Drawing the Lewis Structure for NOFViewing Notes:
Transcript: Let's do the NOF Lewis structure. Nitrogen, on the periodic table, is in group 5 or 15, so it has 5 valence electrons. Oxygen has 6, and Fluorine has 7; for a total of 18 valence electrons. Nitrogen is the least electronegative, that'll go in the center. Put the Oxygen here and then the Fluorine on the other side. We'll put two valence electrons between the atoms to form chemical bonds. We've used four. Around the outside, 6, 8, 10, over here, 12, 14, 16, and then back to the center, 18. We can see Oxygen has eight valence electrons, so it has an octet; as does Fluorine, full outer shell. But Nitrogen only has six valence electrons. If we move these two valence electrons here from the Oxygen into the center and share them with the Nitrogen, that'll make a double bond. By doing so, Oxygen still has eight valence electrons, but now Nitrogen also has eight valence electrons. And the Fluorine didn't change; it also has eight valence electrons. So we've used all 18 valence electrons, and each of the atoms has octets. If we check the formal charges, we'll see that each atom has a formal charge of zero. So this is the best Lewis structure for NOF. This is Dr. B. with the NOF Lewis structure, and thanks for watching. |
|