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Question 1 (4 points)

(4 points) 1. Draw the best Lewis structures for NOF and BrF5 and include formal charges on atoms with non-zero values. Concisely identify at least four steps of the procedure for drawing the Lewis structures.

Note: In the formula of the first molecule, atoms are in the order of their atomic numbers; the given formula does not necessarily reflect the actual arrangement of atoms in the structure.
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Question 2 (3 points)

(1.5 points) 2. (a) Draw at least three plausible resonance contributors for the sulfite ion (SO32-).

(0.5 points) 2. (b) Assign formal charges to each atom in the resonance structures of the sulfite ion (SO32-).

(1 points) 2. (c) How many double bonds are present in the experimental (true) structure of the sulfite ion (SO32-)? Write one sentence to justify your answer.
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Question 3 (5 points)

3. T2O3(s) is the ionic compound formed from oxygen and a metal with the form T(s) at 1.00 bar and 298 K.
(0.5 points) (a) Draw the Lewis structure for T2O3. Assume that all the valence electrons from T are required.
(4.5 points) (b) Use the following information to determine the enthalpy of formation for T2O3(s). Express your answer in kJ/(mol T2O3(s)).
Lattice energy for T2O3(s) = -16439 kJ mol-1
ΔHsub for T(s) = 317 kJ mol-1
First ionization energy for T(g) = 610 kJ mol-1
Second ionization energy for T(g) = 1732 kJ mol-1
Third ionization energy for T(g) = 3638 kJ mol-1
Bond dissociation energy for O2(g) = 498 kJ mol-1
First electron affinity for O = -141 kJ mol-1
Second electron affinity for O = 744 kJ mol-1
As part of your problem work you must show the full equations with phases for all steps in the Born-Haber process and you must label each step. Note that you may need to use some of these labels more than once. The Born-Haber process is shown in section 9.5 in your textbook. The steps can be shown following the example on page 344; a diagram like that on page 345 is not required.
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