Describe briefly what will happen when you try to dissolve...

Describe briefly what will happen when you try to dissolve each of the following compounds in water: a. $\mathrm{KCl} ;$ b. $\mathrm{NbCl}_5$; c. $\mathrm{AlBr}_3 ;$ d. $\mathrm{CBr}_4$; e. $\mathrm{BaI}_2$; f. IF 7 . Which of these would be likely to fume in air and why?

Key Concepts

Solubility and Inertness of Covalent Molecular Compounds

Covalent compounds, particularly those that are nonpolar, display very limited solubility in water. Their molecular structure does not interact strongly with water, leading to poor hydration and little or no dissolution. This concept contrasts with the extensive solvation seen with ionic compounds.

Fuming Due to Hydrolytic Reactions in Air

Some compounds react with trace amounts of moisture in the air via hydrolysis, generating acidic products that can vaporize, appearing as fumes. This phenomenon is commonly observed with reactive metal halides, where the hydrolysis produces volatile acids that are visible as fumes upon exposure to atmospheric moisture.

Ionic Solubility in Water

This concept refers to the ability of ionic compounds to dissociate into their constituent ions when introduced to a polar solvent like water. The process is driven by the inter-molecular interactions between the ions and water molecules (hydration), overcoming the lattice energy that holds the ionic solid together.

Hydrolysis of Metal Halides

Many metal halides, especially those with high oxidation state metals, undergo hydrolysis in water. This is a reaction where water molecules interact with the metal-halide bonds, leading to the formation of metal hydroxides and hydrogen halides. The process often results in acidic solutions and can sometimes release fumes if volatile halogen acids are produced.

Transcript

Please give Ace some feedback