Principles of Chemistry I 3150: EXAM III Tuesday, 8:45AM November 27, 2018

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1 Name Principles of Chemistry I 3150: EXAM III Tuesday, 8:45AM November 27, pts. Instructions: 1. Each student is responsible for following instructions. Read this page carefully. 2. Enter your name on this page and on your scan sheet. SIGN YOUR NAME on the scan sheet. Your signature on the scan sheet states your agreement with the following statement: I certify that I have not given or received aid on this exam, and that all work on the exam is entirely my own. 3. CODE your name (LAST NAME FIRST) on the computer answer sheet using an ordinary (No. 2 or HB) pencil. (No. 1 is also acceptable; No. 2 ½ or 3 is not.) It is very important to code the information correctly!! Use your full name as it is in UA s records, not any nickname. Fill as much of each name as will fit. 4. Put all calculations on the examination pages or scratch paper. Do not make any extra marks on the scan sheet!! 5. This exam consists of 42 multiple-choice questions worth 5 points each. For each multiple-choice question, choose the ONE best or correct answer and both write it on your exam paper and bubble it on the answer sheet. The computer answer sheet is the only one that will be graded! 6. Unless otherwise stated in a question: atoms and molecules are in the ground state; solutions are aqueous; and substances are at 25 C and 1 atm (~100 kpa). 7. This exam booklet consists of 4 pages (including this one) and a Periodic Table/Formula Sheet. Please check to be sure that you have them all! KEEP YOUR EXAM BOOKLET AND ANSWER SHEET COVERED TO PROTECT THE INTEGRITY OF YOUR WORK! PROHIBITED DURING EXAM: watches, food and drink, cell phones, pagers, laptops, PDAs, headphones, hats worn low over the eyes Please put these items away until you have left the room. REALLY, REALLY important information about bubbling your scan sheet: You MUST use a No. 2 pencil to bubble your answer sheet. Sheets completed in ink can not and WILL NOT BE GRADED. Enter your first and last names as far to the LEFT as possible in the fields. WRITE the letters of your name in the boxes at the top of the columns. (Dr. Donovan can not read bubbles.) In the STUDENT ID field, enter two zeros, then your 7-digit UA ID number. (if your ID number has fewer than 7 digits, fill with zeros so that your number is as far to the right as it can go.) That is, enter ID Number as You MUST bubble 3150: in the Dept/Course/Section fields. You MUST bubble the TEST NUMBER AND TEST FORM shown INSIDE THE EXAM. FAILING TO BUBBLE EVERYTHING CORRECTLY WILL PREVENT OR SIGNIFICANTLY DELAY PROCESSING OF YOUR EXAM!! If you erase and change an answer, please try using the white plastic eraser at the front of the room to remove the old mark. The scanner is VERY sensitive to erased marks! Thanks. The Management Warning!!! Doing any of the following will result in earning a score of zero (0) for this test. using INK to complete the bubble sheet not entering your name on the answer sheet not signing your name to the answer sheet not entering the TEST NUMBER and TEST FORM as noted on the first page FINAL EXAM for 8:45 class: Tuesday, December 11, 12:15-2:15pm in MGH 111. Covers all course material. YOU MUST HAVE YOUR ZIP CARD FOR THE FINAL EXAM. NO ZIP CARD=NO EXAM!! DON T FORGET YOUR CALCULATOR!! You will need a calculator and there may NOT be spares available. Reminder: watches and cell phones must NOT be out during exams, including the final exam.

