Describe the process of formation of NaCl with the help of electron dot structure.

The formation of sodium chloride (NaCl) can be explained using electron dot structures:

  • Step 1: Sodium (Na), an alkali metal, has one electron in its outermost shell (1s² 2s² 2p⁶ 3s¹). Chlorine (Cl), a halogen, has seven electrons in its outermost shell (1s² 2s² 2p⁶ 3s² 3p⁵).

  • Step 2: Sodium donates its single valence electron to chlorine, forming a Na⁺ ion (positively charged) and a Cl⁻ ion (negatively charged).

    • Na: Na → Na⁺ + e⁻ (Electron dot structure: Na → [Na]⁺)

    • Cl: Cl + e⁻ → Cl⁻ (Electron dot structure: Cl: [Cl]⁻)

  • Step 3: The electron transfer results in the formation of oppositely charged ions, Na⁺ and Cl⁻. These ions are held together by electrostatic attraction, forming an ionic bond and resulting in the compound NaCl.

Related Questions:

  1. Explain how elements attain stability.
  2. Describe the ways in which bonds may be formed.
  3. Describe the formation of a covalent bond between two non-metallic elements.
  4. Explain with examples single, double, and triple covalent bonds.
  5. Find the number of valence electrons in the following atoms using the periodic table:
  6. Represent the formation of cations for the following metal atoms using electron dot structures:
  7. A sample of sulfur from a volcano was analyzed to give the following composition of isotopes (Atomic No. of S = 16):
  8. An atom of an element has an atomic number of 9 and a mass number of 19:
  9. Define ionic bond and give an example.
  10. Compare and contrast ionic, covalent, and metallic bonds with examples.
  11. Explain the concept of hybridization and its role in molecular geometry.
  12. State octet and duplet rules.
  13. Explain the formation of a covalent bond between two nitrogen atoms.
  14. How does Al form a cation?
  15. Draw an electron cross and dot structure for an H₂O molecule.
  16. Describe the importance of noble gas electronic configuration.
  17. Why do noble gases not form bonds easily?
  18. Explain the difference between polar and non-polar covalent bonds.
  19. What is meant by bond energy, and how does it affect bond strength?
  20. How does electronegativity affect the type of bond formed between two atoms?