FORM A is EXAM I AF, VERSION 2 (v2) 1. DO NOT TURN THIS PAGE UNTIL DIRECTED TO DO SO. 2. These tests are machine graded; therefore, be sure to use a No. 1 or 2 pencil for marking the answer sheets. 3. Completely blacken the answer circle. If you change an answer, erase completely the previous mark. 4. You may remove you answer sheet from this booklet. If you have a pink test, test form A should be darkened (B for Blue), if it is not, notify your instructor immediately. 5. Fill in your last name, first name, and initial. Blacken the corresponding letters below. 6. Fill in your ID number. CAREFULLY, blacken the corresponding numbers below. 7. Fill in the Dept. Course No. and Section. The Dept. = CHEM, the Course No. = 101, and your section refers to your lecture section. 8. If you want your scores posted by a portion of your ID #, mark A under the option column. 9. READ THE TEST CAREFULLY. The time limit on this test is 50 minutes. 10. Use the test for scratch paper. 11. Mark your answers in this booklet as well as on the answer sheet so you can check your score with the key after the test. 12. There are 20 questions. Each of the multiple-choice questions counts 5 points for a total of 100 points. 13. Your score will be calculated from the number of correct answers. There is no penalty for guessing. 14. Turn in your scan sheet, show your ID, and have your calculator checked by the TA listed on the overhead for your last name. 15. A key will be on the electronic class bulletin board about 2pm. This is accessed through the class homepage ( http://chemed.tamu.edu/bb.htm ). The class average will also be posted when it is confirmed. IMPORTANT INFORMATION: F = 1.8 C + 32 λ = h/mv 2 2 7-1 1/ λ = -R [(1/n f ) (1/ni )] and R = 1.097 X 10 m E = -R H [(1/n f 2 ) (1/ni 2 )] and RH = 2.18 X 10-18 J c = 3.00 X 10 8 m/s h = 6.63 X 10-34 J s E n = -R H /n 2 Vickie M. Williamson, All Rights Reserved 1
1. Which sketch(es) could represent a p orbital? A. 4 & 5 B. 2 & 3 C.l, 4, & 5 D. 2, 3, & 4 E. 1 only 2. [Ar]4s 2 3d 10 4p 3 is the electron configuration of: A. V B. Zn C. Sb D. As E. P 3. The ionization energy is higher for oxygen than for beryllium. Which statement(s) account for this: I. An increase in the numbers of electron shells. II. An increase in the effective nuclear charge. III. An increase in the atomic radius. A. II and III. B. III only C. I and XII D. I only E. II only 4. What is the frequency (per second, which is Hz) of electromagnetic radiation necessary to move an electron from n=2 to n=4 in a hydrogen atom? A. 2.18 x 10-18 B. 5.4 x 10-19 C. 6.2 x 10 14 D. 8.2 x 10 14 E. 4.1 x 10-19 5. The density of gold is 19.3 g/cm 3. How many grams of gold are in 1.0 qt of gold? (1 L = 1.056 qt) A. 18 B. 20.4 C. 1.8 x 10-2 D. 19.3 E. 1.8 x 10 4 6. Which particle has 48 electrons? A. 118 50 Sn2+ B. 116 50 Sn4+ C. 112 48 Cd2+ D. 48 68 Ti E. 22 31 Ga 7. The series which correctly lists from left to right a halogen, an alkaline earth, a transition metal, and an alkali metal is A. F, Sr, Fe, Sn B. Br, Ba, Cr, Na C. Cl, K, V, Mg D. O, Ca, Ce, Al E. Cl, Na, Fe, Ca 8. Which one of the following forms of electromagnetic radiation has the shortest wavelength? (frequencies are given in parentheses in HZ or sec -1 ) A. radio waves (10 6 ) B. microwave (10 10 ) C. X ray (10 18 ) D. ultraviolet(10 15 ) E. infrared (10 13 ) Vickie M. Williamson, All Rights Reserved 1
9. How many significant figures should there be in the answer to the following problem? (29.2 20.0) (1.79 x 10 5 ) 1.39 A.2 B.3 C.1 D.5 E.4 10. Which of the following is (are) FALSE? I. Dalton was NOT the first person to describe atoms. II. The Thomson model of the atom contained negative electrons embedded in a positive mass. III. Rutherford s positive particles were deflected by gold foil, showing that the gold atoms had a small dense negative center. IV. Bohr s model of the atom was based on the idea that electrons could contain all energy values since every color of light was given off in the flame tests. A. III, IV B. I,II C. I, IV D. II, III E. all are true 11. The table shown below lists the naturally occurring isotopes of element X. Use this data to calculate the average atomic mass of element X. Mass of Isotope Isotopic Abundance 15.33 amu 28.6% 17.26 amu 13.3% 18.11 amu 58.1% A. 17.65 B. 16.90 C. 17.20 D. 17.11 E. 15.33 12. Elements with the outermost electron configuration ns 2 np 2 are found in which portion of the periodic table? A. R B.S C. Y D. V E. second column in T 13. Select the smallest atom from the following list. A. Rb B. Cl C. Fe D. P E. Na Vickie M. Williamson, All Rights Reserved 2
