Compare and contrast ionic, covalent, and metallic bonds with examples.

  • Ionic Bond:

    • Formation: Occurs when electrons are transferred from one atom to another, resulting in the formation of positive and negative ions.

    • Example: Sodium chloride (NaCl) is formed when sodium donates an electron to chlorine.

    • Properties: High melting and boiling points, electrical conductivity when dissolved in water or molten, usually soluble in water.

  • Covalent Bond:

    • Formation: Occurs when two atoms share electrons to achieve a stable electron configuration.

    • Example: Water (H₂O) is formed when oxygen shares electrons with two hydrogen atoms.

    • Properties: Lower melting and boiling points compared to ionic compounds, poor electrical conductivity, and may be soluble or insoluble in water depending on polarity.

  • Metallic Bond:

    • Formation: Occurs between metal atoms where electrons are delocalized over a lattice structure, forming a “sea of electrons.”

    • Example: Copper (Cu) and iron (Fe) form metallic bonds in their solid state.

    • Properties: High electrical and thermal conductivity, malleability, ductility, and high melting points.

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