posted this question before and wanted to know if I had gotten the right answers.
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.
A) HNO3
B) Still don't understand
C) N2O2 or NO2 not sure
D) NO
E) NH3 any comments will greatly help
Probably compound A is right although I don't think the questions provides data to prove that.
Compound E is right.
Compound B. 21.98 mL x 1.00M HCl = 21.98 millimoles HCl = 21.98 millimoles compound B in 726 mg compound B. That makes the molar mass of compound B what? I get 33. The compound is basic. So if we have an OH and N, how many more H atoms would we need for compound B. I suspect this is hydroxyl amine which has a molar mass of 33.
That leaves compounds C and D. From statement (e), if N is 43.7% and O is 50.0%, what is the extra 6.3%? I don't think NO2 or N2O2 (or NO) will give those percentages. And what have you ignored in the 6.3%? or is that a typo of some kind? And 2.86 x 22.4 = 64. NO, NO2 or N2O2 don't have a molar mass of 64. I hope this is helpful.
Let's go through the provided information and try to identify the compounds one by one.
a) From the information given, we know that compound C and D are ionic compounds, while compound B is a covalent compound.
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, while the formal charge on the only nitrogen atom in compound B is 0.
c) Compounds A and E exist in solution and 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.
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 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 compound C has one more oxygen atom 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 compound C are weakly acidic, solutions of compound A are strongly acidic, and solutions of compound B and E are basic. The titration of 0.726 g of compound B requires 21.98 mL of 1.000 M HCl for complete neutralization.
Now let's try to identify the compounds based on this information:
A) HNO3: This compound fits the description as a strong electrolyte, having nitrogen in its highest oxidation state, and being strongly acidic. Therefore, compound A is HNO3.
B) The information given does not provide enough clues to determine the exact compound, but we know that it is covalent, has nitrogen in its lowest oxidation state, and has a molar mass of 33 g/mol. One possibility is hydroxylamine (NH2OH), which has a molar mass of 33 g/mol and fits the basic nature of the compound.
C) Based on the information provided, compound C has one more oxygen atom than compound D and is an electrolyte. One possible compound fitting this description is nitrous acid (HNO2), which can ionize in solution to give hydrogen ions and nitrite ions. The Lewis structure for HNO2 can be drawn to be consistent with the information given.
D) According to the statement, compound D has a molar mass of 64 g/mol with 43.7% nitrogen and 50.0% oxygen by mass. One compound that meets these criteria is nitric oxide (NO). The Lewis structure can be drawn for NO, which consists of one nitrogen atom and one oxygen atom linked by a double bond.
E) Compound E is ammonia (NH3), which is consistent with the information given. Ammonia is a gas at STP, has a formula with 43.7% nitrogen, and has a density of 2.86 g/L.
To recap, the identified compounds are:
A) HNO3
B) NH2OH
C) HNO2
D) NO
E) NH3
It is important to note that the identification of the compounds is based on the information provided and is subject to interpretation.