UNIT 1: Matter & Lab Safety

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1 Directions: Complete all of the following questions. Turn this in on the day of your final and you can earn up to 10 bonus points on your final. You must correctly answer every questions in order to receive the bonus points. All answer must be hand written and you MUST show ALL work. UNIT 1: Matter & Lab Safety 1. Study the lab safety rules. 2. Know what the following glass wear is and what it is used for: beaker, graduated cylinder, watch plate, evaporating dish, Erlenmeyer flask. 3. Describe the proper way to smell an unknown chemical in lab. 4. What is chemistry? 5. What is qualitative data? 6. What is quantitative data? 7. What are the SI base units for mass, length, and volume? 8. How does one determine the number of significant digits in a number? 9. How many sig figs are in each of the following? a d b e c f What is precision? 11. What is accuracy? 12. Convert the following using dimensional analysis: a. 5000cm km c ml DL b cg g d dm Dm 13. Convert the following using dimensional analysis: a ft into miles b. 37 hours into days c cm into inches 14. What is a physical property? 15. Give 4 examples of physical properties. 16. What is a chemical property? 17. Give 3 examples of chemical properties. 18. What is a physical change? 19. How do you know if a physical change has occurred? 20. What is a chemical change? 21. How do you know if a chemical change has occurred? 22. Label the following as chemical or physical change. a. Silver tarnishing b. Ice melting c. Evaporating water from a salt water solution d. Burning e. Rusting f. Cutting 23. What are the six phase changes of matter? 24. Define each phase change of matter. 25. Define temperature. 1

2 26. Define element. 27. Define compound. 28. Define mixture. 29. Label each of the following as element, compound, or mixture: a. Water f. salad dressing b. Liquid bromine h. carbon dioxide c. Carbon i. Kool-Aid d. Salt water j. Gatorade 30. What is the difference between a compound and a mixture? 31. What is the formula for density? 32. What are the units of density? UNIT 2: Atomic Theory 33. What are all the parts Dalton s atomic theory? 34. What did Aristotle contribute to the atomic theory? 35. What did Chadwick discover? 36. What did Bohr discover? 37. What did Democritus do? 38. What did Rutherford discover? 39. How did Rutherford discover #41? 40. What did Thomson discover? 41. How did Thomson discover #43? 42. What is the law of definite proportions? 43. What are vertical columns called on the periodic table? 44. What are rows called on the periodic table? 45. What is an isotope? 46. What do isotopes have in common? 47. How do isotopes of the same element differ? 48. How do you find the mass number? 49. How do you find the number of neutrons? 50. How do you determine the number of protons? 51. How do you determine the number of electrons? 52. What determines an element s identity? 53. What determines an element s behavior? 54. What have more in common: elements in the same period or elements in the same family? 55. What are the sub atomic particles of an atom? 56. What is the charge on each sub atomic particle in an atom? 57. Where is each sub atomic particle in the atom? 58. How many protons, neutrons, and electrons are in C -4? 59. How many protons are present in a titanium atom with a mass of 48 g/mol? 60. Where are the metals, non-metals and metalloids on the periodic table? 61. What are valance electrons? 62. How many valance electrons does each family on the periodic table contain? 63. What is a nuclear symbol? 64. How many protons, neutrons, and electrons are in the following? 2

