LAST NAME, FirstCHEM 107 (Spring-2007)Final Exam (104 pts)Name: ------------------------------------------------------------------------, Clid # ------------------------------ LAST NAME, First(Circle the alphabet segment of your LAST NAME): A & B C-G H-L M-P R-Z Please answer the following questions:Part I: Multiple Choices (44 pts: 22 @ 2 pts each + 4 pts bonus). Circle the ONE best answer:1. Which of the following species have square planar molecular shape?I) SeF4II) NH4+III) XeF4IV) SO32-a) only III b) only I c) II and III d) I, II and III2. In the above question the hybridization of the central atom in each molecule or ion are as follows:a) sp3d, sp3, sp3d2 and sp3 respectively b) sp3, sp3, sp3d2 and sp2 respectivelyc) sp3d, sp3, sp3d2 and sp2 respectively d) sp3d2, sp3, sp3 and sp2 respectively3. A gold ring has a mass of 5.50 g, it absorbs 2.10 J when heated from 15.0 to 18.0 ºC, What is the specific heat of the gold? (specific heat of gold is 0.129 J/g ºC)a) 0.382 J/g ºC b) -0.129 J/g ºCc) 0.129 J/g ºC d) 1.83 J/g ºC4. Which of the following statements is false?a) An electron transition from n = 4 to n = 2 emits energy.b) Light emitted by an n = 5 to n = 2 transition will have a shorter wavelength than that fromn = 4 to n = 2 transition.c) An atom of group 15 has three unpaired electrons.d) None of the above.5. Which of the following ions is expected to be paramagnetic that corresponds to the presence offive unpaired electrons? a) Cd2+ b) Co2+c) Mn4+d) Cr+6. The ground state electron configuration of osmium, Os (Z = 76) isa. [Xe] 4f146d6 6s2b) [Xe] 4f14 5d6 6s2c) [Xe] 4f14 6p6 6s2d) [Xe] 4f14 5d67. The oxidation numbers of sulfur, S in H2S and S2O32- are:a) 0 and +4, respectively b) +2 and +4, respectively 1c) -2 and +2, respectively d) -2 and +4, respectively 8. Which of the following molecules is expected to be non-polar?a) PCl3b) SF2c) BeF2d) NF3 9. What is the final temperature (°C) is required for the pressure inside an automobile tire to increase from 2.15 at 0 °C to 2.37 atm, assuming the volume remains constant?a) 301 b) -25c) 28 d) no answer was give10. The concentration of cholesterol (C27H46O) in normal blood is approximately 0.005 M. How many grams of cholesterol are in 750 mL of blood? a) 3.75 b) 9.70 x 10-3 c) 1.93 d) 1.4511. Calculate ∆H° for the following reaction using the given enthalpies of formation. 2 C2H2 (g) + 5 O2 (g) 4 CO2 (g) + 2 H2O (g)∆Hf° (kJ/mol): 226.7 -393.5 -241.8b. +862 kJ b) -862 kJc) +2511.0 d) -2511.0 kJ12. Which of the following has the smallest first ionization energy?a) Br b) Sn c) Se d) Cl13. The greatest deviation from the Ideal Gas Law is expected at:a) high T, high P b) low T, high Pc) high T, low P d) low T, low P14. Which name is incorrect?a) (NH4)2SO4: ammonium sulfate b) SeO2: selenium sulfide c) S2F2: disulfur difluoride d) CuO: copper(II) oxide15. The standard enthalpy change for the following reaction is +285.4 kJ. 3 O2 (g) 2 O3 (g) What is the standard enthalpy of formation of O3 (g)?a) +142.7 kJ b) -142.7 kJc) +285.4 kJ d) -285.4 kJ 16. Predict the product formed when calcium, Ca combines with arsenic, As?2a) Ca3As2b) Ca2As3c) CaAs d) CaAs217. What volume, in mL of 0.750 M HCl would be required to neutralize 1.50 g sample of Ca(OH)2?a) 53.5 b) 26.7c) 13.4 d) 35.018. Naturally occurring chlorine consists of two isotopes. The atomic mass of chlorine is approximately 35.5. What are reasonable estimates of the relative percentages of 35Cl and 37Cl, respectively?a) 50, 50 b) 25, 75 c) 75, 25 d) 67, 3319. An atom containing 34 protons and a mass number of 77, would be:a) 77Se b) 43Sec) 77Tc d) 43Tc20. A solution of acetic acid, CH3COOH (60 g/mol), is 50.0% CH3COOH by mass and has a density of 1.15 g/mL. calculate the molarity of the solutiona) 9.58 b) 0.958c) 7.25 d) none of these21. Which of the following ions has the smallest atomic radius?a) Si b) P c) S d) F Questions 22-24: Consider the phase diagram of the substance shown here. 22. Approximately what is the normal boiling point? a) 170 ºCb) 300 ºC c) 460 ºC 23. What is the normal melting point of the substance? a) 170 ºC b) 180 ºC c) 300ºC 24. What is the physical state of the substance of the substance under the conditions of T = 350 K, P = 0.9 atm?3a) solid b) liquid c) gas4Part II. Bonding and Chemical Equations (26 pts):A) Bonding & molecular structure (12 pts):1. Draw the Lewis structure for the SCN- ion, draw the resonance structures, if there is any then predict: a) the molecular shape b) hybridization of the central C atom c) number σ and π bonds d) bond angleB) Chemical Equations (16 pts):2. (8 pts) Balance the following redox equation in acidic solution:MnO4- (aq) + Br- (s) Mn2+ (aq) + Br2 (l),Then identify the oxidizing agent and how many electron(s) are transferred per one mole of the oxidizing agent.5Balanced equation:Oxidizing agent: --------------Number of electrons/mole of oxidizing agent: -------- Lewis Structure & resonance structures (if any)a) Molecular shape: ------------------------b) Hybridization of the central atom: -------c) # of σ bonds ------- and # of π bonds --------d) Bond angle: -----------------2. (6 pts) Write the balanced chemical equation and the net ionic equation for the reaction between aqueous solutions of AgNO3 (aq) and CaBr2 (aq) and then identify the spectator ion(s)Part III. Calculations (30 pts: 5 @ 6 pts each) Show all work for full credit. Please express all answers with the proper units and correct number of significant figures.1. Given the following equations: N2 (g) + 3 H2 (g) 2 NH3 (g) ∆Hrxn° = -92.2 kJ2 H2 (g) + O2 (g) 2 H2O (l) ∆Hrxn° = -571.6 kJ N2 (g) + O2 (g) 2 NO (g) ∆Hrxn° = +180.5 kJ Determine the enthalpy change, ∆Hrxn° for the following reaction: 2 NO (g) + 2 O2 (g) 2 NH3 (g) + 2 H2O (l) ∆Hrxn° = ??6∆Hrxn° = -844.3 kJChemical equation:Net ionic equation:Spectator ion(s):2. Titanium(III) chloride, TiCl3 a substance used as a catalyst for preparing