calc_lab - Lab Practical Name: Chemistry 114 Spring 2010 1....

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Unformatted text preview: Lab Practical Name: Chemistry 114 Spring 2010 1. For each. of the following give 1) the most appropriate Lewis structure, 2) all resonance structures, and 3) formal changes for all atoms having any. a) nitric acid, HNO3' 10'. i ' " u u Vin/51% ', H-0-)p-o: 5mg: utzfir— 311: ~ + ~- (bomb: gonad—.1012: 51:59 A _ Long: 1+ 10’- MIL" “TEL? it ‘k/vwdlses mlowm H La 1m 0? W E ' u “‘3‘ loam») Wade» Alflaom , tillég’ m- H — t)— !0 1 O . ‘ + I b) hydrogen phosphatei n, HPOE’ VFW; Elili Hg pod/{vs a?“ E) \v‘ 4 _‘ ’ Wt ‘A’O-rp’o.‘ :7 H,O_,3-r0 ' ' " ' a .w M“! :0: yo 2:7 Vggg “ ' a .' . 4-0'Q—«0‘5. com: 5 «Jam ‘ p 2. 2. For the following molecules, circle those which have a dipole moment. \ O I ea {Jive—flirt? - i) 20>; a) CH4 Sear-q c Br4 5mg SWL =7 LWENL') 85:35? ‘ 16mm: 3 so: L19) TE’YIZAlol-ébafirk‘ PC12F3 does not have a dipole moment. a) Use VSEPR to. predict, and carefully draw, the structure consistent with this data. Wu viola: 2w Yak/Le» . . a a ‘ I ‘ f"! P? {9 SF? ‘ ‘ " b) Why does your structure have no dipole moment? (‘X~P~% v5 KMW :m hm Wafiéfi 3) V";- Mr ‘5?" an 'e CS sncag G) stfiau: 3 $13 15:? mlflQfib b‘xwaammmv -2- 4. For each of the following give a) the electronic geometry-(electron—group arrangement) for the central atom, b) the molecular geometry (shape), c) all bond angles (when distorted, tell if angle is greater than or less than VSEPR prediction and give the prediction), and d) draw the best three-dimensional structure (omit resonance structures and omit drawing lone pairs of electrons on outer atoms but include them on the central atom). formula distortion (Fm 963Fch vsevasame) MT DETWA’B watt of MM/ @45er We" MT blsTble "imam:th Emu— fLPsWh DEL; 61cm ’ HE‘DYM L. fimmtom. Maw 17%“ mm flaw paws: bl) 9)) M, 03%)} £3) . -3- 5. For each of the following compounds 1) give the hybridization of all atoms marked with a large dot, 2) describe all bonds between numbered atoms, and, if present, 3) circle the portion of any molecule which is conjugated. a) lamb l‘l'. W: C, P”)? Era. 1" ’- cF¢€Q?G 9W ..sp3 6) sH o C'IH2 (I? (IIHZOH HZN—(IZH—g—‘NH—CH—C—NH—CH—COZH CH3 ’5) gram; Spa 1) 5 C\I—I3 5921 spit O/C=C=O CH3 k) 0 H o CH3—C—NH2 b) o 0 ' - ll . ll CH3—C——O——C—CH3 d) O\\ 1’31... 2‘. (fr—RCIHCHQZ ¢$Ffzyl CH C—— ( 3h. C\\O 81:3 f) i h) j) 1) -4- 6. a) Give the ground state electron'configuration of an oxygen atom. b" 1&9" a?“ b) Is an oxygen atom diamagnetic or paramagnetic? Why? megmfiie - A. 52M, ghng 0) Draw the Lewis structure for 02. vmez mittens d) The following is the molecular orbital (MO) energy level (correlation) diagram for the valence electrons of 02. Fill in the valence electrons and completely label the diagram. 2 .- "- 05 __ (mtg wémw w “3, {1* benefit- (9&0qu « “Pr bruimg. JMWKJ$> -5- 7. a) Give the ground state electron configuration of a nitrogen atom. 15%" Rag 9?3 b) Give the ground state electron configuration of an oxygen atom. ’L “2.- la . u 9‘5 N , . 7» 0) Draw the Lewis structure for NO‘. " N : O 5 ,q ., 39214) : \hqxwkg, (9+5-(—l\)5 M .3 " d) The following is the molecular orbital (MO) energy level (correlation) diagram for the valence electrons of NO". Fill in the valence electrons and completely label the diagram. t0 «We \“\’3Lv ‘ 3.2:. M16» 0 mm. “m” (E15 0 awe 6) Fill in the following table “‘7 “fig” Wm ' Wmilfiie bond order m— 9 f) Circle the species with the longest bond: NO NO+ paramagnetic (y/n) -6- 8. Consider the compound CHZCHCHCHZ with the four C atoms forming a chain. a) Determine the number of valence electrons. VMX“ Li“! )+ (a: 9.9.. b) Draw its Lewis structure. 