Question

complete the following table. identify the type of bonding in each substance. click on the radio button identifying the substance with the highest melting point.

substance	bonding	highest melting point
$ccl_{4}$	select
$alcl_{3}$	select
$cf_{4}$	select

Explanation:

Step1: Analyze $S_8$

$S_8$ is a molecular solid. The sulfur - sulfur bonds within the $S_8$ molecule are covalent, and the intermolecular forces between $S_8$ molecules are London - dispersion forces.

Step2: Analyze $CCl_4$

$CCl_4$ is a molecular compound. The carbon - chlorine bonds are covalent, and the intermolecular forces are London - dispersion forces due to its non - polar nature.

Step3: Analyze $AlCl_3$

$AlCl_3$ is a covalent compound in the gas phase and exists as a dimer $Al_2Cl_6$. In the solid, it has some ionic character due to the polarization of the chloride ions by the aluminum ion, but it is mainly covalent with relatively weak intermolecular forces.

Step4: Analyze $CF_4$

$CF_4$ is a molecular compound. The carbon - fluorine bonds are covalent, and the intermolecular forces are London - dispersion forces as it is non - polar.

Step5: Compare melting points

Among these molecular substances, the melting point is related to the strength of the intermolecular forces. The strength of London - dispersion forces increases with the molar mass. The molar mass of $S_8$ ($M = 8\times32\ g/mol=256\ g/mol$), $CCl_4$ ($M=(12 + 4\times35.5)\ g/mol = 154\ g/mol$), $AlCl_3$ ($M=(27+3\times35.5)\ g/mol=133.5\ g/mol$), $CF_4$ ($M=(12 + 4\times19)\ g/mol = 88\ g/mol$). Since $S_8$ has the highest molar mass among them, it has the strongest London - dispersion forces and thus the highest melting point.

Answer:

Substance	Bonding	Highest Melting Point
$CCl_4$	Covalent (intramolecular), London - dispersion (intermolecular)
$AlCl_3$	Covalent (predominantly, with some ionic character), weak intermolecular forces
$CF_4$	Covalent (intramolecular), London - dispersion (intermolecular)