Exam 3 - CHEM 1314 Exam III John III. Gelder , April 5,...

Info iconThis preview shows pages 1–6. 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
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: CHEM 1314 Exam III John III. Gelder , April 5, 2005 1 Lab Section INSTRUCTIONS: 1. This examination consists of a total of 9 different pages. The last two page include a periodic table, some useful equations, a table of standard enthalpies of formation and a solubility table. All work should be done in this booklet. 2. PRINT your name, TA's name and your lab section number no_w in the space at the top of this sheet. DQ NOT SEPARATE THESE PAGES. 3. Answer all questions that you can and whenever called for show your work clearly. Your method of solving problems should pattern the approach used in lecture. 4. No credit will be awarded if your work is not shown in problems 5a, and 5b. 5. Point values are shown next to the problem number. 6. Budget your time for each of the questions. Some problems may have a low point value yet be very challenging. If you do not recognize the solution to a question quickly, skip it, and return to the question after completing the easier problems. 7. Look through the exam before beginning; plan your work; then begin. 8. Relax and do well. Page 2 Page 3 Page 4 Page 5 TOTAL SCORES it. & i % (3’2) (21) (23) (24) CHEM 1314 EXAM III PAGE 2 (12) 1. Write the chemical formula(s) of the product(s) and balance all of the following reactions. Identify all products phases as either (g)as, (l)iquid, (s)olid or 320%. A l a) 35(OH52(aq) + HNOémq) —>;J Hang-5w 5 J~. b) Néorimq) + FéENo3)3(aq) —> N»? , c) Km + NM) —> aLLt‘ I“) d) Na2C03(aq) + Htlqur'll/‘qgiéwié‘fil 1L wit (4) 2. Write the ionic and net ionic chemical equations for 1b). 1b) Ionic equation: I» ,, m K N 1, N y . : ' ,, 3.2;! g} g; Net Ionic equation: ,I ,V {l (A it V , u = C t, ; OHM?) ’r Mm; 3) z (12) 3. Write the complete electron configuration and indicate the number of unpaired electro for each of the following species in their ground state, / i. “Si M 7/‘f X22: unpaired electrons i§L I 30/, . ‘ xix/5‘? l ii. Co -3 a 5 )3 6, I}! unpaired electrons 255% a. ‘4 fr 5 #41? /e \ a»; i K \2 iii. Dy (atomic number 66)_k v“; unpaired electrons ’2 t t'i I.» l (4) 4. Draw the orbital diagram for the yalence electrons in P. [/7 7 x” “4’8. 72,3?» '3 --~~ J“ Page}? / CHEM 1314 EXAM III PAGE 3 (14) 5a. The energy required to break a carbon wchlorine bond (C—Cl) is reported as 328 kJ mol'l. Calculate the energy require to break one C—Cl £4) a W Mw 'g/i tzwirw‘“3t®C2W/O will «It i t '20 b) Calculate the wavelength (in nanometers) of a photon of light that is capable of breaking C—Cl bond. (10) 2{1/ é? Mf\ f/k, _, C s‘ l 4 Vi a ! L (y) \x / ,V ’ , t l ' 0% n 31/ gt / , L 3 2" r / [1 a l., (18) 6a. In the space in the box draw an energy level diagram that shows the transition an electron would undergo when a hydrogen atom emits a photon of light. Provide a brief explanation to support the information provided in the box. (7) CHEM 1314 EXAM III PAGE 4 b) Without doing any calculations explain how you would determine the energy of the photon emitted in Pa“ ‘0' (6) p, A53 .E‘i .3 lzglé/«l \ Mulg (1538 flu? £9me ’3’ If»? ,1; j I f Malia g MC} " " ’ ‘ (A.th Maw 50‘“: (WW ‘3“ “ ' 1F§ /4/[u.la“3fl’3 9%“ COMET??? U .