Chapter 24: Problem 33
Is carbon monoxide isoelectronic with nitrogen \(\left(\mathrm{N}_{2}\right)\) ?
Short Answer
Expert verified
Yes, carbon monoxide (CO) is isoelectronic with nitrogen (N2).
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
Electron Configuration
Electron configuration is a way of describing the arrangement of electrons within an atom. The electrons are organized into shells and subshells around the nucleus. This arrangement follows specific rules based on principles such as the Pauli exclusion principle and Hund's rule.
When two species have the same electron configuration, they are referred to as isoelectronic. Isoelectronic species possess identical numbers of electrons and consequently, very similar chemical properties.
Understanding electron configurations helps predict element behavior, including bonding and the formation of molecules. For example, knowing the electron configuration can explain why carbon monoxide (CO) and nitrogen (N2) are isoelectronic, both having 14 electrons arranged in a way that results in similar interactive properties.
When two species have the same electron configuration, they are referred to as isoelectronic. Isoelectronic species possess identical numbers of electrons and consequently, very similar chemical properties.
Understanding electron configurations helps predict element behavior, including bonding and the formation of molecules. For example, knowing the electron configuration can explain why carbon monoxide (CO) and nitrogen (N2) are isoelectronic, both having 14 electrons arranged in a way that results in similar interactive properties.
Carbon Monoxide
Carbon monoxide (CO) is a simple yet crucial molecule in chemistry. It consists of one carbon (C) atom and one oxygen (O) atom. Carbon's atomic number is 6, providing it with 6 electrons. Oxygen has an atomic number of 8, and thus 8 electrons. Together, CO has a total of 14 electrons.
This compound is a colorless and odorless gas. It is formed through the incomplete combustion of carbon-containing fuels. Despite its simplicity, carbon monoxide is dangerous due to its ability to bind with hemoglobin in the blood, preventing oxygen from doing so.
In chemistry, CO is often used in reactions as a ligand in metal carbonyls or for its reducing properties. Its electron configuration and simple structure make it isoelectronic with nitrogen (N2). This means that it has the same number of electrons arranged in similar configurations, granting it similar characteristics.
This compound is a colorless and odorless gas. It is formed through the incomplete combustion of carbon-containing fuels. Despite its simplicity, carbon monoxide is dangerous due to its ability to bind with hemoglobin in the blood, preventing oxygen from doing so.
In chemistry, CO is often used in reactions as a ligand in metal carbonyls or for its reducing properties. Its electron configuration and simple structure make it isoelectronic with nitrogen (N2). This means that it has the same number of electrons arranged in similar configurations, granting it similar characteristics.
Nitrogen Molecule
The nitrogen molecule (N2) is abundantly found in Earth's atmosphere, making up about 78% by volume. Each nitrogen atom has an atomic number of 7, contributing 7 electrons each to the molecule, resulting in a total of 14 electrons.
This diatomic molecule is stable due to the strong triple bond formed between the nitrogen atoms. This bond arises because both nitrogen atoms share three pairs of electrons, making the N2 molecule challenging to dissociate.
Nitrogen is crucial in chemistry and life sciences, participating in processes such as the nitrogen cycle. In addition to forming compounds and acting as a building block in organic chemistry, the nitrogen molecule is used industrially to create ammonia for fertilizers.
Being isoelectronic with CO, both molecules share the same total number of electrons, giving them similar properties despite having different atomic compositions.
This diatomic molecule is stable due to the strong triple bond formed between the nitrogen atoms. This bond arises because both nitrogen atoms share three pairs of electrons, making the N2 molecule challenging to dissociate.
Nitrogen is crucial in chemistry and life sciences, participating in processes such as the nitrogen cycle. In addition to forming compounds and acting as a building block in organic chemistry, the nitrogen molecule is used industrially to create ammonia for fertilizers.
Being isoelectronic with CO, both molecules share the same total number of electrons, giving them similar properties despite having different atomic compositions.
Atomic Number
The atomic number is a fundamental property of an element, representing the number of protons in an atom's nucleus. It directly determines the element's position in the periodic table and its chemical behavior.
Each proton contributes a positive charge, balancing with the electrons orbiting around the nucleus to make a neutral atom. This balance leads to a stable electron configuration.
For example, carbon has an atomic number of 6, indicating 6 protons and typically 6 electrons in a neutral state. Oxygen's atomic number is 8, meaning it has 8 protons and 8 electrons, while nitrogen has an atomic number of 7.
Understanding atomic numbers is crucial for determining the electron configuration of molecules such as carbon monoxide (14 electrons) and molecular nitrogen, also with 14 electrons, which enables us to identify them as isoelectronic.
Each proton contributes a positive charge, balancing with the electrons orbiting around the nucleus to make a neutral atom. This balance leads to a stable electron configuration.
For example, carbon has an atomic number of 6, indicating 6 protons and typically 6 electrons in a neutral state. Oxygen's atomic number is 8, meaning it has 8 protons and 8 electrons, while nitrogen has an atomic number of 7.
Understanding atomic numbers is crucial for determining the electron configuration of molecules such as carbon monoxide (14 electrons) and molecular nitrogen, also with 14 electrons, which enables us to identify them as isoelectronic.
