NAME (Please print )__________________________________________________ © Keeney-Kennicutt, 2010 A1 CHEMISTRY 101 SPRING 2010 FINAL FORM A DR. KEENEY-KENNICUTT Directions: (1) Put your name on PART 1 and your name and signature on PART 2 of the exam where indicated. (2) Sign the Aggie Code on PART 2 of this exam. (3) Each multiple choice question is actually 2 questions on your scanning sheet. If you are sure of an answer, put the same answer down for both questions for 5 pts. If you cannot decide between two answers, put your BEST answer down for the ODD/FIRST question for 3 pts and your SECOND BEST answer down for the EVEN/SECOND question for 2 pts. If there is an ambiguous multiple choice question, use the last page to explain your answer. (4) Do NOT write on the envelope. (5) When finished, put both parts of the exam in the envelope with the scanning sheet. You can leave during announced times. (6) There are a total of 64 questions (34 actual questions with 2 pts extra credit). Total value is 170 + 2 points. PART 1 1&2. Which of the following is a non-polar covalent bond? (a) Te-I (b) H-Cl (c) O-S (d) Na-Ca (e) P-As 3&4. Titanium (Ti) conducts electricity as a solid. It melts at 1675oC to give a liquid that also conducts electricity. Solid Ti can probably be classified as a ___________ solid. (a) ionic (b) metallic (c) polar (d) molecular (e) covalent 5&6. The correct Lewis dot structure of BeF2 uses a total of _________ valence electrons. (a) 2 (b) 4 (c) 8 (d) 16 (e) 24 7&8. Which element is paramagnetic with 2 unpaired electrons? (a) Mg (b) F (c) B (d) O (e) Be 9&10. In Bronsted-Lowry Theory of acids and bases, a base is defined as: (a) a proton donor (b) a hydroxide donor (c) an electron-pair acceptor© Keeney-Kennicutt, 2010 A2 (d) a water-former (e) a proton acceptor 11&12. One formula unit of K2SO4 contains: (a) 2 ions of K+ (b) 1 mole of K2SO4 (c) 32 g of S (d) 4 moles of SO42- anions (e) Avogadro's number of sulfur atoms 13&14. Which of the following statements is/are true about 56Fe3+? (1) this ion has 29 electrons (2) this ion has 26 neutrons (3) this ion has 26 protons (a) 1 only (b) 1 and 3 only (c) 1 and 2 only (d) 2 and 3 only (e) 3 only 15&16. Which ground state electronic configuration is NOT correct? (a) Po [Xe] 6s2 5d10 6p4 (b) Ni [Ar] 3d8 4s2 (c) Cr [Ar] 3d5 4s1 (d) Mg 1s2 2s2 2p6 3s2 (e) As [Ar] 3d10 4s2 4p3 17&18. Consider the diagram when choosing the CORRECT statement from the following: (a) The vapor pressure is always equal to the atmospheric barometric pressure. (b) Compound A’s vapor pressure is independent of the temperature. (c) The boiling point of Compound A is always equal to or greater than about 56oC. (d) At the top of a very high mountain, the boiling point is about 56oC. (e) In a closed container, the vapor is in equilibrium with the liquid. 19&20. The ionic geometry of SF3− is: (a) trigonal pyramidal (b) trigonal planar (c) trigonal bipyramidal© Keeney-Kennicutt, 2010 A3 (d) T-shaped (e) see-saw 21&22. In the following drawing, the white spheres represent cations and the black spheres represent anions. The following drawing of an ionic compound is a representation of which compound? (a) Ba(ClO3)2 (b) (NH4)2CO3 (c) NaBr (d) AlBr3 (e) Ca3(PO4)2 23&24. Consider this acid-base net ionic equation: 2H+(aq) + Ni(OH)2(s) Æ Ni2+(aq) + 2H2O(l) Which of the following statements is TRUE? (a) The acid is a weak acid. (b) The base is a weak electrolyte. (c) The spectator ion could have been a NO3– ion. (d) The salt is insoluble. (e) The reaction is called a precipitation reaction. 25&26. Determine the oxidation number of sulfur in the sulfate ion, SO42−. (a) +2 (b) +4 (c) +6 (d) +7 (e) +8 27&28.The following set of 4 quantum numbers: n = 5, l = 2, ml = +2, ms = +1/2 could be an appropriate set for the last electron to go into an atom of: (Assume that the element is not an exception to the normal filling rule.) (a) Zr (b) Kr (c) Sr (d) Sn (e) W 29&30. Which one of the following statements about this phase diagram is FALSE? (a) At Point 4, the substance is a gas. (b) Point 5 is called the triple point. (c) At Point 3, the liquid phase is in equilibrium with gas phase. (d) When the substance moves from the conditions at Point 2 to the conditions at Point 4, the substance sublimes. (e) When the conditions change from Point 1 to Point 3, the temperature changes and the pressure stays constant.© Keeney-Kennicutt, 2010 A4 31&32. Give the ions present and their numbers that appear in the correct formula for copper(II) carbonate. (a) 2 Cu2+ and 1 CO32- (b) 2 Cu2+ and 2 CO32- (c) 2 Cu2+ and 3 CO32- (d) 1 Cu2+ and 1 CO32- (e) 1 Cu3+ and 2 CO32- 33&34. Balance the equation with the SMALLEST WHOLE NUMBER COEFFICIENTS possible. Choose the number that is the SUM of the coefficients in the balanced equation. Don’t forget coefficients of one. Na2SO3 + HCl Æ NaCl + H2O + SO2 (a) 5 (b) 7 (c) 9 (d) 12 (e) 15 35&36. Which one of the following statements about gases is FALSE? (a) Gases consist of large numbers of particles in rapid random motion. (b) The volume of the molecules of a gas is very small compared to the total volume in which the gas is contained. (c) The average kinetic energy of the molecules is proportional to the absolute temperature. (d) The average kinetic energies of ideal gases are different at different temperatures. (e) The attractive forces between the molecules of a gas become significant only at high temperatures and low pressures. 37&38. The formula weight of Mg3(PO4)2 is: (a) 168 amu (b) 239 amu (c) 358 amu (d) 214 amu (e) 263 amu© Keeney-Kennicutt, 2010 A5© Keeney-Kennicutt, 2010 A6 39&40. If a system gains 20 J of heat and does 30 J of work on the surroundings, the change in internal energy is (a) −50 J (b) +50 J (c) −10 J (d) +10 J (e) 0 J 41&42. If the pH of a solution is 2.11, what is the molarity of H+ ions in the solution? (a) 7.8 x 10−3 M (b) 0.75 M (c) 0.32 M (d) 0.12 M (e) 2.11 M 43&44. An oxide of iron contains 72.36% Fe by mass. The empirical formula is: (a) FeO (b) Fe3O4 (c) Fe2O3 (d) FeO2 (e) Fe3O2© Keeney-Kennicutt, 2010 A7
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