Chapter 3, Problem 3.7P

L. C. Allen has suggested that a more meaningful formal charge can be obtained by taking into account theelectronegativities of the atoms involved Men’s formula for this type of charge—referred to as the Lewis—Langmuir $\left(\text{L}—\text{L}\right)$ charge —of an atom, A, bonded to another atom, B, is
$\text{L}-\text{Lcharge}=\left(\text{US}\right)\text{ group number of A}—\text{number of unshared electrons on A}-\text{2}{\displaystyle \underset{B}{\overset{}{\sum }}\frac{xA}{xA+XB}\left(\begin{array}{l}\text{number of bonds}\\ \text{between A and B}\end{array}\right)}$
where $X_A$ and $X_B$ designate the electronegativities. Using this equation, calculate the $L-L$ charges for CO, ${\text{NO}}_{-}$ , and HF, andcompare the results with the corresponding formal charges Do you think the $L-L$ charges are a better representation ofelectron distribution? (See L C Alien, J. Am Chem Soc., 1989 111, 9115; L. D. Garner, T.L Meek, B. G. Patrick,THEOCHEM, 2003, 620, 43.)