14amt2k - CHEM 14A YOUR NAME Instructor Dr Laurence Lavelle...

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Unformatted text preview: CHEM 14A YOUR NAME ................................ Instructor: Dr. Laurence Lavelle lD# ............................... FALL 2004 2nd MIDTERM (Total number of pages = 7) (Total points = 50) (Total time = 50 mins) ”Carefully remove last page which is your Periodic Table.** YOUR DISCUSSION SECTION ...................................... YOUR TA’S NAME ...................................... WRITE IN PEN (Show all your work on this paper, check units and significant figures.) Good Luck Constants and Formulas Planck constant, h = 6.63 x 10‘34 J - s Avogadro constant, NA = 6.02 x 1023 mol‘1 Rydberg constant, R = 3.29 x 1015 Hz Gas constant, R = 8.314 J.K‘1.mol'1 Mass of electron, me = 9.1 x 10‘31 kg Speed of light, 0 = 3.0 x 108 m.s’1 0°C=273.15K 1L=1dm3 1atm=101.325 kPa 7t=3.14 h2n2 E=hv E=pC Enzm p=mv hR h En: - 712‘ A: E C=Xv _ MW _ l 2 _h_ pH_pKA+LOGl[AH]INITIALACID E— 2mv AprxZ47t Solution to AX2 + BX + C = o is X = W QlA. What is the shape of CS32— ? /' --.. a ' ‘ / \ If: .. H Z/VS ng"/ap€‘ C 2" :j. ' trigonal planar B. All of the following have an angular shape except: Circle your one answer. HOCl 332— 13- C102— 1] 3x ?:Z/7’-/5616 4 I '. 7 ”a a ’0 / ‘ \ G 1: Circle your one answer. Xng Xe02 '\ \ \ Which of the following is polar ? NHQ” (3pt) (3pt) (3pt) D. For the following molecule give the type of bond and the orbitals used to form the bond. (12190 I? I? H\ _ _ _ '. /C —C C —Q. H Bond Bond Type, Orbitals Used H —C= flo (H1s+Csp2) M N “I“? —C=C— MAT o(Csp2+Csp2) [7‘4“ _ = _ C2 C2 C c ”I 7H p + p) [M = C —' C —C=O (If G (Csp2 + Csp2) Md“ _ C = 0 /4f 0 (Csp2 + Osp2) IWF { g TE(C2p+02p) Wt Q2. Determine the bond orders and use them to predict which species of each of the following pairs has the stronger bond. Show all your work and clearly indicate your answer. A. F2 which one has the stronger bond F2 (2pt) F2 bond orderis fl 0 11W 4): (2pt) Fz- bond orderis 10- : 1L3; 7') Z é/ (2pt) IT 2 7f ¢/Jflzfli1 if 437 flfiiZ/O Ex 12 m-f’y 5 We / '5: Z § :1”— 1y 7’ S 41 02: B. B2 or B2+ which one has the stronger bond £2 (2pt) B2 bond order is g 0 —- 11% W2”) / (2pt) _L _, B2+ bond order is gfl : 1" 3'— Z) ~ '2 (2pt) Q3. Answer the following questions for the complex ion [Cr(en)(ox)Clg]+ A. What is the shape of the complex ? octahedral B. What is the oxidation state of the Cr ? ”5'1" C. Write the n' r this com lex. ’71 l1}? W M dichloro ethylenediamine oxalat Chromiumm Mt M 9% / M” E. Draw one optical isomer. (More than one structure will be zero credit.) (2pt) (2pt) (4pt) (4pt) Q4A. Write the equilibrium constant expression for the following reaction. (2pt) PbS(s) + 02(g) : PbO(s) + 802(g) 2PbS(s) + 302(g) : 2PbO(s) + 2s02(g) /7l/(L K = [SO2(g)]2/[02(g)]3 01/5 ’ 'ZXY /' ’L K : I”: 01 M at)? B. Given: 802(g) + 02(g) 3— SO3(g) At equilibrium at a certain temperature, the concentrations of SO3(g), 802(g), and 02(g) are 0.12 M, 0.86 M, and 0.33 M, respectively. Calculate the value of KC for this reaction. (3pt) 28©2<g> + 02<g> : st3<g> M14 ...
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