CHEM-100 [Aronson] Test 1-2 (Summer 02)

CHEM-100 [Aronson] Test 1-2 (Summer 02) - Kettering...

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Unformatted text preview: Kettering University CHEM 135-05 Summer Term, 2003 Professor C. L. Aronson Exam #1 August 4, 2003 _ Names/7%.- Her 'E . ,x. You fl use a calculator. Please circle the best answer and be sure to utilize the en'odic table attached on the last a e. Note: I poimper answer. . Which one of the following represents a chemical change? (__a_}__boiling water to form steam (b) bleach turns hair yellow " (a melting butter (d) mixing powdered zinc and sulfur at room temperature (e) cutting a bar of sodium meta] into pieces with a knife 2. All of the following are properties of sodium. Which one is a physical property of sodium? {3 It is surface turns black when first exposed to air. 9/1 is a solid at 255C and changes to a liquid when heated to 98"C. (C) When placed in water it sizzles and a gas is formed. (d) When placed in contact with chlorine it forms a compound that melts at SOICC (e) none ofthe above 3. The diameter of an atom is approximately] x 10‘5 cm. What is this diameter when expressed in nanometers? (a) 1 x 10"?nm (b)1><10"’ nm (0)] x 101nm ((1 1x 10'IO nm _ l x 10'] nm 4. Express 7.500 nm as picometers. (a) 150 pm (12075.0 pm (c 7'50 pm sex (@725 x 106 pm L) e) 7.5 x10” pm Dr. C. L. Aronson Exam #1 CHEM 135-05: Summer Term. 3003 Page 1 5. The melting point of bromine is —7CC. What is this in CF? (21)] (b)2 (e) S 7. After carrying out the follovting operations- h0\x-=mar1_\=signifieam figures are appropriate to show in the result? 2.6+0.019 9.221 (21)] £222 (-678 $254 (a) 5 8. The density of mercury is 13.6 gt’cms. Ho“ many quarts does .100 g ong occupy? '3 Given 1 L: lilo qt. H, ’ ,F-QT -" “t? ‘Z ’ 1 {I 1‘ a s (a l44qt ’ fie” ',3__/v .79 X 10" qt 9‘ tc) 'i'.?9 qt _ (d) 6.94 x 10"" qt {6) 1.44 x104 qt (a) — 12.6"}: (b) — 28.] CF (c) 19.4“F 39 CF W of them are within 2"F of the right answer 6. A thermometer scale is calibrated (marked off) in tenths of a degree Celsius from ICC to 50.0 "C. Determine how many significant figures should be used to express the outdoor temperature if that temperature is between 1°C and 9°C. Dr. C. 1.. Axonson Exam #J CHEM 135-05: Summer Term. 2003. Page 2 W 734-91 U 9. How many cubic centimeters of ore containing 0.229} by mass gold must be processed to Obtain $100 \\ orth of gold? The density of the ore is 8.0 gz‘cm“ and the .‘ price of gold is $418 per troy ounce. 14.6 troy oz : 1.0 ordinary pound, called an ,__a— avoirdupois pound. and 1 lb 2 454 g. - [:5/ (a) 42 cm? ‘ ’52”? L -- -\ s (b) 2.? x 10*1 cm’_ W ' t, @120 x 10;ch I \ Ml 6.200 cm" A I. I (L? fight-rt”. .. r' L}, (e)9.3x 10"cm-' ‘tjlt.//5f_r//’5 l L35 I. Q60" #0 10. The elements in a rout of the periodic table are known as: (a) metalloids. period. c noble gases. (d) a group. (e) nonmetals. r355; ll.Which of the following elements is most likely to be a good conductor of electricity? (:1) N (b) S (c) He (1) Cl Fe 12. A cation is defined as: (a) a stable atom. (b) a charged atom or group of atoms with a net negative charge. __ a group of stable atoms. an atom or group of atoms with a net positive charge. (e) none of the above. 