NAME ____________________________________________________ © Keeney-Kennicutt, 2005 A1 CHEMISTRY 101 SPRING 2005 FINAL FORM A SECTIONS 501-511 DR. KEENEY-KENNICUTT Directions: (1) Put your name and signature on PART 1 and 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 one answer down for one question and the other answer down for the other question. If you get one correct you'll get half credit for 2.5 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 everything in the envelope and wait to be excused. At the table, take everything out of the envelope. You can pick up the multiple choice part with the answers outside my office after the exam. (6) There are a total of 59 questions (32 actual questions). PART 1 1&2. The oxidation state of phosphorus in NaHPO3 is _______. (a) +1 (b) +3 (c) +4 (d) 0 (e) -3 3&4. The following ground state atomic configuration: 1s2 2s2 2p6 3s2 3p6 3d10 4s1 corresponds to (a) Cu (b) Cr (c) K (d) Zn (e) Ca 5&6. A sample of CH4 gas behaves most ideally at: (a) 0oC and 1 atm (b) 100oC and 1 atm (c) 0oC and 10 atm (d) 100oC and 10 atm (e) 0oC and 5 atm 7&8. The substance H2O(s) would be classified as a(n) _____________ solid. (a) amorphous (b) covalent (network) (c) ionic (d) metallic (e) molecular© Keeney-Kennicutt, 2005 A2 9&10. An appropriate set of 4 quantum numbers for the "last" electron to go into an atom of platinum (Pt, atomic number 78) could be: n l ml ms (a) 5 3 -3 +1/2 (b) 4 3 0 -1/2 (c) 5 2 2 +1/2 (d) 4 2 -2 -1/2 (e) 5 1 0 -1/2 11&12. Which of the following statements is FALSE concerning the compound Fe(NO3)3? (a) Each formula unit of Fe(NO3)3 contains 9 atoms of oxygen. (b) Each mole of Fe(NO3)3 contains 55.85 g of iron. (c) Each formula unit of Fe(NO3)3 contains 3 nitrate ions. (d) Each mole of Fe(NO3)3 contains 4 moles of ions. (e) Each mole of Fe(NO3)3 contains 6.02 x 1023 atoms of nitrogen. 13&14. A hypothetical molecule, AB3, has two (2) lone pairs of electrons on the center atom, A. The hybridization of A is _______ . (a) sp (b) sp2 (c) sp3 (d) sp3d (e) sp3d2 15&16. Which of the following substances is INSOLUBLE? (a) HNO3 (b) H2S (c) Ba3(PO4)2 (d) Ba(OH)2 (e) all are soluble 17&18. The correct dot structure for SF4 contains ______ lone pair(s) of electrons around the central atom. (a) 0 (b) 1 (c) 2 (d) 3 (e) 4© Keeney-Kennicutt, 2005 A3 19&20. Valence Bond Theory uses the concept of resonance to explain the structure of _______. (a) CH4 (b) SO42- (c) CO32- (d) H2O (e) PO43- 21&22. According to Bronsted-Lowry Theory, which acid is INCORRECTLY matched with its conjugate base? ACID CONJUGATE BASE (a) HCl Cl- (b) H2F+ HF (c) HCO3- CO32- (d) H3O+ OH- (e) H2PO4- HPO42- 23&24. The number of π bonds in a molecule of benzene is: (a) 0 (b) 1 (c) 2 (d) 3 (e) more than 3 25&26. Which of the following species is INCORRECTLY paired with its molecular or ionic geometry? (a) CO2 linear (b) SO2 linear (c) SO3 trigonal planar (d) SO32- pyramidal (e) AsF5 trigonal bipyramidal 27&28. Which statement is WRONG? (a) A carbon atom is smaller than a silicon atom. (b) The most stable calcium ion is Ca2+. (c) A magnesium cation is smaller than a magnesium atom. (d) The atomic weight of oxygen is about 16. (e) Oxygen has a less negative electron affinity than nitrogen.© Keeney-Kennicutt, 2005 A4 29&30. The correct ranking of substances according to their boiling points from lowest boiling point to highest boiling point is: (a) He < CH4 < NH3 < NaCl (b) He < NH3 < CH4 < NaCl (c) He < CH4 < NaCl < NH3 (d) CH4 < He < NH3 < NaCl (e) NaCl < He < CH4 < NH3 31&32. A species having 28 electrons and 30 protons could be: (a) Ni2+ (b) Zn2+ (c) Ni2- (d) Zn2- (e) something else 33&34. Which of the following species is polar? (a) BeF2 (b) CF4 (c) CF3- (d) PF4+ (e) SF6 35&36. What is the percent of oxygen by mass in vanillin, C8H8O3? (a) 31.5% (b) 19.2% (c) 15.8% (d) 25.8% (e) 10.5%© Keeney-Kennicutt, 2005 A5 37&38. Consider the reaction: H2(g) + O2(g) → H2O(g) UNBALANCED The initial system before the reaction began is represented by the following particle view: where is a hydrogen atom is an oxygen atom is a water molecule Give the limiting reactant and the number of molecules of H2O that can be produced. (a) H2, 1 (b) H2, 2 (c) O2, 1 (d) O2, 2 (e) another answer 39&40. How many grams of Na2O2 (FW - 78.0 g/mol) can be produced from the reaction of 10.0 g of sodium metal with excess oxygen gas if the percent yield of the reaction is only 55%? 2 Na + O2 → Na2O2 (a) 5.8 g (b) 12.2 g (c) 8.6 g (d) 6.8 g (e) 9.3 g© Keeney-Kennicutt, 2005 A6 41&42. Air bags for automobiles are inflated during a collision by the explosion of sodium azide, NaN3 (FW = 65.0 g/mol). The equation for the decomposition is: 2NaN3(s) → 2Na(s) + 3N2(g) What mass of sodium azide is needed to inflate a 25.0 L bag to a pressure of 1.40 atm at 20oC? (a) 14.4 g (b) 88.1 g (c) 93.1 g (d) 63.1 g (e) 155 g 43&44. What volume (in mL) of 0.45 M NaBr can be prepared from 25 g of NaBr (FW = 103 g/mol)? (a) 320 mL (b) 480 mL (c) 610 mL (d) 540 mL (e) 270 mL© Keeney-Kennicutt, 2005 A7 45&46. You are given the data for all the isotopes of the newly discovered element, Aggiedaddium: Abundance (%) Isotopic Mass (amu) 10.00 122.00 50.00 125.00 40.00 128.00 The atomic weight of Aggiedaddium (in amu) is (to 4 significant figures): (a) 125.9 (b) 125.0 (c) 125.6 (d) 124.7 (e) 126.0 47&48. A student must prepare a 0.100 N solution of KMnO4 which will be used in this UNBALANCED net ionic reaction occurring in acidic solution: MnO4- + Fe2+ → Mn2+ + Fe3+ How many grams of KMnO4 must be used to make 1000 mL of this 0.100 N solution? (a) 3.16 g (b)
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