The iodine bromide molecule, IBr, is an interhalogen compound. Assume that the molecular orbitals of IBr are analogous to the homonuclear diatomic molecule F2. (c) One of the valence MOs of IBr is sketched here. Determine whether each of the following statements about this orbital is true: i. This is an antibonding orbital. ii. The larger contribution is from the I atom. iii. The energy of the molecular orbital is closer in energy to the valence atomic orbitals of Br than to those of I.

Video transcript

Hello everyone today. We are being given the falling problem. One of the valence molecular orbital's of iodine chloride is shown below. What is the most likely reason why the atomic orbital contributions to this molecular orbital are different in size. So we have to note that iodine and chlorine separately have different quantum numbers. Quantum numbers are represented by the variable N on the periodic table. It is based on the period that the atom or element is in. And so we have the relationship that a larger quantum number indicates a larger sized orbital. So based on the period of of iodine, iodine is in period of five and chlorine is in period three. And so due to them having different quantum numbers, their size of their orbital's will differ. So for our answer We have iodine quantum number of five And Chlorine has a quantum number of three. And so different quantum numbers, which I'll abbreviate as in will result in different sized orbital's in different sized orbital's. And so this would be our final answer. Overall, I hope this helped. And until next time