13. What percentage of the mass of a fluorine-19 atom is contributed by its electrons? Given the mass of an electron is (1H 83.6) amu. (a) 50.0 (b) 0.236% {c 33.0% tel) .0269} e 99.96% Dr. C. L. Aronsnn Exam #1 CHEM 135-05: Summer Term. 2003 all Page 3 l4. Atoms of the same element with different mass numbers are called: (a) ions. {13) neutrons. (c) allotropes. (:1) chemical families. [ [episotopes 15. How many neutrons are there in an atom of lead whose mass number is 208‘? ta‘ 82 @126 't )208 M1290 (e) none of the above 16. An aluminum ion. Alt". has: {a} 13 protons and 13 electrons (b) 2? protons and 24 electrons (c) 16 protons and 13 electrons protons and 10 electrons (e) 10 protons and 13 electrons 17. Which ofthe folloMng pairs of elements would be most liker to form an ionic compound? (a) and Br J Cu and K C and 0 (d) C] and Fe (6) A] and Rb 18. Which is the COITCCI formula for coppertIJ) phosphate? (3) CogPOs te1CutPOsli Dr. C. L. Aronson Exam #1 CHEM 135—05: Summer Term. 2003 Page 4 19. The chemical name for C105 is chlorite ion. Therefore. the name of HClO: is: ydrochlon'c acid " ‘(' )chloroform (c) hydmgen dioxychioride (d) chlorous acid (e) chloric acid 20. The correct name for KSCN is (a potassium carbonate. potassium thiocyanate. (c) potassium cyanide. (d) potassium sulfur carbon nitride. (e) calcium bicarbonate. 21. The Stock system name for Mn307 is: (a) dimanganese heptaoxide. (b) magnesium oxide. r manganeselfl) oxide. e) manganesetlll) oxide. anganeserI) oxide. 22. The stock system name for CrSOi is: (a) chromium sulfide (ll) chromium {11) sulfite hromium (11) sulfate "(-d chromium (III) sulfite (e) chromium sulfur oxide 23. An atom of bromine has a mass about four limes greater than that of an atom of neon. How many grams of neon will contain the same number of atoms as 1.000 g of br0mine‘? (a 4 g Ne (Sign) g Ne "(c 400 g Ne (Cl) 1,000 g Ne (e) 4,000 g Ne Dr. C . ]_. Amnson . n}. t7, 3 i“ ‘ Exam #J CHEM 135-05: Summer Term. 2003 Page 3 34. What is the mass of one copper atom? @2055 x 10‘: g l 63.55 g (c) l amu fl [(1)166 x tO'f‘ g m 9.4?6 x 10~1 g realest number of atoms? ‘1 25. Which of the following samples contains the n’ "/1 .L] 5 moi; eta .100 g of Pb E Itb;2.0 mole of Ar , e .. .f 1‘6) 0.1 mole of Fe 1.71; (d) 5 g of He 1e} 20 million 0; molecules no k-r“ 26. The molar mass of aspirin is 180.2 gfmol. Ho“ man} aspirin-molecules are present in one SOO—milligram tablet? W) my) “of (a) 2.3"? molecules -| (b) 2.77 x 10" molecules ' c] 1.67 x 10:4 molecules "(d 1.6? x 10: molecules (e) None ofthese is correct. 37. How many grams of sulfur are there in 6.0 g of 1363604)}? (a) 2.40 g _Ot"f,.-, " (b) 0.48 g (c) 6.00 g 23. The element oxygen consists of three naturally occurring isotopes: “‘0. 