2 On your answer sheet, right now, enter TEST FORM A and TEST NUMBER 3. Your exam can not be graded without this information. Questions 1-3 pertain to the following choices, which may (or may not) repeat: (A) Al (B) Si (C) P (D) Ge (E) As On your scan sheet, bubble the letter for the atom that has the largest first ionization energy. has the most metallic character. has the fewest valence electrons. Which ion has the smallest radius? (A) Te 2 (B) I (C) Cs + (D) Ba 2+ Which atom has the smallest radius? (A) Te (B) I (C) Cs (D) Ba Which correctly represents the predicted electron configuration of Ni? (A) [Ar] 4s 3d (B) [Ar] 4s 3d (C) [Ar] 4s 3d. (D) [Ar] 4s 3d (E) [Ar] 4s 3d 4p. Which electronic transition in a hydrogen atom corresponds to the largest release of energy? (A) n = 9 n = 7 (B) n = 4 n = 2 (C) n = 1 n = 3 (D) n = 6 n = 8 (E) It is impossible to tell without additional information. Which comparison(s) of radii is/are correct? (A) Br < Cl (B) Cl < Cl (C) both (A) and (B) (D) neither (A) nor (B) What is the electron configuration of Ni 2+? (Take care on this one. Two more questions use it.) (A) [Ar]4s 2 3d 6 (B) [Ar]4p 8 (C) [Ar]4s 1 3d 7 (D) [Ar]3d 8 A ground-state Ni 2+ ion exhibits (A) diamagnetism only. (B) paramagnetism How many unpaired electrons are present in a ground-state Ni 2+ ion? (D) 3 Which could be an excited-state electron configuration for a neutral atom of chlorine? (A) [Ne]3s 2 3p 5 (B) [Ne]3s 3 3p 3 4p 1 (C) [Ne]3s 1 3p 5 4p 1 (D) [Ne]3s 1 3p 5 (E) [Ne]3s 2 3p 6 Being in the same group as chromium, molybdenum has some similar properties. Like Cr, Mo has an electron configuration that is an exception ([Kr]5s 1 4d 5 ) to the general rule. Why does Mo exhibit this behavior? (A) One electron goes into the 5s orbital so that it doesn t have to pair with a 4d electron, since the 4d subshell already contains two pairs of electrons plus one unpaired. (B) In Mo, the 5s orbital is always higher than energy than the 4d orbitals. (C) The 5s and 4d subshells are close in energy, and the number of unpaired electrons with the same spin is maximized with the [Kr]5s 1 4d 5 configuration. (D) It s not possible to explain this exceptional behavior. How many valence electrons does a neutral atom of 84 Po have? (A) 84 (B) 30 (C) 16 (D) 6 Which ion(s) of 81 Tl can be described as having a pseudo-noble-gas configuration? (A) Tl + (B) Tl 3+ (C) both Tl + and Tl 3+ (D) neither Tl + nor Tl 3+ Which element in the third period would have the most acidic oxide? (A) P (B) Si (C) Al (D) Mg (E) Na 3150: Exam III 2 11/27/18

17. 18. Which reaction s energy equals the third ionization energy of Ga?

3 Which reaction s energy equals the third ionization energy of Ga? (A) Ga 3+ (g) + 3e Ga(g) (B) Ga 2+ (g) Ga 3+ (g) + e (C) Ga(g) + 3e Ga 3 (g) (D) Ga 3+ (g) Ga 4+ (g) + e (E) Ga(g) Ga 3+ (g) + 3e Which set of quantum numbers could correctly describe an electron in a 4d orbital? (A) n = 4, l = 2, m l = 1, m s = (B) n = 4, l = 3, m l = +1, m s = +1 (C) n = 4, l = 2, m l = 3, m s = 1 2 (D) n = 4, l = 2, m l = 1, m s = 1 (E) n = 4, l = 3, m l = 1, m s = Bohr s model of the atom could be used to accurately calculate energies in (A) H. (B) He +. (C) both H and He +. (D) neither H nor He If the frequency of electromagnetic radiation were doubled, the wavelength of the radiation would (A) be halved. (B) be doubled. (C) remain the same. (D) be squared. 21. What is the frequency (in Hz) of UV light with a wavelength of nm? (A) Hz Hz (C) Hz (D) Hz (E) Hz 22. What is the ground-state electron configuration of an 77Ir atom? (It s not an exception.) (A) [Xe]6s 2 5f 14 5d 7 (B) [Xe]6s 2 4f 14 6d 7 (C) [Xe]6s 2 5d 7 (D) [Xe]6s 2 4f 14 5d 7 (E) [Xe]6s 2 6f 14 6d A certain element has the successive ionization energies shown. How Ionization Energies/ many valence electrons kj mol does this element have? 1 1 st 999 (A) 3 2 nd 2,252 (B) 4 3 rd 3,357 (C) 5 4 th 4,556 (D) 6 5 th 7,004 (E) 7 6 th 8,496 7 th 27, Which type of orbital is shown? (A) s (B) p (C) d (D) f How many orbitals in an atom could have quantum numbers l = 2 and m l = 3? (D) 5 (E) It depends on the value of n. How many electrons in an atom could have quantum numbers n = 4 and m s = 1 2? (A) 4 (B) 8 (C) 16 (D) 32 (E) none of these Consider the wavelengths of Wavelength/nm radiation listed at right. infrared 100,000 A photon of which radiation orange 600 would have the lowest X-ray 1 energy? (A) infrared radiation (B) orange light (C) X-ray radiation (D) It is impossible to tell without additional information. The bonding in CsF is (A) 100% ionic. (B) mostly ionic. (C) polar covalent. (D) nonpolar covalent. Which bond is the strongest? (A) C O (B) C=O (C) C O (D) all of these bonds are equal in strength. What is the ground-state electron configuration of S 2? (A) [Ne]3s 2 3p 4 (B) [Ne]3s 2 3p 2 (C) [Ne]3s 2 3p 6 (D) [Ne]3s 2 3p 4 4s 2 (E) none of these Which is/are exothermic? (A) electron affinity of F (B) first ionization energy of F (C) both (A) and (B) (D) neither (A) nor (B) 3150: Exam III 3 11/27/18

