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Chapter 10: Problem 123

Which of the following ions possess a dipole moment: (a) \(\mathrm{ClF}_{2}^{+},\) (b) \(\mathrm{ClF}_{2}^{-},\) (c) \(\mathrm{IF}_{4}^{+},\) (d) \(\mathrm{IF}_{4}^{-} ?\)

Short Answer

Expert verified
Among the give ions, only \(\mathrm{ClF}_{2}^{+}\), and \(\mathrm{ClF}_{2}^{-}\) possess a dipole moment, while \(\mathrm{IF}_{4}^{+}\), and \(\mathrm{IF}_{4}^{-}\) do not.

Step by step solution

01

Analyzing the geometry of \(\mathrm{ClF}_{2}^{+}\)

This ion has a bent shaped molecular geometry, like that of water. Because the two Fluorine atoms and the non-bonding pair of electron are not distributed symmetrically around the Chlorine atom, the molecule is polarized and thus has a dipole moment.
02

Analyzing the geometry of \(\mathrm{ClF}_{2}^{-}\)

This ion too has a bent shaped geometry. But due to the extra negative charge, it has one more non-bonding pair of electrons. But like \(\mathrm{ClF}_{2}^{+}\), the Fluorine atoms and the non-bonding pairs of electrons are not distributed symmetrically around the Chlorine atom, creating a dipole moment.
03

Analyzing the geometry of \(\mathrm{IF}_{4}^{+}\)

The electron configuration of Iodine in its ground state allows this ion to form a square planar geometry. In this configuration, the charge distribution is symmetric, cancelling the dipole moments, hence \(\mathrm{IF}_{4}^{+}\) has no dipole moment.
04

Analyzing the geometry of \(\mathrm{IF}_{4}^{-}\)

Like \(\mathrm{IF}_{4}^{+}\), \(\mathrm{IF}_{4}^{-}\) also forms a square planar geometry with symmetric charge distribution, cancelling the dipole moments. Thus, it does not possess a dipole moment.

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Most popular questions from this chapter

Predict the geometries of the following species: (a) \(\mathrm{AlCl}_{3},\) (b) \(\mathrm{ZnCl}_{2}\), (c) \(\mathrm{ZnCl}_{4}^{2-}\).

Both ethylene \(\left(\mathrm{C}_{2} \mathrm{H}_{4}\right)\) and benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) contain the \(\mathrm{C}=\mathrm{C}\) bond. The reactivity of ethylene is greater than that of benzene. For example, ethylene readily reacts with molecular bromine, whereas benzene is normally quite inert toward molecular bromine and many other compounds. Explain this difference in reactivity.

Write the electron configuration of the cyanide ion \(\left(\mathrm{CN}^{-}\right) .\) Name a stable molecule that is isoelectronic with the ion.

Predict the bond angles for the following molecules: (a) \(\mathrm{BeCl}_{2},\) (b) \(\mathrm{BCl}_{3},\) (c) \(\mathrm{CCl}_{4}\), (d) \(\mathrm{CH}_{3} \mathrm{Cl}\), (e) \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\) (arrangement of atoms: \(\mathrm{ClHgHgCl}\) ), (f) \(\mathrm{SnCl}_{2}\), (g) \(\mathrm{H}_{2} \mathrm{O}_{2},\) (h) \(\mathrm{SnH}_{4}\).

Which of these species has a longer bond, \(\mathrm{B}_{2}\) or \(\mathrm{B}_{2}^{+} ?\) Explain in terms of molecular orbital theory.
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