Problem: Draw the lewis structure of XeCl4 showing all lone pairs.XeCl4 molecule isa. polar.b. nonpolar.What are the approximate bond angles in XeCl4?Select all that applya. 90 degreesb. 109.5 degreesc. 120 degreesd. 180 degreesIdentify the molecular geometry of XeCl4a. tetrahedralb trigonal bipyramidalc. T-shapedd. lineare. see-sawf. octahedralg. square pyramidalh. benti. trigonal pyramidalj. square planark. trigonal planar

FREE Expert Solution

For this problem, we need to do the following steps:

Step 1: Determine the central atom in this molecule.

Step 2: Calculate the total number of valence electrons present.

Step 3: Draw the Lewis structure for the molecule.

Step 4: Draw dipole arrows for each bond.

Step 5: Determine the polarity of the molecule.

Step 1: Xe is less electronegative than chlorine so chlorine is the central atom.

Step 2: The total number of valence electrons present in XeCl4 is:

            Group             Valence Electrons

Xe        8A                   1 × 8 e8 e

Cl         7A                   4 × 7 e28 e

Total:  36 valence e

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Problem Details

Draw the lewis structure of XeCl4 showing all lone pairs.

XeCl4 molecule is
a. polar.
b. nonpolar.

What are the approximate bond angles in XeCl4?
Select all that apply
a. 90 degrees
b. 109.5 degrees
c. 120 degrees
d. 180 degrees

Identify the molecular geometry of XeCl4
a. tetrahedral
b trigonal bipyramidal
c. T-shaped
d. linear
e. see-saw
f. octahedral
g. square pyramidal
h. bent
i. trigonal pyramidal
j. square planar
k. trigonal planar

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Molecular Polarity concept. You can view video lessons to learn Molecular Polarity. Or if you need more Molecular Polarity practice, you can also practice Molecular Polarity practice problems.