Chemistry Name Date Period 1. Define matter. Final Exam Review Properties of Matter 2. Classify the following as chemical or physical changes. a. Burning paper d. Boiling water b. Chopping wood e. Iron rusting c. Dissolving sugar f. Cooking food 3. Classify the following as an element, compound. a. BaCl 2 d. Ga e. FeO f. Rn 4. a. Define Density & write its formula. b. A solid has a volume of 276.5cm 3 & a mass of 405.7g. Will the solid float on water? Why or why not? Directions: Identify the letter of the choice that best completes the statement or answers the question. 5. Matter includes all of the following EXCEPT a. air. c. smoke. b. light. d. water vapor. 6. A physical property may be investigated by a. melting ice. c. allowing silver to tarnish. b. letting milk turn sour. d. burning wood. 7. Chemical properties a. include changes of state of a substance. b. include mass and color. c. include changes that alter the identity of a substance. d. can be observed without altering the identity of a substance.
8. Two features that distinguish matter are a. mass and velocity. c. mass and volume. b. weight and velocity. d. weight and volume. 9. One chemical property of matter is a. boiling point. c. reactivity. b. texture. d. density. 10. Which of the following is an intensive physical property? a. volume c. color b. length d. mass 11. An example of a chemical change is a. sanding wood. c. milk going sour. b. melting ice. d. vaporizing gasoline. 12. A physical change occurs when a a. peach spoils. c. bracelet turns your wrist green. b. copper bowl tarnishes. d. glue gun melts a glue stick. 13. The state of matter in which a material has neither a definite shape nor a definite volume is the a. gaseous state. c. elemental state. b. liquid state. d. solid state. 14. A list of pure substances could include a. bread dough. c. vitamin C (ascorbic acid). b. vinegar (5% acetic acid). d. sea water. The Atom Identifying Properties of Atoms 15. Directions: Complete the following table. Atom or Ion # of Protons # of Electrons # of Neutrons Atomic Number Na +2 11 12 Mass Number S -2 18 32 Ne 10 20 16. Who was the schoolmaster who studied chemistry and proposed an atomic theory? a. John Dalton c. Robert Brown b. Jons Berzelius d. Dmitri Mendeleev 17. Experiments with cathode rays led to the discovery of the a. proton. c. neutron. b. nucleus. d. electron. 18. Who discovered the nucleus by bombarding gold foil with positively charged particles and noting that some particles were widely deflected? a. Rutherford c. Chadwick b. Dalton d. Bohr 19. Rutherford's experiments led to the discovery of the a. electron. c. nucleus. b. cathode ray. d. neutron.
20. An atom is electrically neutral because a. neutrons balance the protons and electrons. b. nuclear forces stabilize the charges. c. the numbers of protons and electrons are equal. d. the numbers of protons and neutrons are equal. 21. Most of the volume of an atom is occupied by the a. nucleus. c. electron cloud. b. nuclides. d. protons. 22. Isotopes of an element contain different numbers of a. electrons. c. neutrons. b. protons. d. nuclides. Electron Configurations 23. Electron Configurations Directions: Using the LONG version, write out the ground state electron configuration for the following species. a. Mg b. S c. Th 24. Directions: Using NOBLE GAS notation, write out the ground state electron configuration for the following species. a. Ba b. Ar c. U Directions: Answer the following question or complete the following statements. 25. Define valence electrons? 26. The maximum amount of valence electrons an atom can have is, this is called an of electrons. 27. Why do all atoms want to obtain 8 valence electrons? 28. What two atoms do NOT want 8 valence electrons?
29. How many valence electrons do the following atoms have? a. N b. Br c. K Directions: Identify the letter of the choice that best completes the statement or answers the question. 30. For an electron in an atom to change from the ground state to an excited state, a. energy must be released. b. energy must be absorbed. c. radiation must be emitted. d. the electron must make a transition from a higher to a lower energy level. 31. If electrons in an atom have the lowest possible energies, the atom is in the a. ground state. c. excited state. b. inert state. d. radiation-emitting state. 32. The statement that an electron occupies the lowest available energy orbital is a. Hund's rule. c. Bohr's law. b. the Aufbau principle. d. the Pauli exclusion principle. 33. "Orbitals of equal energy are each occupied by one electron before any is occupied by a second electron, and all electrons in singly occupied orbitals must have the same spin" is a statement of a. the Pauli exclusion principle. c. the quantum effect. b. the Aufbau principle. d. Hund's rule. 34. The statement that no two electrons in the same atom can have the same four quantum numbers is a. the Pauli exclusion principle. c. Bohr's law. b. Hund's rule. d. the Aufbau principle. 35. If the s and p sublevels of the highest main energy level of an atom are filled, how many electrons are in the main energy level? a. 2 c. 16 b. 8 d. 32 36. If an element has an octet of electrons in its highest main energy level, there are electrons in this level. a. 2 c. 10 b. 8 d. 32 37. An element with 8 electrons in its highest main energy level is a(n) a. octet element. c. Aufbau element. b. third period element. d. noble gas.
