QQuestionChemistry
QuestionChemistry
Consider the following Lewis structure for XeO^3 and answer the following three questions.
What is the ideal O-Xe-O bond angle? (Choose the closest value.)
90°
109°
120°
180°
What is the molecular geometry?
tetrahedral
trigonal planar
trigonal pyramidal
T-shaped
Is the XeO^3 molecule polar?
Yes
No
10 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:: Determine the electron geometry of XeO^3.
The Lewis structure for XeO^3 shows that the central atom, Xe, is bonded to three oxygen atoms and has no lone pairs. This means that the electron geometry around the Xe atom is trigonal planar.
Step 2:: Understand the relationship between electron geometry and molecular geometry.
For molecules without lone pairs, the molecular geometry is the same as the electron geometry. Therefore, the molecular geometry of XeO^3 is also trigonal planar.
Step 3:: Calculate the ideal bond angle.
In a trigonal planar molecule, the ideal bond angle is 120°. This is due to the sp^2 hybridization of the central atom, which results in three equal bond angles.
Step 4:: Determine the polarity of the molecule.
Xenon (Xe) is a highly electronegative element, and oxygen (O) is also electronegative. Since XeO^3 has a polar covalent bond between Xe and O, the molecule itself is polar. However, due to the symmetrical shape of the trigonal planar geometry, the dipole moments of the individual bonds cancel each other out. As a result, the overall molecular dipole moment is zero, and the molecule is nonpolar.
Final Answer
- The ideal O-Xe-O bond angle is 120°. - The molecular geometry is trigonal planar. - Despite having polar bonds, XeO^3 is a nonpolar molecule.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students