XeF4 Molecular Geometry and Polarity

The video tutorial explains the polarity of xenon tetrafluoride (XeF4) by examining its Lewis structure, bonding, and molecular geometry. XeF4 has single bonds with four fluorine atoms and two lone pairs on the central xenon atom, allowing for an expanded octet. Despite the electronegativity difference between xenon and fluorine, the molecule's symmetrical shape results in no net dipole, making XeF4 nonpolar.

What is the primary factor in determining if a molecule like XeF4 is polar or nonpolar?

• The type of atoms in the molecule

• The number of atoms in the molecule

• The symmetry of the molecule

• The color of the molecule

In the Lewis structure of XeF4, how many single bonds are formed with fluorine atoms?

• Four

• Three

• Two

• Five

How many lone pairs of electrons are present on the central xenon atom in XeF4?

• Four

• Three

• Two

• One

What allows xenon in XeF4 to have more than eight valence electrons?

• It forms ionic bonds

• It has a high electronegativity

• It is below Period three on the periodic table

• It is a noble gas

Why is the concept of symmetry important in determining the polarity of XeF4?

• It determines the molecular weight

• It changes the state of matter

• It affects the color of the molecule

• It influences the distribution of charge

What is the shape of the XeF4 molecule?

• Square planar

• Tetrahedral

• Trigonal planar

• Linear

How do the lone pairs on the xenon atom in XeF4 affect its geometry?

• They cause the molecule to be bent

• They contribute to the square planar shape

• They have no effect on the geometry

• They make the molecule linear

What is the net dipole moment of XeF4?

• Zero

• Undefined

• Positive

• Negative

Why does XeF4 have no net dipole moment?

• Due to its symmetrical shape

• Because it is a gas

• Because it has no lone pairs

• Due to its high electronegativity

What is the overall polarity of the XeF4 molecule?

• Polar

• Nonpolar

• Ionic

• Metallic