Final answer:
The Lewis structure of carbon dioxide (CO₂) includes a central carbon atom with two double bonds to two oxygen atoms, with each oxygen having two lone pairs. The linear molecular geometry is a result of the two bonding pairs arranged 180° apart, following the VSEPR theory.
Step-by-step explanation
The Lewis structure of carbon dioxide (CO₂) shows the carbon atom in the center with two double bonds connecting it to two oxygen atoms. In the Lewis dot structure, carbon does not have any lone pairs, and each oxygen atom has two lone pairs. These double bonds represent shared pairs of valence electrons between carbon and oxygen atoms.
VSEPR theory explains that with two bonding pairs, the molecular geometry of CO₂ is linear, which is reflected in the structure. The lack of lone pairs on the carbon atom in the Lewis structure promotes this linear shape, as there are no lone pair repulsions to alter the arrangement of the electron groups around the carbon atom.
Illustrating a double bond in the Lewis notation, each oxygen atom is connected to the carbon atom by two lines, signifying four shared electrons, or two electron pairs, forming a strong covalent bond. This arrangement minimizes the repulsion between the electron groups (the bonding pairs), leading to the linear molecular geometry of CO₂.