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The false statement among the following is (1) Λnhydrous ΛlCl3 is covalent. (2) IIydrated ΛlCl36II2O is ionic. (3) \Lambdanhydrous Λ1Cl3 is a Lewis acid. (4) IIydrated ΛlCl36II2O is Lewis acid.

Short Answer

Expert verified
Statement 4 is false. Hydrated AlCl36H2O is not a Lewis acid.

Step by step solution

01

Identify the Covalent and Ionic Compounds

Check if anhydrous AlCl3 and hydrated AlCl36H2O are covalent or ionic. Anhydrous AlCl3 is covalent because it forms a dimer through chlorine bridges. Hydrated AlCl36H2O contains water molecules that coordinate to the Al3+ ions, making the compound ionic.
02

Check if Anhydrous AlCl3 is a Lewis Acid

Identify if anhydrous AlCl3 acts as a Lewis acid. AlCl3 is a Lewis acid as it can accept electron pairs due to the presence of an empty orbital on the aluminum atom.
03

Check if Hydrated AlCl36H2O is a Lewis Acid

Determine if AlCl36H2O can act as a Lewis acid. The hydrate form already has aluminum coordinated with H2O molecules, reducing its ability to act as a Lewis acid effectively compared to the anhydrous form.
04

Identify the False Statement

Compare the statements given: (1) AlCl3 is covalent (true), (2) AlCl36H2O is ionic (true), (3) AlCl3 is a Lewis acid (true), (4) AlCl36H2O is a Lewis acid (false). Thus, the false statement is: \textbf{ii}ydrated AlCl36H2O is a Lewis acid.

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Key Concepts

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

Covalent Compounds
Covalent compounds are created when two or more atoms share electrons, instead of giving them away or taking them. These atoms form molecules where the shared electrons belong to both atoms in the bond. An example of a covalent compound is anhydrous AlCl3, where aluminum and chlorine atoms share electrons, forming a stable molecule.
  • Covalent bonds are typically found in compounds with nonmetals.
  • These bonds can be single, double, or triple, depending on the number of shared electron pairs.
Understanding covalent bonds is crucial in predicting the properties of the compound, such as its melting and boiling points. These compounds generally have lower melting and boiling points compared to ionic compounds.
Ionic Compounds
Ionic compounds are formed when atoms transfer electrons from one to another, resulting in oppositely charged ions that are attracted to each other. This type of bond generally occurs between metals and nonmetals. An example is hydrated AlCl36H2O, where aluminum loses electrons to chlorine, forming Al3+ and Cl ions, with water molecules stabilizing the structure.
  • Ionic bonds create a crystalline lattice, which contributes to high melting and boiling points.
  • These compounds are often soluble in water and conduct electricity when dissolved.
Identifying whether a compound is ionic or covalent helps predict how it will behave in different environments, such as in water or when exposed to heat.
Coordination Chemistry
Coordination chemistry deals with coordination compounds, where a central metal atom or ion is bonded to surrounding molecules or ions, called ligands. These ligands donate pairs of electrons to the metal, creating a complex. For instance, in hydrated AlCl36H2O, water molecules act as ligands, coordinating to the Al3+ ion.
  • The metal-ligand bond is known as a coordinate covalent bond, where both electrons in the bond originate from the ligand.
  • Coordination compounds can exhibit various geometries, such as octahedral or tetrahedral, based on the number of ligands.
Understanding the principles of coordination chemistry is important in many fields, including catalysis and material science.
Hydration of Compounds
Hydration refers to the addition of water molecules to a substance, which can significantly alter its properties. This process is especially important in coordination chemistry, as seen with hydrated AlCl36H2O. In this case, the aluminum ions are surrounded by water molecules, forming a stable hydrated complex.
  • Hydration can change the solubility, reactivity, and phase of a compound.
  • The number of water molecules associated with a compound is often indicated in its chemical formula.
Recognizing the effects of hydration helps in understanding the compound's behavior in aqueous environments and its overall stability.

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