Need help to rewrite

To begin with, the characteristic properties of the quadruple bonds and the electron configuration is that they are very strong but short bonds. They have interesting spectroscopic characteristics such as their bright colors. Mo₂(O₂CCH₃) is a bright yellow and K₄Mo₂Cl₈×2H₂O has a bright magenta color which is due to the d to d* transition. They can also decompose if in air too long.

In each of these compounds, the Mo2 will have a charge of +4 and a total number of electron valence shell of 12 which equates to 8 electrons (4 bonding molecular orbitals). The four d orbitals occupied are s (dz2), p (dxz, dyz), d (dxy). 

Unfortunately, due to equipment and time, the experiment did yeild the highest and best compounds. The only IR that was able to be down was of Mo₂(O₂CCH₃)_4. The IR (3001 cm, 2357 cm -1, 2165 cm -1, and 2023) showed one similar peak (3001 cm-1) similar to molybdenum stretching bond. The final product Mo₂Cl₄ [P(C₄H₉) ₃]₄ was not able to dissolve in chloroform so no NMR was able to be completed.

Some errors may have started since the first synthesis since it was left to sit in a flask for a week. The reaction could have started decomposing, which resulted in such a small yield of (approx. 6%). Another issue that may have arised was during the last synthesis of Mo₂Cl₄ [P(C₄H₉) ₃]₄. During filtering, the reaction flask was dropping resulting in a drop of product. The small amount of final product was not able to be characterized