Let's analyze the compounds given: LiCl (Lithium Chloride) and [tex]\( \text{C}_6\text{H}_{14}\text{O} \)[/tex] (Hexanol).
1. Atomic Masses:
While the difference in atomic masses of the elements making up LiCl and [tex]\( \text{C}_6\text{H}_{14}\text{O} \)[/tex] (Carbon, Hydrogen, and Oxygen) could contribute to differences in properties, this factor alone does not sufficiently explain the distinct behaviors in chemistry and physical properties.
2. Periodic Table Groups:
Although Chlorine (Cl) and Oxygen (O) belong to different groups in the periodic table, this distinction is not the main reason for the significant differences in properties between LiCl and [tex]\( \text{C}_6\text{H}_{14}\text{O} \)[/tex]. This group difference alone does not account for all the contrasting properties observed.
3. Chemical Bonds - Ionic vs. Metallic:
One of the compounds being ionic and the other metallic is not applicable. Hexanol ([tex]\( \text{C}_6\text{H}_{14}\text{O} \)[/tex]) is not a metallic compound. This option can be dismissed.
4. Chemical Bonds - Covalent vs. Ionic:
This is the most accurate explanation. LiCl is an ionic compound, meaning it is formed by the electrostatic attraction between oppositely charged ions (Li[tex]\(^+\)[/tex] and Cl[tex]\(^-\)[/tex]). Ionic compounds typically have high melting and boiling points, and they conduct electricity when dissolved in water.
On the other hand, [tex]\( \text{C}_6\text{H}_{14}\text{O} \)[/tex] is a covalent compound. Covalent compounds are formed by the sharing of electron pairs between atoms. These types of compounds generally have lower melting and boiling points compared to ionic compounds and do not conduct electricity in water.
Thus, the best reason for the difference in properties between LiCl and [tex]\( \text{C}_6\text{H}_{14}\text{O} \)[/tex] is that one compound is covalent, and the other is ionic. The correct answer is:
One compound is covalent, and the other is ionic.
