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Draw the lewis structure molecular geometry, electron geometry, hybridization of the central atom and determine if they are polar or nonpolar of molecules, of the compound icl4-
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## ICl4- Lewis Structure, Geometry, and Polarity:
1. Lewis Structure:
Iodine (I) is the central atom with 7 valence electrons.
Chlorine (Cl) has 7 valence electrons each.
The negative charge adds one more electron.
Total valence electrons = 7 + (4
7) + 1 = 36 electrons
Place the central iodine atom and arrange the four chlorine atoms around it.
Connect each chlorine atom to the iodine with a single bond, using 8 electrons.
Distribute the remaining 28 electrons as lone pairs around the chlorine atoms and the central iodine atom.
Lewis Structure:
[Image of ICl4- Lewis structure]
2. Electron Geometry:
The central iodine atom has 6 electron groups (4 bonding pairs and 2 lone pairs).
The electron geometry is octahedral.
3. Molecular Geometry:
The two lone pairs on the iodine atom create repulsion, forcing the chlorine atoms into a square planar arrangement.
The molecular geometry is square planar.
4. Hybridization:
The central iodine atom has 6 electron groups, requiring 6 hybrid orbitals.
Therefore, the hybridization of the central iodine atom is sp3d2.
5. Polarity:
Even though the individual I-Cl bonds are polar, the square planar molecular geometry results in a symmetrical distribution of electron density.
The molecule is nonpolar.
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