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chem06 - Problem#1(15 points{EX Predict the geometry of...

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Unformatted text preview: Problem #1 (15 points) . {EX Predict the geometry of each of the following molecules. Describe your leasoning in terms of the VSEPR theory. Draw the resultant structure for each. Using words and/or sketches, be careful to indicate any distortions from otherwise symmetric shapes. If bond angles increase or decrease relative to those expected in highly symmetric structures, be sure to indicate the direction in which they change. I (a) Krlz I (b) 0134 - . I 6 (c) NC15 What is the (net) dipole moment of each of the following? 3M6- (d) C02 (6) CH4 W (0 H20 N [OZ’W CD) ' “ Problem #2 (25 1 pts.) KEy (a) Draw the molecular orbital correlation diagram for the molecule, OF, being careful to indicate in your sketch the relative energy locations of both atomic and molecular orbitals. (b) Write the electron configuration of OF. L z'Z. fl 7' 0’“ (9’: 62/9? 77% 772/}! (c) Is OF paramagnetic or diamagnetic? Why? WMMN 977‘?) IT 1644.9 AN aN/A'Mea’ ELM/70¢ 77:3 fix 2: a" 2*: Zr /7 Maw)- [6/ O. Zffic a? 53323-2/2 w (d) Based on their electron configurations/occupied MO's, which should you expect to be more leactive chemically, OF or CF ? - 0F; jr ,2: 0pm Men :19 not: name , @F‘ is camp Matt) Problem #3 (20 points) - , K )/ (a) Arsene is an extremely poisonous substance used in the manufacture of computer chips. Its formula is Ang. Given your knowledge of periodic properties and chemical bonding principles, draw its geometric structure as well as bond angles [at least as limiting (> or <) values] and the location of any lone pairs. PMWR/ ”/ . flWfiWfl/v ’ x _ 4‘9 (M Ma) H/\ V/ ‘ * <l07° H (b) Do the same for TeHz. ,, fl d—p pun/M t 7?; l2 fewer/2m \ ‘ \ \/ H CLIX’e #20) ,. «W l g t , H Kg negative charge, the absolute value tential of K is 4.8 eV, the electron Problem #4 (20 points) At a separation of 2.2 A between a (full) positive and a (full) of the Coulombic interaction energy is 7 eV. The ionization po affinity of F_ is 3.2 eV, the electron eV. In the highly ionic molecule, dissociation energy of KF (a) into neutral atomic pr and F‘)? affinity of F2 is 2.5 eV, and the electron affinity of K2 is 0.5 KP, the equilibrium. bond length is 2.2 A. ' What is the oducts (K + F) and (b) into ionic products (K+ May (a) Let 2 be the interatomic axis in a homonuclear, diatomic molecule. When a ZpZ orbital on one atom interacts with a 2pz orbital on the other atom, what molecular orbital(s) is/are formed? Give the appropriate label(s) to this/these molecular orbitals. Label them in terms of their bonding/antibonding characteristics as well. Sketch it/them. ' Problem #5 (20 points) We .. ’ 1/2 (W é’gpg (b) Repeat all steps in the above exercise for the interaction of a 2px orbital from one of the above atoms with a 2px orbital from the other atom. \‘ , ME (c) Given the follovving information and your knowledge of chemical bonding, draw the structure of methanol, including all bond lengths and all bond angles (give them specific values). end of exam Wall ' fl] ‘ 1,13 :2: CH30 L/f 1.54 v. 0.96 A /C 0” 1.15 A 1.10 A 1.21 A fl anger! AWCB’ H 9666716”! AMI I o flew GMM [‘[0‘4 leE/Cc QI‘Nfi 7M7" deem/u N _ Mt . C . 1.13! ~ 0. ”I? new) (v I' o lee/”020” H \ <10? 