# 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.

The question is asking you to identify the five compounds from hints.
How to start? Start with compound D. e) gives you the percentage composition and mol mass (mass per 22.4 liters).

the descriptions are so detailed that you can determine the compounds A,B,C,D,and E.

A.

B.

C.

D.

E.

When I was in graduate school we called these railroad problems because we thought the purpose was to railroad us out of the class. Look for a tag on all of the information. For this problem, it is compound E. That MUST be NH3. D gives you percent composition (I assume there is 6.3% hydrogen) so you get a simplest formula and that with the density of the material gives the molecular formula. The 21.28 mL of 1.00 M HCl to titrate 0.726 g compound B gives the molar mass of compound B and the fact it is basic is a give-a-way. Repost with any questions you have.

16 years ago

12 years ago

## So far i have not compleatly worked it out.but compound E is NOT NH3.

it is NH2OH, which you can tell only by its titation information.
compound D is N2O2H4 in some order.
compound A is likely Nitric Acid.

9 years ago

9 years ago

7 months ago

## To solve this problem, let's break down the given information:

a) We are told that compounds C and D are ionic, while compound B is covalent. This means that compounds C and D contain ions, while compound B consists of nonmetals sharing electrons.

b) Nitrogen occurs in its highest oxidation state in compounds A and C, and in its lowest oxidation state in compounds C, D, and E. The formal charge on both nitrogen atoms in compound C is +1, and the formal charge on the only nitrogen atom in compound B is 0. This suggests that compounds A and C contain nitrogen in a positive oxidation state, while compounds C, D, and E contain nitrogen in a negative oxidation state.

c) Compounds A and E exist in solutions that give off gases. The commercially available concentrated solution of compound A is normally 16 M, while the commercial, concentrated solution of compound E is 15 M. This information gives some insight into the concentration and behavior of these compounds in solution.

d) Commercial solutions of compound E are labeled with a misnomer that implies a reaction between a binary, gaseous compound of nitrogen and hydrogen with water to produce ammonium ions and hydroxide ions. However, this reaction actually 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. This information allows us to calculate the molecular formula of compound D based on its percentage composition and density.

f) A formula unit of compound C has one more oxygen atom than a formula unit of compound D. Additionally, compounds C and A have one ion in common when compound A is acting as a strong electrolyte. These hints help us determine the composition and relationship between compounds C, D, and A.

g) Solutions of compound C are weakly acidic, solutions of compound A are strongly acidic, and solutions of compounds B and E are basic. Furthermore, the titration of 0.726 g of compound B requires 21.98 mL of 1.000 M HCl for complete neutralization. This information gives us insights into the acidity/basicity of compounds B, C, and A, as well as their molar masses.

Based on these hints, we can start with compound D. We know from e) that compound D has a composition of 43.7% N and 50.0% O by mass, and a density of 2.86 g/L at STP. Since the molar mass of nitrogen is 14.01 g/mol and the molar mass of oxygen is 16.00 g/mol, we can calculate the molecular formula of compound D.

Next, we can analyze the other hints to identify compounds A, B, C, and E. The information about oxidation states, formal charges, solution behavior, and acidity/basicity can provide clues to determine the types and compositions of these compounds.

Remember to utilize the given information and use it as a starting point for each compound. Good luck!

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