170. and “30. The atomic mass of oxygen is 16.0 amu. What can be implied about the relative abundances of these isotopes? (a) More than 509? of all 0 atoms are I70. (b) Almost all 0 atoms are 180. (c) Almost all 0 atoms are 1’0. (d) The isotopes all have: the same abundance. tie. 33.39}. @ The abundances of I O and 1“20 are very small. Dr. C. 1.. Amnson Exam #1 CHEM 135-05: Summer Term. 2003 Page 6 ll 29. The empirical formula of a compound of uranium and fluorine that is composed of 673.69? uranium and 32.49“? fluorine is: (a) use {j i: (b) U333: _ UR: at» ( E) U123 30. What is the coefficient for 03 when the following combustion reaction of a hydrocarbon is balanced with the smallest set of whole numbers?. LC‘Hitt+;O:—>_ZCO:+_$HZO ll?) ” .r. "E {c} 10 ' (d) 21 (e) 36 3]. Balance the following equation. then add together the coefficients. The sum of the coefficients is: LSF‘I-Fil‘lgo —>_L 1435034r in? (a) 4 H (Hi. (b) 6 t t; (c) 7 so @9 32. When 22.0 g NaCl and 21.0 g H3504 are mixed and react according to the equation below. which is the limiting reagent? 3 NaCl + H2504 ~+ Nesso.1 + ZHCl ' ,. 73L €it.{,,.c.i t? e { aCl . - 1" r I. ’I‘.- .{ilfr < .II.. I I Jr _ (C) Nagsoa I 3 Email {I}; L EH H__LF-—t—T A). —(( —_ . 'fyrflo/é- guilt}. (d) HCl .ti (e) Neither reagent is limiting. Dr. C. L. Aronson Exam #] CHEM 135-05: Summer Term. 2003 Page T 33. When C3313: is treated with water- the products are calcium hydroxide and PH;. What is the maximum mass of PH; that can be prepared from 2.00 g of Cang and I . 9 Es . ‘ _ r . L rn. (3)0.0185g f/ 0‘5 i Z . . (1:00.187 52 gm 0.630 g \a . (- .‘. - ill/O‘Emol (“i '3 {e “ 5 El c’ 34. A student prepared bromobenzene. C(J'JfiBr, by the reaction of benzene. Col-lb. with bromine by the reaction: C(BH-b + BF: a C6H5Bl‘ + J'IBT. The student specifically reacted 20.0 g of benzene with excess bromine and obtained 28.0 g of bromobenzene. What is the student‘s i5Ft-_\*iels:l of C¢H5Br3 i®9aa - 2"“ ” ‘J lb) 57.0% (c) 30.4% (d) 75.6% (e) 36.49% (a) 0.037? M (b) 1.39 x L - x 10'” M .0152 M 36. A solution has a density of J .46 gfml. and contains 655 g of potassium hydroxide per liter of solution. What is the 11135592: potassium hydroxide? (8)1059? .- ..(//_ ,_ ’5? HO.» £34» I ,_ ($62.95;: (, / 0 (638.4% ,4" " {57/0 I 35. A 1.00 g sample of sodium carbonate decahydrate was initially dissolved in 20.0 m]. of distilled water. Additional water was added so as to yield a total 250 m]. of solution. What is the/molar concentration of sodium carbonate“? /’ ,/ I Dr. C. L. Aronson Exam #1 CHEM 135-05: Summer Term. 2003 Page 8 37. A sodium chloride so]ution is prepared by mixing 3.65 L of 0.105 M NaC1 with 5.1] L of 0.]62 M NaCl to give 8.76 L of the new solution. HOW many grams of NaCl are contained in 1.00 L of the new solution? "7 y WV ' ., 1 I P 2 _ 235?”;7‘ «b ts‘é‘zfl H AZJ'WOF “ L 38. Calculate the molality of a 20.0% by mass ammonium sulfate solution. The density ofthe solution is 1.117 gme. - x , l (x/u 1-! ,J r- =- (a) m LIKE/x. a. ’1 (b) 1.5] m . if I Z h”: [I 1th ! I i_ .;_ \1 t ' ' ' J 39. Calculate the mole fraction of methanol (CH30H) in a 20.3 M aqueous solution. The density ofthe solution is 0.858 gme. (a) 0.858 . '~ 1, (100.12? (C) 0.2 .637 .762 40. What volume of 5.07 M stock NaOH (aq) solution would you use to prepare 2.00 x 10‘ mL of 0.866 M NaOH (aq)? age/o - 