The charges and sizes of the ions in an ionic compound affect the strength of the electrostatic attraction holding that compound together. based on ion charges and relative ion sizes, arrange these ionic compounds by their expected melting points. a. csbr b. srf2 c. rbf d. sro

SrF2>SrO>RbF>CsBr

Explanation:

Ionic solids have their melting points dependent on:

i) size of the the ion: the smaller the size of the ion, the more closely packed the ionic sphere will be and the greater the melting point.

ii) Charge on the ion, the  higher the charge on the ion the greater the electrostatic attraction between the ions and the greater the melting point.

In the arrangement above, the order of cation sizes are Sr2+<Rb+<Cs+

the order of anion sizes are F-<O2-<Br-

This explains the order of melting points given in the answer.

vanderwaal's forces of attraction are the electrostatic intermolecular forces that exist in a molecule due to the temporary or permanent dipoles that are developed in a molecule. in , the major intermolecular forces are dipole-dipole interactions as the molecule is polar (bent structure). so the vanderwaal's forces of interaction in between molecules are the permanent dipole-dipole interactions that develop due to the dipole that exists in between the polar h - s bond. the positively charged hydrogen atom is attracted towards the negative end of the dipole that is sulfur of the adjacent molecule. therefore, these forces of attraction are relatively stronger than that of london dispersion forces that exist in non polar molecules.

the answer is:  

line graphs show patterns in data with variables that change over time; whereas, circle graphs show data as parts out of a whole (such as out of 100%).