Mu1 Final Exam Review

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SCH 4U1 FINAL EXAM REVIEW ATOMIC STRUCTURE AND MOLECULAR ARCHITECTURE 1. Describe the wave mechanical model of the atom. 2. Write the ground state electron configuration for Br. 3. Explain why the first ionization energy for Ne is significantly greater than Na. 4. Distinguish between ionization energy and electronegativity. 5. How does VSEPR Theory account for the fact that the bond angle in H2O is less than NH3? 6. Which of the following molecules are polar? Include diagrams detailing their molecular shape (according to VSEPR), bond angles and molecular dipole (if present). CO2 BCl3 NF3 AsH3 CCl4 CH2Cl2 N2 H2S 7. Distinguish between intermolecular and intramolecular…show more content…
Calculate the equilibrium constant, Ke. [0.85] 4. If the equilibrium concentration of F2(g) is 1.50 mol/L and H2(g) is 2.5 mol/L, determine the concentration of HF(g) at equilibrium. [1.92 mol/L] F2 (g) + H2 (g) === 2 HF(g) Ke = 0.98 5. If 0.100 mol of hydrogen iodide is placed in a 1.0 L container and allowed to reach equilibrium, find the concentrations of all reactants and products at equilibrium. 2 HI (g) === H2 (g) + I2 (g) Ke = 1.84(10-2 [H2]=[I2]= 1.07(10-2 mol/L, [HI]=7.86(10-2 mol/L 6. A 1.00 L reaction vessel initially contains 9.28(10-3 moles of H2S. At equilibrium, the concentration of H2S of 7.06(10-3 mol/L. Calculate the value of Ke for this system. 2 H2S (g) === 2 H2 (g) + S2 (g) [1.1(10-4] 7. At a given temperature, the following system has an equilibrium constant, Ke, of 0.27. C(g) + B(g) === 2 E(g) The system was established by placing 8.00 moles of C and 5.0 moles of B in a 4.0 L vessel. Calculate the concentration of all substances at equilibrium. [C]= 1.68 mol/L; [B]= 0.62 mol/L; [E]= 0.64…show more content…
9. What is meant by “dynamic equilibrium”? EQUILIBRIUM APPLICATIONS: SOLUBILITY 1. a) Calculate the solubility of AgBr in pure water. Ksp of AgBr is 7.7(10-13 [8.8(10-7 mol/L] b) Calculate the solubility of AgBr in a 0.10 mol/L NaBr solution. [7.7(10-12 mol/L] 2. How many milligrams of PbI2 can you dissolve in 300 mL of water at 25(C? Ksp of PbI2 is 1.4(10-8 [210 mg] 3. Calculate the solubility product constant, Ksp, of SrCl2 if 8.0 mg dissolves in 200 mL to form a saturated solution at 25(C. [6.4(10-11] 4. Seawater is saturated with AgCl. If the [Cl-] in seawater is 0.53 mol/L, calculate the concentration of Ag+ ions in seawater. The Ksp of AgCl is 1.8(10-10 [3.40(10-10 M] 5. The solubility product constant for PbF2 is 3.7(10-8. Calculate the solubility of PbF2 in g/L. [5.1(10-1 g/L] 6. Why is water a good solvent? Explain. 7. 0.50 g of CaSO4 is dissolved in 1.0 L of water. Is this solution saturated? The Ksp of CaSO4 is

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