I stumbled upon this problem:
"The s and p orbitals of Pb are poorly energetically matched, and do not noticeably hybridize. In Pb(II) compounds, the two remaining electrons on Pb reside in an unhybridized s orbital, and bonding utilizes only the p-orbitals. In gaseous PbCl2, what is the approximate angle between the Pb—Cl bonds?"
Answer is ~90 degrees. Can anybody explain why this is so? I figured that the Lewis Dot would look something like lead flanked by two...
Hybridized/Unhybridized orbitals
"The s and p orbitals of Pb are poorly energetically matched, and do not noticeably hybridize. In Pb(II) compounds, the two remaining electrons on Pb reside in an unhybridized s orbital, and bonding utilizes only the p-orbitals. In gaseous PbCl2, what is the approximate angle between the Pb—Cl bonds?"
Answer is ~90 degrees. Can anybody explain why this is so? I figured that the Lewis Dot would look something like lead flanked by two...
Hybridized/Unhybridized orbitals