5.07. C, (d) 90.1 ml (6) 0.222 ml Hr Dr. C. L. Aronson Exam #] CHEM 135—05: Summer Term. 2003 Page 9 I 1! I l—Atomic number 1 e. D Melal C — gymbol D Sermmetal W“ D Nonmetal LMomvc 11.19.1911? ' 22- Ti 4766 39 4O 1' '12 N a g 2 99 21,3 19 2c: 3910 .1 05 . Rh 3' o 7 8 23 24 25 ZE- V Cr Mn Fe 50 94 S2 00 54 9t 55- 85- 41 4s (IV 36 105 Lr 26211 '1 61 62 as 94 (-1. La Nd Sm Eu Gd 1 136.9 1“ 2 14s 9 15011 152: 1 - 91 92 93 -4 95 "‘ , ' 2:11 o 2:15 o 2-97 0 2-“ 1 243 1 Dr. C. L. Aronson Exam #1 CHEM 135-05: Summer Term. 2003 - .- - 1. ' 1 5-5 39 69,72 - .’ '~ 43 44 . 49 5-1 a m 54 Y ZrN‘bMoTc RuthdAng Sb Te . 85191 91722 9291 95 94 98791 10191 “'39 105-1 101-9 112‘ 114.3 12178 127.6 126.9 131.3 - 71 72' 73 74 75 76 177 78 79 SCI 61 62' 63 5-4 65 85 ’ 175.0 1755' 1809 153$ 1862 190.2 192.9 1951 19770 2009 2041 207.2 20970 20970 2100 2220 104 105 105 107 108 109 110 111 112 Rf D1) 83 81: HS Mt Uun Uuu Uub 25191 262‘ 1 953 1 2‘64 1 265 1 25-3 2‘59 2‘72 277 1 1575 152.5 164.9 I} 14 15 16 l7 s E- 7 9 g 1091 12.01 1401 1900 13 14_ 1 s- 16» 1': A] 31 P 8 Cl 25.95 28- 09 so 97 32 or 35. 45 1 M ,. _ 34 :5- Se Br 78 96 79 90 1 1 4 116 Uuq Unh 289 25-9 66 67 68 E? 70 Dy Ho Er Tm 1 30 1671) 156 9 99 100 101 E3 Fm MI? 2529 as: 1 255 K, Page 10 1 Ne 201$ 18 Ar 39 95 3E- I 8? ,80 D (01992 on,“ de1 September 3, 2003: Exam #2 Kettering University CHEM 135-05, Summer Term, 2003 Prof. C. L. Aronson ,_~ Namezr“ J r.» {THC _ f 5" "L Circle the best answer for multiple choice problems. Please use a calculator, attached list of equations and periodic table. Note: each answer = 1 point (60 minutes) (1) Which one ofthe following is most likely to be anionic compound? ; aAs //—‘ SrBrz /. : (cmog 0 (d) C1311; (e) H30 (2) Complete the following statement. Coulomb’s law states that the magnitude of the energy of interaction between two charged bodies is: (a) directly proportional to the product of the charges on the bodies and directly _I_ l‘oportional to the distance separating them. @irectly proportional to the product of the charges on the bodies. and inversely roponional to the square of the distance separating them. (c) inversely proportional to the charges on the bodies, and directly proportiOna] to the ,__ square of the distance separating them. mii‘ectly proportional to the product of the charges on the bodies, and inversely "w/ proportional to the distance separating them. (e) none of the above. (3) Which of the following atoms or ions has the largest radius? (a) Ar flycd-H-Jfiffi (b er _ 1 - (9.) r' fwd”? p.15 . M.) ‘ ” “(tn K: .23” q it; - '\ (6) Sr '+ (it: . I 4;. If: ix .IX. \ .Ill I : L, 51 \ \~ \\ VJ, " Dr. C. L. Aronson CHEM lBS-OS, Summer Term, 2003: Exam #2 Page 1 (4) The Lewis dot symbol for the selenide ion is: 2. (c) Se 2- (d) —~Se— (C) .' Se— (5) Which of the ions listed below has the largest radius? (a) Na + (W Tc) Ca ’"+ ((1) Cl ' (e) F ' (6) Which of the following solids would have the highest melting point? (c1) NIng (C) KP (7") Which of the elements listed below is the least electronegative‘? 