QuestionAugust 6, 2025

Which of the following ions possess a dipole moment?Check all that apply. IF_(4)^+ IBr_(4)^+ IBr_(2)^+ IBr_(4)^- None of the above

Which of the following ions possess a dipole moment?Check all that apply. IF_(4)^+ IBr_(4)^+ IBr_(2)^+ IBr_(4)^- None of the above
Which of the following ions possess a dipole moment?Check all that apply. IF_(4)^+ IBr_(4)^+ IBr_(2)^+ IBr_(4)^- None of the above

Solution
4.3(197 votes)

Answer

\( \mathrm{IF}_{4}^{+} \), \( \mathrm{IBr}_{4}^{+} \), \( \mathrm{IBr}_{2}^{+} \) possess a dipole moment. Explanation 1. Determine molecular geometry Analyze the electron pair geometry for each ion using VSEPR theory. - \( \mathrm{IF}_{4}^{+} \): 5 electron pairs, seesaw shape. - \( \mathrm{IBr}_{4}^{+} \): 5 electron pairs, seesaw shape. - \( \mathrm{IBr}_{2}^{+} \): 3 electron pairs, bent shape. - \( \mathrm{IBr}_{4}^{-} \): 6 electron pairs, square planar shape. 2. Assess dipole moment presence Dipole moments occur in molecules with asymmetrical charge distribution. - Seesaw and bent shapes are asymmetrical, likely possessing a dipole moment. - Square planar is symmetrical, typically no dipole moment.

Explanation

1. Determine molecular geometry<br /> Analyze the electron pair geometry for each ion using VSEPR theory.<br />- \( \mathrm{IF}_{4}^{+} \): 5 electron pairs, seesaw shape.<br />- \( \mathrm{IBr}_{4}^{+} \): 5 electron pairs, seesaw shape.<br />- \( \mathrm{IBr}_{2}^{+} \): 3 electron pairs, bent shape.<br />- \( \mathrm{IBr}_{4}^{-} \): 6 electron pairs, square planar shape.<br /><br />2. Assess dipole moment presence<br /> Dipole moments occur in molecules with asymmetrical charge distribution.<br />- Seesaw and bent shapes are asymmetrical, likely possessing a dipole moment.<br />- Square planar is symmetrical, typically no dipole moment.
Click to rate:

Similar Questions