Multiple Choice
How do lone electron pairs on the central atom affect the molecular shape of a molecule?
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12. Molecular Shapes & Valence Bond Theory
Molecular Geometry
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Which compound below is a polar molecule and has a linear molecular geometry?
A
N2
B
CO2
C
CO
D
C2H2
Verified step by step guidance1
Step 1: Understand the question asks for a molecule that is both polar and has a linear molecular geometry. This means the molecule must have a straight-line shape and an uneven distribution of charge (dipole moment).
Step 2: Analyze each molecule's geometry and polarity: N\_2 is linear but nonpolar because it consists of two identical atoms sharing electrons equally.
Step 3: CO\_2 is linear but nonpolar because the two polar C=O bonds are symmetrically opposite, canceling out the dipole moments.
Step 4: CO (carbon monoxide) is linear and polar because it has a triple bond between C and O with different electronegativities, resulting in a net dipole moment.
Step 5: C\_2H\_2 (acetylene) is linear but nonpolar because the molecule is symmetrical with identical C-H bonds on both ends, leading to no net dipole moment.
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