2.The image below shows two nitrogen atoms. For these two atoms to form a stable molecule, N2, how many electrons would have to be part of covalent bonds?

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01-02-2017
Chemistry

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2.The image below shows two nitrogen atoms. For these two atoms to form a stable molecule, N2, how many electrons would have to be part of covalent bonds?

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jamilashah jamilashah · Answer 1 · 2017-02-01T15:21:30+01:00

Since N2 is a covalent bond, the lewis dot structure of N2 would have a triple bond. Each bond contains 2 electrons, so if it has a triple bond it contains 6 electrons.
Calculate the number of valence electrons of N2
N= 2x 5 = 10
N2 has a total of 10 valence electrons, to become stable each N atom needs 8 electrons.
So, therefore, 6 electrons would have to be a part of covalent bonds because they share 6 electrons in a triple bond.

Stephvelez2 Stephvelez2 · Answer 2 · 2018-11-11T16:09:20+01:00

Stephvelez2 Stephvelez2

11-11-2018

D. 6 electrons

A single nitrogen atom has five electrons in its outer energy level to start, and will be most stable with an octet, or 8 electrons in its outer level.

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