3 UNIT 3: The Periodic Table 65. Be able to label the following on a periodic table: Families/groups, periods, alkali metals, alkaline earth metals, transition metals, halogens, noble gases, lanthanides, actinides, inner transition metals, metals, non-metals, metalloids, charges of families, valence electrons of families, elements that are liquid at room temperature, elements that are gases at room temperature 66. Write the long hand electron configuration, short hand electron configuration, and the orbital diagram for the following: a. Magnesium d. Phosphorous b. Selenium e. Xenon c. Calcium f. Oxygen 67. List the 7 diatomic molecules. 68. What element ends in 3p 3? 69. What element ends in 6s 1? 70. How many valance electrons are in the p orbital of Kr? 71. How many valance electrons are in the s orbital of Rb? 72. List the electron configuration/noble gas configuration/orbital notation for the following elements: Mg, Ca, F, Se, Si, P, S, As 73. What is group 1? What are some characteristics of group 1? 74. What is the possible charge of group 1? 75. What is group 2? What are some characteristics of group 2? 76. What is the charge on group 2? 77. What are groups 3-12 called? And what are some characteristics of these groups? 78. What is group 17 group 7A? What are some characteristics of group 7A? 79. What is the charge on group 17? 80. What is group 18/group 8A? What are some characteristics of group 8A? 81. What are the two sections at the bottom of the periodic table called? 82. Where are the radioactive elements located on the periodic table? 83. What is a cation? 84. What is an anion? 85. What is atomic radius? 86. What are the group and periodic trends of atomic radius? 87. What is ionization energy? 88. What are the group and periodic trends of ionization energy? 89. What is electronegativity? 90. What are the group and periodic trends of electronegativity? 91. What element has the highest electronegativity? 92. What are metalloids? 93. What is the law of conservation of mass? UNIT 4: Bonding and Nomenclature 94. What are ionic compounds composed of? 95. What are covalent molecules composed of? 96. What are acids composed of? 3

4 97. How are ionic bonds formed? 98. How are covalent bonds formed? 99. What are properties of ionic compounds? 100. What are properties of covalent compounds? 101. How do you name ionic compounds? 102. When do you use roman numerals and what do the roman numerals represent? 103. How do you name covalent compounds? 104. What are the 8 prefixes? 105. What do the prefixes in the name represent? 106. What is a lewis structure? 107. How do you draw a lewis structure? 108. What is a single bond? 109. What is a double bond? 110. What is a triple bond? 111. Be able to draw Lewis structures What is a binary acid? 113. What is a ternary acid? 114. What is the difference among a nonpolar and polar bond? 115. How many oxygen atoms are in aluminum hydroxide? 116. How many iron atoms are in Iron (II) sulfate? 117. What is the formula for hydrofluoric acid? 118. What is the formula for chloric acid? 119. What is the formula for perchloric acid? 120. How many lead atoms are in Lead (IV) Sulfate? 121. How many lone pairs on the central atom of Carbon tetrahydride Draw the Lewis structure of nitrogen trifluoride? 123. Draw the Lewis structure of water Be able to calculate molar mass What are the units of molar mass? UNIT 5: Chemical Reactions 126. What is a reactant? 127. What is a product? 128. What is the law of conservation of mass? 129. Why do we balance equations? 130. What is evidence of a chemical change? 131. What are the 5 reaction types and describe each? 132. What are the requirements for each type? 133. What type can be predicted using the activity series? 134. What does soluble mean? 135. What does insoluble mean? 136. What is aqueous? 137. What is a precipitate? 4

5 PROBLEMS: Fill in the chart: Nuclear Symbol Mass Number Atomic Number # Protons # Neutrons # Electrons Ni H Give the number of significant figures: 142) ) ) ) ) ) ) ) Express your answer to the following with the appropriate number of significant figures: 150) 2.21 x 0.3= 151) = 152) 2.90 x x 920= Convert the following: 155) 34 m = cm 156) 0.15 mg = g 157) L = ml 158) 1286 m = km Place the following in scientific notation: 163) ) ) Place the following in standard form: 169) 4.3 x ) 2.5 x ) 1.2 x 10-4 Perform the following calculations: 175) ( 1.10 x 10 3 ) ( x 10 6 ) 176) ( x 10 6 ) (1.81 x 10 9 ) 177) (6.30 x 10 8 ) ( 2.50 x 10 3 ) 178) ( 7.64 x 10 6 ) (1.343 x 10 8 ) 153) 2.02 x = 154) (72) (4.022) = ) 72 cm = m 160) 948 mm = cm 161) 32 Dm = m 162) 87 km = Hm 166) ) ) ) 6.2 x ) 4.4 x ) 1.3 x

