1. Molecular Geometry:
* Central Atom: Iodine (I)
* Surrounding Atoms: One oxygen (O) and five fluorine (F) atoms.
* Electron Groups: Iodine has 7 valence electrons, and it forms 6 bonds (one double bond to oxygen and five single bonds to fluorine). This means there are 6 electron groups around the central iodine atom.
* Shape: With 6 electron groups, the molecular geometry of IOF5 is square pyramidal.
2. Polarity of Bonds:
* Iodine-Oxygen (I=O): This bond is polar because oxygen is more electronegative than iodine.
* Iodine-Fluorine (I-F): This bond is also polar, as fluorine is more electronegative than iodine.
3. Molecular Dipole Moment:
* Symmetry: Due to the square pyramidal shape, the polar I-F bonds are arranged symmetrically around the central iodine. This means their individual dipole moments cancel each other out.
* Net Dipole Moment: However, the polar I=O bond is not canceled out by any other bond.
Therefore, IOF5 has a net dipole moment, making it a polar molecule.
