Question

what intermolecular forces can co₂ exhibit with similar molecules?
o=c=o
only dispersion forces
dispersion forces, dipole-dipole, and hydrogen bonds
only hydrogen bonding
only dispersion and dipole-dipole forces

Explanation:

1. First, analyze the molecular structure of \( \ce{CO2} \). The Lewis structure shows it is a linear molecule (\( \text{O}=\text{C}=\text{O} \)) with a symmetrical arrangement.
2. For a molecule to have a permanent dipole (dipole - dipole forces), it must be polar. In \( \ce{CO2} \), the electronegativity difference between \( \text{C} \) and \( \text{O} \) creates bond dipoles, but due to the linear and symmetrical structure, these bond dipoles cancel each other out. So, \( \ce{CO2} \) is a non - polar molecule.
3. Hydrogen bonding requires a hydrogen atom bonded to a highly electronegative atom (F, O, or N) and another electronegative atom to which the hydrogen can be attracted. \( \ce{CO2} \) has no hydrogen atoms, so it cannot form hydrogen bonds.
4. Dispersion forces (London dispersion forces) are present in all molecules, including non - polar ones, because they arise from temporary fluctuations in electron distribution, creating temporary dipoles. Since \( \ce{CO2} \) is non - polar, the only intermolecular force it can exhibit with similar (non - polar \( \ce{CO2} \)) molecules is dispersion forces.

Answer:

A. only dispersion forces