CHEM 200/202 Exam 3-A November 15, Name (printed): Signature:

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1 HEM 200/202 Exam 3-A November 15, 2014 HEM Lab Section Number: Name (printed): (Last) (irst) Signature: This exam consists of 32 questions at 5 points each for a total of 160 points. Make sure that your test has all of the pages. Please read each problem carefully. There are no intentionally misleading questions; each problem should be taken at its face value. Please mark your answers on the Scantron sheet provided to you and on the actual exam. You will be given a periodic table and an exam information sheet to use during the exam. You may remove it from the exam make it more accessible. You may also use the designated asio fx-300ms-plus calculator or equivalent non-programmable non-graphing scientific calculator during the exam. Use the back pages of the test as scratch paper. You are not allowed to use any devices capable of accessing the internet, textbooks, notes, or homemade reference sheets during the exam. You may leave if you finish the exam early. Give the exam and the information sheet to your TA and leave quietly without disturbing other students. Before leaving, check that all your answers have been properly entered on the Scantron sheet and the exam and that your name is written on every page of the exam and on the Scantron sheet. All cell phones and electronic devices must be turned off and put away. Please remove all hats and caps. Place your books and all papers out of sight under your seat. If the TA believes that you might be looking at your neighbor s paper, you will be asked to move to a new location. Exam scores will be posted on Blackboard as soon as the grading is complete. Your test will be returned to you in the first lab meeting of next week. If you have any questions regarding the grading of your exam, please notify your TA. The time available for the exam is 120 minutes. Good luck!

2 HEM 200/202 Exam 3-A November 15, 2014 Name: Lab Section #: Please mark your answers on the scantron sheet using a #2 pencil and also mark your answers on the exam itself. Mark Test rom A on your scantron. 1. Which of the following is an ionic compound? a) KI b) NH3 c) I2 d) H2S e) l4 2. f these substances, in which are the atoms held together by metallic bonding? a) 2(g) b) Si(s) c) Br2(l) d) S8(s) e) r(s) 3. Which statement below best describes the location of the electrons involved in a covalent bond? a) The electrons are delocalized evenly, everywhere, between all the atoms in the substance. b) The electrons have a higher probability of being found directly between adjacent nuclei. c) The electrons form a straight line bridging the adjacent nuclei. d) The electrons are removed from one atom and found exclusive around the adjacent atom. e) The electrons are on the far sides of the nuclei, which touch to form a covalent bond. 4. What is the molecular formula of the ionic compound formed by barium and nitrogen? a) BaN b) BaN2 c) Ba2N3 d) Ba2N e) Ba3N2 5. The lattice energy for ionic crystals increases as the charge on the ions and the size of the ions. a) increases, increases b) increases, decreases c) decreases, increases d) decreases, decreases e) None of these choices is generally correct. 1 of 9

3 HEM 200/202 Exam 3-A November 15, alculate the lattice energy of magnesium sulfide from the data given below. Mg(s) Mg(g) H = 148 kj/mol Mg(g) Mg 2+ (g) + 2e H = 2186 kj/mol S8(s) 8S(g) H = 2232 kj/mol S(g) + 2e S 2 (g) H = 450 kj/mol 8Mg(s) + S8(s) 8MgS(s) H = kj/mol MgS(s) Mg 2+ (g) + S 2 (g) H lattice =? a) kj/mol b) kj/mol c) kj/mol d) 3406 kj/mol e) None of these choices are correct. 7. The diameter of a chloride ion is 362 pm, and the diameter of a potassium ion is 276 pm. What is the distance between the nuclei of adjacent chloride and potassium ions in solid potassium chloride? a) 1276 pm b) 638 pm c) 319 pm d) 181 pm e) 138 pm 8. Select the element whose Lewis symbol is correctly represented. A B D E r Ra Pb Te He 9. The melting point of Mg is 2852, whereas S2 has a melting point of If quartz (Si2) is a solid with a melting point of 1550, the bonding in quartz is best described as: a) lattice energy b) network attractions c) ionic bonding d) network covalent bonding e) metallic bonding 10. Which of the atoms listed below is the most electronegative? a) Rb b) Li c) As d) Al e) N 2 of 9

4 HEM 200/202 Exam 3-A November 15, The reaction between methane and chlorine gas is exothermic and produces carbon tetrachloride and hydrogen chloride gasses. Given the reaction, its enthalpy, and the respective bond energies, determine the bond energy of the l l bond. H4(g) + 4l2(g) 4Hl(g) + l4(g) H rxn = -440 kj Bond energies: H = 413 kj/mol; l = 339 kj/mol; = 347 kj/mol; H l = 427 kj/mol a) 60.8 kj/mol b) 330 kj/mol c) 243 kj/mol d) 972 kj/mol e) 156 kj/mol 12. Which is the strongest bond of those listed below? a) H l b) H c) H Br d) H At e) H I 13. Select the best Lewis structure for ln. l A B N l N l N l D N l E N 14. Which of the molecules below is not an example of an expanded octet? a) S4 2 b) l3 c) Xe4 d) Pl3 e) P4 3 D 15. Select the Lewis structure in which the formal charges on the atoms in periodate (I4 ) are best minimized. A 1- B 1-1- D 1- E 1- I I I I I 3 of 9

