Arrange the following ionic compounds in order of increasing lattice energy. Exp

Question

Arrange the following ionic compounds in order of increasing lattice energy. Explain your answer. LiF, CsF, RbF, KF, MgO, SeN Based on the trends in first ionization energies which representative element Group IA and VIIA) would you expect to have the lowest ionization energy? The highest? Explain your choices The bromine monofluoride molecule, Brl, has a bond length of 1.78 A. Calculate the dipole moment, Debyes, that results if the charges on Br and F were 1^+ and 1^-; respectively. (1 Debye (D) = 3.34 times 10^30 C-m, 1 e^- = 1.6 times 10^-19 C), 1 A = 1 times 10^-80 m) (include the equation, not just numbers) If the experimentally measured dipole moment is 1.42 D, what is the magnitude (in units of e)of the charges on Br and F (Include the equation, not just numbers)

Explanation / Answer

7. arrangement of ionic compounds in terms of incresing lattice energy

RbF < KF < LiF < CaF2 < MgO < ScN

As the size becomes smaller, lattice energy increases. As the charge of ions goes up, lattice energy goes up.

8. Group IA are alkali metals which have one valence shell electron which tends to loose rather easily to attain an inert gas configuration. So ionization energy of Group IA is lower than group VIIA. The highest ionization energy would be seen for Group VIIA halogens which are one electron short in attaining inert gas configuration so ionization energies of these are extremely high.

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