7’07” MUD; H’ [0?0 [3’ We Tenth/£14 AN‘LQ KW Problem #1 (The Shapes of hiclecules) (30 points) Predict the geometry of each of the following molecules and ions. Describe your reasoning in terms of the VSEPR theory. Draw the resultant structure for each. Using words and/or sketches, be careful to indicate any distortions from otherwise symmetric shapes. If bond angles increase or decrease relative to those expected in highly symmetric structures, be sure to indicate the direction in which they change. (a) Xe03 (c) BrO; (d) PF'6 (f) OI4 mate ’0 ‘39} meat Lem es mm ID?" Seesaw (low—energy, favored) ZethXQ 29: To 649” DIV/Em“; CPA V/‘Nfl / 3N: {a WWAP’C- .94”? Ad“ Aware Ame fA/‘fl T / JRWZc/e fimfl fiWflem, — coma / e 2 120i 00 XX / gmao§ XX Problem #2 [Molecular Orbitals in Diatomic Molecules] (30 pts.) When one electron is added to an oxygen molecule, a superoxide ion, 02, is formed. The addition of two electrons gives a peroxide ion, 0%". Removal of an electron from ()2 leads to 0;. (a) Construct the correlation diagram for 0—2. 9* ~9r< 99 —@—«< a @251 0 0; ’3 0 (b) Give the molecular electron configuration for each of the following: ()2, 02, 02, 0%— 01 (a) (as c 29071,)‘T7r )’ 0a (on) ME?) (02993): (17);? 7729 02; (021} 6&5)’ (0» #91) C759" 07779) t WW C aft/am) (c) Give the bond ordel of each of (09%)(0219 (a; 3/9 (a: 0 (d) Predict which of these species are patamagnetic. QJLQr W OZ one (6) Pl‘CdiCt the order of increasing bond dissociation energy among these species. ~ « + 03 fl; 02 (92 Z _) J J . 7 W fl, Problem #3 [Chemical Bonding: Short Questions] (30 points) (a) An‘ange the (four) hydrogen halides in order of increasing bond energies. ”HI pHfln “£93 ,t/ee //F (b) Which IS more ionic, CsF or Nal‘? Exp in terms “t9“ electonegativities. CSFM WWW yc1s~<yre~ OAK/>74; (c) Since there is always a net energy cost in forming the positive mm and the negative ion which make up a highly lOIliC diatomic molecule, how, then, does an ionic bond between them form? 77¢ MWWW MW ((1) List the tlnee types of chemical bonds and for each define it in terms of open shell/closed shell interactions. O 0%} [3057/ WM m M’ 1,1. 1 g _ M Q >1L021Iic 3% $19M 1, (1W>Qo€fl%¢f 8 (Wm “’ my (6) Sketch the geometly 0 each of the following molecules; CH4, H20, NH3, and C02 and ._..'-—-v indicate the total dipole moment, it, vector direction for each. Use the convention in which the head of the dipole moment vector arrow is the positive end, and the tail of the arrow is the negative end. If it is zero, so state it. H" 01/4: ”6 W 0 ‘l Problem #4 [Transition Metals/Coordination Complexes] (10 points) (a) Treatment of cobalt (II) oxide with oxygen at high temperatures gives C0304. Write a balanced chemical equation for this reaction. What is the oxidation state of cobalt in C0304? 6 COO + 02 —> 2 00304 I The average oxidation state of Co in 00304 is g. This corresponds to two CO3+ g Q“ and one 002+ ion. (b) Determine the oxidation state of the metal in each of the following coordination complexes; Mn2(C0)10, [R63B1‘1213‘, [F6(H20)4(0H)2l+, [C0(NH3)4C12]+- The oxidation state of Mn in Mn2(CO)m is zero; the oxidation state of Re in [R63BI‘12]3— is +3; the oxidation state of the Fe in [Fe(H20)4(OH)2]+ is +3; the oxidation state of the Co in [CO(NH3)4012]+ is + 3. end of exam ...
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