Based on its molecular structure, is XeO3 a polar molecule?A.Yes, because the Xe=O bonds are polar and any molecule with polar bonds is a polar molecule.B.No, because the Xe=O bonds are nonpolar.C.Yes, because the Xe=O bonds are polar and have a geometry that gives the molecule a net dipole.D.No, because the Xe=O bonds are polar but have a geometry that causes the dipoles to cancel.
Question
Based on its molecular structure, is XeO3 a polar molecule?A.Yes, because the Xe=O bonds are polar and any molecule with polar bonds is a polar molecule.B.No, because the Xe=O bonds are nonpolar.C.Yes, because the Xe=O bonds are polar and have a geometry that gives the molecule a net dipole.D.No, because the Xe=O bonds are polar but have a geometry that causes the dipoles to cancel.
Solution
The answer is C. Yes, because the Xe=O bonds are polar and have a geometry that gives the molecule a net dipole.
Here's the step-by-step explanation:
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XeO3, or Xenon trioxide, is a molecule that consists of one Xenon atom (Xe) and three Oxygen atoms (O).
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The electronegativity difference between Xenon and Oxygen makes the Xe=O bonds polar. Oxygen is more electronegative than Xenon, so the electrons in the bond are more attracted to Oxygen, creating a dipole (a separation of charge).
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The geometry of XeO3 is trigonal pyramidal. This is because Xenon has 5 electron pairs in its valence shell: 3 bonding pairs (forming bonds with the Oxygen atoms) and 2 lone pairs.
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In a trigonal pyramidal geometry, the dipoles do not cancel out. Instead, they add up to create a net dipole in the molecule, making the molecule polar.
So, XeO3 is a polar molecule because it has polar bonds and a geometry that results in a net dipole.
Similar Questions
In XeO3, the xenon-oxygen bonds are:A.nonpolar, because the electron affinity of Xe is close to zero.B.nonpolar, because the electronegativities of Xe and O are nearly equal.C.polar, because the electronegativity of Xe is much higher than the electronegativity of O.D.polar, because the electronegativity of Xe is much lower than the electronegativity of O.
Which statement best describes the polarity of the molecule PI3?A.It is nonpolar, because the bonds are polar and the molecular geometry does not affect polarity.B.It is polar, because it is a trigonal-planar molecule and the bond polarities between phosphorus (P) and iodine (I) add together.C.It is nonpolar, because it is a trigonal-planar molecule and the bond polarities cancel each other out.D.It is nonpolar, because the electronegativity difference between phosphorus (P) and iodine (I) is very small.SUBMITarrow_backPREVIOUS
Molecules possessing polar covalent bonds are called dipoles.Question 23Answera.Falseb.True
Which of the following molecules is the most polar?
In order to have dipole-dipole attractions, a molecule mustGroup of answer choiceshave electrons so all things have dipole-dipole attractions.have a permanently uneven distribution of electrons so only polar molecules have dipole-dipole attractions.have a hydrogen bonded directly to N, O, or F.have an accidental dipole so only nonpolar molecules have dipole-dipole attractions.
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