4 Which comparisons of Ge and P are correct? I. electronegativity: Ge < P II. atomic radius: Ge < P III. metallic character: Ge < P IV. first ionization energy: Ge < P (A) I and II (B) I and IV (C) II and III (D) III and IV (E) I, II, and III Which neutral atom could X be? (A) Al (B) P (C) S (D) Cl (E) Ar Draw the Lewis structure of SeF 4. How many lone pairs are there on the central atom? (D) 3 Diamond and quartz are members of what class of crystalline solids? (A) network covalent (B) molecular (C) ionic (D) metallic V 3+ and Ca are isoelectronic. (A) True (B) False Using enthalpies of formation, calculate ΔH of this reaction: CO 2 (g) + 2SO 2 (g) CS 2 (l) + 3O 2 (g) (A) kj (B) kj (C) kj (D) kj (E) kj Calculate the heat for the decomposition of 15.2 g lead(ii) azide, Pb(N 3 ) 2, to form Pb and N 2. Pb(N 3 ) 2 (s) Pb(s) + 3N 2 (g) ΔH = kj (A) 7030 kj (B) 30.4 kj (C) 24.1 kj (D) kj (E) kj ΔH F /kj mol 1 CO 2 (g) CS 2 (l) 87.9 SO 2 (g) Molar Mass/g mol 1 Pb(N 3 ) An exothermic aqueous reaction is carried out in a constant-pressure calorimeter. The temperature of the solution during the reaction. (A) increases (B) decreases (C) does not change A sample of an unknown 1 Specific Heat/ J g 1 K metal required 5 minutes to uranium 0.12 increase in temperature by cesium C in an oven. A sample palladium 0.24 of cesium required 10 rubidium 0.36 minutes to heat in the same manganese 0.48 oven, receiving the same amount of heat per minute. What metal could be the unknown? (A) uranium (B) palladium (C) rubidium (D) manganese When mol of a compound reacted in a constant-pressure calorimeter containing 49.7 g of water, the temperature decreased from 29.7 C to 10.4 C. What is ΔH RXN in kj mol 1? (A) 4010 kj mol 1 (B) kj mol 1 (C) kj mol 1 (D) 38.2 kj mol 1 (E) +579 kj mol 1 Use these data to calculate ΔH for this reaction: 2C(s) + 3H 2 (g) C 2 H 6 (g) 2C 2 H 6 (g) + 7O 2 (g) 4CO 2 (g) + 6H 2 O(l) C(s) + O 2 (g) CO 2 (g) 2H 2 O(l) 2H 2 (g) + O 2 (g) (A) 86 kj (B) 1490 kj (C) 3206 kj (D) +86 kj (E) kj ΔH = 3120 kj ΔH = 394 kj ΔH = +572 kj End of Exam Check to see that you have entered 42 answers on your scan sheet. Make sure that you have bubbled everything correctly, including the ID number, Test Form, and Test Number. Proofread your work. The Test Number may or may not be 3. If you bubbled in ink, redo your scan sheet now (on a fresh sheet) or else earn a zero! You must return your scan sheet before leaving the room. MAKE SURE YOU HAVE ENTERED YOUR ANSWERS ON THIS PAPER so that you can check them against the key, posted online later, and estimate your score. Also, past tests make excellent study tools for the final exam. NOTE: IF YOU ARE TAKING THE EXAM ANYWHERE OTHER THAN MGH 111 AT 8:45AM, YOU MUST HAND ALL PAGES IN TO THE PROCTOR. 3150: Exam III 4 11/27/18

