What about unsymmetrical systems, in which the two atoms are not identical? Again, the coefficients C 1 and C 2 will change. Consider CH 3 F: Since F is the electronegative, the bonds are polarized (unequal). Thus, F likes having a higher electron density around it, so the \(σ\) bond is skewed and no longer symmetrical. By analogy, the exact opposite is true for the \(σ^{*}\). Let’s return to betulin for a moment. Take a minute to look at its structure and think about how complex it would be if we drew molecular orbitals for every bond. That’s why we draw molecules using line-angle notation, a short-hand of the Lewis model of bonding. You just need to recognize where it comes from.