What is the oxidation number of \(\mathrm{N}\) in nitrate, nitrite, \(\mathrm{NO}, \mathrm{N}_{2} \mathrm{O}\) and \(\mathrm{N}_{2}\) ?

Short Answer

Expert verified
The oxidation numbers of Nitrogen in nitrate, nitrite, \(\mathrm{NO, N_{2}O}\) and \(\mathrm{N_{2}}\) are +5, +3, +2, +1 and 0 respectively.

Step by step solution

01

Identify the oxidation number of Nitrogen in Nitrate

The nitrate ion is \(\mathrm{NO_{3}^{-}}\), a polyatomic ion. Following rule 4, the sum of oxidation numbers in this ion equals the charge of the ion, which is -1. There is 1 Nitrogen atom and 3 Oxygen atoms. Oxygen usually has an oxidation state of -2 (rule 5). Therefore, the overall contribution from Oxygen is -6. Let's denote the oxidation number of Nitrogen as x. Hence, \(x - 6 = -1\). Solving for x gives us \(x = +5\). Thus, the oxidation number of Nitrogen in nitrate is +5.
02

Identify the oxidation number of Nitrogen in Nitrite

The nitrite ion is \(\mathrm{NO_{2}^{-}}\), another polyatomic ion. The same rationale applies here, and the overall charge of the ion should be equal to -1. There are 2 Oxygen atoms, contributing -4 overall. Denoting the oxidation number of Nitrogen as x, form the equation: \(x - 4 = -1\). Solving for x gives: \(x = +3\). Thus, the oxidation number of Nitrogen in nitrite is +3.
03

Identify the oxidation number of Nitrogen in NO

The molecule \(\mathrm{NO}\) is a neutral compound. Applying rule 3, the sum of oxidation numbers should be equal to 0. One Oxygen atom contributes -2. Denoting the oxidation number of Nitrogen as x, we have: \(x - 2 = 0\). Solving for x, we get \(x = +2\). Thus, the oxidation number of Nitrogen in \(\mathrm{NO}\) is +2.
04

Identify the oxidation number of Nitrogen in N2O

Similarly, \(\mathrm{N_{2}O}\) is a neutral molecule so the sum of oxidation numbers should be equal to 0. One Oxygen atom contributes -2 while two Nitrogen atoms share the same oxidation number, denoted as x. Form the equation as \(2x - 2 = 0\). Solving for x, we get \(x = +1\). Thus, the oxidation number of Nitrogen in \(\mathrm{N_{2}O}\) is +1.
05

Identify the oxidation number of Nitrogen in N2

In \(\mathrm{N_{2}}\), Nitrogen is in its elemental state. Hence per rule 1, the oxidation number of Nitrogen in \(\mathrm{N_{2}}\) is 0.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Oxidation States
Understanding the oxidation states of elements is critical in chemistry, especially when it comes to redox reactions. An oxidation state, often referred to as oxidation number, is a theoretical charge that an atom would have if all bonds to it were ionic. This concept helps chemists determine how electrons are distributed in a molecule and which atoms are oxidized or reduced during chemical reactions. For instance, in nitrate (o3^-{}o3^-o3^-{}o3^-{}), we determined the oxidation state of nitrogen to be +5. This is because the combined oxidation states of the oxygen atoms total -6, and the overall charge of the ion is -1. The equation we use is based on the known oxidation state of oxygen (-2) and the charge of the ion: o3^-{} = -1). Solving for the nitrogen's oxidation state in such equations allows us to gain insight into the chemical behavior of the substances in reactions.
Redox Chemistry
Redox chemistry is the branch of chemistry that deals with oxidation-reduction reactions, where the transfer of electrons between substances takes place. These reactions are fundamental to numerous processes, including metabolism and corrosion. In the context of determining oxidation numbers, appreciating redox chemistry can help us see why certain elements change their oxidation states. When we say that an element is oxidized, it loses electrons and its oxidation number increases, as seen with nitrogen going from o{} to various nitrogen oxides. Conversely, reduction involves gaining electrons and a decrease in oxidation number. This understanding of electron transfer is key to both predicting and balancing chemical equations for redox reactions.
Polyatomic Ions
Polyatomic ions are charged entities composed of two or more covalently bonded atoms. It is important to know the common oxidation states of the atoms within these ions to determine the overall charge. For example, in both nitrate (o3^-{}) and nitrite (o2^-{}), oxygen has a known oxidation state of -2. Since these ions carry a negative charge, the oxidation states of all atoms must add up to that charge. By understanding the typical oxidation states of oxygen and the rules governing oxidation numbers, we can deduce the less obvious oxidation states of other atoms in the polyatomic ion, like nitrogen, in the various compounds such as o{}, o2^-{}, and o3^-{}. This knowledge is especially useful in predicting the products of chemical reactions and in understanding the structure of chemical compounds.
Chemical Bonding
Chemical bonding is the force that holds atoms together in molecules and compounds. There are several types of chemical bonds, including ionic, covalent, and metallic bonds. The nature of the bond between atoms can affect their oxidation states. For example, in an ionic bond, electrons are transferred completely from one atom to another, leading to clearly defined oxidation states. In contrast, covalent bonds involve the sharing of electrons, and the oxidation state of an atom in a covalent bond is determined by pretending that the shared electrons are assigned to the more electronegative atom. This is the case with polyatomic ions, such as nitrate and nitrite, where nitrogen and oxygen share electrons. Understanding the type of bonding in a substance can aid in predicting its properties and behavior in chemical reactions.

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