Refer to the table given for the ionic radii in your lab manual and approximate the attractive portion of the lattice energy for 1 mole of the following salts. (Consider only one bond if more than one bond exists.)

a) Ca3P2
___J
b) MoCl4
___J
c) Cs2O
___J

To approximate the attractive portion of the lattice energy for 1 mole of the given salts, we need to consider the ionic radii of the ions involved. Unfortunately, without access to the table mentioned in your lab manual providing the ionic radii, I cannot perform the calculations for you.

However, I can guide you on how to obtain the information and calculate the lattice energy approximately:

1. Obtain the ionic radii: Look for the table mentioned in your lab manual. It should provide the ionic radii of cations and anions involved in the formation of the given salts.

2. Identify the ions: For each salt, identify the cation(s) and anion(s) involved. In this case, we have:
a) Ca3P2 - The cation is Ca2+ and the anion is P3-.
b) MoCl4 - The cation is Mo4+ and the anion is Cl-.
c) Cs2O - The cation is Cs+ and the anion is O2-.

3. Determine the ionic radii: Once you have identified the ions, find their respective ionic radii in the table provided. Make sure the units are consistent.

4. Calculate the lattice energy: The lattice energy can be approximated using the formula:
Lattice energy = (1.75 x (Q1 x Q2)) / (r1 + r2)
where Q1 and Q2 are the charges of the ions (in multiples of e), and r1 and r2 are their ionic radii.

5. Plug in the values: Substitute the values of the charges and ionic radii into the formula obtained in the previous step, and calculate the lattice energy in joules (J).

Remember, this is just an approximate calculation as lattice energy depends on various factors, and the mentioned formula is a simplified version. The actual lattice energy calculation may involve more complex equations.

Once you have the ionic radii for the given salts, you can perform the calculations using the steps provided.