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
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Answer
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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.
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.
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