To determine the best reason for the difference in properties between LiCl (Lithium Chloride) and [tex]\( C_6H_{14}O \)[/tex] (Hexanol), it’s important to consider their chemical nature.
1. Atomic Mass Difference: While LiCl and [tex]\( C_6H_{14}O \)[/tex] do have different atomic masses, this is not the most relevant factor when explaining the differences in their chemical properties. Atomic mass does not directly influence the type of bonding or the resultant properties of the compounds.
2. Periodic Table Groups: Although Cl (Chlorine) and O (Oxygen) belong to different groups of the periodic table, this is also not the primary reason for the different properties of LiCl and [tex]\( C_6H_{14}O \)[/tex]. The group memberships indeed influence their electron configurations and reactivities, but the compounds in question are more profoundly distinguished by their bonding types.
3. Ionic vs. Metallic Compound: This option suggests that one compound is ionic and the other is metallic. Lithium Chloride (LiCl) is indeed ionic, however, [tex]\( C_6H_{14}O \)[/tex] (Hexanol) is not metallic. Hexanol is an organic compound that is covalently bonded. Hence, describing [tex]\( C_6H_{14}O \)[/tex] as metallic is inaccurate.
4. Covalent vs. Ionic Compound: This option suggests that one compound is covalent and the other is ionic. This is the most accurate explanation. LiCl is an ionic compound, composed of lithium cations (Li⁺) and chloride anions (Cl⁻), which form a lattice structure due to electrostatic attraction. On the other hand, [tex]\( C_6H_{14}O \)[/tex] is a covalent compound where the atoms share electrons to form bonds, resulting in different intermolecular forces and properties compared to ionic compounds.
Given these explanations, the best reason for the difference in properties of LiCl and [tex]\( C_6H_{14}O \)[/tex] is:
One compound is covalent, and the other is ionic.