6 Density: D=m/V 179) Given that the density of iron is g/cm 3, what would be the volume of a 5.7 gram piece of iron? 180) What is the density of g of water whose volume is 6.80 cm 3? 181) The density of Aluminum is 2.70 g/cm 3. The volume of a solid piece of Al is 1.50 cm 3. What is the mass of this piece? Trends: Circle the element described 182) N P As smallest ionization energy 183) O C N highest ionization energy 184) Al Si P most electronegative 185) Cl Br I least electronegative 186) Na K Li largest atomic radius 187) Na Mg Al smallest atomic radius Bonding and Nomenclature: Write the chemical formula and compound name for the following: 188) Ca and NO 3 193) V 3+ and CrO 4 198) Al and OH 203) Pb 2+ and C 2H 3O 2 189) Ca and PO 4 194) K and ClO 3 199) Fe 2+ and ClO 3 204) NH 4 and C 2O 4 190) K and SO 4 195) Sn 4+ and OH 200)Cu + and SO 4 205) Na and PO 4 191) Ba and NO 3 196) Mg and NO 3 201) K and MnO 4 206) Cr 3+ and NO 3 192) Al and SO 4 197)NH 4 and SO 4 202) Sn 2+ and PO 4 207) Pb 4+ and SO 4 Name the following molecules AND calculate their molar mass: 208) CO 2 209) CCl 4 210) PCl 5 211) SeF 6 212) As 2O 5 213) SO 3 214) ICl 3 215) PBr 5 Write the formula for the following compounds: 216) carbon tetrabromide 217) silicon dioxide 218) tetraphosphorus decoxide 219) diarsenic trisulfide 220) sulfur trioxide 221) diphosphorus pentoxide 222) dinitrogen trioxide Determine what type of bond will exist between the following pairs of atoms (Ionic, Covalent, Acid): 223) H and I 226) S and O 229) K and Br 230) Ca and Cl 224) Se and S 227) C and H 231) I and Br 225) Li and F 228) Cu and S Draw the Lewis structure and predict the polarity for the following molecules: 232) CI 4 233) BCl 3 234) Cl 2O 235) PI 3 6

7 Write the formula for the following acids: 236) Carbonic acid 237) Chlorous acid 238) Iodic acid 239) Hydrobromic acid Write the correct name for the following acids: 244) HBr 245) H 2SO 4 246) HClO 2 247) H 2S 240) Arsenic acid 241) Hydrofluoric acid 242) Sulfurous acid 243) Hypochlorous acid 248) H 2CO 3 249) HCl 250) H 2SO 3 Name the following compounds AND circle the ones that are soluble in water 251) AgCl 255) Sr3(PO4)2 252) Na2SO4 256) K2SO4 253) NH4NO3 257) FeBr3 254) Al(ClO4)3 258) NaCl Using the activity series, determine if the following reactions will occur. If they do, you must balance. 259) Na + AlBr 3 NaBr + Al 260) Li + CuSO 4 Li 2SO 4 + Cu 261) Al + CuSO 4 Al 2(SO 4) 3 + Cu 262) Mg + LiNO 3 Mg(NO 3) 2 + Li Balance AND identify the following reactions: 263) Mg + Zn(NO 3) 2 Zn + Mg(NO 3) 2 264) Mg + AgNO 3 Ag + Mg(NO 3) 2 265) NH 3 N 2 + H 2 266) MgO Mg + O 2 267) K + Cl 2 KCl 268) Al + O 2 Al 2O 3 269) HI H 2 + I 2 270) C 2H 6 + O 2 CO 2 + H 2O 271) Li 2S + AlP Al 2S 3 + Li 3P 272) K 2S + PbO 2 K 2O + PbS 2 273) Al + CuSO 4 Al 2(SO 4) 3 + Cu 274) Pb(NO 3) 2 + NaI PbI 2 + NaNO 3 7

8 Activity Series Halogens Activity Series Metal Activity Series F Fluorine Li Lithium K Potassium Na Sodium Ca Calcium Mg Magnesium Cl Chlorine Al Aluminum C Carbon Zn Zinc Fe Iron Br Bromine Sn Tin Pb Lead H Hydrogen Cu Copper I Iodine Ag Silver Au Gold Pt Platinum 8

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