Why is N2 less reactive at room temperature?
Dinitrogen (N2) IS formed by sharing three electron pairs between two nitrogen atoms.The two nitrogen atoms are joined by triple bond(N≡N). The nitrogen atom is very small in size ,therefore the bond length is also quite small(109.8 pm) & as a result the bond dissociation energy is quite high(946Kj / mol).This reason leads N2 to be very less reactive at room temperature.
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10 Comment(s) on this Question
If the size is small then the bond dissociation enthelpy or energy is high due to the the electrons are tightly bonded and having stronger nuclear charge bcz only the number ofelectrons are much as compared to their size
Give the increasing order acidic stronger of hclo ,hclo2, hclo3 ,hclo4?
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For boards, specific answer is required. Nitrogen forms pÏ-pÏ bond with other nitrogen due to small size and high electronegativity. Thus they exist as a very stable diatomic molecule with Bond enthalpy = 941.4kJ/mol which is very difficult to overcome. Thus they are stable at room temperature and less reactive
reply to simran question dinitrogen is unreactive at room temperature. The room temperature varies according to the conditions in which dintrogen is kept.But with the increase in temperature dintrogen reactivity increases.It Liquefies at 77 K and freezes at63 K
NOT PROPER DUDE IF I ASK YOU AT WHAT TEMP IT REACT THAN WHAT YOU SAY
The nitrogen atom is small in size but the two nitrogen atoms are attached to each other by tripple bond.So three bonds have to be broken to make N2 reactive ,as a result the bond dissociation energy is high.
If the size is small then why is the bond dissociation energy high?
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