Xenon Fluoride Molecular Geometry Concepts

The video tutorial explains the number of lone and bonding pairs in xenon difluoride (XeF2). It highlights that the central atom, xenon, affects the molecular geometry. XeF2 has two bonding pairs and three lone pairs of electrons. Xenon can have an expanded octet, allowing more than eight electrons. The molecular geometry of XeF2 is linear due to the repulsion of lone pairs. The video concludes with a recap of the electron pairs in XeF2.

What is the primary focus when discussing lone pairs and bonding pairs in a molecule?

• The lightest atom

• The heaviest atom

• The outermost atoms

• The central atom

How many bonding pairs of electrons are present in XeF2?

• One

• Four

• Two

• Three

What is unique about xenon's electron configuration in XeF2?

• It has fewer than eight electrons

• It can have an expanded octet

• It follows the octet rule strictly

• It has no lone pairs

How many lone pairs of electrons are found in XeF2?

• Two

• One

• Three

• Four

What is the molecular geometry of XeF2?

• Tetrahedral

• Trigonal planar

• Bent

• Linear

Why does XeF2 have a linear shape?

• Due to the repulsion between three lone pairs

• Because of the small size of fluorine atoms

• Due to the presence of two bonding pairs

• Because of the absence of lone pairs

How do lone pairs affect the shape of a molecule?

• They make the molecule more compact

• They do not affect the shape

• They repel each other and bonding pairs

• They attract bonding pairs

What is the total number of electron pairs around the central xenon atom in XeF2?

• Four

• Five

• Six

• Seven

Which statement correctly summarizes the electron pairs in XeF2?

• XeF2 has no lone pairs

• XeF2 has more bonding pairs than lone pairs

• XeF2 has more lone pairs than bonding pairs

• XeF2 has equal numbers of bonding and lone pairs