Consider BeF2, SO3 and XeF4 molecule

Consider BeF2, SO3 and XeF4 molecule.

a) Draw the Lewis structure.

b) According to VSEPR, predict the geometry of the molecule.

c) Indicate the type of hybrid orbital of the central atom.

The Correct Answer and Explanation is :

Let’s analyze the molecules BeF₂, SO₃, and XeF₄ by addressing each part of your query:

a) Lewis Structures:

1. BeF₂ (Beryllium Fluoride):

• Valence Electrons: eryllium (Be) has 2 valence electrons, and each fluorine (F) atom has 7 valence electrons, totaling 16 valence electrons. – Structure: eryllium forms two single bonds with two fluorine atoms, utilizing all 16 valence electrons.

1. SO₃ (Sulfur Trioxide):

• Valence Electrons: ulfur (S) has 6 valence electrons, and each oxygen (O) atom has 6 valence electrons, totaling 24 valence electrons. – Structure: ulfur forms double bonds with each of the three oxygen atoms, resulting in a resonance structure where the double bonds are delocalized over the three O atoms.

1. XeF₄ (Xenon Tetrafluoride):

• Valence Electrons: enon (Xe) has 8 valence electrons, and each fluorine (F) atom has 7 valence electrons, totaling 36 valence electrons. – Structure: enon forms four single bonds with four fluorine atoms, with two lone pairs remaining on the xenon atom.
  b) VSEPR Geometry:

1. BeF₂:

• Electron Groups: wo bonding pairs and no lone pairs on the central atom. – Geometry: inear arrangement with a bond angle of 180°.

1. SO₃:

• Electron Groups: hree bonding pairs and no lone pairs on the central atom. – Geometry: rigonal planar arrangement with bond angles of 120°.

1. XeF₄:

• Electron Groups: our bonding pairs and two lone pairs on the central atom. – Geometry: quare planar arrangement with bond angles of 90° and 180°.
  c) Hybridization of the Central Atom:

1. BeF₂:

• Hybridization: p hybridization, resulting in a linear geometry.

1. SO₃:

• Hybridization: p² hybridization, leading to a trigonal planar geometry.

1. XeF₄:

• Hybridization: p³d² hybridization, corresponding to a square planar geometry.
  Explanation:
• BeF₂: eryllium, with an electron configuration of [He] 2s², has two valence electrons. In BeF₂, these electrons form two sigma bonds with fluorine atoms, resulting in a linear geometry due to sp hybridization.
• SO₃: ulfur, with an electron configuration of [Ne] 3s² 3p⁴, has six valence electrons. In SO₃, sulfur forms three double bonds with oxygen atoms, utilizing all six valence electrons. The molecule adopts a trigonal planar geometry with sp² hybridization, where each sp² hybrid orbital overlaps with an oxygen p orbital to form a sigma bond.
• XeF₄: enon, with an electron configuration of [Kr] 4d¹⁰ 5s² 5p⁶, has eight valence electrons. In XeF₄, xenon forms four sigma bonds with fluorine atoms and has two lone pairs. The molecule adopts a square planar geometry with sp³d² hybridization, where the d orbitals accommodate the lone pairs, and the sp³d² hybrid orbitals overlap with fluorine p orbitals to form sigma bonds.
  For a visual representation and further explanation of the Lewis structure and VSEPR geometry of XeF₄, you might find the following video helpful:

videoLewis Structure (+VSEPR) for XeF4turn0search5