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) PbS2
b) Ca3P2
c)Ca3N2
To approximate the attractive portion of the lattice energy for 1 mole of salts, we need to consider the ionic radii of the ions involved. However, since I cannot access specific lab manuals or tables, I will provide a general explanation of how to approach this problem.
Lattice energy is the energy released when one mole of an ionic compound is formed from its constituent ions in the gas phase. It depends on the magnitude of the charges on the ions and the distance between them. The greater the charge magnitude and the smaller the distance, the higher the lattice energy.
Ionic radii provide a measure of the size of an ion. Typically, the radii decrease across a period from left to right in the periodic table and increase down a group. Ca2+ is a cation, while S2-, P3-, and N3- are anions.
To approximate the lattice energy, you would need to determine the ionic radii of the cations and anions involved in each compound. Then, you can use the values to compare the sizes of the ions. Generally, a smaller ion size implies a stronger attractive force and a higher lattice energy.
Once you have the ionic radii, you can compare them and make an estimation of the relative values of the lattice energies for each compound.
Please consult your lab manual or any relevant reference material to obtain the specific ionic radii for the ions in question, and then use the provided information to make your estimations.