The polyhalide ion ICl4⁻ is stable in aqueous solution and can be isolated as salts
CHEMISTRY · Multi-part · CBSE · Chemistry · Chemical Bonding and Molecular Structure · Chemical Bonding and Molecular Structure
Problem
The polyhalide ion ICl4⁻ is stable in aqueous solution and can be isolated as salts.
Use principles of chemical bonding to analyze this ion.
(a) Calculate the total number of valence electrons that must appear in a Lewis diagram of ICl4⁻.
(b) Construct a Lewis diagram for ICl4⁻ that satisfies the octet rule for the terminal atoms and shows all lone pairs on the central atom.
(c) Determine the formal charge on the central I atom and on each Cl atom in your diagram from part (b).
(d) Predict whether ICl4⁻ is expected to be polar or nonpolar in three-dimensional space, and justify your answer based on the symmetry of both the electron-domain and molecular geometries.