Without using tabulated numerical values, consider the following bonds: Li–F, Cs–F, and N–O.
(a) Using periodic trends in electronegativity, order the three bonds from greatest to least ionic character. Explain your reasoning.
(b) For the bond you placed in the middle of your ranking, describe the qualitative distribution of electron density between the two atoms and indicate the direction of any bond dipole.
(c) Explain why comparing metallic versus non-metallic elements can sometimes be a more reliable indicator of bond type than relying solely on ΔEN thresholds.