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Hybridization in N2 is:
- a)sp4
- b)sp2
- c)sp3
- d)None
Correct answer is option 'D'. Can you explain this answer?
Verified Answer
Hybridization in N2 is:a)sp4b)sp2c)sp3d)NoneCorrect answer is option '...
The hybridization of O2 ,N2 and F2 is Sp2 , Sp, Sp3 . Steric factor = number of bonded atoms + number of lone pair . The hybridization of O2, N2, and F2are sp2, sp, sp3 respectively. As we know between O-O , there are two bonds one is sigma and other is pi bond.
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Most Upvoted Answer
Hybridization in N2 is:a)sp4b)sp2c)sp3d)NoneCorrect answer is option '...
Hybridization in N2 is None.
Explanation:
Hybridization is the process of mixing atomic orbitals to form new hybrid orbitals that are suitable for bonding. Nitrogen has the electronic configuration of 1s2 2s2 2px1 2py1 2pz1. The 2s and the three 2p orbitals of nitrogen participate in hybridization.
In the case of N2, it does not undergo hybridization. Instead, it forms a triple bond between the two nitrogen atoms. The triple bond consists of one sigma bond and two pi bonds. Each nitrogen atom contributes one electron to form the sigma bond, and the other two electrons form the pi bonds.
The triple bond between the two nitrogen atoms is very strong, and it requires a lot of energy to break it. This is why nitrogen gas (N2) is very stable and unreactive under normal conditions.
In conclusion, the hybridization in N2 is none, as it does not undergo hybridization but instead forms a triple bond between the two nitrogen atoms.
Explanation:
Hybridization is the process of mixing atomic orbitals to form new hybrid orbitals that are suitable for bonding. Nitrogen has the electronic configuration of 1s2 2s2 2px1 2py1 2pz1. The 2s and the three 2p orbitals of nitrogen participate in hybridization.
In the case of N2, it does not undergo hybridization. Instead, it forms a triple bond between the two nitrogen atoms. The triple bond consists of one sigma bond and two pi bonds. Each nitrogen atom contributes one electron to form the sigma bond, and the other two electrons form the pi bonds.
The triple bond between the two nitrogen atoms is very strong, and it requires a lot of energy to break it. This is why nitrogen gas (N2) is very stable and unreactive under normal conditions.
In conclusion, the hybridization in N2 is none, as it does not undergo hybridization but instead forms a triple bond between the two nitrogen atoms.
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Community Answer
Hybridization in N2 is:a)sp4b)sp2c)sp3d)NoneCorrect answer is option '...
The no of bond between N2 is 3.
(one Sigma bond and two pi bond).
We all know
hybridization = (no of Sigma bond with central atom + no of lone pair on central atom)
electronic configuration of N is : 1s^2 2s^2 2p^3.
no of electron in valence shell is 5.
and we above see the no of bond between N2 is 3 and rest of two electron is a pair of electron in valence shell of N.
and hence hybridization of N2 is sp.
(one Sigma bond and two pi bond).
We all know
hybridization = (no of Sigma bond with central atom + no of lone pair on central atom)
electronic configuration of N is : 1s^2 2s^2 2p^3.
no of electron in valence shell is 5.
and we above see the no of bond between N2 is 3 and rest of two electron is a pair of electron in valence shell of N.
and hence hybridization of N2 is sp.
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Hybridization in N2 is:a)sp4b)sp2c)sp3d)NoneCorrect answer is option 'D'. Can you explain this answer? for Chemistry 2025 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about Hybridization in N2 is:a)sp4b)sp2c)sp3d)NoneCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for Chemistry 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Hybridization in N2 is:a)sp4b)sp2c)sp3d)NoneCorrect answer is option 'D'. Can you explain this answer?.
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