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.
I have no idea where to start for this problem. Please help me.
All of the "Railroad" problems have a give away line. This one has two and you need to know enough chemistry to recognize them when you see them.Let me give you the give away lines and a few hints and let you work on it.
A. The give away line is that commercially available stuff is 16M, it is a strong electrolyte, it has N in its highest oxidation state (+5) so this must be HNO3.
E. The give away lines are that commercially available stuff is 15 M AND (the most telling) is part d about gas forming NH4OH (the misnomer) so this must be NH3.
Extra hint: Look at part e. You can calculate a formula for that, both an empirical and a molecular formula.
Another hint: Look at part g. You can calculate a molar mass for compound B.
To solve this problem, we can break it down into smaller parts and analyze the given information. Let's go step by step:
Step 1: Identify the compounds:
Based on the information provided, we need to identify five compounds composed of the elements hydrogen (H), nitrogen (N), and oxygen (O). Let's assign letters to each compound for easier reference: A, B, C, D, and E.
Step 2: Determine the electrolyte properties:
From the information given, we know that all compounds are electrolytes, but not all are strong electrolytes. Compounds C and D are ionic, and compound B is covalent.
Step 3: Identify the oxidation states of nitrogen:
Compound A and C have nitrogen in its highest oxidation state, while compounds C, D, and E have nitrogen in its lowest oxidation state. Both nitrogen atoms in compound C have a formal charge of +1, and the only nitrogen atom in compound B has a formal charge of 0.
Step 4: Identify the gases released from compounds A and E:
Both compounds A and E release gases in solution. Commercially available concentrated solutions of compound A are 16 M, and the solution of compound E is 15 M.
Step 5: Analyze the misnomer in the labeling of compound E:
The commercially available solution of compound E is labeled to suggest that a binary compound of nitrogen and hydrogen reacted with water to produce ammonium ions and hydroxide ions. However, this reaction only occurs to a slight extent.
Step 6: Calculate the mass percentage and density of compound D:
Compound D is composed of 43.7% nitrogen and 50.0% oxygen by mass. If compound D were a gas at STP, it would have a density of 2.86 g/L.
Step 7: Compare the formula units of compounds C and D:
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 the strong electrolyte.
Step 8: Analyze the acidity/basicity of the compounds:
Solutions of compound C are weakly acidic, solutions of compound A are strongly acidic, and solutions of compounds 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.
By following these steps, you should be able to systematically analyze the given information and determine the compounds, as well as draw Lewis structures for each compound.