Question

your answer is incorrect.
decide what kind of crystalline solid each element or compound in the table forms, and what kind of force holds the
then, rank the solids in order of decreasing melting point. that is, select \1\ next to the solid with the highest meltin
highest melting point, and so on. (you may need to use the scrollbar to see all the choices.)

element or compound	type of solid formed	force holding the solid together	melting point of solid
$\ce{hocl}$	molecular	select	select

| $\ce{rh}$ | atomic\
ionic | select | select |

Explanation:

Step1: Analyze \( \ce{F2} \)

Fluorine (\( \ce{F2} \)) is a diatomic molecule composed of non - metal atoms. The type of solid it forms is a molecular solid. In molecular solids, the molecules are held together by intermolecular forces. For non - polar molecules like \( \ce{F2} \), the intermolecular force is London dispersion forces (also called van der Waals forces).

Step2: Analyze \( \ce{HOCl} \)

Hypochlorous acid (\( \ce{HOCl} \)) is a covalent compound made up of molecules. So, it forms a molecular solid. The molecules of \( \ce{HOCl} \) are polar (due to the difference in electronegativity between O and Cl, and O and H). The intermolecular forces holding \( \ce{HOCl} \) molecules together are dipole - dipole interactions (and also London dispersion forces, but dipole - dipole is the dominant intermolecular force for polar molecules in this case).

Step3: Analyze \( \ce{Rh} \)

Rhodium (\( \ce{Rh} \)) is a metal. Metals form metallic solids. In metallic solids, the metal atoms lose their valence electrons, and these electrons form a "sea of electrons" that holds the positively charged metal ions together. The force holding the metallic solid together is metallic bonding.

Step4: Rank by melting point

The strength of the forces holding the solid together determines the melting point. Metallic bonding (in \( \ce{Rh} \)) is generally stronger than dipole - dipole interactions (in \( \ce{HOCl} \)) and London dispersion forces (in \( \ce{F2} \)). Among molecular solids, dipole - dipole interactions (in \( \ce{HOCl} \)) are stronger than London dispersion forces (in \( \ce{F2} \)) because polar molecules have stronger intermolecular forces than non - polar molecules of similar molar mass. So, the order of decreasing melting point is: \( \ce{Rh} \) (metallic solid, metallic bonding) > \( \ce{HOCl} \) (molecular solid, dipole - dipole) > \( \ce{F2} \) (molecular solid, London dispersion forces).

For \( \ce{F2} \):

• Type of solid: molecular
• Force holding together: London dispersion forces

For \( \ce{HOCl} \):

• Force holding together: dipole - dipole interactions

For \( \ce{Rh} \):

• Type of solid: metallic
• Force holding together: metallic bonding

Answer:

For \( \ce{F2} \):

• Type of solid formed: molecular
• Force holding the solid together: London dispersion forces

For \( \ce{HOCl} \):

• Force holding the solid together: dipole - dipole interactions

For \( \ce{Rh} \):

• Type of solid formed: metallic
• Force holding the solid together: metallic bonding

Ranking (from highest to lowest melting point):

1. \( \ce{Rh} \)
2. \( \ce{HOCl} \)
3. \( \ce{F2} \)