The electron-domain geometry and molecular geometry of iodine trichloride are __________ and __________, respectively.

The answer is trigonal bipyramidal, T-shaped, respectively- I do not understand the approach
PLEASE EXPLAIN HOW YOU GOT THE ANSWER!!!

Iodine trichloride is composed of 1 Iodine and 3 Chlorines. Each atom has 7 electrons in their valence electron shell. The chlorine atoms will have six electrons each around them, but the other remaining electron from each chlorine will be able to participate in a bond with Iodine. Iodine in return will share one electron each, with each chlorine, and the remaining four will surround chlorine in two pairs. Since there are 5 groups of two electrons for iodine, 2 lone groups around Iodine and three groups participating in bonds with the chlorines, you look at a chart on the web or in your text and look for the name of the group corresponding to 5 groups of two electrons for the central atom to determine the electron-domain geometry. You look within the group to identify the molecular geometry of the structure for the central atom that has two lone pairs of electrons surrounding it to determine the molecular geometry.

I had a couple of typos that may have made this unclear.

Iodine trichloride is composed of 1 Iodine and 3 Chlorines. Each atom has 7 electrons in their valence electron shell. The chlorine atoms will have six electrons each around them, but the other remaining electron from each chlorine will be able to participate in a bond with Iodine. Iodine in return will share one electron each, with each chlorine, and the remaining four will be in pairs surrounding chlorine. Since there are 5 groups of two electrons for iodine, 2 lone groups around Iodine and three groups participating in bonds with the chlorines, you look at a chart on the web or in your text and look for the name of the group corresponding to 5 groups of two electrons for the central atom to determine the electron-domain geometry. You look within the group to identify the molecular geometry of the structure for the central atom that has two lone pairs of electrons surrounding it.

To determine the electron-domain geometry and molecular geometry of a molecule, we use the VSEPR (Valence Shell Electron Pair Repulsion) theory. This theory states that electron pairs repel each other and arrange themselves in a way that minimizes repulsion.

For iodine trichloride (ICl3), we first need to determine the number of valence electrons. Iodine (I) is in group 7A, so it has 7 valence electrons, and chlorine (Cl) is in group 7A, so each chlorine atom has 7 valence electrons. There are 3 chlorine atoms in ICl3, so the total number of valence electrons is:

1 (iodine) + 3 (chlorine) = 4 + 21 = 25 valence electrons.

Next, we determine the electron-domain geometry by counting the number of electron domains around the central atom (iodine in this case). An electron domain is any region of electron density, including lone pairs and bonds.

In ICl3, the central iodine atom is bonded to three chlorine atoms, and there are no lone pairs on the central atom. Therefore, there are three electron domains around iodine. This corresponds to the trigonal bipyramidal electron-domain geometry, which consists of three equatorial positions and two axial positions.

Now, we determine the molecular geometry by considering the arrangement of atoms around the central atom, ignoring the lone pairs. In ICl3, three chlorine atoms occupy the equatorial positions, whereas the two axial positions remain unoccupied. Since the molecule has a Trigonal Bipyramidal electron-domain geometry, the molecular geometry would be T-shaped.

Therefore, the electron-domain geometry of iodine trichloride is trigonal bipyramidal, and the molecular geometry is T-shaped.

To determine the electron-domain geometry and molecular geometry of a molecule, we follow a step-by-step approach:

Step 1: Draw the Lewis structure of the molecule.
The Lewis structure of iodine trichloride (ICl3) can be determined by counting the total number of valence electrons in the molecule and arranging them to form bonds between atoms. Iodine (I) has 7 valence electrons, and each chlorine (Cl) atom has 7 valence electrons. Since there are three chlorine atoms in ICl3, the total number of valence electrons is 7 + (3 × 7) = 28.

The Lewis structure of ICl3 is as follows:
I:Cl-Cl-Cl

Step 2: Determine the central atom.
In ICl3, iodine (I) is the central atom because it is the least electronegative element. The chlorine atoms (Cl) will be bonded to the central iodine atom.

Step 3: Determine the electron-domain geometry.
To determine the electron-domain geometry, we need to count the total number of bonding and non-bonding electron domains around the central atom.

In ICl3, there are three chlorine atoms bonded to the central iodine atom, resulting in three bonding domains. Additionally, there is one lone pair of electrons on the central iodine atom, contributing one non-bonding domain.

Adding them up, we get a total of four electron domains around the iodine atom.

Based on the electron domain geometry, a molecule with four electron domains will adopt a trigonal bipyramidal electron-domain geometry.

Step 4: Determine the molecular geometry.
To determine the molecular geometry, we need to consider the arrangement of the bonded atoms.

In ICl3, the three chlorine atoms surrounding the central iodine atom form a trigonal planar arrangement. The bond angles between these chlorine atoms are approximately 120 degrees.

However, we also need to consider the influence of the lone pair of electrons on the molecular geometry. The presence of a lone pair creates unequal repulsion between the electron domains.

The lone pair repels the bonding pairs, pushing them closer together. As a result, the molecular geometry of ICl3 is T-shaped, with the three chlorine atoms forming the base of a T, and the lone pair of electrons occupying an axial position above or below the plane.

In summary, the electron-domain geometry of ICl3 is trigonal bipyramidal (due to four electron domains), and the molecular geometry is T-shaped (due to unequal repulsion caused by the presence of a lone pair).