Iodine forms three compounds with chlorine. Choose the correct molecular shapes.
ICl3
ICl5
ICl
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To determine the molecular shapes of these compounds, we need to know the number of electron pairs around the central iodine atom.
For ICl3:
Iodine forms three bonds with chlorine, and there is one lone pair on iodine. This gives us a total of 4 electron pairs around iodine. According to the VSEPR (Valence Shell Electron Pair Repulsion) theory, the molecular shape will be trigonal pyramidal. The three chlorine atoms will form a pyramid around the central iodine atom.
For ICl5:
Iodine forms five bonds with chlorine, and there are no lone pairs on iodine. This gives us a total of 5 electron pairs around iodine. According to the VSEPR theory, the molecular shape will be trigonal bipyramidal. The five chlorine atoms will arrange themselves around the central iodine atom, forming a bipyramid.
For ICl:
Iodine forms one bond with chlorine, and there are no lone pairs on iodine. This gives us a total of 2 electron pairs around iodine. According to the VSEPR theory, the molecular shape will be linear. The chlorine atom will be directly opposite to the central iodine atom in a straight line.
So, the correct molecular shapes are:
ICl3 - trigonal pyramidal
ICl5 - trigonal bipyramidal
ICl - linear