Chapter 8: Problem 75
Write Lewis structures for the reaction $$ \mathrm{AlCl}_{3}+\mathrm{Cl}^{-} \longrightarrow \mathrm{AlCl}_{4}^{-} $$ What kind of bond joins \(\mathrm{Al}\) and \(\mathrm{Cl}\) in the product?
Short Answer
Expert verified
A coordinate covalent bond joins \(\mathrm{Al}\) and \(\mathrm{Cl}\) in \(\mathrm{AlCl}_4^-\).
Step by step solution
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
AlCl₄⁻
The molecule \(\mathrm{AlCl}_4^-\) consists of an aluminum (Al) atom surrounded by four chlorine (Cl) atoms. In its Lewis structure, aluminum serves as the central atom. This central position allows it to bond with the additional chloride ion, forming a stable tetrahedral shape. This structure is crucial because it shows how electrons are shared and arranged while also explaining the molecule's shape.
The process begins with \(\mathrm{AlCl}_3\) and a \(\mathrm{Cl}^-\) ion reacting together. Initially, aluminum has three valence electrons, and its goal is to complete its octet by adding electrons. The reaction forms a complex ion, \(\mathrm{AlCl}_4^-\), which is a product of aluminum's increase in electron count, achieving an 8-electron arrangement.
Understanding the geometry and electron distribution in \(\mathrm{AlCl}_4^-\) is essential for comprehending more advanced concepts in chemistry, such as molecular interactions and chemical reactions.
The process begins with \(\mathrm{AlCl}_3\) and a \(\mathrm{Cl}^-\) ion reacting together. Initially, aluminum has three valence electrons, and its goal is to complete its octet by adding electrons. The reaction forms a complex ion, \(\mathrm{AlCl}_4^-\), which is a product of aluminum's increase in electron count, achieving an 8-electron arrangement.
Understanding the geometry and electron distribution in \(\mathrm{AlCl}_4^-\) is essential for comprehending more advanced concepts in chemistry, such as molecular interactions and chemical reactions.
coordinate covalent bond
A coordinate covalent bond, also known as a dative bond, is a type of covalent bond where both electrons in the bond originate from the same atom. In the reaction creating \(\mathrm{AlCl}_4^-\), this particular bond occurs when the lone pair of electrons from the \(\mathrm{Cl}^-\) ion is donated to form a new bond with the aluminum atom.
This concept is significant because it introduces the idea that atoms can share electrons differently. It showcases the flexibility of chlorine to donate its pair as a whole, completing aluminum's octet smoothly.
Coordinate covalent bonds are a critical part of understanding molecular structures. They provide insight into how flexible electron arrangements can tailor specific chemical needs. These unique bonds often occur in complex molecules, like coordination compounds, and expand the possibilities in chemistry for bonding arrangements.
This concept is significant because it introduces the idea that atoms can share electrons differently. It showcases the flexibility of chlorine to donate its pair as a whole, completing aluminum's octet smoothly.
Coordinate covalent bonds are a critical part of understanding molecular structures. They provide insight into how flexible electron arrangements can tailor specific chemical needs. These unique bonds often occur in complex molecules, like coordination compounds, and expand the possibilities in chemistry for bonding arrangements.
valence electrons
Valence electrons are the outermost electrons of an atom and are responsible for an atom's chemical properties and its ability to form bonds. In the context of \(\mathrm{AlCl}_3 + \mathrm{Cl}^-\), the valence electrons of aluminum and chlorine play vital roles.
Aluminum has three valence electrons, which it uses to form bonds with three chlorine atoms in \(\mathrm{AlCl}_3\). Each chlorine atom, with seven valence electrons, shares one with aluminum to complete its own octet. This sharing enables the chlorine atoms in the product \(\mathrm{AlCl}_4^-\) to maintain a stable outer shell.
Valence electrons are also crucial in understanding Lewis structures. These electrons are represented as dots around the atomic symbol. Knowledge of how many valence electrons belong to each atom aids in predicting molecule formation and chemical behavior, functioning as a fundamental aspect of chemistry.
Aluminum has three valence electrons, which it uses to form bonds with three chlorine atoms in \(\mathrm{AlCl}_3\). Each chlorine atom, with seven valence electrons, shares one with aluminum to complete its own octet. This sharing enables the chlorine atoms in the product \(\mathrm{AlCl}_4^-\) to maintain a stable outer shell.
Valence electrons are also crucial in understanding Lewis structures. These electrons are represented as dots around the atomic symbol. Knowledge of how many valence electrons belong to each atom aids in predicting molecule formation and chemical behavior, functioning as a fundamental aspect of chemistry.
covalent bonds
Covalent bonds are a fundamental concept where atoms share their valence electrons to achieve full outer electron shells. In \(\mathrm{AlCl}_3\), covalent bonds form when aluminum shares its electrons with chlorine atoms. Thus, both elements fulfill their goal of obtaining stable electron configurations.
These bonds, particularly in \(\mathrm{AlCl}_3 + \mathrm{Cl}^-\), result in the tetrahedral structure of \(\mathrm{AlCl}_4^-\). A significant aspect of covalent bonding is the equal sharing of electrons between atoms, which allows molecules to form stable structures.
Understanding covalent bonds helps explain how complex molecules are structured and behave. These bonds act like "glue," holding atoms in place and defining the molecule's geometry. Learning about covalent bonds lays the groundwork for more intricate topics like polarity, hybridization, and molecule interaction.
These bonds, particularly in \(\mathrm{AlCl}_3 + \mathrm{Cl}^-\), result in the tetrahedral structure of \(\mathrm{AlCl}_4^-\). A significant aspect of covalent bonding is the equal sharing of electrons between atoms, which allows molecules to form stable structures.
Understanding covalent bonds helps explain how complex molecules are structured and behave. These bonds act like "glue," holding atoms in place and defining the molecule's geometry. Learning about covalent bonds lays the groundwork for more intricate topics like polarity, hybridization, and molecule interaction.
