Identify The Lewis Acid In This Balanced Equation:$\[ \text{SnCl}_4 + 2 \text{Cl}^- \rightarrow \text{SnCl}_6^{2-} \\]A. \[$\text{SnCl}_4\$\] B. \[$\text{Cr}\$\] C. \[$\text{SnCl}_6^{2-}\$\]

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Understanding Lewis Acids and Bases

In chemistry, a Lewis acid is defined as a species that can accept a pair of electrons to form a covalent bond. On the other hand, a Lewis base is a species that can donate a pair of electrons to form a covalent bond. The concept of Lewis acids and bases was introduced by Gilbert N. Lewis in 1923 and is a fundamental aspect of inorganic chemistry.

The Balanced Equation

The given balanced equation is:

SnCl4+2Cl−→SnCl62−{ \text{SnCl}_4 + 2 \text{Cl}^- \rightarrow \text{SnCl}_6^{2-} }

In this equation, tin(IV) chloride (SnCl4\text{SnCl}_4) reacts with chloride ions (Cl−\text{Cl}^-) to form the hexachlorostannate ion (SnCl62−\text{SnCl}_6^{2-}).

Identifying the Lewis Acid

To identify the Lewis acid in this equation, we need to determine which species can accept a pair of electrons. In this case, the tin(IV) ion (Sn4+\text{Sn}^{4+}) is the central atom in both SnCl4\text{SnCl}_4 and SnCl62−\text{SnCl}_6^{2-}. The tin(IV) ion has a formal charge of +4, which means it has a strong tendency to accept a pair of electrons to form a covalent bond.

Analyzing the Options

Now, let's analyze the options given:

A. SnCl4\text{SnCl}_4 B. SnCl62−\text{SnCl}_6^{2-} C. Cl−\text{Cl}^-

Option A: SnCl4\text{SnCl}_4

In SnCl4\text{SnCl}_4, the tin(IV) ion is bonded to four chlorine atoms. Although the tin(IV) ion has a strong tendency to accept a pair of electrons, it is already bonded to four chlorine atoms, which means it is not available to accept additional electrons. Therefore, SnCl4\text{SnCl}_4 is not the Lewis acid in this equation.

Option B: SnCl62−\text{SnCl}_6^{2-}

In SnCl62−\text{SnCl}_6^{2-}, the tin(IV) ion is bonded to six chlorine atoms. Similar to SnCl4\text{SnCl}_4, the tin(IV) ion in SnCl62−\text{SnCl}_6^{2-} is already bonded to six chlorine atoms, which means it is not available to accept additional electrons. Therefore, SnCl62−\text{SnCl}_6^{2-} is not the Lewis acid in this equation.

Option C: Cl−\text{Cl}^-

In the given equation, the chloride ions (Cl−\text{Cl}^-) are the species that donate a pair of electrons to form a covalent bond with the tin(IV) ion. However, the question asks us to identify the Lewis acid, which is the species that accepts a pair of electrons. In this case, the tin(IV) ion is the species that accepts a pair of electrons from the chloride ions, making it the Lewis acid.

Conclusion

In conclusion, the Lewis acid in the given balanced equation is the tin(IV) ion (Sn4+\text{Sn}^{4+}), which is present in both SnCl4\text{SnCl}_4 and SnCl62−\text{SnCl}_6^{2-}. The tin(IV) ion has a strong tendency to accept a pair of electrons to form a covalent bond, making it the Lewis acid in this equation.

Key Takeaways

  • A Lewis acid is a species that can accept a pair of electrons to form a covalent bond.
  • The tin(IV) ion (Sn4+\text{Sn}^{4+}) is the central atom in both SnCl4\text{SnCl}_4 and SnCl62−\text{SnCl}_6^{2-}.
  • The tin(IV) ion has a strong tendency to accept a pair of electrons to form a covalent bond.
  • The chloride ions (Cl−\text{Cl}^-) donate a pair of electrons to form a covalent bond with the tin(IV) ion.

