Final answer:
Sodium (a metal) and chlorine (a nonmetal) react to form the ionic compound sodium chloride (NaCl), which has a giant ionic lattice structure with alternating Na+ and Cl− ions held together by electrostatic forces. Ions in sodium chloride crystal lattice have oppositely charged neighbors, resulting in the compound's properties which are vastly different from its elemental constituents. A comparison table outlines the properties of sodium, chlorine, and sodium chloride
Step-by-step explanation:
Understanding Sodium Chloride Formation
The reaction between sodium and chlorine results in the formation of sodium chloride (NaCl), a compound with a giant ionic lattice structure.
a. Structures of Sodium and Chlorine
Pure sodium is a metal with a soft and silvery-white appearance, and chlorine is a nonmetal forming a yellow-green gas. Sodium and chlorine have atomic structures that enable sodium to lose an electron easily and chlorine to gain an electron, leading to the formation of Na+ cations and Cl− anions.
b. Ionic Bonding in Sodium Chloride
In sodium chloride, ions are held together by electrostatic attraction in a regular three-dimensional array known as a crystal lattice. Each sodium ion (Na+) is surrounded by six chloride ions (Cl−), and each chloride ion is similarly surrounded by six sodium ions.
c. Electron Arrangement in Ions
As a sodium ion, Na+ has lost its outermost electron, resulting in a stable electronic arrangement with a positive charge. Conversely, a chloride ion, Cl−, has gained an extra electron, completing its valence shell and resulting in a negative charge.
d. Comparative Properties Table
- Sodium: Soft, silvery-white metal, vigorous reaction with water and air.
- Chlorine: Yellow-green gas, corrosive, toxic.
- Sodium Chloride: White, crystalline, essential to life, dissolves in water without reacting vigorously.