Which of the following would you expect to show dispersion forces? Dipole forces? (a) \(\mathrm{GeBr}_{4}\) (b) \(\mathrm{C}_{2} \mathrm{H}_{2}\) (c) \(\mathrm{HF}(g)\) (d) \(\mathrm{TeCl}_{2}\)

We will analyze the molecular structure and electronegativity differences of each compound to determine its polar or nonpolar status: (a) \(\mathrm{GeBr}_{4}\): GeBr4 is a tetrahedral molecule with equal electronegativity distribution, making it nonpolar. (b) \(\mathrm{C}_{2} \mathrm{H}_{2}\): C2H2 is a linear molecule with the triple bond between the two carbon atoms and hydrogen atoms at the ends. The electronegativity difference between carbon and hydrogen is small, making the molecule nonpolar. (c) \(\mathrm{HF}(g)\): HF is a diatomic molecule with a significant electronegativity difference between hydrogen and fluorine, making it polar. (d) \(\mathrm{TeCl}_{2}\): TeCl2 is a bent molecule with an electronegativity difference between tellurium and chlorine, making it polar.

Now we will identify the intermolecular forces present in each compound: (a) \(\mathrm{GeBr}_{4}\): Since GeBr4 is nonpolar, it has only dispersion forces present. (b) \(\mathrm{C}_{2} \mathrm{H}_{2}\): Since C2H2 is nonpolar, it has only dispersion forces present. (c) \(\mathrm{HF}(g)\): Since HF is a polar molecule, it exhibits dipole forces. However, it does not show dispersion forces since it's a gas. (d) \(\mathrm{TeCl}_{2}\): Since TeCl2 is a polar molecule, it exhibits dipole forces. Additionally, it also shows dispersion forces because it is non-gaseous and all molecules possess some degree of dispersion forces. In summary: (a) \(\mathrm{GeBr}_{4}\): Dispersion forces only. (b) \(\mathrm{C}_{2} \mathrm{H}_{2}\): Dispersion forces only. (c) \(\mathrm{HF}(g)\): Dipole forces only. (d) \(\mathrm{TeCl}_{2}\): Dipole forces and dispersion forces.