115 Exam II Fa07 - llS—M - Exam 2 (Test 55} - 10/17/07 1....

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Unformatted text preview: llS—M - Exam 2 (Test 55} - 10/17/07 1. Which element has the electron configuration 13232210635231}? (81) Mg (b) S (c) Si (d) Se (e) Ga 2. The X3" ion with the following electron configuration is formed from: [Net (a) oxygen. (b) nitrogen. (c) phosphorus. (d) aluminum. (e) magnesium. The figure is a portion ofa plot of: LJJ Atomic Number (a) Highest principal quantum number vs. atomic number. (b) 1st iouization energy vs. atomic number. (c) Electron affinity vs. atomic number. (d) Atomic radius vs. atomic number. (6) Atomic charge vs atomic number. 4. Place the following atoms in order of INCREASING atomic radii: Ca, Mg, P, and C]. (a) Ca<Cl<P<Mg (b) Mg<P<Cl<Ca (C) Ca<Mg<P<Cl (d) P<C1<Mg<Ca (e) C1<P<Mg<Ca llS-M ~ Exam 2 (Test 55) - 10/17/07 5. An element in period 2 has the following values of its first four ionization energies: 1131 = 0.80 MJ/mol IE2 2* 2.42 Mil/moi IE3 = 3.66 MJ/niol IE4 = 25.02 MJ/mol What is the element? (a) Be (13) B (c) C (d) N (61 0 6. What is the formula of the oxide of Al? (a) A10 (b) A102 (0) A103 (d) A1202 (63) A1203 7. Censider the following data for lattice energies of alkaline earth oxides: (kJ/mol The trend in this data can best be explained by the following: (a) The electron configuration of each atom (h) The electron affinity of each atom. (c) The radius of each atom, (d) The radius of each ion. (e) The charge on each ion. 115-M — Exam 2 (Test 55) ~ 10/17/07 8. Use the following information to calculate the first ionization energy of Li. LiF(s) we Li+(g) + F ‘(g) 1050 kJ/mol LiF Li(s) + V; F2(g) we LiF(s) —617 kI/mol Li thg) —+ 2 Mg) 160 kJ/mol F2 Li(s) —> Li(g) 161 kJ/niol Li Hg) w-r F Kg) M328 kJ/mol F (a) 216 kJ/mol Li (b) 346 kJ/mol Li (c) 426 kJ/mol Li (d) 440 kJ/mol Li (e) 520 lei/11101 Li 9. Determine the bond length of F2 from the Morse curve: C) | w (J .105 —140 Potential energy, kJImol a: -1?5 O 100 200 300 400 F-F Inter nuclear dlstance. pm (a) 52 pm (1)) 128 pm (C) 384 pm (:3) “"120 kJ/mol (e) 155kJ/mol l0. Which of these molecules is NOT planar? (21) N13 (b) XeF4 (C) BFs (d) 803 (B) CFZZCFZ l ISvM ~ Exam 2 (Test 55) - 10(17/07 11. 12. 13. Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of iodine trichloride, ICl3. I l l (e) T-shaed Identify the geometry about atoms X and Y: /—\ 0" \_/ r—\ O A 0.. CHs—‘(IEHZ-wCH2---(.‘.Br=(.‘IH2 atom X atom y - (b) What are the O-SWO bond angles in 803‘? (a) All equal to 109.5 degrees. (b) All equal to 120 degrees. (c) All smaller than 109.5 degrees. (d) Two are greater than 120 degrees and one is less than 120 degrees. (e) Two are less than 120 degrees and one is greater than 120 degrees. ] 15-M - Exam 2 (Test 55) - 10/?7/07 34. Which compound contains both ionic and covalent bonds? (a) CaClz (b) CH3C02H (c) GINO; (5) K28 (e) NaNO; 15. Which is the structure for butene? (c) Rik/\V/ (e) 16. What is the formal charge 0n the C atom in this structure of the CNO' ion? [ C = NED] (a) W2 (13) —1 (C) 0 ((1) +1 (e) +2 17. What is the molecular formula for the following structure? o/ (a) CSHH (b) C4Hs (C) CSHIG (d) C4H10 (9) C5H9 llS-M - Exam 2(T95155)- 10/17/07 18. What can you say about the energy change in the following reactiozi‘? H2 + H20=CH2 --> H30"CH3 C-C = 346 kJ/mol C=C = 6lOkJ/mol C—H = 413 kJ/mol Heel-l = 436 kJ/mol (a) This reaction is isothermic. (b) This reaction is endothermic. (c) This reaction is exothermic. (d) This reaction is energy neutral (AH = 0). (e) The energy change will depend on which isomer is present. 19. Identify an isomer of the foliowing molecule: an an CHy—CH—CHEMCH—CHg We M (b) / (e) M (E) /\\H\m ilS-M — Exam 2 (Test 55) — 10/17/07 20. Which of the functional groups listed are present in the following molecule? \ /\ / NH2 0 I. hydroxyl Ill. carboxylic acid II. carbonyl 1V. amine (a) 1, IV (b) I, 11, IV (c) I, III, IV ({3} n, 111, IV (e) 111, IV END OF EXAM 1) Please make sure that you have entered 20 answers on your scan sheet 2) Make sure that you have entered your name, ID number, and lab section number (4 digits). 3) You MUST turn the scan sheet in to your TA before leaving the exam! ...
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This note was uploaded on 02/05/2012 for the course CHEM 115 taught by Professor L during the Fall '02 term at Purdue University-West Lafayette.

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115 Exam II Fa07 - llS—M - Exam 2 (Test 55} - 10/17/07 1....

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