# Urgent: Hybridisation

The problem is as follows:

Decide if the following pairs of orbitals overlap to form a σ bond, π bond, or no bond at
all. Explain your reasoning in each case, including a sketch of the orbitals. Assume the
bond lies along the z-axis.

(a) 2pz and 2pz
(b) 2py and 2px
(c) sp3 and 2pz
(d) 2py and 2py

And here are what I think the solutions are:

(a) 2pz and 2pz will form a σ bond as they are on the same axis and will over lap end-on-end

(b) 2py and 2px will form a π bond as they will over lap side by side

(c) sp3 and 2pz will not form a bond as the next hybridisation is sp3d orbital which contains an electron from a d orbital

(d) 2py and 2py will form a σ bond as they are on the same axis and will over lap end-on-end

If these are wrong could, could you please hint to why, and if I have managed to get something from the textbook (i.e., they are right) could you please help with expanding on the ideas.

Many thanks for your time and replies

chemisttree
Homework Helper
Gold Member
...(d) 2py and 2py will form a σ bond as they are on the same axis and will over lap end-on-end

Remember the question stated...
Assume the bond lies along the z-axis.

It might help to draw a picture of these two orbitals approaching each other along the z axis and then determine what type of interaction you might expect.

thank you, i have now solved the problem as i didn't quite understand what the problem was asking
and i realised i have posted this in wrong section of the forum, sorry