Question

what is the best reason for the difference in properties of licl and c6h14o?
licl and c6h14o have different atomic masses.
cl and o belong to different groups of the periodic table.
one compound is ionic, and the other is metallic.
one compound is covalent, and the other is ionic.

Explanation:

• For the option "LiCl and \(C_6H_{14}O\) have different atomic masses": Atomic mass differences do not explain the fundamental property differences (like melting point, conductivity etc.) between an ionic and a covalent compound.
• For the option "Cl and O belong to different groups of the periodic table": While Cl (Group 17) and O (Group 16) are in different groups, this alone does not account for the property differences between \(LiCl\) (ionic) and \(C_6H_{14}O\) (covalent). The bonding type is more relevant.
• For the option "One compound is ionic, and the other is metallic": \(C_6H_{14}O\) is a covalent (organic) compound, not metallic. Metallic compounds have a sea - of - electrons model which is not applicable here.
• For the option "One compound is covalent, and the other is ionic": \(LiCl\) is an ionic compound (formed by the transfer of electrons from \(Li\) to \(Cl\), with strong electrostatic forces between ions). \(C_6H_{14}O\) is a covalent compound (formed by the sharing of electrons between \(C\), \(H\) and \(O\) atoms). The difference in bonding (ionic vs covalent) leads to significant differences in properties such as melting point (ionic compounds generally have high melting points, covalent compounds have relatively low melting points), solubility (ionic compounds often dissolve in polar solvents, covalent organic compounds may dissolve in non - polar solvents) and electrical conductivity (ionic compounds conduct electricity in molten or aqueous state, covalent compounds do not conduct electricity in general).

Answer:

One compound is covalent, and the other is ionic.