This seems like a misprint. IF6 will have one electron too many to attain an octahedral structure with 90 degree bond angles. SF6 is octahedral, for example, and does have 90 degree angles, as does PF6(-1). Perhaps IF6(+1) is the molecule in question, which will have the proper number of electrons.
90, 120, 180.
The approximate bond angles for BrF5 is approximately 90 degrees because there would be one lone pair of electrons left over, making the molecular shape square pyramidal... This gives an approximate bond angle of 90 degrees. AX5E, sp3d2 hybridized.
The bond angles are 120 degrees
The molecule of iodine heptafluoride has a bi-pyramidal pentagonal shape. All of the F-I-F angles between two fluorine atoms in axial and equatorial planes are equivalent to 90 degrees. Therefore there is five of them.
Acute angles are angles less than 90 degrees an obtuse angles are greater than 90 degrees
90 and 180 are the approximate bond angles.
SeF6 is a regular octahedron , all bond angles are 90 degrees
90, 120, 180.
The bond angles in IF4^- (iodine tetrafluoride) are approximately 90 degrees.
90 is the smallest one
The value of the bond angle in XeF2 is 180 degrees.
The approximate bond angles for BrF5 is approximately 90 degrees because there would be one lone pair of electrons left over, making the molecular shape square pyramidal... This gives an approximate bond angle of 90 degrees. AX5E, sp3d2 hybridized.
90 degree angles.90 degree angles.90 degree angles.90 degree angles.
The bond angles are 120 degrees
90 degress
Angles that are less than 90 degrees are acute angles. Angles that are 90 degrees are right angles, and angles that are greater than 90 degrees are obtuse angles.
If it is non polar, the bond angles are as follows:I-P-I bond angles: 120ºBr-P-Br bond angles: 180ºI-P-Br bond angles: 90º