CHEM 133-Lesson Questions

CHEM 133-Lesson Questions Calculate the Lattice Energy of KCl(s) given the following data using the Born-Haber cycle: ΔHsublimation K = 79.2 kJ/mol IE1 K = 418.7 kJ/mol Bond EnergyCl–Cl = 242.8 kJ/mol EACl = 348 kJ/mol ΔHKCl(s) = –435.7 kJ/mol  A. 828 kJ/mol  B. 707 kJ/mol  C. 629 kJ/mol  D. -165 kJ/mol  E. 288 kJ/mol Answer Key:B Feedback: See Chapter 07 Question 2 of 25 4.0/ 4.0 Points Of the following elements, which has the highest electronegativity?  A. Sc  B. P  C. As  D. S Answer Key:D Feedback: See Chapter 07 Question 3 of 25 4.0/ 4.0 Points Consider the following reaction: A2 + B2 → 2AB ΔH = –321 kJ Bond energy (A2) = 1/2AB Bond energy (B2) =393 kJ/mol. What is the numerical value for Bond energy (A2) ?  A. 714 kJ/mol  B. -161 kJ/mol  C. 238 kJ/mol  D. 554 kJ/mol Answer Key:C Feedback: See Chapter 07 Question 4 of 25 4.0/ 4.0 Points Which of the following bonds would be the most polar without being considered ionic?  A. Si-O  B. C-O  C. N-O  D. Mg-O  E. O-O Answer Key:A Feedback: See Chapter 07 Question 5 of 25 0.0/ 4.0 Points What is the formal charge on the central nitrogen atom in the most favorable Lewis structure for the fulminate ion, CNO– , based on minimizing formal charge overall?  A. +2  B. -1  C. -2  D. 0 