The Periodic Table 38. Directions: Label the following on the periodic table: halogens transition metals noble gases metals alkaline earth metals alkali metals actinides nonmetals lanthanides metalloids 39. According to the modern periodic table, the elements are arranged in periods according to their A. electron configurations B. atomic masses C. atomic numbers D. valence electrons 40. The most reactive metal is A. Fr B. Ca C. F D. Li 41. A group on the periodic table is the same as a(n) A. period B. row C. family D. line 42. Hydrogen is placed separately from the other elements on the periodic table because A. it is a gas B. it has 1 electron C. it has unique properties D. it is colorless 43. The most reactive nonmetal is A. Ne B. O C. Fr D. F Directions: Circle the atom with the LARGEST electronegativity. 44. Li K Na 45. O C N 46. List the steps for drawing Lewis structures.
47. What is the shape of a water molecule? a. Linear c. Tetrahedral b. Bent d. Trigonal Pyramidal 48. What is the shape of a hydrogen molecule? a. Linear c. Tetrahedral b. Bent d. Trigonal pyramidal 49. What is the shape of an ammonia molecule (NH 3 )? a. Linear c. Tetrahedral b. Bent d. Trigonal pyramidal 50. What is the shape of a methane molecule (CH 4 )? a. Linear c. Tetrahedral b. Bent d. Trigonal pyramidal Polarity 51. The chemical bond formed when two atoms share electrons is called a(n) a. ionic bond. c. Lewis structure. b. orbital bond. d. covalent bond. 52. If two covalently bonded atoms are identical, the bond is a. nonpolar covalent. c. nonionic. b. polar covalent. d. coordinate covalent. 53. If the atoms that share electrons have an unequal attraction for the electrons, the bond is called a. nonpolar. c. ionic. b. polar. d. dipolar. 54. In which of these compounds is the bond between the atoms NOT a nonpolar covalent bond? a. Cl 2 c. HCl b. H 2 d. O 2 `55. If electrons are transferred between two atoms, the resulting bond is a. nonpolar. c. ionic. b. polar. d. dipolar. 56. If the difference in electronegativity values of two atoms are 0.3, the bond would be. a. nonpolar. c. ionic. b. polar. 57. (Polar / Nonpolar) molecules are will dissolve in water.
Naming and Formula Writing For each of the following, provide either the correct chemical name or chemical formula. 58. cadmium nitrate 59. dinitrogen monoxide 60. potassium bromide 61. nitrous acid 62. PCl 3 63. V 2 O 5 64. HClO 4 65. BaSO 4 66. sulfur hexafluoride 67. sulfuric acid 68. BaO 69. SrSO 3 70. acetic acid 71. CBr 4 72. (NH 4 ) 2 SO 4 6H 2 O 73. calcium hydroxide 74. Na 2 CO 3 75. Cu 3 P 76. HI 77. lead(ii) acetate 78. List 4 types of chemical reactions: Types of Chemical Reactions a. b. c. d. 79. a. A + B AB is an example of a(n) reaction. b. AB A + B is an example of a(n) reaction. c. A + BC AC + B is an example of a(n) reaction. d. AB + CD AD + CB is an example of a(n) reaction.
80. Classify the following reactions. a. 2CuO(s) 2Cu(s) + O 2 b. Ba(s) + 2HCl(aq) H 2 (g) + BaCl 2 (aq) c. Ca(NO 3 ) 2 (aq) + 2NaI(aq) CaI 2 (s) + Na(NO 3 )(aq) 81. What do the following symbols represent in a chemical reaction. (s) = (g) = (l) = (aq)= 82. Balance the following chemical reactions. Balancing Equations a. N 2 + H 2 NH 3 b. Na + H 2 O NaOH + H 2 c. Pb(NO 3 ) 2 (aq) + KI(aq) PbI 2 (s) + KNO 3 (aq) Molar Mass Calculations 83. Directions: Find the molar masses of the following compounds. Compound BaCO 3 Molar Mass (NH 4 ) 2 SO 4 Conversions using Molar Mass Directions: Complete the following molar conversions. Be sure to show your work. 84. How many grams BaCO 3 of are in 6.5moles of BaCO 3? 85. How moles BaCO 3 of are in 76.5g of BaCO 3? 86. How many formula units of BaCO 3 are in 0.536 mols of BaCO 3? 87. How many grams BaCO 3 of are in 3.76 X 10 22 formula units of BaCO 3?