( o 4 Nat tea. 7 C) Would the energ that is calculated for the transi ' othermicZExplain. I}. p , I If»: ital?! ! 9‘: fl jig. ’3: V490" $5 r“mf-W’é”;’ (12) 7. Explain each of the following. a) The atomic radius of S i V ' ller than the atomic radius of Se. (6) i ” '3‘“ :‘fli‘ ‘ b) The first ionization/egg’y of Mg is smaller than the first ionization energy for C1. (6) ’l r» l A my in ‘pa fl. lug?" lI‘X flaf huv‘ V ’ 1/“ 51???? 3%" l‘ g r 2 ~ 7 “‘1 eh i “may! (in filg’x“"§r’§fli‘é“~- ‘5 will“? LL/jLUO/ ‘ / $ “We? "fir’ikfif mm; famv “i “W " "’ " ' ' bemu C " . W T/f/é‘l ((Dnizatfgnc affix CHEM 1314 EXAM Ill PAGE 5 Multiple Choice: 5 8 12 10. . C, 9, t- . 2%, 13. A) B) C) D) E) Print the letter (A, B, C, D, E) which corresponds to he answer selecte/dX 10, Z 11. F 2 14. K 15. 5 ONLY THE ANSWERS IN THE AREA ABOVE WILL BE GRADED. Select the most correct answer for each question. Each question is worth 3 points. . A 100.0 g sample of an unknown metal initially at 95.0 "C is placed into an OSU calorimeter containing 130 g of water at 23.8 °C. The heat capacity of the OSU calorimeter is 25.0 J °C'1. If the final temperature of the mixture after adding the unknown metal to the water is ,30.1 °C, calculate the specific heat of the unknown metal. A) 0331 J g-1°C-1 B) 0. «528 J g-1 °C-1 C) 0.552 J g-1 °C-1 D) 0934 J g-1 °C-1 E) 0.958 J g-1 °C-1 9. Given AH° for the following reactions AH° = +167 kJ mol'1 AH° = +341 kJ mol'1 AH° = —43.4kJ mol'1 2C1F(g) + 02(g) 2C1F3(g) + 202(8) 2F2(g) + 202(3) ’9 Clzotg) + F2009) —> C120(g) + 3F20(g) —* 2F20(g) Calculate AH for the reaction ClF(g) + F2(g) +130. kJ mol-1 +218 kJ mol'1 +465 kJ mol-1 —276 kJ mol'1 —109 kJ mol'1 9 C1F3(g) Which of the following represents a standard formation reaction? A) Fe(s) + 1/202(g) —> FeO(s) B) CH4(g) + HC1(g) —> CH3C1(g) + H2(g) C) 2N02(g) —* N204(g) D) E) 2N2(g) + 02(3) —> 2N20(g) 2C(graphite) + 4H2(g) + 02(g) —> 2CH3OH(l) 11. When organic matter that contains phosphorus decomposes, phosphine, PH3, is produced. Phosphine is a colorless gas that smells like rotten fish. Phosphine ignites in the presence of oxygen in air according to the following reaction, 4PH3(g) + 802( g) A) —2.69 x 103 kJ mol-1 B) —4.68 x 103 kJ mol'1 C) —4.41 X 103 kJ mol'1 D) +4.41 X 103 kJ mol'1 E) +4.68 x 103 kl mol'1 —> P4010(s) + 6H20(l) CHEM 1314 EXAM III PAGE 6 12. When calcium carbonate is heated it decomposes to calcium oxide and carbon dioxide. What mass of CaO can form when 1220 k] of heat is transferred? CaCO3(s) —> CaO(aq) + C02(g) AH° = 461 kJ mol'1 A. 0.0472 g B. 2.65 g C. 148 D. 265 g E. 5.62 x 105 g 13. What is the maximum number of electron in the n = 4shell? A. 8 B. 16 C. 32 D. 64 E. 128 14. The effective nuclear charge for an electron in the n = 3 level for a copper atom is, M l x {9 n “v, s‘ 1:.w~« (a 2.5 a w mm» :54 A. +1 B. +8 C. +11 D. +19 E. +27 15. Of the following, which gives the correct order from largest to smallest for atomic radius for Mg, K, P, Si and Ne? A Mg>K>P>Si>Ne B. Si>P>Ne>K>Mg C. Ne>P>Si>Mg>K D. Ne>Si>P>K>Mg E K>Mg>Si>P>Ne ...
View Full Document

Page1 / 6

Exam 3 - CHEM 1314 Exam III John III. Gelder , April 5,...

This preview shows document pages 1 - 6. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online