Chapter 9. Chemical Bonds

End-of-Chapter Material

Additional Exercises

  1. Explain why iron and copper have the same Lewis electron dot diagram when they have different numbers of electrons.
  2. Name two ions with the same Lewis electron dot diagram as the Cl− ion.
  3. Based on the known trends, what ionic compound from the first column of the periodic table and the next-to-last column of the periodic table should have the highest lattice energy?
  4. Based on the known trends, what ionic compound from the first column of the periodic table and the next-to-last column of the periodic table should have the lowest lattice energy?
  5. P2 is not a stable form of phosphorus, but if it were, what would be its likely Lewis electron dot diagram?
  6. Se2 is not a stable form of selenium, but if it were, what would be its likely Lewis electron dot diagram?
  7. What are the Lewis electron dot diagrams of SO2, SO3, and SO42−?
  8. What are the Lewis electron dot diagrams of PO33− and PO43−?
  9. Which bond do you expect to be more polar: an O–H bond or an N–H bond?
  10. Which bond do you expect to be more polar: an O–F bond or an S–O bond?
  11. Use bond energies to estimate the energy change of this reaction.

    C3H8 + 5O2 → 3CO2 + 4H2O

  12. Use bond energies to estimate the energy change of this reaction.

    N2H4 + O2 → N2 + 2H2O

  13. Ethylene (C2H4) has two central atoms. Determine the geometry around each central atom and the shape of the overall molecule.
  14. Hydrogen peroxide (H2O2) has two central atoms. Determine the geometry around each central atom and the shape of the overall molecule.
  15. Determine the molecular dipole moments for the following molecules:

    dipole_moment_questions

  16. What is the hybridization in the central atom of:
    1. HCN
    2. NH4
    3. TeBr2
  17. Draw the molecular orbital electron configuration energy diagram of He2 and determine the bond order.
  18. Draw the molecular orbital electron configuration energy diagram of O2 and determine the bond order.

Answers

  1. Iron has d electrons that typically are not shown on Lewis electron dot diagrams.
  1. LiF
  1. It would be like N2:

    \chemfig{\Lewis{4:,P}~\Lewis{0:,P}}

  1. \chemfig{\Lewis{2:4:,O}=\Lewis{6:,S}=\Lewis{0:6:,O}}, \chemfig{\Lewis{4:6:,O}=[:30]S(=[:90]\Lewis{0:2:,O})=[:-30]\Lewis{0:6:,O}},\text{ and }\chemfig{\Lewis{2:4:6:,O}-\ce{S^{2-}}(=[:90]\Lewis{0:4:,O})(=[:-90]\Lewis{0:4:,O})-\Lewis{0:2:6:,O}}
  1. an O–H bond
  1. −2,000 kJ
  1. trigonal planar about both central C atoms
  1. dipole_moment_solutions
  1. He2_MO_config_001
    bond order = 0

License

Icon for the Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License

Introductory Chemistry - 1st Canadian Edition Copyright © 2014 by Jessie A. Key is licensed under a Creative Commons Attribution-NonCommercial-ShareAlike 4.0 International License, except where otherwise noted.

Share This Book