Stoichiometry & Mole Ratios 88. In the reaction Zn + H 2 SO 4 ZnSO 4 + H 2, what is the mole ratio of zinc to sulfuric acid? a. 1:6 c. 1:2 b. 1:1 d. 3:1 89. In the reaction C + 2H 2 CH 4, what is the mole ratio of hydrogen to methane? a. 1:1 c. 1:2 b. 2:1 d. 2:4 90. The Haber process for producing ammonia commercially is represented by the equation N 2 (g) + 3H 2 (g) 2NH 3 (g). To completely convert 9.0 mol hydrogen gas to ammonia gas, how many moles of nitrogen gas are required? a. 1.0 mol c. 3.0 mol b. 2.0 mol d. 6.0 mol 91. In the equation 2KClO 3 2KCl + 3O 2, how many moles of oxygen are produced when 3.0 mol of KclO 3 decompose completely? a. 1.0 mol c. 3.0 mol b. 2.5 mol d. 4.5 mol 92. For the reaction C + 2H 2 CH 4, how many moles of hydrogen are required to produce 10 mol of methane, CH 4? a. 2 mol c. 10 mol b. 4 mol d. 20 mol 93. For the reaction 2Na + 2H 2 O 2NaOH + H 2, how many grams of sodium hydroxide are produced from 3.0 mol of water? a. 40. g c. 120 g b. 80. g d. 240 g 94. For the reaction SO 3 + H 2 O H 2 SO 4, how many grams of sulfur trioxide are required to produce 4.00 mol of sulfuric acid? a. 80.0 g c. 240. g b. 160. g d. 320. g 95. For the reaction HCl + NaOH NaCl + H 2 O, how many moles of hydrochloric acid are required to produce 150. g of water? a. 1.50 mol c. 8.32 mol b. 4.16 mol d. 12.2 mol
96. For the reaction SO 3 + H 2 O H 2 SO 4, how many grams of sulfuric acid can be produced from 200. g of sulfur trioxide and 100. g of water? a. 100. g c. 245 g b. 200. g d. 285 g 97. For the reaction 2Zn + O 2 2ZnO, how many grams of zinc oxide can be produced from 100. g each of zinc and oxygen? a. 100. g c. 189 g b. 124 g d. 200. g Kinetic Molecular Theory 98. Pressure is the result of the of gas molecules with walls of a container or surrounding objects. 99. When gas molecules are at a constant temperature, the speed of the molecules a. gradually increases c. gradually decreases b. remains constant 100. Increasing the volume of a gas causes the pressure to (increase / decrease / remain constant). 101. Decreasing the temperature of a gas causes the volume to (increase / decrease / remain constant). 102. Increasing the pressure of a gas causes the temperature to (increase / decrease/ remain constant). 103. The process by which a gas is able to spread throughout a space is called. 104. The process by which a gas is able to escape through a tiny opening is called. 105. On the graph shown to the right a. where is the kinetic energy increasing? b. where is a change in state occurring? c. where is the substance a liquid? Gas Laws 106. States that the volume of a gas is directly proportional to its Kelvin temperature when pressure & amount are held constant.
107. States that the pressure of a gas is directly proportional to its Kelvin temperature when volume & amount are held constant. 108. States that pressure of a gas is inversely proportional to its volume when temperature & amount are held constant. 109. States that the volume of a gas is directly proportional to its amount when pressure & temperature are held constant. This law also states that 1 mole of any gas at STP contains 6.02 x 10 23 molecules, and occupies a volume of 22.4 Liters 110. Law that combines, Boyle s, Charles, & Gay-Lussac s laws. 111. For each of the following gas laws, tell whether it is an example of a direct or indirect relationship: a. Charles Law c. Gay-Lussac s Law b. Boyle s law d. Avogadro s Law 112. Draw the graph of a direct relationship: Draw the graph of an indirect relationship: 113. List the standard pressure in atmospheres & standard temperature in Kelvin: 114. The molar volume of a gas is at STP. 115. 25 o C = K
Gas Law Problems 116. Using Boyle s Law, calculate the new volume of a gas when its pressure is changed to 530mmHg. The initial pressure & volume of the gas was 250mmHg and 125.mL. 117. Using the Ideal Gas Law, calculate the volume of a 0.200 mol sample of gas at 10.0ºC and a pressure of 2.30 atm. 118. A 5.0 L propane tank on a camping stove contains propane at a pressure of 2.0 atm when the temperature is 14.0 C (in the morning). During the day the tank warms up to a temperature of 34.0 C. What is the pressure of the propane gas inside the tank when the temperature is 34.0 C? Use Gay-Lussac s law to solve. 119. A balloon contains 500 ml of helium at 20 C. To what temperature should you increase the balloon to give a volume of 550 ml? Use Charles Law to solve. 120. Imagine you blow up a balloon at sea level where there is 1 atm of pressure to a volume of 450 ml. On a scuba diving trip, you decide to take the balloon with you. If the pressure of the ocean is 2.5 atm, what is the new volume of the balloon? Use Boyle s law to solve.
121. If 15 liters of helium are collected at 70 0 C, what will the volume of this gas be after it cools to 12 0 C? 122. Argon gas occupies a volume of 300.mL with a pressure of 3.2atm. To what pressure should the gas be raised to bring the volume to 100.mL? 123. A ball has an internal pressure of 1.25 atm and a volume of 3.0 L. If the temperature of the ball is 17 0 C, what will happen to the volume when the ball to taken to an altitude where the pressure is 0.75 atm and the temperature is 10 0 C? 124. Determine the molarity of these solutions: Solutions a.) 0.10 mol of NaCl in 1.0 L of solution b.) 0.50 mol of NaCl in 500. ml of solution c.) 25 grams of NaCl in 250 ml of solution 125. Determine the molality of these solutions: a.) 25 g C 6 H 12 O 6 in 0.25 L water b.) 50 g C 6 H 12 O 6 in 500. ml water