5 1A (1) 1 H Li Na K Rb Cs Fr (223) 2A (2) 4 Be Mg Ca Sr Ba Ra [226] 3B (3) 21 Sc Y Lu Lr (262) 4B (4) 22 Ti Zr Hf Rf (267) Activity Series of Metals Li(s) Li + (aq) + e K(s) K + (aq) + e Ba(s) Ba 2+ (aq) + 2e Ca(s) Ca 2+ (aq) + 2e Na(s) Na + (aq) + e Mg(s) Mg 2+ (aq) + 2e Al(s) Al 3+ (aq) + 3e Mn(s) Mn 2+ (aq) + 2e Zn(s) Zn 2+ (aq) + 2e Cr(s) Cr 3+ (aq) + 3e Fe(s) Fe 2+ (aq) + 2e Co(s) Co 2+ (aq) + 2e Ni(s) Ni 2+ (aq) + 2e Sn(s) Sn 2+ (aq) + 2e Pb(s) Pb 2+ (aq) + 2e H 2 (g) 2H + (aq) + 2e Cu(s) Cu 2+ (aq) + 2e Ag(s) Ag + (aq) + e Hg(l) Hg 2+ (aq) + 2e Pt(s) Pt 2+ (aq) + 2e Au(s) Au 3+ (aq) + 3e 57 La Ac [227] 5B (5) 23 V Nb Ta Db (268) 6B (6) 24 Cr Mo W Sg (271) 58 Ce Th INCREASING ACTIVITY 59 Pr Pa B (7) (8) Mn Fe Tc (98) 75 Re Bh (270) 60 Nd U Ru Os Hs (269) N A = Pm (145) 93 Np [237] 8B (9) (10) Co Ni Rh Ir Mt (278) 62 Sm Pu (244) 46 Pd Pt Ds (281) 1B (11) 29 Cu Ag Au Eu Am (243) 111 Rg (281) 2B (12) 30 Zn Cd Hg Gd Cm (247) 112 Cn (285) 3A (13) 5 B Al Ga In Tl Tb Bk (247) 113 Nh (286) 4A (14) 6 C Si Ge Sn Pb Dy Cf (251) 114 Fl (289) 5A (15) 7 N P As Sb Bi Ho Es (252) 115 Mc (289) 6A (16) 8 O S Se Te Po (209) 68 Er Fm (257) 116 Lv (293) 7A (17) 9 F Cl Br I At (210) 69 Tm Md (258) 117 Ts (294) 70 Yb No (259) Note: notation such as g mol 1 is read grams per mole. T K = T C T F = 9 5 T C + 32 T C = 5 9 [T F 32] E = q + w q = mc T w = P V H = E + P V H = n H F (products) n H F (reactants) M 1 V 1 = M 2 V 2 H = nd(bonds broken) nd(bonds formed) 1 1 cal = J specific heat of water = J g 1 K M = mol/l 8A (18) 2 He Ne Ar Kr Xe h = J s c = m s 1 R H = J 1 c = ν E = hν E RH 2 n PV = nrt D = P RT M 1 1 r r n A B PV T = PV 2 2 T 1 2 B M M 1 R = L atm mol 1 K 1 atm 760 torr = 760. mmhg = kpa = 14.7 psi = mbar P i = X i P T P T = P i P 1 /P T = n 1 /n T 1 in 2.54 cm (exact) actual % yield = 100% BO = 1 theoretical 2 [#bonding e #antibonding * e ] A 86 Rn (222) 118 Og (294) 3150: Exam III 5 11/27/18

Principles of Chemistry I 3150: EXAM III Tuesday, 10:15AM November 27, 2018

Name Principles of Chemistry I 3150:151-006 EXAM III Tuesday, 10:15AM November 27, 2018 205 pts. Instructions: 1. Each student is responsible for following instructions. Read this page carefully. 2. Enter