EM 1314 Name Exam III TA Name John III. Gelder November 16, 1992 Lab Section INSTRUTIONS: 1. This examination consists of a total of 7 different pages. The last page includes a periodic table and some useful information. All work should be done in this booklet. 2. PRINT your name, teaching assistant's name and lab section now in the space at the top of this sheet. DO NOT SEPARATE TESE PAGES. 3. Answer all questions that you can and whenever called for show your work clearly. Your method of solving problems should pattern the approach used in lecture. You do not have to show your work for the multiple choice or short answer questions. 4. Point values are shown next to the problem number. 5. Budget your time for each of the questions. Some problems may have a low point value yet be very challenging. If you do not recognize the solution to a question quickly, skip it, and return to the question after completing the easier problems. 6. Look through the exam before beginning; plan your work; then begin. 7. Relax and do well. Page 2 Page 3 Page 4 Page 5 Page 6 TOTAL SORES (25) (26) (22) (15) (12) (100)
EM 1314 EXAM III PAGE 2 (9) 1. Write the chemical formula(s) of the product(s) and balance each of the following four reactions. Identify all product phases as either (g)as, (l)iquid, (s)olid or (aq)ueous. a) NO 3 (aq) + Ba(O) 2 (aq) b) Al(NO 3 ) 3 (aq) + Na 2 O 3 (aq) c) Ba(s) + l(aq) (4) 2. Write the ionic and the net ionic equation for any one of the equations in Problem #1. (12) 3. Draw a Lewis electron-dot structure for each of the covalent molecules below. Include all resonance structures if they are needed to adequately represent the bonding in the molecule. (a) BrO 3 (b) 2 O 2 (c) lno 2
EM 1314 EXAM III PAGE 3 (18) 4. omplete the following table ompound Name of molecular geometry Bond angle(s) ybridization on the central atom Polar or nonpolar? IF 3 N 2 PO 3 4 N 2 O O 3 (8) 5. Given the following Lewis structure, : O 1 N bond angle #2 bond angle #1 2 a) how many σ-bonds and how many π bonds. σ-bonds π-bonds : b) indicate the hybridization on each of the following atoms. 1 2 O N c) indicate the ideal bond angle for; bond angle #1 bond angle #2 :
EM 1314 EXAM III PAGE 4 (14) 6. Answer each of the following statements. a. Explain the term effective nuclear charge and use it to explain why the atomic radius of l is smaller than the atomic radius of Al. b. Define the term ionization energy and indicate the overall trend in the first ionization energy for the elements in a period. Also, explain why the first ionization energy for boron is less than the first ionization energy for beryllium. (8) 7. Indicate the atomic and/or hybrid orbitals on each atom in the following molecules which are involved in forming the covalent bond. a. 2 O b. N 2
EM 1314 EXAM III PAGE 5 (15) 8. Short answer. a. Write the electron configuration for, i. P 3 ii. Fe 3+ iii. Po b. Draw a Lewis structure for the ion SN and determine the formal charge on each of the atoms. c. Write the set of quantum numbers for the last electron added to complete the ground state electron configuration for a neutral Zr atom. d. An unknown neutral element, X, has only 3 electrons in its p subshell. What is the formula of the compound formed between this unknown element and hydrogen?
EM 1314 EXAM III PAGE 6 Multiple hoice: Print the letter (A, B,, D) which corresponds to the answer selected. 9. 10. 11. 12. 13. 14. ONLY TE ANSWERS IN TE AREA ABOVE WILL BE GRADED. Select the most correct answer for each question. Each question is worth 2 points. 9. Which of the following are reasonable values for the first four ionization energies for Mg? 1st 2nd 3rd 4th A) 496 kj 4562 kj 6912 kj 9543 kj B) 578 kj 1817 kj 2744 kj 11,577 kj ) 738 kj 1451 kj 7733 kj 10,540 kj D) 657 kj 1269 kj 2136 kj 2752 kj 10. Which of the following species has the largest radius? A) Ne B) O 2 ) Li + D) N 11. Which of the following atoms has a negative electron affinity? A) e B) Be ) Ne D) F 12. The shortest bond length in the following is A) F B) l ) Br D) I 13. The molecular geometry of a molecule is best described in terms of the location of the atomic nuclei. What geometries are possible for compounds with a central atom which can be described as using sp 2 hybrid orbitals? A) trigonal planar or bent B) tetrahedral, bent, or trigonal pyramidal ) square planar, tetrahedral, or trigonal planar D) trigonal bipyramidal or unsymmetrical tetrahedron 14. Which of the following species violates the octet rule? A) N + 4 B) NO 2 ) lo 3 D) N 2 O 4
EM 1314 EXAM III PAGE 7 Useful Information 1 2 3 4 5 6 7 IA 1 1.008 3 6.94 11 IIA 4 Li Be 9.01 12 Na Mg 22.99 24.30 19 20 K a 39.10 40.08 37 Rb Sr 38 85.47 87.62 55 56 s Ba 132.9 137.3 87 88 Fr (223) Ra 226.0 IIIA IVA VA VIA VIIA 4.00 5 6 7 8 B N O F 9 10 Ne 10.81 12.01 14.01 16.00 19.00 20.18 13 14 15 16 17 18 IIIB IVB VB VIB VIIB VIII IB IIB 26.98 28.09 30.97 32.06 35.45 39.95 21 22 23 24 25 26 27 28 29 Sc Ti V r Mn Fe o Ni u 30 31 32 33 34 35 36 Zn Ga Ge As Se Br Kr 44.96 47.88 50.94 52.00 54.94 55.85 58.93 58.69 63.55 65.38 69.72 72.59 74.92 78.96 79.90 83.80 39 Y Zr 40 41 42 43 44 45 46 47 Nb Mo Tc Ru Rh Pd A g 48 49 50 51 52 53 54 d In Sn Sb Te I Xe 88.91 91.22 92.91 95.94 (98) 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3 57 72 73 74 76 77 78 79 81 82 83 84 85 86 La Periodic Table of the Elements f Al Si P S l VIIIA 2 Ta W Re 75 Os Ir Pt Au g 80 Tl Pb Bi Po At Rn 138.9 178.5 180.9 183.8 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 (209) (210) 89 Ac 104 105 106 227.0 (261) (262) (263) e Ar (222) Lanthanides Actinides 58 59 60 61 62 63 64 e Pr Nd Pm Sm Eu Gd 65 66 67 68 69 70 71 Tb Dy o Er Tm Yb Lu 140.1 140.9 144.2 (145) 150.4 152.0 157.2 158.9 162.5 164.9 167.3 168.9 173.0 175.0 90 91 92 93 94 95 96 Th Pa U Np Pu Amm 97 98 99 100 101 102 103 Bk f Es Fm Md No Lr 232.0 231.0 238.0 237.0 (244) (243) (247) (247) (251) (252) (257) (258) (259) (260) Solubility Table Ion Solubility Exceptions NO 3 soluble none lo 4 soluble none l soluble except Ag +, g 2+ 2, *Pb 2+ I soluble except Ag +, g 2+ 2, Pb 2+ SO 2 4 soluble except a 2+, Ba 2+, Sr 2+, g 2+, Pb 2+, Ag + O 3 2 insoluble except Group IA and N 4 + PO 3 4 insoluble + except Group IA and N 4 - O insoluble except Group IA, *a 2+, Ba 2+, Sr 2+ S 2 insoluble except Group IA, IIA and N + 4 Na + soluble none N + 4 soluble none K + soluble none *slightly soluble
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