[Busch] Chemistry Exam #4 - Fall 2006

[Busch] Chemistry Exam #4 - Fall 2006 - NAME '1 Chemistry...

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Unformatted text preview: NAME '1 Chemistry 1301 Fall 2006 Exam #4 PLEASE READ THESE INSTRUCTIONS CAREFULLY BEFORE BEGINNING THIS EXAMINATION. Select the best response to each question. There is only one best response to each question unless otherwise indicated in the question. There are 33 questions on this examination worth 3 points each. (Total of 100 points.) Check your test booklet to be sure that you have a complete exam with all 39 questions. Write your NAME and TEST NUMBER on your Scantron. Write your name on the first page of the test booklet also. Work each problem carefully on the test booklet or on the scratch paper provided. Then select the answer, which you feel is the best response. If none of the choices is close to your calculated answer, or if none is correct, then select the response "none of the above." ALL ANSWERS MUST APPEAR ON THE SCANTRON. Your grade will be determined only by what appears on the Scantron, not by work on the test booklet. Look over your exam and work the easiest problems first, saving the more difficult ones for last. Be sure that you have correctly indicated your final choices on the Scantron before turning in your paper. If a question is incorrectly marked on the Scantron, it will be counted wrong even if it was correctly marked on the test booklet. If you have any questions about any of the problems on this exam, it is your responsibility to ask for a clarification from the instructor during the examination. 1. \thfligneofthefoUowdngconflflnafionsofquananinnnben;doesggtrepnwentanaflowed solution of the Schrodinger equation for the electron in the hydrogen atom (i.e., which combination of quantum numbers is not allowed)? n 1 fly n“ a) 8 -4— 1/2 9 b) 8 2 2 1/2 @ 6 —5 —1 1/2 J1: 0,52,3fifi maquklix: me 6 d) 5 —5 1/2 e) All are allowed. Choose only if a—d are all allowed. 2. How many d—orbitals can one atom can have in the n = 3 shell? w 2 i: 7— : 30 xvi—"viaiho ‘ C d) 20 Hogan; 5- Edodot‘lnla ° Q 18 3. What name is given to a region of an electron probability density graph where the probability of finding the electron is zero? a) wave function b) orbital @ node d) lobe e) something else 4. When n = 3, all possible values of l are a) +1,0,-1 b) +2,+1,0,-1,—2 “DAL 3;), “:5 @ 0,1,2 ' , A .., M \ ‘<“’ 36:2 \ 2x iCx‘wm u Came, d) 0,1 0 Qt ) vi ‘ w e) none of the above 5. What is the maximum number of electrons that can be placed in fig single 5p orbital? . . ‘1 @ two érfifiésk‘gkfGVXI?C\\¥\%§3&Q b) seven ‘ (V - ’RQXELW‘QOJ‘Q‘ 'fp,orfl_Q/,‘E(ftfl‘f‘ c) eight H 0* y _ N9}. C) '3 a: a cl) fourteen r 5 Ix e) none of the above 6. How many valence electrons are there in one atom of Sn? a) 2 GVW fi :1 4 : :1: vamca Aadww d) 5 . e) 6 7. Which of the following is the correct ground state electron configuration for the neutral copper atom? a) [Ar] 3d104s2 b) [Ar] 3d94s2 @ [Ar] 3d104s1 d) [Arl 3d10430 e) none of the above 8. Which one of the following series represents an isoelectronic series? a) Al, Si, P, S b) Be, Mg, Ca, Sr c) Al, Ge, Sb, Po d) Mg: Mg, Mgfi Mg2+ Nah Mg2+,AI3+, 814+ mm it QSQW 9. Which (me of the following atoms has the largest second ionization energy? a) Mg 3.63:5; {met b) er 2,297 m/m C) S 2.151H3/met C0 C3 LIQStuHSIVWJX @ Na bazdttss mm mm malt ab 21061 4.5qu Mil/met 10. Which of the following best describes the variation of atomic radius of the main group elements with respect to their position on the periodic table? a) Increases across a period, increases down a group. b) Increases across a period, decreases down a group. c) Decreases across a period, decreases down a group. Decreases across a period, increases down a group. 6) None of the above. 11. Which gig of the following subshellélgations reflects an atom in the ground state? 