Draw all resonance structures for the nitryl fluoride molecule, no2f.(a) explicitly draw all h atoms.(b) include all valence lone pairs in your answer.(c) do not include overall ion charges or formal charges in your drawing.(d) do not draw double bonds to oxygen unless they are needed for the central atom to obey the octet rule.(e) draw one structure per sketcher. (f) add additional sketchers using the drop-down menu in the bottom right corner.(g) separate resonance structures using the ↔ symbol from the drop-down menu.

Resonance structures are represented in the picture below.

Explanation:

When there is a double pair of electrons shared between atoms in a molecule, the position of these electrons can be changed, without changing the molecule conformation. This occurs to stabilization, the electrons are relocated. These structures are called resonance structures.

In the molecule of NO₂F, nitrogen has 5 electrons in its valence shell, so it needs 3 electrons to be stable. Oxygen has 6 electrons and needs 2 to be stable, and fluor has 7 electrons and needs one electron to be stable.

Nitrogen still has electrons after the sharing, so it can also share one pair and will have a partial positive charge. One of the oxygens will not complete the octet, so will share only one pair f electron and will have a partial negative charge, that will compensate the positive charge in nitrogen.

The two resonance structures are shown below: