Part Ia) SF4Chemistry 101 –Final Exam December 14, 2019 Part I 1. Carbon dioxide (CO2(g)) dissolves in water to produce carbonic acid H2CO3. CO2 + H2O → H2CO3 While carbonic acid is not stable it does do acid-base reactions in water until the CO2 is consumed. Aluminum carbonate, Al2(CO3)3(s), can be used as an antacid (not the best choice however!). How many grams of aluminum carbonate can be formed from combination of 10.0 L of CO2(g) at STP with 500. ml of 0.543 M Al(OH)3?2 2. Given the data: N2(g) + O2(g) → 2 NO(g) ∆H = +180.7 kJ 2 NO(g) + O2(g) → 2 NO2(g) ∆H = −113.1 kJ 2 N2O → 2 N2(g) + O2(g) ∆H = −163.2 kJ i. Use Hess’s law to calculate ∆H for the desired reaction below: N2O(g) + NO2(g) → 3 NO(g) ii. Using the desired equation from (i), how much heat is needed if one starts with 22.0g N2O and an excess of NO2? iii. What volume of NO(g) is produced if 100.kJ are required at 25°C and 1.00 atm for the reaction below? N2O(g) + NO2(g) → 3 NO(g)3 3. For each formula below: i. Draw the best Lewis structure ii. Calculate the Formal charge on all the atoms for your Lewis structure iii. Give the molecular geometry name iv. Circle if it has a dipole v. Indicate if resonance structures exist by circling yes or no vi. Give the hybridization of the central atom (where indicated). a) SF4 i. Lewis Structure: ii. Formal Charges: iv. Dipole: Polar Non-polar v. Resonance: Yes No iii. Molecular Geometry Name: b) CO32− i. Lewis Structure: ii. Formal Charges: iv. Dipole: Polar Non-polar v. Resonance: Yes No vi. Hybridization: iii. Molecular Geometry Name: c) ClO3 i. Lewis Structure: ii. Formal Charges: iv. Dipole: Polar Non-polar v. Resonance: Yes No vi. Hybridization iii. Molecular Geometry Name:4 1. A beaker is known to have a weight of 126 grams. To the beaker is added 13.3 grams of substance A and 1.57 grams of substance B. Properly expressed in terms of significant figures, the total weight of beaker and contents is now (in grams): a) 140 b) 141 c) 140.8 d) 140.9 e) 140.87 2. Correct names for the following compounds are: CCl4, FeCO3 Al(NO3)3 a) monocarbontetrachlorine, iron(III) carbonate, aluminum nitrate b) carbon tetrachlorine, iron carbontrioxide, aluminum(III) nitrate c) tetrachlorocarbon, iron(III) carbontrioxide, aluminum trinitrate d) carbon tetrachloride, iron(II) carbonate, aluminum nitrate e) tetrachlorocarbon, iron(II) chlorate, aluminum nitrate 3. For reaction of H3PO4 with KOH the coefficients in the balanced chemical equation are: aKOH + bH3PO4 → cK3PO4 + dH2O a) a = 2, b = 2, c = 2, d = 3 b) a = 1, b = 2, c = 2, d = 1 c) a = 1, b = 1, c = 1, d = 1 d) a = 2, b = 1, c = 1, d = 2 e) a = 3, b = 1, c = 1, d = 3 4. The number of moles of hydrogen atoms in 1.0g of glucose, C6H12O6, is: a) 0.13 b) 0.083 c) 0.0056 d) 12 e) 0.067 5. In the reaction of 1.00 mole of O2 with 2.00 mole of H2, if 30.0g of H2O is formed, what is the percent yield? 2H2 + O2 → 2H2O a) 83.3% b) 167% c) 50.0% d) 88.9% e) 100% 6. How many mL of 0.125M H2SO4 are needed to neutralize 100.mL of 0.0500M NaOH? a) 10.0mL b) 40.0mL c) 100.mL d) 20.0mL e) 50.0mL5 7. Place the following gases in order of increasing average molecular speed at 25°C: Ne, HBr, SO2, NF3, CO a) NF3 < SO2 < HBr < CO < Ne b) Ne < CO < HBr < SO2 < NF3 c) HBr < SO2 < CO < NF3 < Ne d) Ne < CO < SO2 < NF3 < HBr e) HBr < NF3 < SO2 < CO < Ne 8. How many different orbitals can have the principal quantum number n = 3? a) 9 b) 4 c) 6 d) 5 e) 18 9. The number of 5d electrons in the electronic configuration of element 75 (Re) is: a) 2 b) 3 c) 7 d) 5 e) 10 10. Which of the following is not a valid set of quantum numbers for an orbital in an atom? a) n = 3, ℓ = 1, mℓ = -1 b) n = 1, ℓ = 0, mℓ = 0 c) n = 6, ℓ = 1, mℓ = 0 d) n = 5, ℓ = 4, mℓ = -4 e) n = 2, ℓ = 2, mℓ = 1 11. A possible set of four quantum numbers (n, ℓ, mℓ, ms) for the highest energy electron in arsenic, As, is: a) 4, 1, 2, 1/2 b) 4, 1, -1, 1/2 c) 3, 1, 0, 1/2 d) 4, 0, 0, 1/2 e) 4, 2, 1, -1/26 12. The number of unpaired d-electrons in the ground state electron configuration decreases in the following order: a) d8 > d10 > d2 b) d9 > d1 > d5 c) d6 > d9 > d10 d) d10 > d4 > d3 e) d9 > d3 > d2 13. What is the electron configuration of Fe2+? a) [Ar]4s23d4 b) [Ar]3d6 c) [Ar]4s23d6 d) [Ar]3s13d5 e) [Ar]3d7 14. Which of the following statements provides an accurate statement comparing the atomic radius of Ca with that of K? a) Ca is larger because it has more electrons. b) Ca is larger because its effective nuclear charge is greater. c) K is larger because its effective nuclear charge is less. d) K is larger because it has fewer electrons. e) Ca and K are essentially the same size. 15. The ionic compound formed between calcium and chlorine has the formula: a) CaCl b) Ca2Cl c) CaCl2 d) CaCl3 e) Ca2Cl2 16. From the following groups, the largest atom will be, (K, Li, Cs), (Pb, Sn, Si), (F, O, N) a) K, Sn, F b) K, Sn, O c) Cs, Pb, F d) Li, Si, N e) Cs, Pb, N7 17. Which of the following ions has the largest ionic radius? a) Mg2+ b) Li+ c) Al3+ d) Co3+ e) K+ 18. Choose the correct molecular geometry and hybridization for ICl2+. a) linear, sp hybridization b) linear, sp3d hybridization c) bent, sp2 hybridization d) pyramidal, sp3 hybridization e) bent, sp3 hybridization 19. The molecular geometry of BrF3 is: a) T shaped b) pyramidal c) trigonal planar d) tetrahedral e) linear 20. The correct Lewis dot structure for PCl3 has around phosphorus: a) one lone pair (non bonding) and three bonding pairs b) two lone pairs (non bonding) and two bonding pairs c) two lone pairs (non bonding) and three bonding pairs d) three lone pairs (non bonding) and two bonding pairs e) one lone pair (non bonding) and two bonding pairs 21. The hybridization around Sn in the SnO2 molecule