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Magazine Chapter 4: Problem 47
Nitric acid is a strong oxidizing agent. State which of the following species is least likely to be produced when nitric acid reacts with a strong reducing agent such as zinc metal, and explain why: \(\mathrm{N}_{2} \mathrm{O}, \mathrm{NO}, \mathrm{NO}_{2}\), \(\mathrm{N}_{2} \mathrm{O}_{4}, \mathrm{~N}_{2} \mathrm{O}_{5}, \mathrm{NH}_{4}^{+}\).
Short Answer
Expert verified
\(\mathrm{NH}_4^+\) is least likely produced due to extreme reduction required.
Step by step solution
01
Identifying Species Likely Produced
In a reaction with a reducing agent, nitric acid \( \mathrm{HNO}_3 \) can be reduced to various nitrogen species. These reduced forms are usually in lower oxidation states compared to nitric acid. Commonly produced species in such reactions are \( \mathrm{NO} \), \( \mathrm{N_2O} \), and occasionally \( \mathrm{NO_2} \).
02
Analyzing Oxidation States
The oxidation state of nitrogen in each species must be considered.\( \mathrm{HNO_3} \) has nitrogen in +5 oxidation state. - In \( \mathrm{NO} \), nitrogen is in +2 oxidation state. - In \( \mathrm{N_2O} \), it's in the +1 oxidation state.- In \( \mathrm{NO_2} \), nitrogen is in the +4 oxidation state.- In \( \mathrm{N_2O_4} \) and \( \mathrm{N_2O_5} \), nitrogen remains high at +4 and +5 respectively.- \( \mathrm{NH}_4^+ \) has nitrogen in the -3 oxidation state.
03
Determining the Least Likely Species
Consider the reducing capacity of zinc and the stability of products.\( \mathrm{NH}_4^+ \) involves reducing nitrogen all the way to -3, which is highly unlikely in one step with zinc. Meanwhile, others involve less drastic reductions.Species \( \mathrm{N_2O_4} \) and \( \mathrm{N_2O_5} \) are usually formed as dimeric or oxygen-rich forms which are less favored with a typical reducing environment.
04
Conclusion
Amongst these possibilities, \( \mathrm{NH}_4^+ \) is the least likely to be produced with zinc as it would require an extremely strong reduction which normally involves hydrogen, not zinc.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Oxidation States
Understanding oxidation states is crucial when predicting the products of a chemical reaction involving an oxidizing and reducing agent. The oxidation state indicates the degree of oxidation of an element in a compound. In the case of nitric acid \( \mathrm{HNO_3} \), nitrogen is in a +5 oxidation state. This is a very high oxidation state, meaning nitrogen can gain electrons to become less positive.
Different nitrogen species have varying oxidation states, and these changes play a central role in their formation:
Different nitrogen species have varying oxidation states, and these changes play a central role in their formation:
- In \( \mathrm{NO} \), nitrogen is found in a +2 oxidation state, showing it has gained three electrons from its original form in nitric acid.
- \( \mathrm{N_2O} \) has nitrogen in a +1 oxidation state.
- In \( \mathrm{NO_2} \), nitrogen holds a +4 oxidation state.
- \( \mathrm{N_2O_4} \) and \( \mathrm{N_2O_5} \) maintain nitrogen at +4 and +5, close to its original form.
- \( \mathrm{NH}_4^+ \) has nitrogen in a -3 oxidation state, indicating a substantial gain of electrons and is highly reduced compared to the others.
Reducing Agents
Reducing agents are substances that donate electrons to other reactants during a chemical reaction. Zinc is an example of a strong reducing agent, having the ability to effectively donate electrons. In reactions with nitric acid, zinc not only pushes forward the electron transfer process but also determines the extent of reduction of nitric acid.
The strength of a reducing agent helps dictate which products of nitrogen can potentially form. Zinc, given its properties:
The strength of a reducing agent helps dictate which products of nitrogen can potentially form. Zinc, given its properties:
- Can reduce nitrogen in nitric acid to lower oxidation states.
- Promotes reactions that form products like \( \mathrm{NO} \) and \( \mathrm{N_2O} \).
- Struggles to substantially reduce nitric acid to form \( \mathrm{NH}_4^+ \), as this would require an advanced reduction process not typical unless an even stronger reducing agent, such as elemental hydrogen, is in play.
Reaction Products
When nitric acid reacts with zinc, the nature of nitrogen species produced as products is quite interesting. The reaction typically yields gases, illustrating the transfer of electrons from zinc to the nitrogen species.
Possible reaction products include:
Possible reaction products include:
- \( \mathrm{NO} \)
- \( \mathrm{N_2O} \)
- \( \mathrm{NO_2} \)
Zinc Metal
Zinc is a common and effective reducing agent used in many chemical reactions, known for its ability to readily donate electrons. In the context of reactions with nitric acid:
- Metallic zinc can easily be oxidized, which means it effectively loses electrons.
- These lost electrons can then reduce other elements or ions, especially in compounds like nitric acid.
- As it gets oxidized, the zinc itself turns into \( \text{Zn}^{2+} \), while the nitric acid is reduced to various nitrogen oxides.
Oxidizing Agents
Oxidizing agents are substances that accept electrons from other species during a chemical reaction. Nitric acid, \( \mathrm{HNO_3} \), serves as a very strong oxidizing agent due to its high nitrogen oxidation state of +5. When paired with a reducing agent like zinc:
- Nitric acid can accept electrons and undergo reduction through the reaction process.
- The high affinity for electron acceptance facilitates the conversion of nitrogen to lower oxidation states, resulting in species like \( \mathrm{NO} \) or \( \mathrm{N_2O} \).
- Its oxidizing power is why the reaction seldom proceeds to \( \mathrm{NH}_4^+ \), as this would require absorption of a large number of electrons beyond typical nitrogen reactions involving zinc.
