To determine the best reason for the difference in properties between LiCl and [tex]\( C_6H_{14}O \)[/tex], we need to consider the nature of the chemical bonding in each compound:
1. LiCl (Lithium Chloride):
- Lithium (Li) is a metal, and Chlorine (Cl) is a non-metal.
- When these elements combine, Li donates one electron to Cl, forming Li⁺ and Cl⁻ ions.
- The electrostatic attraction between the positively charged Li⁺ ion and the negatively charged Cl⁻ ion results in an ionic bond.
- Ionic compounds, such as LiCl, generally have high melting and boiling points, conduct electricity when molten or dissolved in water, and are typically soluble in water.
2. [tex]\( C_6H_{14}O \)[/tex] (Hexanol):
- This molecule contains carbon (C), hydrogen (H), and oxygen (O), all of which are non-metals.
- The bonds within hexanol are covalent; electrons are shared rather than transferred.
- Covalent compounds, like [tex]\( C_6H_{14}O \)[/tex], generally have lower melting and boiling points compared to ionic compounds, do not conduct electricity, and their solubility varies depending on the specific nature of the covalent bonds (e.g., polarity).
Considering these points, the disparity in their properties can be attributed to the fundamentally different types of bonding:
- Ionic Bonding in LiCl:
- Results from the transfer of electrons and the resulting electrostatic attraction between ions.
- Covalent Bonding in [tex]\( C_6H_{14}O \)[/tex]:
- Involves the sharing of electrons and lack of charged particles.
Therefore, the best reason for the difference in properties between LiCl and [tex]\( C_6H_{14}O \)[/tex] is:
One compound is covalent, and the other is ionic.
So, the correct answer is:
One compound is covalent, and the other is ionic.
