Describe the formation of a covalent bond between two non-metallic elements.

The formation of a covalent bond between two non-metallic elements involves the sharing of electrons between atoms. Non-metals typically have relatively high electronegativity, meaning they tend to attract electrons strongly. In order to achieve a stable electron configuration (often resembling that of the nearest noble gas), atoms of non-metals will share their outermost electrons to fill their valence shells.

For example, let’s take the formation of a covalent bond between two chlorine (Cl) atoms:

  • Each chlorine atom has 7 valence electrons, as it is in Group 17 of the periodic table.

  • In order to complete their octet, two chlorine atoms will share one pair of electrons, with each chlorine contributing one electron to the shared pair.

  • This shared electron pair forms a single covalent bond, denoted as Cl-Cl.

The result is that both chlorine atoms achieve a stable electron configuration, each having 8 electrons in their valence shell, which is a stable configuration similar to that of argon (a noble gas). This kind of bond, formed by the sharing of electrons, is called a covalent bond.

In the case of a double bond or triple bond, the same principles apply, but more pairs of electrons are shared between the atoms. For instance, in an oxygen molecule (O₂), the two oxygen atoms share two pairs of electrons, resulting in a double bond. The key concept in covalent bonding is that the atoms share electrons to achieve a full valence shell, which gives them greater stability.

Related Questions:

  1. Explain the formation of a covalent bond between two nitrogen atoms.
  2. Explain how elements attain stability.
  3. Describe the ways in which bonds may be formed.
  4. State octet and duplet rules.
  5. How does Al form a cation?
  6. Draw an electron cross and dot structure for an H₂O molecule.
  7. Describe the importance of noble gas electronic configuration.
  8. Why do gases have neither a definite shape nor a definite volume?
  9. The electronic configurations listed below are incorrect. Explain the mistakes in each and write the correct electronic configurations.
  10. Which orbital in each of the following pairs is lower in energy?
  11. Draw Bohr’s Model for the following atoms, indicating the locations of electrons, protons, and neutrons:
  12. Write the electronic configuration for the following elements:
  13. State the importance and uses of isotopes in various fields of life.
  14. The atomic number of an element is 23, and its mass number is 56.
  15. The atomic symbol of aluminum is written as Al. What information do you get from it?
  16. Write the valence shell electronic configuration of an element present in the 3rd period and Group IIA.
  17. Define halogens.
  18. Which atom has a higher shielding effect, Li or Na?
  19. Explain why Na has higher ionization energy than K.
  20. Alkali metals belong to the S-block in the periodic table. Why?