# But what are anti-bonding pi-orbital? In search for an intuitive explanation [closed]

Imagine that you want to explain to an undergraduate why they have to to shade the pi-orbitals in a symmetrical way, i.e. dark on top (+), white on bottom (-) for two neighbouring pi-orbitals because they are bonding (or anti bonding), but then the student asks: why?!.. Can anyone explain why this is without knowing about quantum mechanics and diving into molecular orbital theory? Intuitively, it makes no sense that an electron should 'care' why if they are 'on top' or 'on the bottom' of the nucleus.

I have a hard time both intuitively understanding, but also explaining why we care about bonding and anti-bonding orbitals. I know that I should draw them, and that one is stabilising while the other is destabilising. However, for a person with limited chemistry knowledge my reasons for why is simply: 'because it is so'. This is not very satisfying. I think this has something to do with the phase and wave equations (..etc) - but again,..this seems to go into heavy chemistry (..or?).

Question: Does someone have a nice analogy, or way of explaining why this is - and what anti-bonding orbitals are without any very high-level chemistry concepts?

I think there are others struggling with this concepts, as I found a few questions here on stack exchange that failed to give a satisfying answer. This might be because the concept is extremely complexes and not possible to understand without quantum mechanics... but thats why I want to ask the question here in hope of an intuitive explanation.

• Just a thought: You are asking in the same place where you were unable to find a simple enough answer.. – Safdar Sep 11 '20 at 14:44
• Would you accept the wave-particle duality? Probably I can explain it I guess – Soumyadwip Chanda Sep 11 '20 at 15:20
• Electrons do not exist as either particles or waves.. See Wave-particle duality. Attempting to answer something that has its basis in a different level of theory using outdated versions is dangerous and may lead to unneeded misconceptions.. – Safdar Sep 11 '20 at 16:21
• The problem with analogies is that you have to draw upon experience, which is naturally rooted in the macroscopic world. However, this is of limited experience for quantum mechanical concepts. At best, with an analogy, your understanding is incomplete, and at worst, you develop misconceptions due to the baggage of constructing the analogy. – Zhe Sep 11 '20 at 16:51
• Can anyone explain why this is without knowing about quantum mechanics and diving into molecular orbital theory? I'm afraid that won't be possible. If you are talking about orbitals, you need a basic understanding of orbitals. The most basic ones will be atomic orbitals, but looking at molecules you will need molecular orbitals. Since this is an approximation to the wave function, you will need (at least some) understanding of quantum mechanics. – Martin - マーチン Sep 11 '20 at 16:53

To clarify, the red and blue orbitals don't totally collapse each other and disappear - just where they might "touch". So each orbital, red and blue, still contains one (negative) electron, but there is no continuity of electron travel from and around one nucleus to the other, because there is a gap, a node, a location where there is no electron density, where they might come in contact. This represents two atoms that have been dissociated from their bonded state as a molecule. They could have been bonded together using two red-flashing orbitals, but got excited by some energy input that brought one electron up to a blue energy which is now out of sync with the red orbital, and finds it repulsive. A $$pi$$ bond between two carbon atoms would show the two upper lobes of each atomic orbital to have the same color and the two lower lobes of each atomic orbital to have the other color: both upper and lower regions would be bonding. A $$pi$$ antibond would have a red and a blue in the upper region and a blue and a red in the lower region: repulsive!