Consider the molecules AsF3, F2, BrF3, SF4, and SF6.?

Question

Consider the molecules AsF3, F2, BrF3, SF4, and SF6.
(a) Which has bonds that are the most polar?
AsF3
F2
BrF3
SF4
SF6
(b) Which have a molecular dipole moment? (Select all that apply.)
AsF3
F2
BrF3
SF4
SF6

Answer 1

The most polar bond will be between the atoms with the greatest difference in electronegativity.

F2 has bond that is not polar since the electrons are equally shared between the two identical atoms. The electronegativity series is As
As belongs to the same family as N. Thus in AsF3 it forms 3 single bonds and also has 1 lone pair. So the electron-group arrangement is tetrahedral but since there are only 3 identical bonds there will be a net dipole moment.

I already explained why F2 has no dipole moment

BrF3 has trigonal bipyramid electron group arrangment (3 bonds+2 lone pairs) but not corners are occupied by identical atoms (2 have lone pairs of Br) so the dipole moments do not cancel out and the molecule has a net dipole moment

SF4 has again trigonal bipyramid electron group arrangement(4 bonds + 1 lone pair) with one lone pair at one of the corners so it has a net dipole moment

SF6 has octahedral electron group arrangement (6 single bonds)
and since all corners have F atoms the dipole moments of the bonds cancel each other and the molecule has no net dipole moment.

Answer 2

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RE:
Consider the molecules AsF3, F2, BrF3, SF4, and SF6.?
Consider the molecules AsF3, F2, BrF3, SF4, and SF6.
(a) Which has bonds that are the most polar?
AsF3
F2
BrF3
SF4
SF6
(b) Which have a molecular dipole moment? (Select all that apply.)
AsF3
F2
BrF3
SF4
SF6

Answer 3

molecules asf3 f2 brf3 sf4 sf6: https://giveme.im/e11/consider-the-molecules-asf3-f2-brf3-sf4-and-sf6

Answer 4

Sf6 Dipole Moment

Answer 5

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a) they are all fluorides (which is the least positive charged nucleus to which they are attached; hint: group 4,5,6 elements are involved b) which molecules have a symmetrical arrangement of F's; write octet structures for all, but BrF3 (are you sure this is not BF3)

Answer 6

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