CS2 Lewis Structure

CS2 Lewis Structure

The Correct Answer and Explanation is :

The Lewis structure of carbon disulfide (CS₂) represents the arrangement of valence electrons in the molecule, illustrating how atoms are bonded and the distribution of lone pairs.

Steps to Draw the Lewis Structure of CS₂:

1. Determine the Total Number of Valence Electrons:

• Carbon (C) is in Group 14 of the periodic table, so it has 4 valence electrons.
• Sulfur (S) is in Group 16, so each sulfur atom has 6 valence electrons.
• Total valence electrons = 4 (from C) + 6 × 2 (from two S atoms) = 16 electrons.

1. Choose the Central Atom:

• Carbon is less electronegative than sulfur, making it the central atom.

1. Connect the Atoms with Single Bonds:

• Place carbon in the center with single bonds to each sulfur atom. Each single bond consists of 2 electrons, using up 4 electrons (2 bonds × 2 electrons per bond).

1. Distribute the Remaining Electrons as Lone Pairs:

• After forming the bonds, 12 electrons remain (16 total – 4 used in bonds).
• Distribute these electrons as lone pairs on the sulfur atoms. Each sulfur atom will have three lone pairs (6 electrons), totaling 12 electrons.

1. Convert Lone Pairs to Double Bonds to Satisfy the Octet Rule:

• Carbon needs 4 more electrons to complete its octet.
• Each sulfur atom can share one lone pair with carbon, forming a double bond.
• This conversion uses 4 electrons (2 electrons per double bond × 2 bonds), completing the octet for both carbon and sulfur atoms.

1. Verify the Structure:

• Each sulfur atom has two lone pairs and shares two electrons with carbon, satisfying the octet rule.
• Carbon shares four electrons with each sulfur atom, completing its octet.

Final Lewis Structure:

The Lewis structure of CS₂ is linear, with carbon in the center forming double bonds with each sulfur atom. Each sulfur atom has two lone pairs, and carbon has no lone pairs.

Hybridization and Molecular Geometry:

• Hybridization:
• The carbon atom undergoes sp hybridization, forming two sp hybrid orbitals that overlap with sulfur’s p orbitals to form sigma bonds. The remaining p orbitals on carbon overlap with p orbitals on sulfur to form pi bonds.
• Molecular Geometry:
• The molecule adopts a linear geometry with a bond angle of 180°, resulting from the sp hybridization of carbon.

Polarity:

CS₂ is a nonpolar molecule. Despite the polar bonds between carbon and sulfur, the linear geometry causes the dipoles to cancel out, resulting in no net dipole moment.

Understanding the Lewis structure of CS₂ provides insights into its chemical bonding, molecular geometry, and polarity, which are essential for predicting its chemical behavior and interactions.