945.33 kJ/mol
positive
triple bond between the nitrogen atoms
Covalent bond
Nitrogen bases bond by the help of covalent or hydrogen bonds
A ionic bond
Nitrogen Is Uncreative beacuase of the triple bond between 2 nitrogen atom,which have a bond enthalpy of 945kjmol-1,and this result for a fewer reactions of nitrogen.
Enthalpy is the measurement of total energy change of a reaction. The energy of bond formation and bond breaking can be used to calculate the bond enthalpy of the reaction. Bond enthalpy is the enthalphy change when 1 mol of bond is broken. Therefore the general equation to calculate the enthalpy change is energy of bond broken subtract by energy of bond formation.
This might not be of much help, but it is longer than Nitrogen monoxide, as the bond enthalpy is higher in a N-O bond. There is not much on this issue on the Internet unfortunately.
The reason for this lies in the bond dissociation enthalpy of Nitrogen molecule, The two atoms are bonded by a triple bond whose enthalpy is 941.4 KJ mol-1 . So the two atoms are not very free to bond with others Not only this, the higher tendency of P to form catenation is its bigger size than N which makes the bond cleavage with other atoms easy.
the enthalpy of atomisation of hydrogen is equal and (in principle) identical to the bond dissociation enthalpy of the H-H bond. However, IF the first is measured by calorimetry and the second by spectrometry there might be a systematic difference.
positive
Bond enthalpy is the energy required to break a chemical bond whereas lattice energy is the enthalpy of formation of one mole of an ionic compound from gaseus ions under standard conditions.
no
Molar bond enthalpy shows the change in a bond association. For example, if one mole of bond is broken, the energy change that results is DHd (degree).
Nitrogen is not a bond; it is the single element Nitrogen.
This bond is covalent.
The length of nitrogen-to-nitrogen bond is approx. 100 pm.