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This is due to its bonding, which is unique among the diatomic elements at standard conditions in that it has an N≡N triple bond. Triple bonds have short bond lengths (in this case, 109.76 pm) and high dissociation energies (in this case, 945.41 kJ/mol), and are thus very strong, explaining dinitrogen's low level of chemical reactivity. [28] [45]
A triple bond in chemistry is a chemical bond between two atoms involving six bonding electrons instead of the usual two in a covalent single bond. Triple bonds are stronger than the equivalent single bonds or double bonds, with a bond order of three. The most common triple bond is in a nitrogen N 2 molecule; the second most common is that ...
The less well-characterised ways involve dinitrogen donating electron pairs from the triple bond, either as a bridging ligand to two metal cations (μ, bis-η 2) or to just one (η 2). The fifth and unique method involves triple-coordination as a bridging ligand, donating all three electron pairs from the triple bond (μ 3-N 2).
Nitrogen can be fixed by lightning converting nitrogen gas (N 2) and oxygen gas (O 2) in the atmosphere into NO x (nitrogen oxides). The N 2 molecule is highly stable and nonreactive due to the triple bond between the nitrogen atoms. [81] Lightning produces enough energy and heat to break this bond [81] allowing nitrogen atoms to react with ...
Similar to carbon–carbon bonds, these bonds can form stable double bonds, as in imines; and triple bonds, such as nitriles. Bond lengths range from 147.9 pm for simple amines to 147.5 pm for C-N= compounds such as nitromethane to 135.2 pm for partial double bonds in pyridine to 115.8 pm for triple bonds as in nitriles. [2]
For example, with the benzo-fused unsaturated nitrogen heterocycles, pyrrole provides indole or isoindole depending on the orientation. The pyridine analog is quinoline or isoquinoline, and the class of analogues with two nitrogen atoms is known as the benzodiazines. For azepine, benzazepine is the preferred name.
Since nitrogen is more electronegative than carbon, metal-nitrosyl complexes tend to be more electrophilic than related metal carbonyl complexes. Nucleophiles often add to the nitrogen. [2] The nitrogen atom in bent metal nitrosyls is basic, thus can be oxidized, alkylated, and protonated, e.g.: (Ph 3 P) 2 (CO)ClOsNO + HCl → (Ph 3 P) 2 (CO ...
For this reason, few examples exist of complexes containing both CO and N 2 ligand. Transition metal-dinitrogen complexes can contain more than one N 2 as "end-on" ligands, such as mer-[Mo(N 2) 3 (PPr n 2 Ph) 3], which has octahedral geometry. [15] In another example, the dinitrogen ligand in Mo(N 2) 2 (Ph 2 PCH 2 CH 2 PPh 2) 2 can be reduced ...