2 - N... K e z Student ID Number LAB Sec. # _; TA: ;Lab...

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: N... K e z Student ID Number LAB Sec. # _; TA: ;Lab day/time: Dr. Dorte Madsen Winter 2009 CHEMISTRY 2A (Section B) Exam II Instructions: CLOSED BOOK EXAM! No books, notes, or additional scrap paper are permitted. All information required is contained on the exam. Place all work in the space provided. If you require additional space, use the back of the exam. A scientific calculator may be used (if it is a programmable calculator, its memory must be cleared before the exam). (1) Read each question carefully. (2) For Parts I and 11 there is no partial credit given, and ONLY ANSWERS ON THE FRONT PAGE ARE GRADED (3) Use the correct number of significant digits in your answers (4) The last page contains a periodic table and some useful information. HHHI You may remove it for easy access. (5) If you finish early, RECHECK YOUR ANSWERS! U.C. Davis is an Honor Institution Possible Points #1—10. (2 poi ts each) #1 1-15 (6 points each) #16—18 (6+ 12+6points) #19-22 (6+ 6+ 6 +18 points) # 23 (30 points) I 140 otal Score Name: Exam I (Page 2 of 9) Part I: True/False Questions, Concepts (2 points each) Write either “T” if the statement is True or “F” is the statement is False on the front page 1. A solid formed from a mixture of solutions is called a precipitate I 2. The angular momentum quantum number, 8, determines the angular shape of the electronic wave function r’ 2 f "WW/e £> 0 =9 f-mfiHvz T- l P) [0’ of 9+! . 3. The hydroxides of group I metals are all strong bases , T 2"an H470 "9 WWW WWI) [Y 5+0»? [3019 4. An aqueous solution of carbon dioxide is acidic 4 _ T (gait/7590 ‘3 ’55”; ’37)? * #503 arc/901,1 5. The symbol “n” in the Bohr theory of atomic structure refers to the number of electrons in a shell Y) 2 fwd/Va Q (mu-MM )3 a )fi 6. The electron configuration of F e3+ is [Ar] 452 3d3 6 +3 q j 5‘ F thgaw at ~:> Fc {N M 7. When an atom absorbs a photon an electron is promoted to a higher lying energy level 7 8. 0.5 moles of hydrochloric acid is exactly neutralized by 0.§ moles of calcium h droxide 05/40; H at [Ma] M [140/ w; /m/ K W2 5 0.1””! F p40} pa [WI [9’ 2,101 0/7' ‘— Caév’flz 9. An atom with an even number of electrons is always diamzig-netic A , c ['5 74” 6‘ gm :77an r ‘5” F632“ El EHZJEI P' “fl WW»! 2 10. The nitrogen atom has three unpaired electrons T N awn“ : 1:2 232,03 : 30mm“ (9 Name: Exam 1 (Page 3 of 9) Part 11: Multiple Choice, Concepts (6 points each) Select the Qe_s_t_ answer and enter it on the front page (either a, b, c, d, e, or i) - No partial credit 11. (6 pts) Which of the following is the correct orbital diagram for the ground state electronic configuration of phosphorous? (a) We] {New ELL Fo/L'w Haw/T Pvt/6’5 (c) We! m M (d) [Ne] E (e) None of the above 01“ 12. (6 pts) For an ideal gas, if the volume is doubled but the temperature and number moles stays the same P V 2 V) 117‘ (6’ Pressure is doubled /(,b)/ The gas constant is doubled F (2 V3 3 V) )2 7‘ M The pressure is squared (d’f The molecules moves slower none of the above 13. (6 pts) Which of the following orbitals does NOT have lobes aligned along the y-axis? dry (13) dx2_y2 (c) py ((1) None of the above are aligned along the y—axis (e) All of the above are aligned along the y-axis 14. (6 pts) Which of the following species have unpaired electrons? («{F at)” Ca2+ t4; Kiev/fl (c) Fe2+ ——> C3 BEBE} E1 53 MY 82" (e) None of the above Name: Exam I (Page 4 of 9) 15. (6 pts) Which graph best represents the distribution of molecular speeds for the gases argon and methane when both are in the same flask with a total pressure of 600 mmHg and a partial pressure of 450 mmHg for the argon? [Note: The vertical line on each curve represent the root mean square velocity, um] ' 2 (“3- CH. cm i 31 '5 C a 5 A! ° Ar 5 E E E E :3: molecuizrspend (My )1}; ’5 ‘5 E E “a “5 E; E .1 E moitculz: speed 0,0(7 fry/0f} Thai k gappové‘r fir 270%"0/ owL melanin: :pccd Name: Exam