Nitrogen Electrons

How many electrons are unpaired in the orbitals of nitrogen?

1. Nitrogen Electrons Configuration

Electron Configuration of Nitrogen and Oxygen Nitrogen has 7 electrons and has an electron configuration of 1s2 2s2 and 2p3 In the video I use the diagonal r. Biological nitrogen fixation can be represented by the following equation, in which two moles of ammonia are produced from one mole of nitrogen gas, at the expense of 16 moles of ATP and a supply of electrons and protons (hydrogen ions): N 2 + 8H+ + 8e-+ 16 ATP = 2NH 3 + H 2 + 16ADP + 16 Pi.

2 Answers

Explanation:

Nitrogen atom has total #7# electrons. Two will fill up the #n=1# level, and then there are five electrons in the #n=2# level.

Nitrogen can bond three times with other electrons to fill up it's shell with 8, (8-5=3). And these are those #3# unpaired electrons which were residing the #2p# sub-shell of the Nitrogen atom , before the formation of #3# bonds.

The #2p_x#, #2p_y# and #2p_z# orbitals of the Nitrogen atom have #1# unpaired electron in each of them as shown below :-

Thus, the total no. of unpaired electrons in Nitrogen atom is #3#.

Hope that helps!

Explanation:

From the Periodic Table or other description of the electron shells of nitrogen we see that its configuration is #1s^2 2s^2 2p^3#.

That means that it has only 3 electrons in the 2p orbitals. Per Hund's Rule, they will not become paired until each available orbital has one electron in it. Thus, nitrogen contains 3 unpaired electrons - one in each of the available p orbitals.

Nitrogen Electrons Configuration

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