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Magazine Chapter 9: Problem 64
Write Lewis structures for the reaction $$ \mathrm{AlCl}_{3}+\mathrm{Cl}^{-} \longrightarrow \mathrm{AlCl}_{4}^{-} $$ What kind of bond is between \(\mathrm{Al}\) and \(\mathrm{Cl}\) in the product?
Short Answer
Expert verified
The bond type is a coordinate covalent bond.
Step by step solution
01
Identify the participants
For the reaction \( \mathrm{AlCl}_{3} + \mathrm{Cl}^{-} \longrightarrow \mathrm{AlCl}_{4}^{-} \), we first examine the reactants \( \mathrm{AlCl}_{3} \) and \( \mathrm{Cl}^{-} \). \( \mathrm{AlCl}_{3} \) is aluminum trichloride with three chlorine atoms bonded to one aluminum atom, and \( \mathrm{Cl}^{-} \) is a chloride ion.
02
Draw the Lewis structure for \( \mathrm{AlCl}_{3} \)
\( \mathrm{AlCl}_{3} \) has aluminum (\( \mathrm{Al} \)) at its center, which shares electrons with three chlorine atoms. Each \( \mathrm{Cl} \) atom shares one electron with \( \mathrm{Al} \), forming three covalent bonds (Al-Cl). Aluminum in \( \mathrm{AlCl}_{3} \) is electron deficient, typically having only six valence electrons.
03
Draw the Lewis structure for \( \mathrm{Cl}^{-} \)
The \( \mathrm{Cl}^{-} \) ion is simply a chlorine atom that has gained one extra electron, giving it a total of eight valence electrons, making it a negatively charged ion with a stable octet electron configuration.
04
Form the \( \mathrm{AlCl}_{4}^{-} \) complex
In \( \mathrm{AlCl}_{4}^{-} \), the \( \mathrm{Cl}^{-} \) ion donates a pair of electrons to \( \mathrm{AlCl}_{3} \), forming a coordinate covalent bond with aluminum. This interaction completes the octet for aluminum, resulting in a stable configuration where aluminum is surrounded by four chlorine atoms and has a formal charge of \( -1 \).
05
Determine the bond type in \( \mathrm{AlCl}_{4}^{-} \)
The bonds between \( \mathrm{Al} \) and \( \mathrm{Cl} \) in \( \mathrm{AlCl}_{4}^{-} \) are covalent, specifically with one being a coordinate covalent bond鈥攚here the electron pair comes from the \( \mathrm{Cl}^{-} \) ion to the electron-deficient aluminum.
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Key Concepts
These are the key concepts you need to understand to accurately answer the question.
AlCl3
Aluminum chloride, represented by the formula \( \mathrm{AlCl}_3 \), consists of one aluminum atom and three chlorine atoms. It's important to understand that each chlorine atom shares an electron with the aluminum to form a covalent bond.
In the Lewis structure of \( \mathrm{AlCl}_3 \), aluminum is at the center of the structure. It uses three of its electrons to bond with three chlorine atoms. This forms three \( \text{Al-Cl} \) covalent bonds.
In the Lewis structure of \( \mathrm{AlCl}_3 \), aluminum is at the center of the structure. It uses three of its electrons to bond with three chlorine atoms. This forms three \( \text{Al-Cl} \) covalent bonds.
- Chlorine atoms complete their octet by sharing one electron.
- Aluminum in \( \mathrm{AlCl}_3 \) is electron-deficient, having only six electrons around it rather than eight.
Cl-
The chloride ion \( \mathrm{Cl}^- \) is a simple yet essential player in this reaction. It is a chlorine atom that has gained an extra electron, resulting in a stable octet electron configuration.
The Lewis structure for \( \mathrm{Cl}^- \) shows chlorine with eight valence electrons, giving it a negative charge:
The Lewis structure for \( \mathrm{Cl}^- \) shows chlorine with eight valence electrons, giving it a negative charge:
- This extra electron ensures stability, as the octet rule is satisfied.
- \( \mathrm{Cl}^- \) can donate a pair of electrons in a bond, as seen in \( \mathrm{AlCl}_4^- \).
Covalent bond
Understanding covalent bonds is crucial for grasping the basic structure of both \( \mathrm{AlCl}_3 \) and \( \mathrm{AlCl}_4^- \). Covalent bonds involve the sharing of electron pairs between atoms. In the case of \( \mathrm{AlCl}_3 \), each chlorine atom forms a single covalent bond with aluminum by sharing one electron each.
Covalent bonds can vary in strength and stability, which influences the reactivity and properties of a substance. In simple terms:
Covalent bonds can vary in strength and stability, which influences the reactivity and properties of a substance. In simple terms:
- The shared electrons hold the atoms together.
- These bonds result in the formation of stable molecules.
AlCl4-
The \( \mathrm{AlCl}_4^- \) ion is a product formed in the reaction between \( \mathrm{AlCl}_3 \) and \( \mathrm{Cl}^- \). In this complex ion, a chloride ion \( \mathrm{Cl}^- \) introduces an additional pair of electrons to the aluminum-centered structure.
When forming this ion:
When forming this ion:
- The aluminum center gains an electron pair from \( \mathrm{Cl}^- \), resulting in four bonds around \( \text{Al} \).
- This donation forms a coordinate covalent bond, supporting a complete octet for aluminum.
- The entire ion acquires a negative charge \( -1 \).
Coordinate covalent bond
A coordinate covalent bond, or dative bond, is a fascinating concept essential to the reaction. Unlike typical covalent bonds where each atom contributes one electron, a coordinate bond is when one atom supplies both electrons in the shared pair.
This bond plays a pivotal role in the formation of \( \mathrm{AlCl}_4^- \):
This bond plays a pivotal role in the formation of \( \mathrm{AlCl}_4^- \):
- The \( \mathrm{Cl}^- \) ion donates a full pair of electrons to aluminum.
- This electron pair helps aluminum complete its octet, providing what's missing from \( \mathrm{AlCl}_3 \).
