Nitrogen typically forms three covalent bonds because it has five valence electrons, with three unpaired electrons available for bonding. This allows nitrogen to form three single bonds, or combinations such as one single and one double bond, or a triple bond, to complete its octet
. However, nitrogen can also form a fourth bond in certain cases through a coordinate covalent bond, where nitrogen donates a lone pair of electrons to another atom that has an empty orbital. An example of this is the ammonium ion (NH4+), where nitrogen forms four bonds, one of which is a coordinate bond
. In rare and complex cases, such as in some metal cluster compounds, nitrogen can be coordinated to more than four atoms (up to six or even seven), but these are exceptions involving coordination chemistry rather than typical covalent bonding
. Summary:
- Normal covalent bonds nitrogen can form: 3 bonds (most common)
- Can form 4 bonds including a coordinate covalent bond (e.g., ammonium ion)
- Rarely, nitrogen can be bonded to more atoms in complex coordination compounds (up to 6 or 7)
Thus, under typical conditions, nitrogen forms three bonds, but it can form up to four bonds when including coordinate bonding
