Indicate which orbitals overlap to form the s bonds in each compound. a. BeBr2 b. HgCl2 c. ICN

Video transcript

Hi everyone here we have a question asking us to determine the orbital's which compromise the sigma bonds in each molecule, A methane, be boron, tri chloride and see xenon die fluoride. So we're gonna start here with methane. So we have carbon in the middle Attached to four hydrogen and our carbon has tetra khedr electron geometry. So it is a sp three hybridization. Our carbon hydrogen bonds, Our carbon is sp three plus our hydrogen is an S orbital. So that is our answer for a. Now we have B boron tri chloride. It has boron in the middle Attached to three Corinne's And each chlorine has three lone pairs boron has diagonal planner electron geometry. So it has sp two hybridization. It's boron chlorine bonds. It's B Is sp two hybrid orbital plus it's chlorine is p orbital. So that is our answer for P lastly we have C. Zenon de fluoride. It has xenon Attached to two Florins And each flooring has three long pairs And the scene on has three lone pairs. Xenon is Trigana by parameter electron geometry. So sp three D hybridization. The xenon flooring bonds. The xenon is S. P three D hybrid orbital plus the flooring is p orbital. And that is our answer for C. Thank you for watching. Bye