Dipole–dipole forces Transitional Reasoning Practice

Questions

1. 1.

   A student compares the physical properties of two triatomic compounds, carbon dioxide ($\text{CO}_2$) and sulfur dioxide ($\text{SO}_2$), to evaluate how molecular polarity influences intermolecular attractions. Although both compounds contain polar covalent bonds, sulfur dioxide condenses into a liquid at $-10^\circ\text{C}$ under normal atmospheric pressure, whereas carbon dioxide sublimes directly into a gas at $-78.5^\circ\text{C}$. Based on molecular structure and intermolecular forces, which statement correctly explains this difference in behavior?

   • A) $\text{CO}_2$ has a bent geometry that cancels its bond dipoles, preventing it from forming permanent dipole–dipole interactions.
   • B) Both substances possess net permanent dipoles, but $\text{SO}_2$ forms strong intermolecular hydrogen bonds between sulfur and oxygen atoms.
   • C) Dipole–dipole attractions in $\text{CO}_2$ are disrupted because oxygen is more electronegative than carbon, leading to repulsive electrostatic interactions.
   • D) $\text{SO}_2$ has a bent geometry with a net molecular dipole, allowing permanent dipole–dipole attractions that require more thermal energy to overcome than the dispersion forces in linear $\text{CO}_2$.

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