Observing the trend of boiling points of the compounds listed, choose the appropriate terms to fit into the blanks: \begin{array}{lr} \text{Compound}& \text{boiling point}\\\hline \ce{H2Te} & −2\ ^{\circ}\mathrm{C}\\ \ce{H2Se} & −41.5\ ^{\circ}\mathrm{C}\\ \ce{H2S} & −60.7\ ^{\circ}\mathrm{C}\\ \ce{H2O} & 100\ ^{\circ}\mathrm{C}\\ \end{array} The ___ the compound, the stronger the __ present between molecules. The stronger the ___, the higher the boiling point of the compound?
More polar, smaller, London dispersion forces, larger, less polar, dipole-dipole and ion-dipole forces
I noticed that the electronegativity for each compound increases from top to bottom, so higher electronegativity = higher boiling point?
I've also tried putting more polar the compound, stronger the dipole-dipole & ion forces. No luck, I still got it wrong.