Question

licl(s)
electrostatic attraction
ccl₄(s)
electron cloud
an ionic
covalent bond
electrostatic repulsion
ar(s)
ch₃oh(s)
a molecular
an atomic
match the items in the left column to the appropriate blanks in the sentence on the right.
among ar(s), ccl₄(s), licl(s), and ch₃oh(s),
will have the highest melting
point because it is
compound that tends to have a strong
in solids
reset
help

Explanation:

Step1: Analyze the types of solids

• LiCl(s): It is an ionic compound. Ionic compounds have strong electrostatic attractions (ionic bonds) between ions. These strong forces result in relatively high melting points compared to molecular solids.
• CCl₄(s): It is a non - polar molecular solid. The intermolecular forces in non - polar molecular solids are London dispersion forces (weak forces due to temporary electron cloud distortions).
• Ar(s): It is an atomic solid (a noble gas solid). The only intermolecular forces are London dispersion forces (very weak as Ar atoms have a stable electron configuration and small electron clouds).
• CH₃OH(s): It is a polar molecular solid. It has hydrogen bonding (a relatively strong type of dipole - dipole interaction in addition to London dispersion forces).

Step2: Compare melting points based on intermolecular/intramolecular forces

• Ionic compounds (LiCl) generally have higher melting points than molecular solids (CCl₄, Ar, CH₃OH) because ionic bonds (electrostatic attractions between ions) are stronger than the intermolecular forces in molecular solids.
• Among the molecular solids, CH₃OH has hydrogen bonding (stronger than the London dispersion forces in CCl₄ and Ar). CCl₄ has stronger London dispersion forces than Ar (because CCl₄ has more electrons, so more polarizable electron cloud).

Answer:

Among \(Ar(s)\), \(CCl_{4}(s)\), \(LiCl(s)\), and \(CH_{3}OH(s)\), \(LiCl(s)\) will have the highest melting point because it is an ionic compound that tends to have strong electrostatic attraction in solids.