___________ m 3.1 cg = _______.0031_______ Dg 10. Complete the following: 1 2 3 4 5 6 7 8 9 10 cm Smallest unit on ruler? Hundreds, tens, ones, tenths, hundredths Estimated significant figure? Hundreds, tens, ones, tenths, hundredths Measurement: __3.95cm____________ 11. What are the volumes of water, measured to the correct significant figure? 2.35mL 81.2mL 12. Calculate the density of a cube that has a volume of 27 cm3 and a mass of 4 grams. 4g/27 cm3=.15g/ cm3 13. What does the slope of this graph represent? Density 14. Which line represents a substance with a greater density?1 15. In the graph above, what is the mass of 10 mL of the substance represented by Line 1? 70g Unit 2: Atomic Structure and Periodicity 16. What is the charge, location and mass of a proton? ___________________________________________ 17. What is the charge, location and mass of a neutron? __________________________________________ 18. What is the charge, location and mass of an electron? _________________________________________ 19. What is an energy level? _________________________________________________________________ How can you determine how many an element has? __________________________________________ 20. What atomic particle determines the identity of the element? __________________________________ 21. What atomic particle is active in bonding and determines the chemical properties of the atom? ______ 22. Define “atomic number”__________________________________________________________________ Where is an atom’s atomic number on the periodic table? ______________________________________ 23. Define “atomic mass”____________________________________________________________________ Where is an atom’s atomic mass on the periodic table?________________________________________ What is the different between atomic mass and average atomic mass? __________________________ 24. Define “isotope”________________________________________________________________________ 25. Define “ion” ___________________________________________________________________________ 26. Define “cation”_________________________________________________________________________ 27. Define “anion” _________________________________________________________________________ 28. Define “period” ________________________________________________________________________ 29. Define “group/family” ___________________________________________________________________ What are the general characteristics of Group 1/Alkali Metals? ______________________________________________________________________________________ What are the general characteristics of Group 2/Alkaline Earth Metals? ______________________________________________________________________________________ What are the general characteristics of Group 7/Halogens? ______________________________________________________________________________________ What are the general characteristics of Group 9/Nobel Gases? ______________________________________________________________________________________ 30. Where are the metals, transition metals, metalloids and non-metals located on the periodic table? _____________________________________________________________________________________ 31. What are the properties of metals? ________________________________________________________ 32. What are the properties of metalloids? ____________________________________________________ 33. What are the properties of non-metals? ____________________________________________________ 34. Define “shielding” ______________________________________________________________________ How does shielding change as you move across a row on the periodic table? ______________________ How does shielding change as you move down a column on the periodic table? ____________________ 35. Define “nuclear charge” _________________________________________________________________ 36. Define “atomic radius” ___________________________________________________________________ How does atomic radius change as you move across a row on the periodic table? __________________ Why? ______________________________________________________________________________ How does atomic radius change as you move down a column on the periodic table? ________________ Why?______________________________________________________________________________ 37. Define “Ionization energy”_______________________________________________________________ How does Ionization energy change as you move across a row on the periodic table? _______________ Why? ______________________________________________________________________________ How does Ionization energy change as you move down a column on the periodic table? _____________ Why?______________________________________________________________________________ 38. Define “Electronegativity” ________________________________________________________________ How does Electronegativity change as you move across a row on the periodic table? _______________ Why? ______________________________________________________________________________ How does Electronegativity change as you move down a column on the periodic table? _____________ Why?