5 HEM 200/202 Exam 3-A November 15, Which is the proper representation of bromine trifluoride? A B B Br Br D Br E Br 17. What is the formal charge of the nitrogen atom in nitric acid (HN3)? a) -2 b) -1 c) 0 d) +1 e) +2 N H 18. Which molecule below does not have a resonance structure? a) 3 b) l4 c) P4 3 d) 2 e) S f the bond angles listed below, which is not a bond angle between chlorine atoms, predicted by the VSEPR structure, on Pl5? a) 90 b) c) 120 d) 180 e) All these bond angles are found in Pl Which of the molecules listed below has a square planar structure? a) NH4 + b) Xe4 c) S4 2 d) Xe22 e) I Which one of the molecules below is not correctly paired with its predicted VSEPR structure? a) S4 2 : tetrahedral b) I4 + : see-saw c) 3 2 : trigonal planar d) H2 : linear e) S6 : octahedral 4 of 9

6 HEM 200/202 Exam 3-A November 15, Which one of the molecules listed below does not have a central atom with sp 3 hybridization? a) Bl3 b) NH3 c) H3 + d) Pl3 e) H4 23. What is the hybridization of the carbon atom in thiocyanate (SN )? a) sp b) sp 2 c) sp 3 d) sp 3 d e) The carbon atom is not hybridized 24. Which of the following will result in the least, or no, disruption to the ideal bond angles around a central atom? a) A lone pair of electrons. b) A double bond to oxygen. c) A double bond to sulfur. d) A single bond to hydrogen. e) Nothing disrupts bond angles. 25. Which one of the molecules below exhibits molecular polarity? a) NH4+ b) 2 c) S4 2 d) N e) B3 26. Which statement pertaining to sigma bonds is incorrect? a) Methane (H4) contains four sigma bonds. b) Sigma bonds have very high electron density along the axis of the bond. c) Sigma bonds form from the direct overlap of any two orbitals on adjacent atoms. d) All bonds between atoms contain sigma bonds. e) Double bonds are the result of a pair of sigma bonds between the same two atoms. 27. How many sigma and pi bonds are there in a molecule of S3? a) Three sigma bonds and zero pi bonds. b) Two sigma bonds and one pi bond. c) ne sigma bond and two pi bonds. d) Three sigma bonds and three pi bonds. e) our sigma bonds and two pi bonds. 5 of 9

7 HEM 200/202 Exam 3-A November 15, 2014 Use the molecular orbital diagram below to assist in answering the next three questions. 28. Using the M diagram, determine the bond order for the BN (boronitride) molecule? a) 0 b) 1 c) 1.5 d) 2 e) Which one of the following diatomic molecules is paramagenetic? a) N2 b) N c) BN d) 2 e) B2 30. How many electrons does the diatomic ion N2 have in anti-bonding molecular orbitals? a) 0 b) 1 c) 2 d) 3 e) 4 Energy 6 of 9

8 HEM 200/202 Exam 3-A November 15, 2014 The following problems are extra credit. You will not be penalized for wrong answers. 31. What is the hybridization of the iodine atom in I4 +? a) sp b) sp 2 c) sp 3 d) sp 3 d e) sp 3 d In the figure below the curved line represents the potential energy of the bond in a molecule of H2. Which point on the figure (represented by the letters) shows the optimal length of the H H bond? A Potential Energy (kj/mol) B D E Internuclear Distance (pm) 7 of 9

9 HEM 200/202 Exam 3-A November 15, 2014 This Left Blank or alculations 8 of 9

10 HEM 200/202 Exam 3-A November 15, 2014 This Left Blank or alculations 9 of 9

11 San Diego State University HEM 200 Exam/Quiz Information Sheet all 2013 Physical Quantities atomic mass unit (amu) = x kg Avogadro s number = x universal gas constant (R) = J/K mol = L atm/k mol absolute zero = = 0 K specific heat capacity of water (ch 2 ) = J/g K speed of light (c) = x 10 8 m/s Planck s constant (h) = x J s onversion actors 1 angstrom (Å) = m 1 atm = x 10 5 Pa = bar = 760 Torr 1 calorie = J 1 joule = 1 kg m 2 /s 2 Equations PV = nrt P A = X A P total d = (molar mass) P RT u rms = 3RT molar mass E = q + w H rxn = H f (products) - H f (reactants) heat capacity = q/ T specific heat capacity (c) = q/(mass T) speed of light (c) = x E photon = h = hc E electron = x J ( Z2 n 2) = h mu 1 = x 107 m -1 ( 1 n n2 ), where n 2 > n

12 2008 San Diego State University, Department of hemistry Periodic Table of the Elements H He Li Be B N Ne Na Mg Al Si P S l Ar K a Sc Ti V r Mn e o Ni u Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc [98] 44 Ru Rh Pd Ag d In Sn Sb Te I Xe s Ba * 71 Lu Hf Ta W Re s Ir Pt Au Hg Tl Pb Bi Po [209] 85 At [210] 86 Rn [220] 7 87 r [223] 88 Ra [226] ** 103 Lr [262] 104 Rf [261] 105 Db [262] 106 Sg [266] 107 Bh [264] 108 Hs [277] 109 Mt [268] Metals Non Metals * Lanthanoids 57 La e Pr Nd Pm [145] 62 Sm Eu Gd Tb Dy Ho Er Tm Yb ** Actinoids 89 Ac [227] 90 Th Pa U Np [237] 94 Pu [244] 95 Am [243] 96 m [247] 97 Bk [247] 98 f [251] 99 Es [252] 100 m [257] 101 Md [258] 102 No [259]

Name (printed): Signature:

CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem