NaCl is an example of

Ionic solid

NaCl, or sodium chloride, is a classic example of an ionic compound. To understand why, let's break down the key concepts behind the formation of ionic compounds.

Ionic Bond Formation

An ionic compound is formed when atoms of metals and non-metals transfer electrons. This transfer leads to the formation of charged particles called ions. In the case of NaCl:

• Sodium (Na), a metal, loses an electron to form a positively charged ion (Na⁺).
• Chlorine (Cl), a non-metal, gains this electron to form a negatively charged ion (Cl⁻).

The oppositely charged ions (Na⁺ and Cl⁻) are held together by strong electrostatic forces of attraction, known as ionic bonds. This bond forms the crystal lattice structure of NaCl.

Structure and Properties of NaCl

• Crystal Lattice: In NaCl, the Na⁺ and Cl⁻ ions are arranged in a regular, repeating pattern that forms a three-dimensional lattice. This structure is highly stable due to the strong Coulombic forces of attraction between the positive and negative ions.
• High Melting and Boiling Points: The ionic bonds in NaCl are strong, requiring a large amount of energy to break the bonds. As a result, NaCl has high melting and boiling points.
• Electrical Conductivity: When dissolved in water or melted, NaCl conducts electricity. This happens because the ions become free to move, allowing the flow of electrical current.
• Solubility in Water: NaCl is highly soluble in water. The polar water molecules surround the Na⁺ and Cl⁻ ions, separating and dissolving them.

NaCl is an ionic compound because it is made up of ions (Na⁺ and Cl⁻) that are held together by strong electrostatic forces. This ionic bond gives NaCl its characteristic properties, such as high melting points and electrical conductivity when in molten or aqueous form.