Question

Order the following molecules from lowest to highest oxidation state of the nitrogen atom: \(\mathrm{HHO}_{3}, \mathrm{NH}_{4} \mathrm{Cl}, \mathrm{N}_{2} \mathrm{O}, \mathrm{NO}_{2}\) \(\mathrm{NaNO}_{2}\)

Short answer

The correct order of the molecules from lowest to highest oxidation state of the nitrogen atom is: \(NH_4Cl\), \(N_2O\), \(NaNO_2\), \(NO_2\), \(HHO_3\).

Step-by-step solution

Understanding the rules for calculating oxidation states

Each atom in a molecule has an oxidation state which helps in keeping track of electrons in a chemical reaction. The following rules should be followed to assign oxidation states: 1. The oxidation state of any pure element (in its elemental form) is 0. 2. The oxidation state of a monatomic ion is equal to its charge. 3. Oxygen usually has an oxidation state of -2, with some exceptions. 4. Hydrogen has an oxidation state of +1 when bonded to non-metals and -1 when bonded to metals. 5. The sum of the oxidation states of all atoms in a compound is equal to the overall charge on the compound. Now, we can apply these rules to find the oxidation states of nitrogen in the given molecules.

Calculating the oxidation state of nitrogen in each molecule

1. HHO3: In this molecule, H (hydrogen) has an oxidation state of +1 and O (oxygen) has an oxidation state of -2. Since there are 3 oxygen atoms, the total contribution from O atoms is 3*(-2) = -6. The contribution from H atoms is 1*1 = 1. Hence, the oxidation state of N (nitrogen) is x + 1 - 6 = 0; x = 5. 2. NH4Cl: The compound can be written as (NH4)+ (Cl)- to show that it's an ionic compound, where (NH4)+ is the ammonium ion and (Cl)- is the chloride ion. In this compound, Cl has an oxidation state of -1. In the ammonium ion (NH4)+, the contribution from four H atoms is 4*1 = 4. Hence, the oxidation state of N is x + 4 = 1; x = -3. 3. N2O: In this molecule, O has an oxidation state of -2. So, the oxidation state of N is x + x - 2 = 0; x = 1. 4. NO2: In this molecule, O has an oxidation state of -2. Since there are 2 oxygen atoms, the total contribution from O atoms is 2*(-2) = -4. Hence, the oxidation state of N is x - 4 = 0; x = 4. 5. NaNO2: Here, we have an ionic compound Na+ (NO2)-, where Na has an oxidation state of +1. The NO2- ion contribution is -1, since it's a nitrite ion. In the NO2- ion, O has an oxidation state of 2*(-2) = -4. Therefore, the oxidation state of N is x - 4 = -1; x = 3.

Arrange the molecules from lowest to highest oxidation state

Now that we have the oxidation states of nitrogen in each molecule, we can arrange them from lowest to highest: 1. Lowest oxidation state: NH4Cl (-3) 2. N2O (1) 3. NaNO2 (3) 4. NO2 (4) 5. Highest oxidation state: HHO3 (5) So, the correct order is: \(NH_4Cl\), \(N_2O\), \(NaNO_2\), \(NO_2\), \(HHO_3\).

Key concepts

Chemistry Rules

When it comes to chemistry, there are fundamental rules that help scientists understand the behavior of molecules and atoms. One of these key ideas is the concept of oxidation states, which serve to track how electrons are distributed in a chemical reaction or compound. Here are some essential rules for determining oxidation states:

• The oxidation state of a pure element is always 0. For example, in the molecule \(O_2\), each oxygen atom has an oxidation state of 0.
• A monatomic ion has an oxidation state equal to its charge, like \( ext{Cl}^-(\) which has an oxidation state of -1.
• Oxygen usually carries an oxidation state of -2 unless it's found in peroxides or certain other rare compounds.
• Hydrogen typically has an oxidation state of +1 when bonded to non-metals, and -1 when bonded to metals.
• The sum of all oxidation states in a neutral compound must add up to 0, while in an ion, it equals the ion's charge.

These rules provide a framework that helps chemists unmask the oxidation states in various substances and understand their behavior in reactions.

Oxidation State Calculation

Calculating the oxidation state of an element within a compound requires careful attention to the rules of oxidation mentioned previously. Let's explore how you can determine the oxidation state of nitrogen in different chemical compounds.First, take each molecule and apply the standard rules to deduce the oxidation state for nitrogen. In compounds like \(HHO_3\), hydrogen has an oxidation state of +1 and oxygen is -2. With three oxygen atoms, the total contribution from oxygen becomes -6. Calculating for nitrogen's oxidation state involves balancing the equation to satisfy the charge neutrality of the compound.In \(NH_4Cl\), understanding the ionic structure aids significantly. Recognize the ammonium ion \(NH_4^+\) and chloride ion \(Cl^-\) separately. Use the sum of oxidation states for hydrogen in the ammonium ion, which totals +4, to determine nitrogen's oxidation state. The exercise continues similarly for \(N_2O\), \(NO_2\), and \(NaNO_2\), each requiring the application of these rules to identify nitrogen's oxidation state precisely.

Nitrogen Compounds

Nitrogen is an essential element in chemistry and is found in a multitude of compounds, each with distinct properties and structures. Its versatility is demonstrated by the variety of oxidation states it can exhibit, contributing to the complexity of nitrogen chemistry.For example, in \(NH_4Cl\), nitrogen is part of an ammonium ion, bearing a stable negative oxidation state of -3. This differs greatly from its presence in \(NO_2\), where it has an oxidation state of +4, due to the two oxygen atoms bonded with it, exerting their own oxidation influence.Nitrogen also plays a significant role in the structure of nitrous oxide \(N_2O\) and nitrite ion \(NO_2^-\) in \(NaNO_2\), where it displays unique oxidation states of +1 and +3 respectively. Each compound showcases nitrogen's ability to adjust its oxidation state according to the surrounding elements, reacting and combining in varied ways.

Chemical Reactions Tracking

Understanding oxidation states is not only useful for identifying the state of an element in a compound but also critical in tracking chemical reactions. Oxidation states provide insight into how electrons are transferred during reactions, helping to predict the products and balance reactions properly. In redox reactions, which involve oxidation and reduction, determining the oxidation state changes allows chemists to track electron transfer. For instance, when nitrogen changes oxidation states across different compounds during a reaction, it directly indicates which species gets oxidized and which gets reduced. By thoroughly understanding and calculating oxidation states, we can gain deeper knowledge of the underlying electron movement in reactions. This not only helps predict reaction products but also aids in synthesizing desired compounds and optimizing reaction conditions in laboratories.