5% a a \ 0/";— Qd\ / H 14 ’ (L T» 0 \ H ’ H '0) Give the hybridization of each carbon atom. (1) Which bonds are 0' bonds? 016'- am C—H) 3 (:«c/ e) How many 0' electrons are there? . a (l): lg f) How many 7: electrons are there? mm 1% w 9% g) Each 7: electron is initially in an unhybridized carbon p orbital. How many 7: molecular Ll sp“ 0/ t M mo’s h) Draw the a molecular orbitals, clearly showing all nodes. Number the MO’s and label them as bonding, antibonding, nonbonding (all need not apply). orbitals can be made? ' i) Draw a line for the energy of each 7: MO ordered from bottom to top with increasing energy. Number and label them as you did for part h. Fill with the 7: electrons and indi- cate the HOMO and LUMO energies. Is this molecule diamagnetic or paramagnetic? Why? VAL fill] Ea «Sigma: .«zi W " Ll z; [2} Lame p _ - l3 Ea. 14/me Diamaawmle» M e!” 3 6 ll; PWQED ' j) Circle the description which best fits the molecular orbital which contains one node. nonbonding antibonding -7- 9. Consider the ion NO; which has equal N — 0 bond lengths. a) Determine the number of valence electrons. VR’L, “v 5 A: gig} .. La ['3 = l (2' b) Draw the Lewis structure including all resonance structures. , l R) " I” \ \ " v at” \ \ Q. ‘0‘: “ “a \ ‘D \ .I c) Give the hybridization of the nitrogen atom and the molecular shape of the ion. 3 pl ') mm d) Which bonds are 0' bonds, what orbitals are overlapped to form them, and how many electrons are involved in the sigma bonds. EEC/R we Has A game imam F-eum engrave? or: 5??» on o {MOD 532100 0 $16” {3; ate); Ll Gene e) Which atoms have eleCtrons isolated on them (i.e., lone electrons) and give the total'num— ber of such electrons (be sure to interpret your resonance structures carefully). to HA5 \mm? PM; (we give—cu e We a.» mega wmea‘fiwes" ID mmww .13 Peer W T.“ 5:15ng“? ID D Show how molecular orbital theory provides a description of the equivalent bonding to oxygen that is different from the use of resonance structures by constructing delocalized 7: molecular orbitals. To do this: 1) Determine the number of unhybridized p orbitals. 3 2) Draw the 7: molecular orbitals, clearly showing all nodes. Number the MO’s and label them as bonding, antibonding, nonbonding (all need not apply). EDUDWOQ 1001) whine 3) Determine the number of 7: electrons. \‘8 \ Ll v \0 w, L} 4) Draw a line for the energy of each 71' MO ordered from bottom to top with increasing energy. Number and label them as you did for part h. Fill with the It electrons. ‘ 21a“ 19 ‘W 3mm E} 32.45;” ' a “ Ti" e; Pan Um fiewhiflé mama 5) How does the MO description incorporate both "resonance" structures from part b? we same. “(WOW Tr {Sewn :3 Deteea'cteefe (New, 0 DO We THM' we: “ Lime" Page m3 0 » H106;- euom Weeeeww w at? W amen, emcee ...
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This note was uploaded on 04/13/2010 for the course CHEM 114 taught by Professor Jursich during the Spring '08 term at Ill. Chicago.

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calc_lab - Lab Practical Name: Chemistry 114 Spring 2010 1....

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