______________________________________________________________________________ 39. Define “Reactivity” _____________________________________________________________________ What is the most reactive metal? __________ Why? _______________________________________ What is the most reactive non-metal? ______ Why? _______________________________________ 40. What are the 2 conclusions Rutherford made about the structure of the atom after his Gold Foil Experiment? ___________________________________________________________________________ ______________________________________________________________________________________ 41. What is the mass of the atom? ____________ How many protons does it have? _____ How many neutrons does it have? ______ How many electrons does it have? ____ How would the symbol change if this atom gained an electron? Unit 3 Nomenclature (“The Language of Chemistry”): 42. What is the difference between an element and a compound? __________________________________ 43. Define “valence electron” ________________________________________________________________ How do you determine how many valence electrons an atom has? _______________________________ 44. Complete the table about bonding. What elements are involved? How are their valence electrons interacting? Naming Rules Formula Writing Rules Ionic Bonding Covalent Bonding 45. Complete the table about formula writing: Ionic or Covalent? Chemical Name Chemical Formula Iron (III) chloride Lead (IV) oxide Dinitrogen tetraoxide 43.Complete the table about naming: Ionic or Covalent? Chemical Name Chemical Formula Pb(NO3)2 P2 O5 CaCl2 46. List the number of atoms of each element in the compound: (NH4)3PO4 47. List the number of elements in the compound: (NH4)3PO4 ______ ________ Unit 4: Chemical Mole 48. Define “Molar Mass” ____________________________________________________________________ How do you determine the molar mass? ____________________________________________________ 49. Complete the following Mole Conversion Fact: 1 mole of C2H5 = ______________ grams 1 mole of C2H5 = 6.02 x 10 23 _____________________(molecules or atoms) *pick the correct unit!! 1 molecule of C2H5 = _______________ atoms 50. Complete the following Mole Conversion Fact: 1 mole of C = ______________ grams 1 mole of C = 6.02 x 10 23 _____________________(molecules or atoms) *pick the correct unit!! 51. Calculate the molar mass of: (NH4)2CO3 52. Calculate the number of moles in 96.0 g of Carbon. 53. How many grams are there in 0.00150 moles (NH4)2CO3? 54. A 4.07 gram sample of C2H5 contains how many C2H5 molecules? 55. You have 1 mole of zinc and 1 mole of copper. Which one represents the most mass? 56. You have 1 mole of zinc and 1 mole of copper. Which one represents the most particles? Unit 5: Chemical Reactions: 57. Define “endothermic” ___________________________________________________________________ 58. Define “exothermic” ____________________________________________________________________ 59. Define “activation energy” _______________________________________________________________ 60. Define “catalyst” _______________________________________________________________________ Concepts: 61. Define “Law of Conservation of Mass” ______________________________________________________ 62. Label the Energy Graph A _________________________________________ B _________________________________________ C _________________________________________ D _________________________________________ How will the curve change if you use a catalyst? Draw a new line. Does this graph illustrate an endothermic or endothermic reaction? How will the curve change if this was the other –thermic reaction? Draw a new line. 63. What are the 4 signs that a chemical reaction occurred? _______________________________________ ______________________________________________________________________________________ 64. Identify AND Balance: __________ _____Al + _____CuCl2 _____AlCl3 + _____Cu 65. Identify AND Balance: __________ _____Na + _____Cl2 _____NaCl 66. Identify AND Balance: __________ _____C4H10 + _____O2 _____CO2 + _____H2O 67. Identify AND Balance: __________ _____Fe2O3 _____Fe + _____O2 68. Identify AND Balance: __________ _____MgCl2 + _____ZnO _____MgO + _____ ZnCl2 69. When is a Double Replacement reaction successful? __________________________________________ What tool can help you determine this? _____________________________________________________ 70. When is a Single Replacement reaction successful? ___________________________________________ What tool can help you determine this? _____________________________________________________ For each of the following: A. Identify the type of reaction B. Determine if the reaction will be successful or not. C. If successful, write the formulas for reactants and products (leave a blank line for balancing) D. Balance 71. Type of Reaction _______________ _______ C3H8 + ______ O2 72. Type of Reaction _______________ _____ Mg + ______ HCl 73. Type of Reaction _______________ ______ MgCl2 + ________ Ba(OH)2 74. Type of Reaction _______________ _____ AlCl3 + _____ H3PO4 75. Type of Reaction _______________ _____ CuCl2 + _____ Zn Unit 6 Stoichiometry: 76. Define “limiting reactants” _______________________________________________________________ How do you determine the limiting reactant for a chemical reaction? ____________________________ 77. Define “ percent yield” ___________________________________________________________________ What is the formula for percent yield? ______________________________________________________ 78. What do the coefficients in chemical equation represent? ______________________________________ 79. Balance the reaction and use it to answer the rest of the questions. ____ H2O + ____ Mg3N2 → ____ Mg(OH)2 + ____ NH3 80. How many moles of Mg3N2 are needed to react with 15.2 moles of H2O? 81. If 10.5 grams of Mg3N2 are reacted, how many grams of Mg(OH)2 will be formed? 82. In lab, 10.5 grams of Mg3N2 react with enough water to form 1.8 grams of NH3. What is the % yield of NH3 in this lab? 83. If 15 moles of H20 and 4 moles of Mg3N2 are reacted together, how many moles of NH3 will be formed? Which is the limiting reactant?
