[Midzik]

Experimental evidence suggests that the nitrogen atom in ammonia, NH3, has four orbitals in the shape of a pyramid or tetrahedron.
I was wondering if someone could confirm this for me. Would it look like this?
I use slashes to represent an electron.

Nitrogen
1s X
2s X
2p / / /

Hydrogen (x3)
1s /
1s /
1s /


Whereby when combined looks like this...

NH3
1s X
2s X
2p XXX

Is this correct? Does this illustration suggest that Nitrogen has four orbitals? or am i missing some sort of hybridization? If hybridization occurs is the new hybrid bond called s3p3 ( three S orbitals combine with 3 P orbitals)?

Thanks!

[Schrödinger]

The s- and p- orbitals of Nitrogen hybridize to for 4 hybrid sp3 orbitals, which overlap with the 1s orbital from each H atom.

[Cat in the Lab]

It will be much more easy if you consider the lewis structure before you predict NH3's shape.
There're 3 single bonds in NH3, while N is the center of all, with a lone pair.
and by VSEPR, NH3 is tetrahedral.
Therefore, there're 5 electrons available for bonding, which is 2s2 and 2p3.
in order to form a tetrahedral arrangement, there should be 4 orbital around N.
Thus it's a sp3 hybridization as followed:
X(lone pair)
/(overlapped with 1s of hydrogen)
/(same)
/(same)

[Midzik]

Thank you!