Be sure to answer all parts. Which of the following ions possess a dipole moment? (a) ClF2+ (b) ClF2− has a dipole moment has no dipole moment cannot be determined has a dipole moment has no dipole moment cannot be determined (c) IF4+ has a dipole moment has no dipole moment cannot be determined (d) IF4− has a dipole moment has no dipole moment cannot be determined

In order to determine if a specie has dipole moment or not there is the need for us to draw the Lewis structure, please check attached file for the Lewis structures of each species.

(A). ClF2+: it HAS dipole moment because of Asymmetry. Note that the Fluorine atoms are more Electronegative that the chlorine atom.

(B). ClF2− : Normally, it should have a dipole moment because Fluorine atoms are more Electronegative that the chlorine atom on each side BUT due to its geometry (according to VSEPR theory) which makes it to have a linear geometry, the dipole moment will cancel out ,hence, NO DIPOLE MOMENT.

(C). IF4+ : it HAS dipole moment. Although, the dipole moment of two out of the four Fluorine will cancel out the other two will not cancel out making it to have Dipole moment.

(D). IF4-: it has no dipole moment because the four bonds are in opposite directions

ahsan57900 ahsan57900 · Answer 2 · 2021-10-21T04:06:42+02:00

ClF2+ and IF4+ has dipole moment whereas ClF2− and IF4− has no dipole moment.

ClF2+ has dipole moment because of Asymmetry i.e. the Fluorine atoms has higher electronegativity value that the chlorine atom.

ClF2− has no dipole moment due to its geometry i.e. it has a linear geometry, the dipole moment will cancel out and no dipole moment occur.

IF4+ has dipole moment because the dipole moment of two out of the four Fluorine will cancel out but the other two will not cancel out making it to have Dipole moment.

IF4- has no dipole moment because the four bonds are in opposite directions.

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