<p> EXAM I - THIS IS YOUR REFERENCE SHEET/SCRATCH PAPER</p><p>Planck’s Constant = 6.63 x 10-34 J Sec Speed of light = 3.00 x 108 Rydberg constant = 2.18 x 10-18 J</p><p> page 1 Chemistry 112 Fall 2013 CLS Name______EXAM I</p><p> page 2 Chemistry 112 Fall 2013 CLS Name______EXAM I ______Show all your work. There are 9 Pages to this exam including the reference sheet and cover sheet</p><p>(40 points) 1. SHORT ANSWER/MULTIPLE CHOICE (1) Give the Orbital Diagram for a Sn(IV) ion. </p><p>(2) Write the set of quantum numbers for each electron lost when Cuo forms a Cu(II) ion.</p><p>(3) Atoms only emit certain wavelengths of light when they are excited. This describes the ______</p><p>Theory. In which the energy of photons is said to be______.</p><p>(4) Write an orbital diagram that violates only Pauli Exclusion Theorem</p><p>FOR THE FOLLOWING MULTIPLE CHOICE QUESTIONS, CIRCLE THE CORRECT ANSWER (5) How many different values of ml = in the 5f sublevel? a. 1 b. 7 c. 4 d. 6 e. 2</p><p>(6) Which of the following is diamagnetic a. Sn(II) b. I c. N d. Cr e. None of the above are diamagnetic</p><p>(7) Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error. a. n = 4, l = 0, ml =-1 b. n = 4, l = 4, ml =0 c. n = 5, l = 3, ml =-3 d. n = 3, l = 1, ml = -2 e. n = 3, l = 2, ml =+3</p><p> page 3 (8) Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n=4 and the atom emits a photon of light with a wavelength of 486 nm.</p><p> a. 1 b. 4 c. 2 d. 5 e. 3</p><p>(9) Use the standard reaction enthalpies given below to determine ΔH°rxn for the following reaction:</p><p>2 S(s) + 3 O2(g) → 2 SO3(g) ΔH°rxn = ?</p><p>Given: SO2(g) → S(s) + O2(g) ΔH°rxn = +296.8 kJ</p><p>2 SO2(g) + O2(g) → 2 SO3(g) ΔH°rxn = -197.8 kJ</p><p> a. -791.4 kJ b. 1583 kJ c. -692.4 kJ d. -293.0 kJ e. -494.6 kJ</p><p>(10) Which of the following processes have a ΔS < 0? a. water freezes b. methanol (g, at 555 K) → methanol (g, at 400 K) c. isopropyl alcohol condenses d. carbon dioxide (g) → carbon dioxide (s) e. All of the above processes have a ΔS < 0.</p><p>(11) Which of the following is the strongest reducing agent?</p><p> a. Zn(s) b. Mg(s) c. Mg2+(aq) d. Al(s)</p><p> page 4 e. Al3+(aq)</p><p>(12) The electrolysis of molten AlCl3 for 2.00 hr with an electrical current of 12.0 A produces ______g of aluminum metal.</p><p> a. 72.5 g b. 0.298 g c. 24.2 g</p><p> d. 2.24 × 10-3 g e. 8.06 g</p><p>(13) How many orbitals are contained in the third principal level (n = 3) of a given atom?</p><p> a. 3 b. 7 c. 9 d. 5 e. 18</p><p>(12 pts) 2]. Calculate Δ G for a galvanic cell at standard conditions from following half-reactions:</p><p>- 2- S2O8 + 2e ⇄ 2SO4 E° = 2.01 V - + - 2+ MnO4 + 8 H + 5e ⇄ Mn + 4H2O E° = 1.49 V</p><p> page 5 (12 points) 3] Calculate the emf for the following cell at 25oC:</p><p>- Pt| Fe(NO3)2 (1.00 M) | Fe(NO3)3 (0.010 M)|| Cl2 (1.5 atm) | Cl ((0.050M) | Pt</p><p>(12 points) 4] For the following cell: </p><p>Calculate the pH if the cell potential is 0.45 V</p><p>- 2+ 3+ The [NO3 ]= 0.10 M [Fe ]= 0.30 M PNO = 1.2 atm [Fe ] = 0.15 M</p><p>- + 2+ 3+ NO3 + 4H + 3Fe ⇄ NO + 2H2O + 3Fe</p><p> page 6 -19 (10 points) 5] Calculate the Eo for the following reaction if Keq = 1.00 x 10 : - - + I2 + 5Br2 + 6H2O ⇄ 2IO3 + 10Br + 12H </p><p> page 7 (15 points) 6] For the diagram shown below: a. Calculate the potential for the cell below</p><p> b) Is this a galvanic or electrolytic cell?</p><p> c) Draw the picture of the above cell (1) showing the location of each species (2) all components of the cell (3) flow of electrons (4) write the half-rxn to each beaker (5) show the flow of electrons (6) label the cathode and anodes (7) label the oxidation and reduction rxns (8) label the positive and negative electrodes</p><p>Zno Zno</p><p>0.33 M Zn(NO3)2 3.45 M Zn(NO3)2</p><p> page 8 (6 points) 7] Give and explain the experiment that showed that photons possess both particle and energy properties.</p><p> page 9</p>