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.