Let’s break down the Lewis structure for IF5 and answer the related questions step by step.
a. How many valence electrons are there?
Iodine (I) has 7 valence electrons, and each Fluorine (F) atom has 7 valence electrons. Since there are 5 Fluorine atoms, the total number of valence electrons is:
7 (Iodine) + 5 × 7 (Fluorine) = 7 + 35 = 42 valence electrons.
b. What is the electron geometry?
The electron geometry of IF5 is octahedral. This is because there are 6 regions of electron density around the central Iodine atom (5 bonding pairs and 1 lone pair).
c. What is the molecular geometry?
The molecular geometry of IF5 is square pyramidal. This is due to the presence of 5 bonding pairs and 1 lone pair of electrons on the central Iodine atom, which distorts the shape from a perfect octahedron.
d. What are the hybridized orbitals?
The central Iodine atom in IF5 undergoes sp3d2 hybridization. This means that one s orbital, three p orbitals, and two d orbitals hybridize to form 6 equivalent sp3d2 hybrid orbitals.
e. Is the molecule polar or nonpolar?
IF5 is a polar molecule. The presence of a lone pair on the central Iodine atom creates an asymmetrical distribution of electron density, resulting in a net dipole moment.