How do I draw a Born-Haber Cycle for diphosphorous pentasulfide? Formula: P2S5, but you knew that!

Thanks in advance!

I tried find one on the web for P2S6 but no luck. Here is one for NaCl. Use it as a template for P2S5.

http://chemistry.bd.psu.edu/jircitano/BH.html

I appreciate your help, but I've got several examples already. Drawing a Born-Haber Cycle for NaCl seems to be very different from drawing one for P2S5. I don't understand how to use the IE's (Ionization energies), especially because both P ions and S ions would have a 3- and 2- charge respectively. I understand that you can't or won't GIVE answers, but any hint would be greatly appreciated. (What would my teacher tell me to do?)

I think I just figured out what my teacher would do if I asked him how to do this; he would laugh. If I'm not mistaken, you can only draw Born-Haber Cycles for ionic compounds. P2S5 is covalent, so it's impossible. Any input? Is that true?

To draw a Born-Haber cycle for diphosphorous pentasulfide (P2S5), you need to understand the steps involved in the formation of the compound and the corresponding energy changes that occur. Here's how you can draw a Born-Haber cycle for P2S5:

1. Determine the individual elements involved in the formation of P2S5 and their standard states (S8, P4).

2. Start with the reactants on the left side of the cycle. In this case, you have P4(solid phosphorus) and S8(solid sulfur). You can represent them as P4 and S8 with the corresponding phase notation.

3. The first step is to convert the reactants into their respective gaseous atoms. This involves breaking the P4 molecule and the S8 molecule into individual atoms. Each bond-breaking process requires energy, so you need to indicate it as an uphill arrow (ΔH).

4. Next, you need to ionize the atoms to form gaseous ions. Phosphorus atoms lose electrons to form P5+ ions, and sulfur atoms gain electrons to form S2- ions. These ionization processes are also endothermic and should be indicated as uphill arrows.

5. After ionization, the next step is to form the ionic compound P2S5. This involves the combination of the P5+ and S2- ions to form P2S5(s). The formation of an ionic compound releases energy as it involves the formation of ionic bonds. This release of energy is indicated as a downhill arrow (ΔH).

6. Finally, you can add the overall reaction of the formation of P2S5 at the bottom of the cycle, indicating the energy change accompanying the reaction (enthalpy change, ΔHf).

Remember to label each energy change (ΔH) with the corresponding values that can be obtained from reference sources or calculated using appropriate chemical equations.

Keep in mind that the Born-Haber cycle is a visual representation, so you can adjust the size of the arrows and the energy scales to proportions that make the cycle clear and understandable.

Note: Since I am an AI text-based bot, I cannot provide a graphical representation of the Born-Haber cycle. However, I hope the steps outlined above are helpful in guiding you to draw the Born-Haber cycle for diphosphorous pentasulfide (P2S5).