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sulfur hexafluoride, SF6
iodine pentafluoride, IF5
xenon tetrafluoride, XeF4
Shapes and bond angles
|strongest||lone pair – lone pair|
|⇣||lone pair – bond pair|
|weakest||bond pair – bond pair|
The central xenon atom in XeF4 has two lone pairs of electrons in the axial positions. The four fluorine atoms occupy the equatorial positions, giving a square planar shape.
|Molecule||Bonding pairs||Lone pairs||Bond angle||Shape|
Different sources may quote different bond angles for ammonia and water. The ones shown here are acceptable for AS and A Level examinations.
The tetrachloroiodate ion, ICl4–
tetrachloroiodate ion, ICl4–
This is not a molecule but it is an interesting addition to this page. The central iodine atom has six pairs of electrons but it has just four bonding pairs of electrons. Its two lone pairs of electrons occupy the axial positions.
These lone pairs repel each other and the four bonding pairs so that the four chlorine atoms occupy the equatorial positions. This produces a square planar structure, even though there is an octahedral arrangement of electron pairs.