I (Page 5 of 9) Part III: Fill in the Blank Fill in your result in the assigned space — Partial credit may be given (If) 16. (6 pts) Aqueous solutions of copper sulfate and sodium carbonate are mixed. Predict if a reaction is likely to occur. If so, write the net ionic equation. If not, explain (“+20”) + C03- @ ’9 [5) 1”” a 3 .r Home “.3 [a {on +~ Malagw ~> wazgow + 6.403(5) \0 (‘74 17. (12 pts) Balance the following reaction in acidic solution F’“W##e I’(aq) +Mn04‘(aq) —+ Mn“ (aq) + 12 (s) O¥rda+fofl 3—— 1 I24” —————3 IMO +2 5‘ 1 V? “Mw‘ge‘ + 3W -) MNOW‘Z‘v’) 9 M”+(:w+ “50 a) j x 2 Sat/*4 : + - .. “a! l «FILHW-l‘ lfl/‘loflgfi2-f— [army-9 511(5) ) c"+2MN+é)+f/,l}gi : + — ' mm” H7 H( 7‘ ll’wofi 1"" I x —7 512(5) *lM/V” +XH;0/g) 18. (6 pts) For each of the following pairs, circle the ion or atom that has the larger size (a) Te or Br (b) K+ or @ Exam I (Page 6 of 9) Name: Z / 0 '4 19. (6 pts) Write the electron configuration for selenium (Se) {/4 "1 L115 gd Lie 1? H 20. (6 pts) How many electrons can have n = 2 and m3 = — 2 who” n27. £2 0 ’"110 :my;-/,L : O Angular nodes: 0 K's/ Radial nodes: 3 ("\"C’L Part IV: Long Answer Please show all work gor calculations. Fill in your result in the box (remember units!) — Partial credit may be given 22. (18 pts) The energy levels for the hydrogen atom, in joules, are given by the equation —13 En a —2.l782x10 J n A photon with wavelength 2166 nm is emitted from a hydrogen atom in energy level n = 7. What is the energy level of the @afier the photon is emitted? (I +0» E ’2.I7X‘Ho‘/6~T L, H .300- 2 I — lb] 770 0 C7) (7)2 zé 3'1 : 5”" ‘ Ea his 24,9 120 f5)[%,07/D /5) _’ 6],)77¥)0 2°3- / 7,)96 )‘10’ 1m ‘ F : ‘Hv‘I‘i‘ho'UJ- 0/.177 w”? : 4,56 Lino—'75 7‘ 2 - - 5 [)2- n": 19.? me N I Wfl—"l‘l age total Name: Exam I (Page 7 of 9) 23. (30 pts) Carbon monoxide gas and hydrogen gas are mixed in an evacuated 25.0 L reaction vessel at 25°C. The initial partial pressure of carbon monoxide is 0.350 atm and the initial total pressure is 1.32 atm. The mixture reacts according to the reaction: 3 CO (e) + 7 H2 (2;) -* C3Hs (g) + 3 H20 (1) (a) What is the partial pressure of hydrogen in the initial reaction mixture (before the reaction takes place)? P7544 :- p”; + FCC) l432a'lm2 P» + 0:35‘0 2 PM 3 0'97a‘im (b) What type of reaction is this? (Circle ONE correct answer) Combustion Neutralization Precipitation (0) What is the final number of moles of C3Hs produced in the reaction? Plvnnwm (bevéw) = "W )2 [2w 3m) co ‘ H25»; 50 Tie) DH}: C),qu r0) H; a 7/0, Hz. Pco V: [760 fiT @,3§o)(29~.w) 2n“ Ailey” ' if» 6+;fl' nzv> 0.353;») <0 MJ'TM C015 L)‘”*/ (2% a 7 4 a2 (/4 3979.160 IM £er 2,113» H 2N2) (0 Name: Exam I (Page 8 of 9) The following two pages contain conversions, constants, equations, and a periodic table which may be useful to you. You may remove it for easy access. Conversions: 1 atm = 760 Torr = 760 mmHg = 101,325 Pa 1010 A =1 m = 1012 pm = 100 cm 1.00 in=2.54 cm 1cm3 = 1 mL 101.325 J= 1 L atm llb=453.6g lcal=4.184J 1gal=3.785 L T(K) = t(°C) + 273.15 t(°F) =9/5 t(°C) + 32 Constants: R = 8.3145 J / mol K = 0.08206 L atm / mol K c = 2.9979 x108 m / s h=6.626x10_34 Js g=9.81m/s N,1,=6.022x1023 mol‘l d (H20) = 1.00 g / cm3 m(electron) = 9.109 x 10‘31 kg RH = 2.179 x 10’18 J Equations: 11 a: Mm d = 1’1 V E = hv v = g A u = 172 = 251 m M Pm, 2P, xA=iA- AxApz—h— zefl=z—S I x,,,, 4:: Solubility Rules: 1. Salts of group 1 cations (with some exceptions for [{2} and the NH4+ cation are soluble ,,/ . Nitrates, acetates, and perchlorates are soluble Salts of silver, lead, and mercury(I) are insoluble 2 3 4. Chlorides, bromides, and iodides are soluble 5 Carbonates, phosphates, sulfides, oxides, and hydroxides are insoluble (sulfides of group 2 cations and hydroxides of Ca”, S122 and Ba2+ are slightly soluble) 6. Sulfates are soluble except for those of calcium, strontium, and barium ...
View Full Document

Page1 / 8

2 - N... K e z Student ID Number LAB Sec. # _; TA: ;Lab...

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