Draw the Lewis Dot Structure for H2SO4 and Provide the Following Information: A) Number of Valence Electrons, B) Hybridization, C) Electron Geometry, D) Molecular Geometry, E) Polarity

To draw the Lewis dot structure for sulfuric acid (H₂SO₄), we start by determining the total number of valence electrons.

A) Number of Valence Electrons

In H₂SO₄:

• Hydrogen (H): 1 electron × 2 = 2 electrons
• Sulfur (S): 6 electrons
• Oxygen (O): 6 electrons × 4 = 24 electrons

Total = 2 + 6 + 24 = 32 valence electrons.

B) Hybridization

The sulfur atom in H₂SO₄ undergoes hybridization to form four sp³ orbitals that accommodate its bonding pairs and lone pairs. There are no lone pairs on sulfur in this structure, making it sp³ hybridized.

C) Electron Geometry

The arrangement of the electron pairs around the sulfur atom is tetrahedral. This is due to the four regions of electron density (two single bonds with hydrogen and two double bonds with oxygen).

D) Molecular Geometry

Despite having a tetrahedral electron geometry, the molecular geometry is considered to be tetrahedral too since there are no lone pairs on the sulfur atom. The angles around sulfur are approximately 109.5 degrees.

E) Polarity

H₂SO₄ is a polar molecule. The difference in electronegativity between sulfur and oxygen creates polar bonds. Additionally, the symmetrical shape helps maintain the overall polarity, as the dipoles do not cancel out completely.

This gives us a comprehensive understanding of the Lewis dot structure of H₂SO₄ along with its valence electrons, hybridization, electron geometry, molecular geometry, and polarity.