Identify the five compounds of H, N, and O described below. For each compound, write a Lewis structure that is consistent with the information given:

1. Nitrogen occurs in its highest possible oxidation state in compounds A and C.
2. Nitrogen occurs in its lowest possible oxidation state in compounds C, D, and E.
3. The formal charge on both nitrogens in compound C is +1.
4. The formal charge on the only nitrogen in compound B is 0.

The compounds are inferred to be Nitric Acid (HNO3), Nitrogen Gas (N2), Ammonia (NH3) and Hydrazine (N2H4). The nitrogen's oxidation state varies across these, with the highest being in HNO3, zero in N2, and the lowest in NH3 and N2H4. Lewis structures were provided for each.

Explanation:

Based on the information given, we can infer the following compounds:

Compounds A and C: Nitrogen is in its highest oxidation state. A possible compound can therefore be Nitric Acid (HNO3), for which the Lewis structure is: : O = N (+) - O : - H (^+) - O :
Compound B: Nitrogen is in zero oxidation state and the Lewis structure would correspond to Nitrogen gas (N2), which would be : N ≡ N :
Compounds D and E: Nitrogen is in its lowest oxidation state. The compounds can thus be Nitrogen hydrides such as NH3 (Ammonia) and N2H4 (Hydrazine), with the Lewis structures as follows: : N - H : and H2 - N - N - H2 respectively.

The overall pattern shows the diversity of compounds that can be formed with just the elements Hydrogen, Nitrogen, and Oxygen through the variability of Nitrogen's oxidation state.

Learn more about Nitrogen Compounds here:

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