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The electron group geometry of ICl3 is trigonal bipyramidal.

The molecular shape of ICl3 is T-shaped.

The I-Cl bond is polar.

The Cl-I-Cl bond angle is approximately 90â° and 120â°.

An ICl3 molecule is polar.

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02:32

Complete the table of bond angles and molecular shapes. Some bond angles and molecular shape names may not be used, and some bond angles and molecular shape names may be used multiple times.

Number of Electron GroupsIdeal Bond Angles 180Â°Bonded Atoms Lone PairsVSEPR Molecular ShapeAnswer Bank8trigonal planar2 / 0linear3 / 0trigonal planarsquare planar120Â°2 /benttetrahedral109.59Â°4 / 0tetrahedral109.52Â°3 / 1trigonal planarsquare pyramidal2 / 2bentlinear120Â°5 / 0trigonal bipyramidal90Â°4 / 1see-sawsquare bipyramidal120Â°3 / 2T-shapedlinear180Â°45Â°2 / 36 / 0octahedraltrigonal pyramidal5 / 1square bipyramidal90Â°90Â°4 / 2trigonal bipyramidaltrigonal bipyramidalbent

03:54

Sketch a good Lewis structurefor ICl4- and use it to answer thefollowing … {Note Cl is chlorine, not a carbon and andiodine}.The electron pair geometry around the central atom is__________________.Select one:lineartrigonal pyramidaltrigonal bipyramidalsee sawT-shaped

02:52

Draw the Lewis structure of CH2Cl2, then answer the following questions.

The electron group geometry of CH2Cl2 is:A. linearB. bent or angularC. trigonal planarD. tetrahedralE. trigonal pyramid.

The molecular shape of CH2Cl2 is:A. linearB. bent or angularC. trigonal planarD. tetrahedralE. trigonal pyramid.

The C-Cl bond is:A. polarB. nonpolar.

The Cl-C-Cl bond angle is approximately:A. 90Â°B. 109Â°C. 120Â°D. 180Â°.

A CH2Cl2 molecule is:A. polarB. nonpolar

02:20

Draw the Lewis dot structure for CH2Cl2 . Determine the electrongeometry of CH2Cl2 . trigonal planar tetrahedral linear Determinethe molecular geometry of CH2Cl2 . trigonal planar tetrahedrallinear bent trigonal pyramidal Identify the bond angle in CH2Cl2 .90° 120° 180° 109.5°

Transcript

Hi there in this question we have i c l 3, and we have several questions about this molecule. So the first thing we need to do is draw its lewiston structure. To do that, we need to add up the total valence electrons. We have to work with. Iodine is a halogen, so it’s in group 7 a and has 7 valence electrons, each chlorine also being a halogen. Each of those has 7, but there are 3 of them. So 7 plus 21 gives us 28 valence electrons or in other words, since we use dots to represent valence, electrons or completed structure needs 28 dots. The iodine is going to be in the center and it’s going to be surrounded by the 3 chlorine’s. We know we need to have at least a single bond holding each chlorine to the iodine, and then we can start completing a tetes, we’ll start with our atoms on the outside here and give them each an octet of 8 electrons that uses up 24 of our Total electrons, but we have 28 point so the left over dots. If we have extra dots, they always go on the central atom. So, looking at the iodine here, that’s our central atom. We see that the iodine has 3 atoms bonded and 2 lone pairs, giving us a total of 5 electron domains. Any time we have 5 electron domains or electron groups. If you will, since it looks like this question, is calling them groups, the electron group geometry is going to be the trigonal by parametalokay. So that is our first answer. Trigonal by parameter would be the electron group geometry. Let’S take a second and see what that would look like, so it means we have 1 or we have our central atom and we have 3 electron groups around the center. So there’s a group coming out back here in center center back and then we…

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