What hybrid orbitals are used by nitrogen in the following species
a) NH3
b) H2N-NH2
c) NO3
To determine the hybrid orbitals used by nitrogen in each of the given species, we need to follow a few steps:
Step 1: Count the number of electron groups (bonding pairs and lone pairs) around nitrogen.
Step 2: Determine the type of hybridization based on the number of electron groups.
Step 3 (optional): Check for the presence of any pi bonds.
Let's go through these steps for each species:
a) NH3:
1. Count the number of electron groups around nitrogen: There are three bonding pairs and one lone pair, totaling four electron groups.
2. Determine the type of hybridization: For four electron groups, nitrogen undergoes sp3 hybridization.
3. Check for the presence of any pi bonds: NH3 does not have any pi bonds.
Therefore, nitrogen in NH3 is sp3 hybridized.
b) H2N-NH2:
1. Count the number of electron groups around nitrogen: There are two nitrogen atoms bonded to each other, so there is one electron group for each nitrogen. Additionally, there is one lone pair on each nitrogen, totaling three electron groups.
2. Determine the type of hybridization: For three electron groups, nitrogen undergoes sp2 hybridization.
3. Check for the presence of any pi bonds: H2N-NH2 has a double bond (pi bond) between the two nitrogen atoms.
Therefore, nitrogen in H2N-NH2 is sp2 hybridized.
c) NO3-:
1. Count the number of electron groups around nitrogen: There are three oxygen atoms bonded to nitrogen, so there are three electron groups.
2. Determine the type of hybridization: For three electron groups, nitrogen undergoes sp2 hybridization.
3. Check for the presence of any pi bonds: NO3- has a double bond (pi bond) between nitrogen and one of the oxygen atoms.
Therefore, nitrogen in NO3- is sp2 hybridized.
In summary:
a) NH3: sp3 hybridized nitrogen
b) H2N-NH2: sp2 hybridized nitrogen with a pi bond
c) NO3-: sp2 hybridized nitrogen with a pi bond