Molecular geometry determines if a molecule is linear. VSEPR theory states that electron pair repulsion (bond pairs and lone pairs around the central atom) dictates this geometry.
Analysis of each molecule:
H2O: Oxygen, bonded to two hydrogens and possessing two lone pairs, results in a bent shape due to electron repulsion, not linear.
CO2: Carbon, double-bonded to two oxygens with no lone pairs, exhibits a linear shape due to symmetrical bond distribution.
NH3: Nitrogen, bonded to three hydrogens and having one lone pair, forms a trigonal pyramidal shape, not linear.
SO2: Sulfur, bonded to two oxygens and possessing a lone pair, adopts a bent shape, not linear.
Therefore, CO2 is the linear molecule.
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