1. Write the electron configurations for the following: Si^{4+}, Si^{4–}, Sn^{2+}, Pt^{4+}, Pb^{2+}.

2. Find all of the Russell-Saunders terms for the p^{3} configuration and energy order them.

3. The boiling points for a series of metals is shown below. Based on this data, should boiling point be considered a periodic property? Why or why not?

Metal |
Boiling Point (°C) |

Mn |
2061 |

Fe |
2861 |

Co |
2927 |

Ni |
2913 |

Cu |
2562 |

Zn |
907 |

4. For the following compounds, draw the Lewis dot structure, estimate all of the bond angles, determine the hybrid on the central atom, and give the point group: a) POCl_{3}; b) ClO_{2}^{–}; c) GeCl_{4}; d) AsF_{5}; e) OF_{2}.

5. Estimate the order of the boiling points for N_{2}, NO, NO_{2}, and NH_{3}. Explain your reasoning.

6. Draw the molecular orbital energy level diagram for S_{2}. What is the bond order?

7. Find the irreducible representations for the σ bonds in SiF_{2}Cl_{2}.

8. Find the irreducible representations for the s orbitals for I, Br, and Cl in *trans*-IBr_{2}Cl_{2}^{–}. Use projection operators to find the functional form of the group orbitals and energy order all of the group orbitals.