Question

what is the predominant intermolecular force in cbr₄?
a) hydrogen bonding
b) dipole - dipole forces
c) ion - dipole forces
d) london dispersion forces

Explanation:

• Hydrogen bonding: Occurs when \(H\) is bonded to \(N\), \(O\), or \(F\). \(CBr_4\) has no \(H\) atoms, so this is not applicable.
• Dipole - dipole forces: Require a polar molecule. \(CBr_4\) has a symmetrical tetrahedral structure (\(C\) in the center, \(Br\) atoms at the vertices). The bond dipoles cancel out, making \(CBr_4\) non - polar. So, dipole - dipole forces are not present.
• Ion - dipole forces: Need ions and polar molecules. \(CBr_4\) is a neutral non - polar molecule, so no ion - dipole forces.
• London dispersion forces: Present in all molecules. Since \(CBr_4\) has no hydrogen bonding, dipole - dipole, or ion - dipole forces, London dispersion forces are the predominant intermolecular force.

Answer:

d) london dispersion forces