[Bush] Chemistry Exam #4 - Spring 2007

[Bush] Chemistry Exam #4 - Spring 2007 - NAME 1 Chemistry...

Info iconThis preview shows pages 1–8. Sign up to view the full content.

View Full Document Right Arrow Icon
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 2
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 4
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 6
Background image of page 7

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 8
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: NAME 1 Chemistry 1301 Spring 2007 Exam #4 iknu54 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 30 questions on this examination worth 3.33 points each. (Total of 100 points.) Check your test booklet to be sure that you have a complete exam with all 30 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. What is the relationship between wavelength A, frequency v,and the velocity of light c? a) = A/v O ' Czll) 1‘I’C = AN . C) C = V/}\. ers 0'? d)c = V + x . ‘y +WYSL, e) c = V _ k )W ends 1) m UNH vbGfifley! 2. Which one of the following observations most clearly supports the conclusion that electromagnetic radiation has particle properties? a)the emission spectrum of hydrogen C:>the photoelectric effect c)the scattering of alpha particles by metal foil d)diffraction e)the existence of cathode “rays” 3. 2 Which one of the following observations most clearly supports the conclusion that electrons in atoms have quantized energies? C) the emission spectrum of hydrogen 13) C) d) e) the photoelectric effect the scattering of alpha particles by metal foil diffraction the existence of cathode "rays" 4. The fact that electrons behave as though they had spin was shown by a) calculations using the Bohr model of the atom. b) the Heisenberg Uncertainty Principle. (:) laboratory experiments using magnetic fields. d) calculations using the Schrodinger wave equation. 9) agreement of the Balmer equation with theory. 5. According to the experiments concerned with the photoelectric effect, what was the result of increasing the frequency of the light striking the metal surface? a) The number of electrons emitted was increased. The energy of the electrons emitted was increased. Both the number and energy of the electrons was increased. Both the number and energy of the electrons was decreased. There was no change in the number or energy of the . electrons. 6. Our modern concept of the atom treats electrons as three— dimensional waves. The equation that describes the electron as a wave was developed by a) b) Henry Aufbau Niels Bohr c) Albert Einstein d) Werner Heisenberg (:D Erwin Schrodinger 7. What type of orbital has the quantum numbers: n = 4, l = 3 l, m] = 0? a) 4s 4p c) 4d d) 4f e) none of the above 8. How many 4f orbitals can be found in the same atom? a) one b) three 0) five seven e) nine 9. 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) psi 10. When n = 2, all the allowed values of l are: a) +1, 0, —l b) +2, +1, 0, —l, —2 c) O, l, 2 (d))0, 1 e) l, 2 11. The nu quantum number determines the a) number of valence electrons in the atom. b) number of orbitals in the shell. (j) orientation of the orbital. d) electron spin. e) none of the above 12. l3. 14. 15. 4 Which one of the following elements shows the greatest tendency to form an anion? a) magnesium b) aluminum c) sulfur chlorine e) argon Which one of the following compounds most probably does not exist? a) BaIz b) BiCl5 c) SnCl4 d) AlBr3 LiF2 @ Which one of the bonds below will be ionic? b) C to Cl c) Br to Br d) P to Cl e) H to C Which one of the following represents the correct electron configuration for the ground state (lowest energy state) of a neutral atom of copper (element number 29)? 3d 4s 4p [Ar] (T T )(T T)(T T)(T T)(T T) (T ) ( X. )( ) b) [Ar] (T T)(T T)(T )(T )(T ) (T ) (T )(T )(T ) c) [Ar] (T T )(T T)(T T)(T T)(T ) (T T) ( )( )( ) d) [Ar] (T )(T )(T )( )( ) (T T) (T T)(T T)(T T) e) [Ar] (T )(T )(T )(T )(T ) ( ) (T T)(T T)(T T) 16. Which one element listed below is predicted to have the 5 greatest tendency to form a cation? (Which one loses an electron most easily?) a) lithium b) carbon c) helium potassium e) oxygen 17. Which one of the following represents the correct electron configuration for the ground state (lowest energy state) of a neutral phosphorus atom? 3s 3p a>[Ne1 (M) (T )(T )(T) b) [Ne] (T) (HM )(T) c>[Ne1 (M) (MM >( ) d>[Ne1 (H) (HM )( ) e) [Ne] (H) (T m )(T) 18. Two different ions of the element 33As are commonly found. Consider the electron configuration of this element and predict what these two ions will be. a) As+ and As2+ b) AsZ+ and A54+ (:> As3+ and A55+ d) As2+ and A33+ e) As+ and As3+ 19. The outer electron configuration of elements in Group VIA is: a) nsznp6 b) nsznp5 (:3 nsznp4 d) ns2 e) something else 20. Which one of the following represents the equation 6 associated with the electron affinity of Cl? a) cl(s) "-9 Chg) b) C12(g)—> 2cl(g> + __ c) Cl (9) + Cl («3) % C12(g) Cl(g) +e~ *> Cl_(g) e) Cl<g> -e_ —> Cl+(g) 21. Consider the following isoelectronic ions and atoms. Which one has the largest ionic radius? Isoelectronic means they have the same number of electrons. a) Caz+ b) K+ c) Ar d) c1- 22. Which one of the following atoms should be the most electronegative? 0 b)S c) Se d) Te e) P0 23. Which one of the following species is best described by drawing resonance structures? a) NH3 w or b CO ) O , //O\ u 4W5. /O\ a (5) 3 ’0; O, :0 \Q d) C02 ‘. ‘ ’¢ I " e) HCl 24. 25. 26. 27. a double bond between the oxygens. In the Lewis structure for molecular oxygen (02) there is 7 a) a single bond between the oxygens. oo ., GHQ 09 .0 c) a triple bond between the oxygen. d) e) a partial multiple bond between the oxygens. none of the above Which one of the following has an incomplete octet in its Lewis structure? a) 802 b) IBr c) C02 d) F2 If you were drawing a Lewis dot structure for the molecule CH3C02H, what is the total number of electrons that must be accounted for? 24 at: 2643):?) b)18 4H:4C¢3=4‘ c)w torme=n d) 20 2% e) 8 Which of the following elements could have expanded octets: C, N, P, S, O, F? a) C and N b) O and F c) P and O ‘ll’P and S e) C and S 28. What is the formal charge on the iodine in the periodate 8 ion as shown below? I? I 7 «Mug ch‘wcxm Io~2lE=oi W 69; Warbwdocfl IO: 00 .- gtC‘ : a) +7 b) +6 g) +3 @9 +1 e) —l 29. Using the bond dissociation energies below, estimate the standard molar enthalpy of formation of NF3. 1/2 NEN(g)+ 3/2 F—F(g) -9 NF3(g) Bond Dissociation Energy ng/mol) NEN 946 F—F 159 N—F 272 Z: :2: :30: M12 BIO—F locméq 17ZMZJ) mo ' “L :: 4- @ —104 kJ/mol Wk '2. CD”MKCM&$) 1 - d) —578 kJ/mol mmk‘ 3 (pg: :3. (A ISQ ‘43) e) ~618 kJ/mol 2. __~iE_____i.v_wu«~wmt - \O‘PSWLD 30. Predict which of the following bonds would be the strongest. a) C—C b) C=C @ c.=.c ...
View Full Document

This note was uploaded on 04/08/2008 for the course CHE 1301 taught by Professor Klausmeyer during the Spring '08 term at Baylor.

Page1 / 8

[Bush] Chemistry Exam #4 - Spring 2007 - NAME 1 Chemistry...

This preview shows document pages 1 - 8. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online