The Alkaline Metal Cations that the more likely to be more soluble are the ones that are: [HIGHER or LOWER] on the periodic table. The Halogens that the more likely to have a stronger (more negative) electron affinity are the ones that are: [HIGHER or LOWER] on the periodic table.

What process is illustrated by the following figure? Explain how that can occur

#17 Please describe the property of electronegativity and relate this property to ionization energy, discussing the nature and trends which occur in each. Just a brief explanation thanks.

Place the following compounds in order of increasing lattice energy (from smallest to largest):  LiF, LiBr, NaI, MgF2, MgO.

How does the acidity of the binary acid of an element vary as a function of the electronegativity of the element?  How does this relate to the position of the element in the periodic table?

Arrange the following in order of increasing radius and increasing ionization energy.a. N+, N, N-b. Se, Se- , Cl, Cl+c. Br- , Rb+ , Sr2+

Calculate the lattice energy of KCI(s) using the following thermodynamic data (all data is in kJ/mol) K(s) AHsublimation = 69 kJ/mol K(g) Ionization energy = 399 kJ/mol CI-CI(g) Bond energy = 223 kJ/mol Cl(g) Electron affinity = -369 kJ/mol KCI(s) AH°r= -457 kJ/mol kJ/mol