which of the following statements are supported by the data? select all that apply.
the compounds in which bromine bonds with a metal have lower melting points than the compounds in which bromine bonds with a nonmetal.
the compound with the lowest melting point is made up of molecules held together by intermolecular attractions.
the melting point of cbr4 suggests that it can be classified as an ionic compound.
all of the compounds exist in the gas state at -100°c.
it takes more energy to overcome the attractive forces between particles of solid libr than it does to overcome the attractive forces between particles of solid pbr3.
the compound with the highest melting point is made up of ions held together by ionic bonds.

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# Brief Explanations:
- **Ionic vs. Molecular Compounds**: Ionic compounds (formed between metals and non - metals) generally have higher melting points due to strong ionic bonds. Molecular compounds (formed between non - metals) have lower melting points as they are held together by weaker intermolecular forces.
- **Analysis of Options**:
    - **Option 1 (The compound with the highest melting point is made up of ions held together by ionic bonds)**: Looking at the melting points, $MgBr_2$ has the highest melting point ($711^{\circ}C$). $Mg$ is a metal and $Br$ is a non - metal, so $MgBr_2$ is an ionic compound. This statement is correct.
    - **Option 2 (It takes more energy to overcome the attractive forces between particles of solid $LiBr$ than it does to overcome the attractive forces between particles of solid $PBr_3$)**: $LiBr$ (melting point $550^{\circ}C$) is ionic ($Li$ is a metal, $Br$ is a non - metal), and $PBr_3$ (melting point $- 41^{\circ}C$) is molecular ($P$ and $Br$ are non - metals). Higher melting points mean more energy is required to overcome the forces. So, this statement is correct.
    - **Option 3 (The compounds in which bromine bonds with a non - metal have lower melting points than the compounds in which bromine bonds with a metal)**: Non - metal - non - metal (molecular) compounds ($HBr$, $PBr_3$, $CBr_4$) have lower melting points ($-87^{\circ}C$, $-41^{\circ}C$, $91^{\circ}C$) compared to metal - non - metal (ionic) compounds ($AgBr$, $LiBr$, $MgBr_2$) which have higher melting points ($432^{\circ}C$, $550^{\circ}C$, $711^{\circ}C$). This statement is correct.
    - **Option 4 (The compound with the lowest melting point is made up of molecules held together by intermolecular attractions)**: $PBr_3$ has the lowest melting point ($-41^{\circ}C$) and is molecular (intermolecular forces). This statement is correct.
    - **Option 5 (The melting point of $CBr_4$ suggests that it can be classified as an ionic compound)**: $CBr_4$ (melting point $91^{\circ}C$) is molecular ($C$ and $Br$ are non - metals). Ionic compounds have much higher melting points. So, this statement is incorrect.
    - **Option 6 (All of the compounds exist in the gas state at $-100^{\circ}C$)**: $MgBr_2$ ($711^{\circ}C$), $LiBr$ ($550^{\circ}C$), $AgBr$ ($432^{\circ}C$) have melting points much higher than $-100^{\circ}C$, so they will be solids. This statement is incorrect.

# Answer:
The correct statements are:
- The compound with the highest melting point is made up of ions held together by ionic bonds.
- It takes more energy to overcome the attractive forces between particles of solid $LiBr$ than it does to overcome the attractive forces between particles of solid $PBr_3$.
- The compounds in which bromine bonds with a non - metal have lower melting points than the compounds in which bromine bonds with a metal.
- The compound with the lowest melting point is made up of molecules held together by intermolecular attractions.

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