This is part of a marathon problem, we have to identify the five compunds of H, N, and O described below. For each compound, I have to write a Lewis structure that is consistent with the information given.

a.) All the compunds are electrolytes, although not all of them are strong electrolytes. Compunds C and D are ionic and compund B is covalent.

b.) Nitrogen occurs in its highest possible oxidation state in compunds A and C; nitrogen occurs in its lowest oxidation state in compunds C,D, and E. The formal charge on both nitrogen in compund C is +1; the formal charge on the only nitrogen in compund B is 0.

c.) Compund A and E exist in solution. Both solutions give off gases. Comercially available concentrated solutions of compund A are normally 16 M. The commercial, concentrated solution of compound E is 15 M.

d) Commercial solutions of compund E are labeled witha misnomer that implies that a binary, gaseous compund of nitrogen and hydrogen reacted with watert to produce ammonium ions and hydroxide ions. Actually this reaction occurs to only a slight extent.

e) Compound D is 43.7% N and 50.0% O by mass. If compound D were a gas at STP, it would have a density of 2.86 g/L.

f) A formula unit of compund C has one more oxygen than a formula unit of compound D. Compounds C and A have one ion in common when compound A is acting as the strong electrolyte.

g) Solutions of C are weakly acidic; solutions of compound A are strongly acidic; solutions of compound B and E are basic. The titration of .726 g of compound B requires 21.98 ml of 1.000 M HCl for complete neutralization.

This is due tomm and I have no idea what the question is asking or how to start.

To solve this problem, we need to analyze the given information and use it to identify the compounds. Let's break down the information step by step:

a) From the given information, we know that compounds C and D are ionic, compound B is covalent, and all compounds are electrolytes.

b) The information states that nitrogen occurs in its highest oxidation state in compounds A and C, and in its lowest oxidation state in compounds C, D, and E. It also mentions the formal charges on nitrogen in compound C and B. Based on this, we can conclude that compounds A, C, D, and E all contain nitrogen, while compound B does not.

c) Compounds A and E exist in solution, giving off gases. Additionally, it provides the concentration of commercially available solutions of A and E. We can infer that compounds A and E are soluble in water and form gases when dissolved.

d) Compound E's commercial solution is labeled with a misnomer, implying a reaction with water that produces ammonium ions and hydroxide ions to a slight extent. This suggests that compound E is a weak base.

e) Compound D is given as containing 43.7% N and 50.0% O by mass. If it were a gas at STP, it would have a density of 2.86 g/L. This tells us the elemental composition and density of compound D.

f) It states that compound C has one more oxygen than compound D, and that compounds C and A have one ion in common when A is acting as a strong electrolyte. This suggests that compounds C and A share an ion, which implies a similarity in their chemical formulas.

g) Solutions of compound C are weakly acidic, compound A is strongly acidic, and compounds B and E are basic. It also provides a titration calculation involving compound B and HCl. This tells us about the acid-base properties of the compounds and gives us an indication of the strength of their acidity.

By considering all the provided information, we can infer the following:
- Compounds C and A share an ion, suggesting they are related in some way.
- Compound B has nitrogen.
- Compound E is a weak base.
- Compound D is a gas with a specific composition and density.
- Compound A is a strong electrolyte.

Now, with this understanding, we can proceed to identify and draw the Lewis structures for the five compounds based on their properties and compositions.