identifying hybridized v unhybridized


Moderators: Chem_Mod, Chem_Admin

ZachMoore1C
Posts: 30
Joined: Fri Apr 06, 2018 11:04 am

identifying hybridized v unhybridized

Postby ZachMoore1C » Fri Jun 01, 2018 5:42 pm

How can you tell whether an orbital is hybridized or unhybridized?

jadam_1E
Posts: 30
Joined: Fri Apr 06, 2018 11:01 am

Re: identifying hybridized v unhybridized

Postby jadam_1E » Sat Jun 02, 2018 1:37 am

If you draw the Lewis structure of a molecule or formula unit then you can find the number of bonds that are responsible for the creation of the compound. Look at the number of unpaired electrons for the center atom in its ground state, ie Carbon's 2Px and 2Py orbitals have unpaired electrons. If the number of bonds on the center atom is greater than the number of unpaired valence electrons for the center atom in its ground state, then that atom must have a hybridized orbital. Carbon is known to have a tetrahedral arrangement of bonds (4 atoms bound to it) so carbon definitely has hybridized orbitals (2SP3) in order to have four orbitals with unpaired electrons.


Return to “Hybridization”

Who is online

Users browsing this forum: No registered users and 2 guests