3? (a) Sr (b) V 5 (61 Dr. C. 1.. Aronson CHEM Ufa—05. Summer Term, 2003: Exam #2 (8) A polar covalent bond would form between which one of the Following pairs of atoms? (a) Cl-Cl (b) SinSi _{c Ca-Cl fir-Br '; e) C] (9) What type of chemical bond holds the atoms together within a water molecule? (a) Ionic bond (b) Nonpolar covalent bond olar covalent bond d) Hydrogen bond (6) None of the above (10) A non-polar (pure) covalent bond would form between which one of the following pairs of atoms? (a) Na—CI (b) H-C] (c) Li-B d SewBr Br-Br (l 1) The covalent bond with the greatest polarity would Form between which of the atom pairs below? «(ea—81%?- (b) 8—0 (c) C—P (d) C-0 (6) -O (12) The electron dot formula for Sbl] shows: (complete) (a atotal of210 electron dots . - - ~ I - - x“ )t ree single bonds and 10 lone pairs _' ’ T .' 0 two single bonds, one double bond, and 9 lone pairs (d) one single bond, two double bonds, and 8 lone pairs 2 (c) three single bonds and one lone pair ’ . Dr. C. L. Aronson CHEM [35-05. Summer Term. 2003: Exam #2 Page 3 (13) The Lewis structure for the iodate ion,103 ' should show single bond(s), — dOUble bond(3), and lone pail-(s). (a 1", 10 ' I ’ . .- glfigjiOfi _ Ajfl _ - (c) 2, 1, s . T 1/(d) 3, 0. 10 I (6) 2, 1,11 i 1:): (14) In a molecule of formaldehyde (HZCO), the total number of bonding electrons is and the total number of nrm~bondin g electrons is (15) The formal charge on the sulfur atom in the resonance structure of SO: which has one single bond and one double bond is: (a O .1, /' _ _ c. (531 s3 #0- 64 _ . t (d) +2 (e) —2 (16) Each of the three resonance structures of the nitrate ion, N03 ', has how many 6 pairs of electrons? I‘_.~r.. _ 1 Jr" ' 1 )s '-:_,)H'r’|'\,"‘“ (C) 9 _ _ t- ((1)10 E (e) 13 ; (1'?) Which response includes all the molecules below that do not follow the octet rule in their respective Lewis structures? f—‘r-w. J -—"'—"'—:::\\ amaze l/fziBCl'; We; (4) ea 212,3 'b) ,4 c)1,2 ’7}. (“i (d)3,4 xii—1b tr (e) L4 (' «if— 67 Dr. C. L. Aronson CHEM 135-05. Summer Term. 2003: Exam #2 Page (18) (51) ns (b) ns (1) ns (6) ns (19) s m to H N I.) J The general electron configuration for atoms of all elements in Group 6A is: ( np’ 5 TI p4 1113' Which of the following is the general electron configuration for the outermost electrons of elements in the alkali earth metal group? (c) ns‘ np‘1 (cl)ns2 rip5 (eons3 np" (n—1)ct6 (20) Which one of the following make an lsoelectronic pair: Cl ', 0231:, Cat”, Fe“? (a) Ca3+ and Fe3+ .F (b) " and F F and Cl ' d) c: ' and Ca3+ (e) None of the above (21) (21) Al 90:) P (c) As (22) Dr. C. L. Aronson Which of the elements listed below has the smallest atomic radius? Which of the following elements has the smallest ionization energy? CHEM 135-05. Summer Term. 2003: Exam #2 Page 5 (23) Which of the following atoms will have the greatest electron affinity (largest positive value)? (c) As ((1) Ar (6) I (24) Which of the elements below occupies a position on the periodic table that is not consistent with its chemical properties? * He “(c/i Ar (d) A] (e) U (25) Which of the following substances is being considered as a replacement fuel for gasoline? flDgO - (b),H2 to No; (d) E: (c) He The electron configuration of a Co3+ ion is: ( 26) (e) [Ar] 453 3d” fi (2?) The maximum number of electrons that have the following quantum numbers are: Ml—ms 4 3 Q '/2 (i1) 0 ..