N₂²⁻, or the dinitrogen dianion, is generally considered to be unstable. The formation of N₂²⁻ involves adding two electrons to the nitrogen molecule, which can lead to significant repulsion between the negatively charged species and destabilize the bond. While theoretical studies suggest it can exist under certain conditions, it is not commonly encountered in practice due to its high reactivity and tendency to decompose.
Elements prefer to live in their natural forms.N2 and O2 are more stable than NO.Added:Air is a mixture of N2 and O2 molecules, where NO is a compound, chemically formed by reaction: N2 + O2 --> 2 NO. This reaction does not take place at normal conditions as in the air around us.
The s electrons in N2 are unbonded; there are four of them in each nitrogen atom and therefore 8 in the molecule N2.
The bond order of N2 is 3, and the bond order of O2 is 2.
Three: The reaction equation is N2 + 3 H2 -> 2 NH3
N2 + 3H2 ==> 2NH3moles N2 = 1.20 molesmoles NH3 formed = 1.20 moles N2 x 2 moles NH3/1 moles N2 = 2.40 moles NH3mass NH3 = 2.40 moles x 17 g/mole = 40.8 g NH3
n2-3n+2
Three pairs of electrons.
(N2) + 3(H2) = 2(NH3)
Elements prefer to live in their natural forms.N2 and O2 are more stable than NO.Added:Air is a mixture of N2 and O2 molecules, where NO is a compound, chemically formed by reaction: N2 + O2 --> 2 NO. This reaction does not take place at normal conditions as in the air around us.
The s electrons in N2 are unbonded; there are four of them in each nitrogen atom and therefore 8 in the molecule N2.
Nitrogen gas (N2) consists of a covalent bond between two nitrogen atoms. This bond involves the sharing of electrons between the atoms, resulting in a stable molecule.
N2+ and N2- I just did it on mastering chem and it worked I'm pretty sure its because when you count the valence electrons in N2+ and N2- you get 9 and 11 respectively because these are odd there has to be an unpaired electron in each
More NO would form
n2-1 and n2-4 are trivial cases because of n2-m2=(n-m)(n+m). So the only prime of the form n2-1 is 3 and of the form n2-4 is 5.
The bond order of N2 is 3, and the bond order of O2 is 2.
Nitrogen is a diatomic molecule, meaning it exists naturally as N2 because it is more stable when bonded to another nitrogen atom. Each nitrogen atom in the molecule shares three pairs of electrons with the other nitrogen atom, resulting in a stable molecular structure.
n2 + 11n + 18 = n2 + 2n + 9n + 18 = n(n+2) + 9(n+2) = (n+9)*(n+2)