Frequently Asked Questions

Q: What is a Lewis acid?

A: A Lewis acid is a species that can accept a pair of electrons to form a covalent bond.

Q: What is the difference between a Lewis acid and a Lewis base?

A: A Lewis acid is a species that can accept a pair of electrons, while a Lewis base is a species that can donate a pair of electrons.

Q: Which species is the Lewis acid in the given balanced equation?

A: The tin(IV) ion (Sn4+\text{Sn}^{4+}) is the Lewis acid in the given balanced equation.

Q: Why is the tin(IV) ion the Lewis acid?

Q: What is a Lewis acid?

A: A Lewis acid is a species that can accept a pair of electrons to form a covalent bond. This means that a Lewis acid is a molecule or ion that has an incomplete octet, i.e., it has fewer than eight electrons in its outermost energy level.

Q: What is the difference between a Lewis acid and a Lewis base?

A: A Lewis acid is a species that can accept a pair of electrons, while a Lewis base is a species that can donate a pair of electrons. In other words, a Lewis acid is a electron acceptor, while a Lewis base is an electron donor.

Q: What are some common examples of Lewis acids?

A: Some common examples of Lewis acids include:

  • Boron trifluoride (BF3)
  • Aluminum chloride (AlCl3)
  • Tin(IV) chloride (SnCl4)
  • Iron(III) chloride (FeCl3)

Q: What are some common examples of Lewis bases?

A: Some common examples of Lewis bases include:

  • Water (H2O)
  • Ammonia (NH3)
  • Hydroxide ions (OH-)
  • Cyanide ions (CN-)

Q: How do Lewis acids and bases interact with each other?

A: Lewis acids and bases interact with each other through a process called Lewis acid-base reaction. In this reaction, the Lewis acid accepts a pair of electrons from the Lewis base, forming a covalent bond.

Q: What are some common types of Lewis acid-base reactions?

A: Some common types of Lewis acid-base reactions include:

  • Protonation reactions: In this type of reaction, a Lewis acid (such as a proton) accepts a pair of electrons from a Lewis base (such as a water molecule).
  • Coordination reactions: In this type of reaction, a Lewis acid (such as a metal ion) accepts a pair of electrons from a Lewis base (such as a ligand).
  • Substitution reactions: In this type of reaction, a Lewis acid (such as a metal ion) accepts a pair of electrons from a Lewis base (such as a ligand), replacing an existing ligand.

Q: What are some real-world applications of Lewis acids and bases?

A: Lewis acids and bases have many real-world applications, including:

  • Catalysis: Lewis acids and bases are often used as catalysts in chemical reactions.
  • Materials science: Lewis acids and bases are used to synthesize new materials with unique properties.
  • Pharmaceuticals: Lewis acids and bases are used to synthesize new pharmaceuticals.
  • Environmental science: Lewis acids and bases are used to clean up environmental pollutants.

Q: How can I determine if a molecule is a Lewis acid or a Lewis base?

A: To determine if a molecule is a Lewis acid or a Lewis base, you can use the following criteria:

  • Lewis acids: Have an incomplete octet (i.e., fewer than eight electrons in their outermost energy level).
  • Lewis bases: Have a complete octet (i.e., eight electrons in their outermost energy level).

Q: What are some common mistakes to avoid when working with Lewis acids and bases?

A: Some common mistakes to avoid when working with Lewis acids and bases include:

  • Confusing Lewis acids and bases with Bronsted-Lowry acids and bases.
  • Failing to consider the stereochemistry of Lewis acid-base reactions.
  • Ignoring the effects of solvent on Lewis acid-base reactions.

Q: How can I learn more about Lewis acids and bases?

A: To learn more about Lewis acids and bases, you can:

  • Read textbooks and online resources on inorganic chemistry.
  • Take online courses or attend workshops on Lewis acid-base chemistry.
  • Join online communities or forums to discuss Lewis acid-base chemistry with other chemists.
  • Conduct experiments and research on Lewis acid-base reactions.