What hybrid orbitals are used by nitrogen and phosphorous atoms in the following species?
(a) NH3, (b) PCl4+, (c) H2N-NH2
http://www.youtube.com/watch?v=QvqNUQAzars
To determine the hybrid orbitals used by the nitrogen and phosphorus atoms in the given species, we need to follow a few steps. Here's how:
(a) NH3 (Ammonia):
1. Nitrogen forms three sigma bonds with three hydrogen atoms in NH3.
2. The electronic configuration of nitrogen is 1s2 2s2 2px1 2py1 2pz1.
3. The three sigma bonds require three hybrid orbitals, which will be a combination of the 2s, 2p, and 2p orbitals.
4. Since there are three sigma bonds, nitrogen in NH3 undergoes sp3 hybridization.
Hence, the nitrogen atom in NH3 uses sp3 hybrid orbitals.
(b) PCl4+ (Phosphorus tetrachloride cation):
1. Phosphorus forms four sigma bonds with four chlorine atoms in PCl4+.
2. The electronic configuration of phosphorus is 1s2 2s2 2p6 3s2 3p3.
3. The four sigma bonds require four hybrid orbitals, which will be a combination of the 3s, 3p, and 3p orbitals.
4. Since there are four sigma bonds, phosphorus in PCl4+ undergoes sp3 hybridization.
Hence, the phosphorus atom in PCl4+ uses sp3 hybrid orbitals.
(c) H2N-NH2 (Diazane):
1. There are two nitrogen atoms in H2N-NH2, connected by a single bond.
2. Each nitrogen forms two sigma bonds, one with hydrogen and one with the other nitrogen atom.
3. The electronic configuration of nitrogen is 1s2 2s2 2px1 2py1 2pz1.
4. The two sigma bonds require two hybrid orbitals. The remaining two unhybridized p orbitals on each nitrogen atom form the pi bond.
5. Since there are two sigma bonds, each nitrogen in H2N-NH2 undergoes sp hybridization.
Hence, the nitrogen atoms in H2N-NH2 use sp hybrid orbitals.
In summary:
(a) NH3: Nitrogen uses sp3 hybrid orbitals.
(b) PCl4+: Phosphorus uses sp3 hybrid orbitals.
(c) H2N-NH2: Nitrogen uses sp hybrid orbitals.