14. Calculate the wavelength of a baseball of mass 5.25 oz traveling at 92.5 miles per hour. (1 mile = 1609 m and 1 kg = 2.205 lb) (Hint: convert both to the units you need.) A. 1.08 x 10-34 m B. 9.26 x 10 33 m C. 1.36 x 10-34 m D. 6.63 x 10-34 m E. 4.81 x 10-35 m 15. What is the Fahrenheit temperature that corresponds to 0 K? A. 549 F B. 523 F C. 434 F D. 459 F E. 120 F 16. Which element from the following list has the greatest electronegativity and what is the reason? Si, Mg, P, S, K A. Mg, because it smaller than K and only has 2 outer shell electrons. B. K, because it is the largest and needs to get rid of 1 electron to have a complete outer electron shell. C. S, because it is the smallest and has a more complete main electron shell. D. Mg, because it is the smallest metal and will not accept an electron easily. E. S, because it is the largest nonmetal and will lose an electron easily. 17. Which one of the following represents a possible set of quantum numbers (in the order n, 1, m 1, m s ) for an electron in an atom? A. 2,2,0,1/2 B.2,1,0,0 C. 2,1,-1,1/2 D. 2,0,1,-l/2 E. 3,3,0,-1/2 18. How many orbitals in an atom can have the set of quantum numbers n = 2, l = 1, m 1 = -1? A. 3 B. 1 C. 5 D. 7 E. 2 19. An atom of Fe has two 4s electrons and six 3d electrons. How many unpaired electrons would there be in the Fe 3+ ion? (hint: draw orbital diagrams) A. 3 B. 2 C. 1 D. 5 E. 4 20. Which one of the following is the electron configuration (in order of increasing energy) f or the Co 2+ ion? A. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 9 B. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 0 3d 7 C. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 6 D. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5 E. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 0 3d 5 Vickie M. Williamson, All Rights Reserved 3
Key question 5pts each 1 B (D=3pts) 2 D 3 E (A=3pts) 4 C 5 E (A, C =3pts) 6 A 7 B 8 C 9 A 10 A (C,D =3pts) 11 C 12 D 13 B 14 A 15 D 16 C 17 C 18 B 19 D 20 B Vickie M. Williamson, All Rights Reserved 4
58 59 60 61 62 63 64 65 66 67 68 69 70 71 Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu 140.12 140.91 144.24 (145) 150.36 151.97 157.25 158.93 162.50 164.93 167.26 168.93 173.04 174.97 90 91 92 93 94 95 96 97 98 99 100 101 102 103 Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr 232.04 231.04 238.03 (237) (244) (243) (247) (247) (251) (252) (257) (258) (259) (262) Periodic Table of Elements IA VIIA 0 (1) (17) (18) 1 1 1 2 1 H IIA H IIIA IVA VA VIA H He 1.008 (2) 1.008 (13) (14) (15) (16) 1.008 4.003 3 4 5 6 7 8 9 10 2 Li Be B C N O F Ne 6.941 9.012 10.81 12.01 14.01 16.00 19.00 20.18 11 12 VIIIB 13 14 15 16 17 18 3 Na Mg IIIB IVB VB VIB VIIB IB IIB Al Si P S Cl Ar 22.99 24.31 (3) (4) (5) (6) (7) (8) (9) (10) (11) (12) 26.98 28.09 30.97 32.07 35.45 39.95 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36 4 K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr 39.10 40.08 44.96 47.88 50.94 52.00 54.94 55.85 58.93 58.69 63.55 65.39 69.72 72.61 74.92 78.96 79.90 83.80 37 38 39 40 41 42 43 44 45 46 47 48 49 50 51 52 53 54 5 Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe 85.47 87.62 88.91 91.22 92.91 95.94 (98) 101.07 102.91 106.42 107.87 112.41 114.82 118.71 121.75 127.60 126.90 131.29 55 56 57 72 73 74 75 76 77 78 79 80 81 82 83 84 85 86 6 Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 132.91 137.33 138.91 178.49 180.95 183.85 186.21 190.2 192.22 195.08 196.97 200.59 204.38 207.2 208.98 (209) (210) (222) 87 88 89 104 105 106 107 108 109 110 111 112 113 114 115 116 117 118 7 Fr Ra Ac Rf Db Sg Bh Hs Mt Ds Rg Cn (223) (226) (227) (267) (268) (271) (272) (270) (276) (281) (280) (285) (284) (289) (288) (293) (292) (294) Department of Chemistry Texas A&M University