Identify the type of solid for AgCl, networking atomic solid ionic solid nonbonding atomic solid metallic atomic solid molecular solid
The Correct Answer and Explanation is:
Correct answer: Ionic solid
Explanation:
Silver chloride (AgCl) is classified as an ionic solid. This classification is based on the nature of the bonding and the structure of the compound.
AgCl consists of silver ions (Ag⁺) and chloride ions (Cl⁻) arranged in a crystal lattice. In an ionic solid, the particles are positive and negative ions held together by strong electrostatic forces known as ionic bonds. These bonds form when one atom transfers electrons to another, resulting in oppositely charged ions that attract each other. In AgCl, silver loses one electron to become Ag⁺, and chlorine gains that electron to become Cl⁻. The resulting attraction between these ions forms a stable solid structure.
Properties that support AgCl being an ionic solid:
- High melting point: Ionic solids have high melting points due to the strong attraction between ions. AgCl has a melting point of about 455 °C.
- Brittleness: When an ionic solid like AgCl is struck, layers of ions shift. Like charges may end up next to each other, causing the solid to shatter.
- Electrical conductivity: AgCl does not conduct electricity in its solid form because the ions are fixed in place. However, when melted or dissolved in water, the ions are free to move, allowing the substance to conduct electricity.
- Solubility in water: Many ionic compounds, including AgCl (though only slightly soluble), can dissolve in water, forming hydrated ions.
AgCl is not a molecular solid, because it is not made of neutral molecules held by intermolecular forces. It is also not a metallic solid, since it lacks a sea of delocalized electrons. It is not a covalent network solid, which involves atoms joined by a continuous network of covalent bonds. Lastly, it is not a nonbonding atomic solid, as those are typically made of noble gases with very weak dispersion forces.
