Explanation:

Dipole moment is a measure of the separation of positive and negative charges in a molecule. It is a vector quantity and is represented by an arrow pointing towards the negative end of the molecule.

To determine the number of compounds that have a non-zero dipole moment, we need to first understand the molecular geometry and the electronegativity of the atoms involved in the molecule.

XeF2:
- The molecular geometry of XeF2 is linear, with the two fluorine atoms on either side of the xenon atom.
- The electronegativity of fluorine is greater than that of xenon, so the electrons are pulled towards the fluorine atoms, creating a dipole moment.
- Therefore, XeF2 has a non-zero dipole moment.

XeF4:
- The molecular geometry of XeF4 is square planar, with the four fluorine atoms surrounding the xenon atom in a plane.
- The electronegativity of fluorine is greater than that of xenon, so the electrons are pulled towards the fluorine atoms, creating a dipole moment.
- However, the dipole moments of the four fluorine atoms cancel each other out, resulting in a molecule with a zero dipole moment.
- Therefore, XeF4 does not have a non-zero dipole moment.

XeF6:
- The molecular geometry of XeF6 is octahedral, with the six fluorine atoms surrounding the xenon atom.
- The electronegativity of fluorine is greater than that of xenon, so the electrons are pulled towards the fluorine atoms, creating a dipole moment.
- However, the dipole moments of the six fluorine atoms cancel each other out, resulting in a molecule with a zero dipole moment.
- Therefore, XeF6 does not have a non-zero dipole moment.

XeO3:
- The molecular geometry of XeO3 is trigonal pyramidal, with the three oxygen atoms surrounding the xenon atom.
- The electronegativity of oxygen is greater than that of xenon, so the electrons are pulled towards the oxygen atoms, creating a dipole moment.
- Therefore, XeO3 has a non-zero dipole moment.

XeO4:
- The molecular geometry of XeO4 is tetrahedral, with the four oxygen atoms surrounding the xenon atom.
- The electronegativity of oxygen is greater than that of xenon, so the electrons are pulled towards the oxygen atoms, creating a dipole moment.
- However, the dipole moments of the four oxygen atoms cancel each other out, resulting in a molecule with a zero dipole moment.
- Therefore, XeO4 does not have a non-zero dipole moment.

XeO2:
- The molecular geometry of XeO2 is linear, with the two oxygen atoms on either side of the xenon atom.
- The electronegativity of oxygen is greater than that of xenon, so the electrons are pulled towards the oxygen atoms, creating a dipole moment.
- Therefore, XeO2 has a non-zero dipole moment.

XeOF4:
- The molecular geometry of XeOF4 is square pyramidal, with the four fluorine atoms and one oxygen atom surrounding the xenon atom.
- The electronegativity of oxygen and fluorine is greater than that