———(‘o) l c) 6 e) 10 Dr. C. L. Aronson CHEM 135-05. Summer Term, 2003: Exam #2 (28) A possible set of quantum numbers for the last electron added to complete an atom of germanium in its ground state is: 1 4 0 0 + 1/2 (El- __3- —0 +1 _ 1/2 ...——-(c) 4 l -1 + 1/2 _(t1)_._._3__.. _.1 +1 — [/2 (e) 4 2 +2 - 1/2 (29) The maximum number of electrons that can occupy an energy level described by the principal quantum number, n. is: (a) n (b) n+1 (c) 211 \(d 2113 (e) n2 (30) How many orbitals are allowed in a subshell if the angular momentum quantum number, m, for electrons in that subshell is 3? {fl 1 ‘ (1:03 (c) 5 ~=——- (d) t (a) 9 (31) The ground state electron configuration for an atom of calcium is: .J t W95;— (9 [Ar] 45‘ 3d' xfcti‘jmr] 452 Te) [Ar] 3d2 -.I I (32) What is the energy injoules of a mole of photons associated with visible light of wavelength 486.1 11211? f. J22. (a) 6.46 x 10"‘jJ "’ fl It. (b) 6.46 x 101% —- a? p 92;r,_.___,__._:,23 (c)2.46>< 1041 E 5-” " trig; J, mag) “ ' (d [2.41:] J ‘ €§246 k1 - ELK?" Dr. C. L. Aronson CHEM 135—05. Summer Term, 2003: Exam #2 (33) Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n : 6 to the n = 3 principal energy level. (a) 1.64 x 10% (b) 9.13 x 10‘3rs (c) 3.65 x10'4fs 2’; i J. 8/5! 7.176)“? (d) 1.82 X 1049.15 W6 KHZ" 14 - 41 4—7,? .7 @‘mxlo KS 4.1: 36; .2119“ "J’, > f ' 31"» (34) The orbital diagram for a ground state oxygen atom is: is 2S 2L ‘(ar-——T¢—___....---.. .. m. . . T T T 3 (b) Ti Ti H Ti Ll -— -(c)—--——’t:L--~--- m an T .. 3... or H Ti Ti T T Li (6') Tl-‘v- t-i- -- m- m t 3f (35) n atom of iron has unpaired electrons and is . diamagnetic (b) 6, diamagnetic ' (c) 3, paramagnetic (cl) 5, paramagnetic -9(e) 4, paramagnetic Dr. C. L. Aromon CHEM [3505. Summer Term. 2003: Exam #2 l Extra Credit (36) The flotation process used in metallurgy involves: a roasting of sulfides ."$fieparation of gangue from ore. c) leaching. (d) Chemical reduction of a metal. (8) zone refining. (3'?) Metallic potassium is obtained commercially from molten potassium chloride by: (a) chemical reduction with magnesium. (b) flotatioa. (c) ele rolysis. (w one refining. fling. (38) Three means used to concentrate ores are flotation, ferromagnetic separation, and amalgamation. (a T e False (39) The Hall process involves the reduction of A1303 to aluminum (Al) by: (a) carbon (coke). (b) carbon monoxide. (c) molecular hydrogen. ((1) sodium. @lectrolysis. N.._/' (40) Aluminum hydroxide Al(OH)3 is: (a) an acid. 461) both (a) and (b) (e) used primarily to make amalgams. Dr. C. L. Aronson CHEM 135-05. Summer Term, 2003: Exam #2 Page ...
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This note was uploaded on 04/29/2008 for the course CHEM 135 taught by Professor Aronson during the Summer '02 term at Kettering.

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CHEM-100 [Aronson] Test 1-2 (Summer 02) - Kettering...

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