To understand why \( \text{LiCl} \) and \( \text{C}_6 \text{H}_{14} \text{O} \) have different properties, let's first examine their chemical nature and bonding.
1. Lithium Chloride (\( \text{LiCl} \)):
- Chemical composition: Lithium chloride consists of lithium (Li) and chlorine (Cl).
- Bonding: Lithium (Li), a metal, loses an electron to become \( \text{Li}^+ \), and chlorine (Cl), a non-metal, gains an electron to become \( \text{Cl}^- \). The electrostatic attraction between \( \text{Li}^+ \) and \( \text{Cl}^- \) ions forms an ionic bond.
- Properties: As an ionic compound, \( \text{LiCl} \) typically has high melting and boiling points, and it conducts electricity when molten or dissolved in water (as it dissociates into ions).
2. Hexanol (\( \text{C}_6 \text{H}_{14} \text{O} \)):
- Chemical composition: Hexanol is an organic compound consisting of carbon (C), hydrogen (H), and oxygen (O).
- Bonding: Hexanol features covalent bonds where electrons are shared between carbon, hydrogen, and oxygen atoms. The structure entails a carbon backbone with hydrogen atoms and a single hydroxyl group (OH) attached.
- Properties: As a covalent compound, hexanol typically has lower melting and boiling points compared to ionic compounds and does not conduct electricity in its pure form.
Given these details, the best reason for the difference in properties between \( \text{LiCl} \) and \( \text{C}_6 \text{H}_{14} \text{O} \) is related to the type of bonding and the resulting structural and physical properties.
Therefore, the correct option is:
- One compound is covalent, and the other is ionic.
This explains the fundamental reason for their differing properties.
