Provide the resonance structure including formal charges denoted in the illustration shown below. Which is the major contributor to the resonance hybrid of the compound shown?

Provide the two resonance structures for nitromethane, CH₃NO₂. Give the formal charge of the atoms in each structure (no need to show zero formal charges). 

Give all the possible resonance structures (some will not obey the octet rule) for pyrrole. Show the curve arrows to represent the conversion of one structure to another.

The skeleton of 1,2-difluorobenzene is given below

It has two fluorines replacing adjacent hydrogens in the ring. Does it have resonance structures? If yes, draw all of them.

Draw the resonance hybrid for the cyanate ion (OCN^–).

Draw the Lewis structure for H₂SO₄, HSO₄^–, and SO₄^2–. For each species, determine the maximum number of equivalent resonance structures. Sulfur is the central atom in all three species. On the other hand, if the molecule contains hydrogen atoms they are attached to the oxygen atoms. Only include the best structures, e.g. a structure with bad formal charges should not be included. 

The molecule H₂SO₄ has______ equivalent Lewis structures.

The molecule HSO₄^– has______ equivalent Lewis structures.

The molecule SO₄^2– has______ equivalent Lewis structures

The SNO⁻ ion and the NSO⁻ ion are two simple ions from a large family of compounds called the NSO compounds. These compounds are mainly found in geological formations within asphaltenes and other mixtures. The SNO⁻ ion is more stable than the NSO⁻ ion. Draw Lewis structures for both ions including any resonance forms. Use formal charges to determine why SNO⁻ ion is more stable than the NSO⁻ ion.