Solving Hybridisation: 2pz, 2px, sp3, 2py Bonds

[pavadrin]

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
pavadrin

 

[chemisttree]

...(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.

 

[pavadrin]

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