Understanding Melting Point
Melting point is the temperature at which a solid transitions into a liquid. The stronger the intermolecular forces holding the molecules together, the higher the melting point.
Intermolecular Forces
* London Dispersion Forces: Present in all molecules, but weakest. Increase with molecular size.
* Dipole-Dipole Forces: Occur between polar molecules (molecules with uneven electron distribution). Stronger than London dispersion forces.
* Hydrogen Bonding: A special type of dipole-dipole interaction involving hydrogen bonded to a highly electronegative atom (like oxygen, nitrogen, or fluorine). The strongest type of intermolecular force.
Analyzing the Compounds
* C2H6 (Ethane): Nonpolar, only London dispersion forces.
* Cl2 (Chlorine): Nonpolar, only London dispersion forces.
* AsCl3 (Arsenic Trichloride): Polar, has dipole-dipole forces (and weaker London dispersion forces).
* Ne (Neon): A noble gas, only very weak London dispersion forces.
* Ver (Not a known compound): We can't assess this.
Determining the Highest Melting Point
* AsCl3 will have the highest melting point because it has the strongest intermolecular forces (dipole-dipole).
In Summary:
The compound with the highest melting point is AsCl3 (Arsenic Trichloride) due to its polar nature and the presence of dipole-dipole interactions.
