CHEM133 Week 9 Lesson 4 Quiz

1. Question: Which one of the following is most likely to be an ionic compound? 2. Question: The phosphorus atom in PCl3 would be expected to have a 3. Question: The phosphorus atom in PCl3 would be expected to have a give CH3Cl and hydrogen chloride. 4. Question: How many of the following molecules have no dipole moment? 5. Question: Atoms having equal or nearly equal electronegativities are expected to form 6. Question: Element A has an electronegativity of 0.8 and element B has an electronegativity of 3.0. Which statement best describes the bonding in A3B? 7. Question: Of the following elements, which has the highest electronegativity? 8. Question: In which case is the bond polarity incorrect? 9. Question: Calculate the Lattice Energy of KCl(s) given the following data using the Born-Haber cycle: 10. Question: A chlorine atom in Cl2 should have a. 11. Question: Which one of the following is most likely to be a covalent compound? 12. Question: Which is the longest bond? 13. Question: The compound IF5 contains 14. Question: Draw the Lewis structure for SO42-. How many equivalent resonance structures can be drawn? 15. Question: Identify the correct statement. 16. Question: The compound ICl contains 17. Question: Which of the following represent the Lewis structure for N? 18. Question: In the Lewis structure for BeCl2 , what is the formal charge on the Be atom? 19. Question: Which of the following contains an atom that does not obey the octet rule? 20. Question: How many lone pairs of electrons are on the Br atom in BrF5? 21. Question: Which ionic compound would be expected to have the highest lattice energy? 22. Question: How many lone pairs of electrons are on the I atom in IF4+? 23. Question: In the Lewis structure of CH3OH, how many lone pairs of electrons are there? 24. Question: Use the bond energies provided to estimate ΔH°rxn for the reaction below: 25. Question: The arsenic atom in AsCl3 would be expected to have a