When Nitrogen makes bonds to three other atom, the geometry form is
tetrahedral angle due to the disproportionate influence of the
non-bonding lone pair. Each of the four-sp3 hybrid orbitals takes one electron
each, and that leaves us with 1 more electron. Then, this goes into one of the sp3
hybrid orbitals that already contains 1 electron, giving it a total of 2
electrons. The lone pair on nitrogen is stereo-chemically active. Therefore, 1s
orbital and 3p orbitals create four degenerate sp3 orbitals, but bonding occurs
to only 3 other atoms, and those in the non-bonding orbital do not participate. Therefore, the geometry
shape of a molecule depends on the spatial positioning of covalent bonds
to atoms.
