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Nitrogen is a diatomic gas at room temperature. These nitrogen atoms are bond by a triple bond. It needs more energy to break this bond. So nitrogen is less reactive.
Ammonia molecule: NH32 NH3 N2 + 3 H2Nitrogen molecule N2 , each molecule containing 2 atoms (of the element) N
nitrogen gas is formed when two nitrogen atoms bond together...thus resulting in atriple bond between the nitrogen atoms. these triple bonds together have a very high bond enthalpy(energy needed to break bonds). so the energy needed to break the bonds is very high. since chemical reactions occur on the basis that bonds need to be broken for new bonds to form....the nitrogen molecule does not react readily under normal circumstances. it was once considered an inert gas before the discovery of the Born-Haber process...as a result of its natural "unreactivity". hence a lot of energy has to be given to the nitrogen molecules for them to dissociate and become atoms .. so that they can react- the central idea behind the Born-haber process. (british)
Yes,Whenever an organism dies, decomposers break down the corpse into nitrogen in the form of ammonia. This nitrogen can then be used again by nutrifying bacteria to fixnitrogen for the plants
Firstly, N2 is treated sometimes as an inert gas as it is used to create an inert atmosphere so that no reactions take place. But nitrogen has many compounds as it is more chemically reactive than helium or any other inert gases. Its compounds: e.g. Ammonia, Nitric Acid etc. More on: http://en.wikipedia.org/wiki/Nitrogen
A Nitrogen molecule(N2) has a triple bond between it Nitrogen will only react only if the bond is broken. And since Chlorine cannot break this triple bond, under normal conditions, it does not react with nitrogen readily.
Nitrogen is chemically less reactive. This is because of the high stability of its molecule, N2. In N2, the two nitrogen atoms form a triple bond. This triple bond has very high bond strength, which is very difficult to break. It is because of nitrogen's small size that it is able to form pπ−pπ bonds with itself. This property is not exhibited by atoms such as phosphorus. Thus, phosphorus is more reactive than nitrogen.
The reason why nitrogen gas is inert at room temperature is because the triple bond between the two nitrogen atoms in each nitrogen molecule (N2) is very strong, and therefore it takes a lot of energy to break that bond, and until that bond is broken, the nitrogen cannot react with any other chemical.
we can't breathe in and break a triple bond
A Nitrogen molecule has a triple bond.So high amount of energy is needed to break down this bond.Bond dissociates naturally in occasions like lightning.So Nitrogen's reactivity is very low.Nitrogen has a little bit high molecular mass.So it has a high escape velocity.As a result of those Nitrogen remains in atmosphere in huge amount.
green plants do not have the "power" to break the triple bond of N2 molecule. in better words, they do not have suitable enzymes. on the other hand, some bacteria have, the so colled "nitrogen fixing bacteria", living on legume plant roots.
It is unreactive because diatomic nitrogen is bonded by a triple bond. This triple bond takes so much energy to break, that it does not likely naturally react with other substances
Nitrogen is a diatomic gas at room temperature. These nitrogen atoms are bond by a triple bond. It needs more energy to break this bond. So nitrogen is less reactive.
Ammonia molecule: NH32 NH3 N2 + 3 H2Nitrogen molecule N2 , each molecule containing 2 atoms (of the element) N
Although the bond holding the nitrogen atoms together is difficult to break, some types of bacterium are able to break the triple covalent bond of N2 gas. The bacteria bind nitrogen atoms to hydrogen creating "fixed" nitrogen, ammonia (NH3) in a process called Nitrogen Fixation. Oxygen ruins this process, so considering our bodies are roughly 65% oxygen, we can't do it.
Because the double bond between nitrogen is very strong
Biology relies on chemistry. The nitrogen must be able to attach to the receptor molecule to be used. Nitrogen fixation renders nitrogen into a less s table form so that it can break bonds and attach to other molecules.