2 2 2 1 255M W903 a) Is 28 2p 33 W «99% b) 1522822p63s3 V fiwa :53 c) 1322s23s2 ~ Zij‘m '_ E 1822822p63823d5“ 3P WE . @ 1822822p6 12. Which 9&9 of the following is a d—block element? Ac b) Ce mamaao \ eke c) U ackxméa d) Ra mngmap mm c) Tl mwjva (soak 13. Which reaction is associated with the first ionization energy? - \r . @ Atom in ground state(g) —> Ion+(g) + e (mi: Q Eim‘fi b) Ion)r in ground state(g) —> Ion2+(g) + e' r {takimwx 0) Atom in ground state(g) + e' —> Ion-(g) d) Ion_ in ground state(g) —> Atom(g) + e~ e) none of the above 14. Which one of the following represents the correct electron configuration for the ground state (lowest energy state) of a neutral sulfur atom? 38 3p M’Um . . a)[Nel (M) (TXMXT) .1 vewmawxqumfi‘fi b)[Nel (M) (mom) “kafixebmmx tram-irate“? , c)[Nel (H) (HXMX > ~ Rm»; &.b‘cir\¢lp£¢3 Hm (Eula d)[Nel (M) (HXle) - muflpwimlw ‘41- @Ne1 (H) (mer) on 15. Which element has the highest Pauling electronegativity in the Periodic Table? a) H @ F c) At d) Fr e) something else not listed above 16. Which (fl of the following is a main group metal? a) radon mash Cfiw raw-e. magma; b) uranium qq/JgLWéfl c) mercury Wfifiififi rx‘krarteti . f d cerium Wklm {Mg-Q - u u ! 7 Indium mtg; 17. Which (fl of the following atoms is expected to be paramagnetic? a) Zn ) Sr 63 p d) Ne e) Be 18. The valence electron configuration for a member of the group designated 5A is 5 a) nsznp5 b) nsOnp5 c) (n—1)d5 d) nsl np4 @ nsznp3 l9. Metallic character is related to the first ionization energy of an element. In the list below, the element with the most metallic character is a) Al b) Fe c Sr Cs e) Zn 20. In drawing a Lewis dot structure for the phosgene molecule COClg, how many total electron: must be used (i.e., accounted for) in the entire molecule? 24 b) 18 4 Cc) a. (,0) c) 32 3U d) 8 W" 3H- e) none of the above 21. Which one of the following species has an odd number of electrons? a) 802 ® NO area it c) SO3 d) NO— + 6) NO 22. Which (fl of the following has an atom with an electron deficient octet? 6 a) S F4 b) B rF c) CF4 d) XeF4 BeF2 23. What is the maximum number of triple bonds that one carbon atom can form? a) 4 ® 1 - 0?: C) 0 d) 2 e) 3 24. Which bond is expected to be the longest? a) C—C single bond b) C=C double bond c) CEC triple bond or single bond 3 avg? sim'de in $13 e) C—H single bond I flag“ ll m“ C, 25. Which is the best Lewis structure for the molecule COS? (Formal charges are not shown.) map” I -" La - W27 A ~‘ meal Coo-13‘) :B- , « ‘\-€ l e a . _7 Q’ 123’ c) A)‘ )9 49 CC) 00 oo 00 oo o. . O— : I. as s=c=o :c=o=s c=s=o :SEc—o: ‘ i’. C_O ‘ in (o) o. o. 00 .. ., .. f x Q'- m FC 0 0 0 IL 4230- 0 {:29 mg é “0069+, ‘ (335.39???” 26. Resonance forms must be written for which E of the following molecules? 21) HF w ‘6 b) NH3 5 1 5'5 \ C)‘ 6a \ N a R 0'51 ) $02 a '1 1 aka 0 e) PF5 27. Which one of the following elements could not have an expanded octet? 7 c b) C) d) 6) Br P S all of the above could have expanded octets 28. Draw the Lewis formula for “chlorate ion, ClO3‘, showing all single bonds from Cl to O. For this structure, what is the formal charge on the Clggom? 72. c\ +2 900:: fig» b) +3 ’ 3" l6.— (chip-£33 c) +5 icL‘“ (3:0 2;: c u . d) -3 l” \ (a e) something else ‘7 & lacgitd Y’ Far. 4 2 7 e.“ 6:29 29. Which one of the following compounds most probably does not exist? a) b) C) d) GD B2112 BiCl5 SnCl4 Mg3N2 A1132 30. Which one of the following compounds exhibits bonding that is best described as ionic? a) c) d) 6) CH4 Bl‘z NF3 SF2 31. 32. 33. The six—step enthalpy diagram below involves the formation of solid sodium chloride 8 crystals. Which step in the cycle corresponds to the lattice energy of sodium chloride? C) @ Nat-g) + _> Na+ —) @ 71 (9) \l’ @D 1 1 1 Naig) + flag) <‘ Nam) + EClzm e Nam) + EClzm @ a) step 1 @ step 2 c) step 3 (1) step 4 e) step 5 Using the bond dissociation energies below, estimate the standard molar enthalpy of formation of NF3. All NF bonds in the NF3 molecule are single. 1/2 N-E:N(g)+ 3/2 F——F(g) —> NF3(g) Bond Dissociation Ener kJ/mol Nt-EN 946 F--F 159 N—F 272 mole/s 5 Mel: may: MC, V; MEN gem. baggy 3/7.. ‘37“ WVW 2, ( .53. as) + amass“) - 2:07.2‘433 w a - $04.32 q w moi» Atoms having the same electronegativities are expected to form: a) 833 kJ/mol b) 440. kJ/mol @104 kJ/mol d) —S78 kJ/mol e) —618 kJ/mol a) no bonds b polar covalent bonds @ nonpolar covalent bonds d) ionic bonds e) something else ...
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This note was uploaded on 04/08/2008 for the course CHE 1301 taught by Professor Klausmeyer during the Fall '08 term at Baylor.

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[Busch] Chemistry Exam #4 - Fall 2006 - NAME '1 Chemistry...

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